C1021 General Chemistry

Faculty of Science
Autumn 2008
Extent and Intensity
4/0/0. 4 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
Mon 18:00–19:50 A,01026, Wed 10:00–11:50 A,01026
Prerequisites
Knowledge of chemistry on secondary school level
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 19 fields of study the course is directly associated with, display
Course objectives
The course objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Assessment methods
23(24) non-obligatory lectures with 10 running optional homeworks. Final written examination (test on the computer).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is also listed under the following terms Autumn 2004, Autumn 2006.

C1021 General Chemistry

Faculty of Science
Autumn 2006
Extent and Intensity
4/0/0. 4 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
Mon 12:00–13:50 A,01026, Thu 12:00–13:50 A,01026
Prerequisites
Knowledge of chemistry on secondary school level
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 25 fields of study the course is directly associated with, display
Course objectives
The aim of the course is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • Atkins, Peter William - Jones, Loretta. Chemical principles : the quest for insight. New York : W.H. Freeman, 2004. ISBN 0-7167-5701-X
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
  • VACÍK, Jiří. Obecná chemie. 1. vyd. Praha: Státní pedagogické nakladatelství, 1986, 303 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Assessment methods (in Czech)
Zkouška je písemná.
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is also listed under the following terms Autumn 2004, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2004
Extent and Intensity
4/0/0. 4 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.
Chemistry Section – Faculty of Science
Timetable
Mon 12:00–13:50 U-aula, Wed 12:00–13:50 U-aula
Prerequisites
Knowledge of chemistry on secondary school level
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 25 fields of study the course is directly associated with, display
Course objectives
The aim of the course is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • Atkins, Peter William - Jones, Loretta. Chemical principles : the quest for insight. New York : W.H. Freeman, 2004. ISBN 0-7167-5701-X
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
  • VACÍK, Jiří. Obecná chemie. 1. vyd. Praha: Státní pedagogické nakladatelství, 1986, 303 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Assessment methods (in Czech)
Zkouška je písemná.
Language of instruction
Czech
Follow-Up Courses
Further Comments
Study Materials
The course is taught once in two years.
The course is also listed under the following terms Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2016

The course is not taught in Autumn 2016

Extent and Intensity
4/0/0. 4 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
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2015

The course is not taught in Autumn 2015

Extent and Intensity
4/0/0. 4 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
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2014

The course is not taught in Autumn 2014

Extent and Intensity
4/0/0. 4 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
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2013

The course is not taught in Autumn 2013

Extent and Intensity
4/0/0. 4 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
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2012

The course is not taught in Autumn 2012

Extent and Intensity
4/0/0. 4 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
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Prerequisites
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2011

The course is not taught in Autumn 2011

Extent and Intensity
4/0/0. 4 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
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2010

The course is not taught in Autumn 2010

Extent and Intensity
4/0/0. 4 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
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2009

The course is not taught in Autumn 2009

Extent and Intensity
4/0/0. 4 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
Knowledge of chemistry on secondary school level
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 19 fields of study the course is directly associated with, display
Course objectives
The course objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2007

The course is not taught in Autumn 2007

Extent and Intensity
4/0/0. 4 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
Prerequisites
Knowledge of chemistry on secondary school level
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 25 fields of study the course is directly associated with, display
Course objectives
The aim of the course is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • Atkins, Peter William - Jones, Loretta. Chemical principles : the quest for insight. New York : W.H. Freeman, 2004. ISBN 0-7167-5701-X
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
  • VACÍK, Jiří. Obecná chemie. 1. vyd. Praha: Státní pedagogické nakladatelství, 1986, 303 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Assessment methods (in Czech)
Zkouška je písemná.
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2005

The course is not taught in Autumn 2005

Extent and Intensity
4/0/0. 4 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.
Chemistry Section – Faculty of Science
Prerequisites
Knowledge of chemistry on secondary school level
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 25 fields of study the course is directly associated with, display
Course objectives
The aim of the course is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • Atkins, Peter William - Jones, Loretta. Chemical principles : the quest for insight. New York : W.H. Freeman, 2004. ISBN 0-7167-5701-X
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
  • VACÍK, Jiří. Obecná chemie. 1. vyd. Praha: Státní pedagogické nakladatelství, 1986, 303 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Assessment methods (in Czech)
Zkouška je písemná.
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2011 - acreditation

The course is not taught in Autumn 2011 - acreditation

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

Extent and Intensity
4/0/0. 4 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
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2010 - only for the accreditation

The course is not taught in Autumn 2010 - only for the accreditation

Extent and Intensity
4/0/0. 4 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
! C1020 General Chemistry
Knowledge of chemistry on secondary school level
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 objective is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 3rd ed. New York: W.H. Freeman and Company, 2005, 1 sv. ISBN 071675701X. info
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Teaching methods
23(24) non-obligatory lectures with 10 running optional home works.
Assessment methods
Final written examination (multiple choice e-test; 25 questions) lasts 100 minutes. Maximum of points will be 50 (A: 50-41; B: 40-36; C: 35-31; D: 30-26; E: 25-21; F: 20-0 pints; P: 50-16; N: 15-0 points).
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.

