C4660 Physical Chemistry I

Faculty of Science
Spring 2025
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
In-person direct teaching
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
prof. RNDr. Jan Hrbáč, Ph.D. (seminar tutor)
Mgr. Jakub Nagy (seminar tutor)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
A mathematics course within the scope of the first semester of bachelor study programs in chemistry, biochemistry, biophysics or environmental studies.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 42 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
The subject consists of 14 lectures. With them, the presentations are only supplementary material, the most important thing is the oral interpretation with notes on the virtual board. Teachers use colored pens (black, red, blue, green, and orange), and having a similar range of colors available for notes is useful. Attendance at lectures is optional. However, practice shows that attending lectures significantly increases the probability of success or getting a good grade on an exam.
Assessment methods
Final written test lasting 110 minutes. It contains mostly open theoretical questions and calculation tasks. The minimum required score for successful completion is 60% points. Voluntary oral re-examination allows the grade to be improved by 1, exceptionally by 2 grades.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
Listed among pre-requisites of other courses
Teacher's information
Course C3150 Physical Chemistry I - seminar is strongly recommended as a significant aid to the successful completion of course C4660.
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024.

C4660 Physical Chemistry I

Faculty of Science
Spring 2024
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
prof. RNDr. Jan Hrbáč, Ph.D. (seminar tutor)
Mgr. Jakub Nagy (seminar tutor)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Mon 19. 2. to Sun 26. 5. Tue 16:00–17:50 B11/132
Prerequisites
A mathematics course within the scope of the first semester of bachelor study programs in chemistry, biochemistry, biophysics or environmental studies.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 42 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
The subject consists of 14 lectures. With them, the presentations are only supplementary material, the most important thing is the oral interpretation with notes on the virtual board. Teachers use colored pens (black, red, blue, green, and orange), and having a similar range of colors available for notes is useful. Attendance at lectures is optional. However, practice shows that attending lectures significantly increases the probability of success or getting a good grade on an exam.
Assessment methods
Final written test lasting 110 minutes. It contains mostly open theoretical questions and calculation tasks. The minimum required score for successful completion is 60% points. Voluntary oral re-examination allows the grade to be improved by 1, exceptionally by 2 grades.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
Teacher's information
Course C3150 Physical Chemistry I - seminar is strongly recommended as a significant aid to the successful completion of course C4660.
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2025.

C4660 Physical Chemistry I

Faculty of Science
Spring 2023
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
doc. Mgr. Ondřej Klíma, Ph.D. (assistant)
prof. Mgr. Petr Hasil, Ph.D. (assistant)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 16:00–17:50 B11/132
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of chemistry, biochemistry, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 42 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2024, Spring 2025.

C4660 Physical Chemistry I

Faculty of Science
Spring 2022
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
prof. RNDr. Jan Hrbáč, Ph.D. (seminar tutor)
RNDr. Erik Kalla (seminar tutor)
Mgr. Milan Říha (seminar tutor)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 16:00–17:50 B11/132
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of chemistry, biochemistry, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 42 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2023, Spring 2024, Spring 2025.

C4660 Physical Chemistry I

Faculty of Science
Spring 2021
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Mon 1. 3. to Fri 14. 5. Tue 14:00–15:50 B11/206
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of chemistry, biochemistry, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 42 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Physical Chemistry I

Faculty of Science
Spring 2020
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
prof. RNDr. Jan Hrbáč, Ph.D. (seminar tutor)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
Mgr. Jakub Stošek, Ph.D. (seminar tutor)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 16:00–17:50 B11/132
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of biochemistry, chemistry, biology, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 42 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2019
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
Mgr. Jakub Stošek, Ph.D. (seminar tutor)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Mon 18. 2. to Fri 17. 5. Tue 16:00–17:50 B11/132
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of biochemistry, chemistry, biology, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
spring 2018
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
Mgr. Jakub Stošek, Ph.D. (seminar tutor)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 16:00–17:50 B11/132
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of biochemistry, chemistry, biology, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2017
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
doc. Mgr. Dominik Heger, Ph.D. (lecturer)
prof. RNDr. Jan Hrbáč, Ph.D. (lecturer)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Mon 20. 2. to Mon 22. 5. Tue 16:00–17:50 B11/132
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of biochemistry, chemistry, biology, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2016
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
doc. Mgr. Dominik Heger, Ph.D. (alternate examiner)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (alternate examiner)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 16:00–17:50 B11/132
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-45; B: 44-40; C: 39-35; D: 34-30; E: 29-25; F: 24-0 points; P: 50-20; N: 19-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2015
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 17:00–18:50 B11/132
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-45; B: 44-40; C: 39-35; D: 34-30; E: 29-25; F: 24-0 points; P: 50-20; N: 19-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2014
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Thu 12:00–13:50 B11/132
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-45; B: 44-40; C: 39-35; D: 34-30; E: 29-25; F: 24-0 points; P: 50-20; N: 19-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
Study Materials
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2013
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 11:00–12:50 B11/132
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-45; B: 44-40; C: 39-35; D: 34-30; E: 29-25; F: 24-0 pints; P: 50-20; N: 19-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2012
Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 11:00–12:50 B11/132
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 41 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2011
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Wed 16:00–17:50 B11/132
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P; DE PAULA, Julio. Atkins' physical chemistry. 9th ed. Oxford : Oxford Univ. Press, 2010. 972 s. ISBN 9780199543373
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2011; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
    not specified
  • ATKINS, P. W. The elements of physical chemistry. 3rd ed. Oxford: Oxford University Press, 2001, xiii, 548. ISBN 0198792905. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2010
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Wed 13:00–14:50 B11/132
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 26 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2010
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Fri 14:00–15:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 18 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
    not specified
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 bodů; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2009
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Thu 12:00–13:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-42; B: 41-37; C: 36-32; D: 31-27; E: 26-22; F: 21-0 pints; P: 50-17; N: 16-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2009
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Thu 10:00–11:50 G2,02003
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 18 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-42; B: 41-37; C: 36-32; D: 31-27; E: 26-22; F: 21-0 pints; P: 50-17; N: 16-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2008
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Thu 12:00–13:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods
Twelve non-obligatory lectures with twelve running optional homeworks. Final written examination (test on the computer).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2008
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Wed 16:00–17:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 18 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmanns statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou přednášky doplněné možností průběžného procvičování látky e-testy v IS.
Ukončení předmětu (zkouškou i kolokviem) má formu e-testu (100 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2007
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Thu 12:00–13:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Ukončení předmětu (zkouška i kolokvium) má formu e-testu (100 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2007
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Zdenka Michaličková (assistant)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Wed 16:00–17:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 18 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmanns statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou přednášky doplněné možností průběžného procvičování látky e-testy v IS.
Ukončení předmětu (zkouškou i kolokviem) má formu e-testu (100 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2006