C1021 General Chemistry

Faculty of Science
Autumn 2007 - for the purpose of the accreditation

The course is not taught in Autumn 2007 - for the purpose of the accreditation

Extent and Intensity
4/0/0. 4 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
Prerequisites
Knowledge of chemistry on secondary school level
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 25 fields of study the course is directly associated with, display
Course objectives
The aim of the course is to introduce students to a variety of chemical principles, in preparation for more detailed chemistry study in later years. Description of concepts and facts seeks the understanding of chemical world on an atomic and molecular level based on qualitative quantum theory. The molecular approach supports the comprehension of macroscopic phenomena and laws firmly depicted by thermodynamics and chemical kinetics.
Syllabus
  • 1. Contemporary Chemistry and its Prospect. Chemical Information. Composition of matter. Molecular Entity, Substance and Amount of Substance.
  • 2. Quantum Theory, Operators, States and Energy Levels, Schrödinger Equation, Stationary States.
  • 3. Hydrogen atom. Atomic Structure and Atomic Orbitals. Periodic Table and Trends, Categories of Elements.
  • 4. Description of Molecular Structure, Molecular Sates. Isomers. Molecular Symmetry, Chirality.
  • 5. Molecular Orbitals, Electron Density Distribution. Orbital Interactions, Electron Count. Pauli Principle.
  • 6. Diatomic and Triatomic Molecules. Photoelectron Spectroscopy.
  • 7. Polyatomic Molecules. Mass Spectrometry. Ionic and Metallic Substances. Relativity in Chemistry.
  • 8. VSEPR, Hybridization and Ligand Field. VB-methods. Quantum Chemical Calculations. Density Functional.
  • 9. Molecular Assemblies. Intermolecular Forces. Statistics in Chemistry, Boltzmann Distribution.
  • 10. Photon Absorption and Emission, the Spectral Line. Change of Rotational, Vibrational and Electronic Molecular State. Spectroscopy. NMR.
  • 11. Gases, Equation of State. Molecular Motion. The Kinetic Model of Gases. Liquids.
  • 12. Solids. Crystalline Solids. Unit Cells. X-Ray Diffraction. Liquid Crystals.
  • 13. Laws of Thermodynamics. Heat and Work. State Functions. The First Law. Enthalpy and Thermochemistry. Reaction Enthalpies and Standard Enthalpies of Formation. Bond Enthalpies.
  • 14. Entropy and Spontaneous Change, the Second Law. Gibbs Energy. The Third Law.
  • 15. Ideal and Real systems, Fugacity, Activity. Colligative Properties. Chemical Potential.
  • 16. Phase Equilibrium and Diagrams, Phase rule. The Vapor Pressure of a Binary Liquid Mixture, Azeotropes.
  • 17. Chemical Equilibrium, Equilibrium Constant and Reaction Quotient. Response to Conditions, Le Chatelier's Principle.
  • 18. Acid and Bases, Autoprotolysis. Donors and Acceptors. Solvents. Solubility.
  • 19. Ions in Solution, Conductivity of Electrolytes. Homogeneous and Heterogeneous Electron Transfer. Electrodes and Electrochemical Cells.
  • 20. Reactivity, Reaction Rates, Mechanisms and Molecularity. Photochemical, Chain, Catalytic, and Oscillation Reactions. Molecular Beams.
  • 21. Reaction Coordinate, Transition state, Activated Complex, Activation Energy. Potential Energy Surface.
  • 22. Chemical Synthesis. Supramolecular Chemistry. Biomolecules. Materials.
Literature
  • POLÁK, Rudolf and Rudolf ZAHRADNÍK. Obecná chemie : stručný úvod. Vyd. 1. Praha: Academia, 2000, 224 s. ISBN 8020007946. info
  • Atkins, Peter William - Jones, Loretta. Chemical principles : the quest for insight. New York : W.H. Freeman, 2004. ISBN 0-7167-5701-X
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie [Klikorka, 1989] a. 2. nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
  • VACÍK, Jiří. Obecná chemie. 1. vyd. Praha: Státní pedagogické nakladatelství, 1986, 303 s. info
Bookmarks
https://is.muni.cz/ln/tag/PříF:C1021!
Assessment methods (in Czech)
Zkouška je písemná.
Language of instruction
Czech
Follow-Up Courses
Further Comments
The course is taught once in two years.
The course is taught: every week.
The course is also listed under the following terms Autumn 2004, Autumn 2006, Autumn 2008.
  • Enrolment Statistics (recent)