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Zdenka Michaličková (assistant)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Tue 11:00–12:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Ukončení předmětu (zkouška i kolokvium) má formu e-testu (100 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2006
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Zdenka Michaličková (assistant)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Wed 13:00–14:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 18 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmanns statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Ukončení předmětu (zkouška i kolokvium) má formu e-testu (90 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2005
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Zdenka Michaličková (alternate examiner)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Chemistry Section – Faculty of Science
Timetable
Tue 13:00–14:50 A,01026
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Ukončení předmětu (zkouška i kolokvium) má formu e-testu (90 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2005
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: k (colloquium). Other types of completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Chemistry Section – Faculty of Science
Timetable
Tue 13:00–14:50 02004
Prerequisites
! C3140 Physical Chemistry I
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 17 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Kvantová chemie. Kvantová teorie, pozorovatelné veličiny a operátory, Schrödingerova rovnice, vlastní funkce a energie, orbitaly, elektronová struktura atomů a molekul, repulze elektronů, spin. (2) Struktura molekul. Jaderná a elektronová struktura molekul, PES, symetrie molekul, vibrace, rotace, translace, elektronová hustota, mezimolekulové síly. (3) Statistická termodynamika. Populace, konfigurace, váha, Boltzmannova statistika, partiční funkce. (4) Interakce molekul s fotony. Spektroskopie, výběrová pravidla, rotační, vibrační a elektronová spektra, fluorescence a fosforescence, magnetická resonance, difrakční techniky. (5) Fenomenologická termodynamika. Termodynamický systém a jeho popis, termodynamické děje, 0. a 1. věta, teplo a práce, stavové funkce, entalpie, tepelné kapacity, termochemie, reakční a slučovací entalpie, standardní stav. (6) Termodynamické kritérium samovolnosti. Entropie, 2. věta, Clausiova nerovnost, Gibbsova a Helmholtzova funkce, maximální práce, 3. věta, absolutní entropie. (7) Ideální a reálné systémy. Spojená formulace 1. a 2. věty, závislost Gibbsovy funkce na teplotě a na tlaku, chemický potenciál, fugacita, aktivita, roztoky, změna složení. (8) Fázová rovnováha. Podmínka fázové rovnováhy, Gibbsův zákon fází, fázové diagramy jedné a více složek. (9) Chemická rovnováha. Reakční a standardní reakční Gibbsova funkce, reakční kvocient, rovnovážná konstanta a její závislost na teplotě. (10) Elektrochemie. Ionty, meziiontové interakce, iontová síla, elektrody a jejich potenciály, elektrochemické články. (11) Chemická dynamika. Transport, difúze, reakční kinetika jednoduchých reakcí, mechanismus, teorie aktivovaného komplexu, reakční koordináta, aktivační energie. (12) Disperzní systémy. Fázové rozhraní, adsorpce, makromolekuly, polyelektrolyty, koloidy, micely.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Zkouška má písemnoum (30 min.) a ústní část (dvě otázky vylosované ze zveřejněného seznamu). Obsahem kolokvia je rozprava ke 2 otázkám, které si student vylosuje ze zveřejněného seznamu.
Language of instruction
Czech
Further comments (probably available only in Czech)
The course is taught annually.
General note: tento předmět je obsahem ekvivalentní předmětu C3140 Fyzikální chemie I v PS.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2004
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: k (colloquium). Other types of completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 17 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Kvantová chemie. Kvantová teorie, pozorovatelné veličiny a operátory, Schrödingerova rovnice, vlastní funkce a energie, orbitaly, elektronová struktura atomů a molekul, repulze elektronů, spin. (2) Struktura molekul. Jaderná a elektronová struktura molekul, PES, symetrie molekul, vibrace, rotace, translace, elektronová hustota, mezimolekulové síly. (3) Statistická termodynamika. Populace, konfigurace, váha, Boltzmannova statistika, partiční funkce. (4) Interakce molekul s fotony. Spektroskopie, výběrová pravidla, rotační, vibrační a elektronová spektra, fluorescence a fosforescence, magnetická resonance, difrakční techniky. (5) Fenomenologická termodynamika. Termodynamický systém a jeho popis, termodynamické děje, 0. a 1. věta, teplo a práce, stavové funkce, entalpie, tepelné kapacity, termochemie, reakční a slučovací entalpie, standardní stav. (6) Termodynamické kritérium samovolnosti. Entropie, 2. věta, Clausiova nerovnost, Gibbsova a Helmholtzova funkce, maximální práce, 3. věta, absolutní entropie. (7) Ideální a reálné systémy. Spojená formulace 1. a 2. věty, závislost Gibbsovy funkce na teplotě a na tlaku, chemický potenciál, fugacita, aktivita, roztoky, změna složení. (8) Fázová rovnováha. Podmínka fázové rovnováhy, Gibbsův zákon fází, fázové diagramy jedné a více složek. (9) Chemická rovnováha. Reakční a standardní reakční Gibbsova funkce, reakční kvocient, rovnovážná konstanta a její závislost na teplotě. (10) Elektrochemie. Ionty, meziiontové interakce, iontová síla, elektrody a jejich potenciály, elektrochemické články. (11) Chemická dynamika. Transport, difúze, reakční kinetika jednoduchých reakcí, mechanismus, teorie aktivovaného komplexu, reakční koordináta, aktivační energie. (12) Disperzní systémy. Fázové rozhraní, adsorpce, makromolekuly, polyelektrolyty, koloidy, micely.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Zkouška má písemnoum (30 min.) a ústní část (dvě otázky vylosované ze zveřejněného seznamu). Obsahem kolokvia je rozprava ke 2 otázkám, které si student vylosuje ze zveřejněného seznamu.
Language of instruction
Czech
Further comments (probably available only in Czech)
The course is taught annually.
The course is taught: every week.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Physical Chemistry

Faculty of Science
Spring 2003
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Chemistry Section – Faculty of Science
Course Enrolment Limitations
The course is only offered to the students of the study fields the course is directly associated with.
fields of study / plans the course is directly associated with
there are 15 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Kvantová chemie. Kvantová teorie, pozorovatelné veličiny a operátory, Schrödingerova rovnice, vlastní funkce a energie, orbitaly, elektronová struktura atomů a molekul, repulze elektronů, spin. (2) Struktura molekul. Jaderná a elektronová struktura molekul, PES, symetrie molekul, vibrace, rotace, translace, elektronová hustota, mezimolekulové síly. (3) Statistická termodynamika. Populace, konfigurace, váha, Boltzmannova statistika, partiční funkce. (4) Interakce molekul s fotony. Spektroskopie, výběrová pravidla, rotační, vibrační a elektronová spektra, fluorescence a fosforescence, magnetická resonance, difrakční techniky. (5) Fenomenologická termodynamika. Termodynamický systém a jeho popis, termodynamické děje, 0. a 1. věta, teplo a práce, stavové funkce, entalpie, tepelné kapacity, termochemie, reakční a slučovací entalpie, standardní stav. (6) Termodynamické kritérium samovolnosti. Entropie, 2. věta, Clausiova nerovnost, Gibbsova a Helmholtzova funkce, maximální práce, 3. věta, absolutní entropie. (7) Ideální a reálné systémy. Spojená formulace 1. a 2. věty, závislost Gibbsovy funkce na teplotě a na tlaku, chemický potenciál, fugacita, aktivita, roztoky, změna složení. (8) Fázová rovnováha. Podmínka fázové rovnováhy, Gibbsův zákon fází, fázové diagramy jedné a více složek. (9) Chemická rovnováha. Reakční a standardní reakční Gibbsova funkce, reakční kvocient, rovnovážná konstanta a její závislost na teplotě. (10) Elektrochemie. Ionty, meziiontové interakce, iontová síla, elektrody a jejich potenciály, elektrochemické články. (11) Chemická dynamika. Transport, difúze, reakční kinetika jednoduchých reakcí, mechanismus, teorie aktivovaného komplexu, reakční koordináta, aktivační energie. (12) Disperzní systémy. Fázové rozhraní, adsorpce, makromolekuly, polyelektrolyty, koloidy, micely.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Zkouška má písemnoum (30 min.) a ústní část (dvě otázky vylosované ze zveřejněného seznamu). Obsahem kolokvia je rozprava ke 2 otázkám, které si student vylosuje ze zveřejněného seznamu.
Language of instruction
Czech
Further comments (probably available only in Czech)
The course is taught annually.
The course is taught: every week.
General note: http://cheminfo.chemi.muni.cz/ktfch/kubacek/C4660/index.htm.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/ktfch/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Physical Chemistry

Faculty of Science
Spring 2002
Extent and Intensity
2/0/0. 3 credit(s). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Marie Studničková, CSc. (lecturer)
Guaranteed by
doc. RNDr. Marie Studničková, CSc.
Chemistry Section – Faculty of Science
Prerequisites (in Czech)
Je vhodné mít zkoušku z obecné a anorganické chemie.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 21 fields of study the course is directly associated with, display
Course objectives
Physical chemistry for biology students contains themes from equilibrium thermodynamics and electrochemistry, an introduction into non-equilibrium themodynamics, themes from chemical kinetics and spectral methods.
Syllabus (in Czech)
  • 1. Thermodynamika. Makroskopické soustavy a okolí. Stavové funkce. První věta- práce a teplo, vnitřní energie. Stavová rovnice - objem , tlak, teplota. Intenzivní a extenzivní veličiny. parciální molární veličiny směsi. Stav rovnováhy. Energie, enthalpie a tepelná kapacita. 2. První zákon thermodynamiky a chemické reakce. Reakční teplo (enthalpie). Standardní stavy. Slučovací (tvorná) tepla a spalná tepla. Entropie, Gibbsova energie a chemické reakce. Chemická rovnováha. Le Chatelierův a Braunův princip. Druhý zákon thermodynamiky. Třetí zákon. Chladicí zařízení. Tepelná pumpa. 3. Aktivita složky. Rovnovážná konstanta. Chemická rovnováha ideálních a neideálních soustav. Standardní stavy a aktivity čistých složek ve směsi. 4. Fázové rovnováhy. Tání, vypařování a sublimace. Výparné teplo. Troutonovo pravidlo. Gibbsovo fázové pravidlo.Fázová rovnováha jednosložkové soustavy a Clapeyronova rovnice. Kapalné krystaly. 5. Ideální roztoky a Raoultův zákon. Změna teploty tání, teploty varu a tenze par (koligativní vlastnosti). Osmotický tlak. Vant Hoffova rovnice. 6. Reálné roztoky a thermodynamika mísení. Dodatkové funkce. Roztoky polymerů. Dělení složek směsi. Limitní zákony zředěných roztoků: Nernstův rozdělovací, Henryho zákon. 7. Ionika - rovnováhy v roztocích elektrolytů. Slabé kyseliny, pufry, Hendersonova a Haselbalchova rovnice. Rovnováhy rozpustnosti. Silné elektrolyty. Iontové aktivity. Iontová síla. Debyeův a Huckelův limitní zákon pro aktivitní koeficient. 8. Elektrodika. Galvanický článek. Nernstova rovnice. Typy elektrod. Iontové elektrody 1. a 2. druhu. Iontově selektivní elektrody. Redoxní elektrody. Vodíková elektroda. Solný můstek. Suchý článek. Vratné články - olověné akumulátory. Převodová čísla a elektroforéza. 9. Základy nerovnovážné thermodynamiky. Lokální rovnováha. Produkce entropie difuzí, tepelnou vodivostí, viskositou a chemickými reakcemi. Lineární závislost toků na silách. Princip symetrie Curie a Prigogina. Onsagerův vztah vzájemnosti. Minimum produkce entropie ve stacionárních stavech (Prigogine). Aktivní transport přes membrány. Disipativní struktury. 10. Kinetika chemických reakcí. Řád reakce, molekularita, mechanismus. Vliv teploty na rychlostní konstantu. Arrheniova rovnice. Srážková theorie a theorie aktivovaného komplexu. 11. Disperzní soustavy, jejich druhy podle fázových směsí. Charakteristiky disperzí oproti roztokům. Rozptyl světla na částicích. Emulze o/v a V/o. Stabilita disperzních soustav. 12. Interakce světla s látkou. Elektromagnetické záření podle energie fotonů, lom, absorpce a rozptyl světla. Barevnost látek. Fotochemické reakce. Fotosyntzéza, fotografický proces. Spektrální metody. Absorpční a emisní spektra.
Literature
  • FISCHER, Oldřich. Fyzikální chemie : (termodynamika, elektrochemie, kinetika, koloidní soustavy). 1. vyd. Praha: Státní pedagogické nakladatelství, 1984, 333 s. info
  • VODRÁŽKA, Zdeněk. Fyzikální chemie pro biologické vědy. Vyd. 1. Praha: Academia, 1982, 565 s. URL info
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Dvouhodinová jednosemestrální přednáška je doplněna dvouhodinovým laboratorním cvičením. Zápočet ze cvičení by měl předcházet zkoušku. Zkouška má písemnou a ústní část. K písemné zkoušce je možno si vypočítat příklady, které jsou opatřeny výsledky pro kontrolu.
Language of instruction
Czech
Further Comments
The course is taught annually.
The course is taught: every week.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Physical Chemistry

Faculty of Science
Spring 2001
Extent and Intensity
2/0/0. 3 credit(s). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Marie Studničková, CSc. (lecturer)
Guaranteed by
doc. RNDr. Marie Studničková, CSc.
Chemistry Section – Faculty of Science
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 23 fields of study the course is directly associated with, display
Course objectives
Physical chemistry for biology students contains themes from equilibrium thermodynamics and electrochemistry, an introduction into non-equilibrium themodynamics, themes from chemical kinetics and spectral methods.
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Language of instruction
Czech
Further Comments
The course is taught annually.
The course is taught: every week.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2018

The course is not taught in Autumn 2018

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of biochemistry, chemistry, biology, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
autumn 2017

The course is not taught in autumn 2017

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
Mathematics course in the extent of the first semester of bachelor's study fields of biochemistry, chemistry, biology, or biophysics.
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
A. Understanding basic concepts of chemical thermodynamics and kinetics with a relation to previous, simultaneous and following courses. B. Step-by-step development of abstract thinking.
Learning outcomes
After completing this course students will understand, at an introductory level, fundamental concepts of chemical thermodynamics and kinetics. Students will be able to solve corresponding computational exercises and will develop skills to derive basic thermodynamic relationships.
Syllabus
  • (1) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work. (2) State functions. Enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (3) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (4) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (5) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (6) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (7) Transport. Diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Fyzikální chemie. Vyd. 1. Praha: Vysoká škola chemicko-technologická v Praze, 2013, xxvi, 915. ISBN 9788070808306. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
    not specified
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • KUBÁČEK, Pavel and Zdena MICHALIČKOVÁ. Základy fyzikální chemie. Elportál. Brno: Masarykova univerzita, 2011. ISSN 1802-128X. URL info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Thirteen non-obligatory lectures.
Assessment methods
Written test (non-electronic one) in 100 minutes length. Both open and closed questions will be included, covering both computational and theoretical questions. A minimum score of 50% points is required for a successful completion of the course.
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2016

The course is not taught in Autumn 2016

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 points; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2015

The course is not taught in Autumn 2015

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 points; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2014

The course is not taught in Autumn 2014

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 points; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2013

The course is not taught in Autumn 2013

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second law, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 points; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2012

The course is not taught in Autumn 2012

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2011

The course is not taught in Autumn 2011

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 36 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
spring 2012 - acreditation

The information about the term spring 2012 - acreditation is not made public

Extent and Intensity
2/0/0. 2 credit(s) (plus extra credits for completion). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught each semester.
The course is taught: every week.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2011 - acreditation

The information about the term Autumn 2011 - acreditation is not made public

Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 26 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2010 - only for the accreditation
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 26 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2011 - only for the accreditation
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 18 fields of study the course is directly associated with, display
Course objectives
After completing this course students will understand, at an introductory level, fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
    recommended literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
    not specified
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
  • Comprehensive dictionary of physical chemistry. Edited by Ladislav Ulický - Terence James Kemp. 1st pub. New York: Ellis Horwood, 1992, 472 s. ISBN 0-13-151747-3. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Teaching methods
Twelve non-obligatory lectures with twelve running optional home works (e-tests).
Assessment methods
Final written examination (multiple choice e-test; 38 questions) lasts 100 minutes. Maximum of points will be 50 ((A: 50-44; B: 43-39; C: 38-34; D: 33-29; E: 28-24; F: 23-0 pints; P: 50-19; N: 18-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught each semester.
The course is taught: every week.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2008 - for the purpose of the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Spring 2008 - for the purpose of the accreditation
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 18 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmanns statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 8th ed. Oxford: Oxford University Press, 2006, xxx, 1064. ISBN 0198700725. info
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou přednášky doplněné možností průběžného procvičování látky e-testy v IS.
Ukončení předmětu (zkouškou i kolokviem) má formu e-testu (100 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.

C4660 Basic Physical Chemistry

Faculty of Science
Autumn 2007 - for the purpose of the accreditation
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
none
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
there are 31 fields of study the course is directly associated with, display
Course objectives
The course introduces fundamental concepts of theoretical chemistry to real chemical systems with an emphasis on the relationships between the microscopic structure and macroscopic properties of matter. Topics will include quantum theory, chemical statistics, thermodynamics, electrochemistry, and kinetics.
Syllabus
  • (1) Quantum chemistry. Quantum theory, observables and operators, Schrödinger equation, eigenfunctions and eigenvalues, orbitals, electron structure of atoms and molecules, electron repulsion, spin. (2) Molecular structure. Nuclear and electron structure of molecules, PES, molecular symmetry, molecular vibrations, rotations, translations, electron density, intermolecular forces. (3) Statistical thermodynamics. Population, configuration, weight, Boltzmann's statistics, partition function. (4) Interaction of molecules and photons. Spectroscopy, selection rules, rotational, vibrational and electronic spectra, fluorescence and phosphorescence, magnetic resonance, X-ray diffraction. (5) Equilibrium thermodynamics. Thermodynamic system and its description, thermodynamic processes, zeroth and first law, heat and work, state functions, enthalpy, heat capacity, thermochemistry, reaction and formation enthalpy, standard state. (6) Thermodynamic criterion for spontaneity. Entropy, second low, Clausius inequality, Gibbs and Helmholtz function, maximum work, third law, absolute entropy. (7) Ideal and real systems. Combined first and second laws, temperature and pressure dependence of Gibbs function, chemical potential, fugacity, activity, solutions, change of composition. (8) Phase equilibrium. Condition of phase equilibrium, Gibbs phase rule, phase diagrams for one and more components. (9) Chemical equilibrium. Reaction and standard reaction Gibbs function, reaction quotient, equilibrium constant and its temperature dependence. (10) Electrochemistry. Ions, interaction between ions, ionic strength, electrodes and their potentials, electrochemical cells. (11) Chemical dynamics. Transport, diffusion, kinetics of simple reactions, mechanism, activated complex theory, reaction coordinate, activation energy. (12) Dispersion systems. Phase boundary, adsorption, macromolecules, polyelectrolytes, colloids, micelles.
Literature
  • ATKINS, P. W. and Julio DE PAULA. Atkins' physical chemistry. 7th ed. Oxford: Oxford University Press, 2002, xxi, 1150. ISBN 0198792859. info
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
  • Atkins, Peter William - Paula, Julio de. Physical chemistry for the Life Sciences. 1st ed. N.Y. : W. H. Freeman and Company, 2006, 699. ISBN 0-1992-8065-9
  • ATKINS, P. W. Fyzikálna chémia. 6. vyd. Bratislava: Slovenská technická univerzita v Bratislave, 1999, 308 s. ISBN 80-227-1238-8. info
  • Kubáček, Pavel. Základy fyzikální chemie. Hypertext, MU 2004; http://cheminfo.chemi.muni.cz/ianua/ZFCh
  • MOORE, Walter J. Fyzikální chemie. 2. vyd. Praha: Nakladatelství technické literatury, 1981, 974 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C4660!
Assessment methods (in Czech)
Předmět je vyučován formou klasické přednášky. Ukončení předmětu (zkouška i kolokvium) má formu e-testu (100 min.)
Language of instruction
Czech
Follow-Up Courses
Further comments (probably available only in Czech)
The course is taught each semester.
The course is taught: every week.
General note: Předmět lze absolvovat také v JS.
Listed among pre-requisites of other courses
Teacher's information
http://cheminfo.chemi.muni.cz/kubacek/C4660/index.htm
The course is also listed under the following terms Spring 2008 - for the purpose of the accreditation, Spring 2011 - only for the accreditation, Autumn 2010 - only for the accreditation, Spring 2001, Spring 2002, Spring 2003, Spring 2004, Spring 2005, Autumn 2005, Spring 2006, Autumn 2006, Spring 2007, Autumn 2007, Spring 2008, Autumn 2008, Spring 2009, Autumn 2009, Spring 2010, Autumn 2010, Spring 2011, Spring 2012, Autumn 2011 - acreditation, spring 2012 - acreditation, Spring 2013, Spring 2014, Spring 2015, Spring 2016, Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2024, Spring 2025.
  • Enrolment Statistics (recent)