F1AC1_15 General and Inorganic Chemistry

Faculty of Pharmacy
Autumn 2024
Extent and Intensity
3/3/0. 8 credit(s). Type of Completion: zk (examination).
In-person direct teaching
Teacher(s)
PharmDr. Tomáš Goněc, Ph.D. (lecturer)
Mgr. Aleš Kroutil, Ph.D. (lecturer)
PharmDr. Tomáš Goněc, Ph.D. (seminar tutor)
Mgr. Aleš Kroutil, Ph.D. (seminar tutor)
Mgr. Michal Greguš (seminar tutor)
RNDr. Eva Havránková, Ph.D. (seminar tutor)
Mgr. Jaroslava Jamrichová (seminar tutor)
Mgr. Veronika Murgašová (seminar tutor)
PharmDr. Jan Otevřel, Ph.D. (seminar tutor)
Mgr. Karolína Šeligová (seminar tutor)
Ing. Vít Šťáva, Ph.D. (seminar tutor)
Mgr. Hubert Veselý (seminar tutor)
Ing. Eliška Růžičková (assistant)
Guaranteed by
PharmDr. Tomáš Goněc, Ph.D.
Department of Chemical Drugs – Departments – Faculty of Pharmacy
Supplier department: Department of Chemical Drugs – Departments – Faculty of Pharmacy
Timetable
Tue 15:00–17:30 44-056
  • Timetable of Seminar Groups:
F1AC1_15/01: Mon 16. 9. to Fri 4. 10. Mon 8:00–10:30 44-249, Mon 7. 10. to Fri 13. 12. Mon 8:00–10:30 44-342, T. Goněc, E. Havránková, A. Kroutil, V. Murgašová, E. Růžičková
F1AC1_15/02: Mon 16. 9. to Fri 4. 10. Tue 8:00–10:30 45-221, Mon 7. 10. to Fri 13. 12. Tue 8:00–10:30 44-342, T. Goněc, A. Kroutil, E. Růžičková, V. Šťáva, H. Veselý
F1AC1_15/03: Mon 16. 9. to Fri 4. 10. Wed 8:00–10:30 44-249, Mon 7. 10. to Fri 13. 12. Wed 8:00–10:30 44-342, T. Goněc, J. Jamrichová, A. Kroutil, E. Růžičková
F1AC1_15/04: Mon 16. 9. to Fri 4. 10. Wed 11:00–13:30 44-249, Mon 7. 10. to Fri 13. 12. Wed 11:00–13:30 44-342, T. Goněc, J. Jamrichová, A. Kroutil, E. Růžičková
F1AC1_15/05: Mon 16. 9. to Fri 4. 10. Thu 7:50–10:20 44-249, Mon 7. 10. to Fri 13. 12. Thu 7:50–10:20 44-342, T. Goněc, A. Kroutil, E. Růžičková, K. Šeligová
F1AC1_15/06: Mon 16. 9. to Fri 4. 10. Thu 10:35–13:05 44-249, Mon 7. 10. to Fri 13. 12. Thu 10:35–13:05 44-342, T. Goněc, A. Kroutil, E. Růžičková, K. Šeligová
F1AC1_15/07: Mon 16. 9. to Fri 4. 10. Thu 14:00–16:30 44-249, Mon 7. 10. to Fri 13. 12. Thu 14:00–16:30 44-342, T. Goněc, A. Kroutil, J. Otevřel, E. Růžičková
F1AC1_15/08: Mon 16. 9. to Fri 4. 10. Wed 14:00–16:30 44-249, Mon 7. 10. to Fri 13. 12. Wed 14:00–16:30 44-342, T. Goněc, A. Kroutil, V. Šťáva
F1AC1_15/09: Mon 16. 9. to Fri 4. 10. Fri 7:15–9:45 44-249, Mon 7. 10. to Fri 13. 12. Fri 7:15–9:45 44-342, T. Goněc, M. Greguš, A. Kroutil, E. Růžičková
Prerequisites (in Czech)
FAKULTA(FaF) || OBOR(MUSFaF)
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
Course objectives
The students will be acquainted with the subject of chemistry including the basic branches of chemistry and the importance of chemistry for pharmacists. The course will focus on the following items: fundamental chemical terms and laws, equations for calculating the quantity of substance and concentration, atomic structure, radioactivity, basic equations used in spectral analysis, models of atomic orbitals, chemical bond including hybridization, physical states of matter, the periodic law and the classification of elements including forms and the division of the periodic system into groups, and the properties of individual elements in the periodic table.
Seminars will concentrate on problems such as calculating the amount of substance, composition of solutions, diluting and mixing solutions, formation of chemical formulas and balancing equations for stoichiometric calculations, and the calculation of the pH. During practical exercises, the students will be acquainted with the basics of laboratory work and will also prepare some inorganic compounds according to calculated equations. The students will elaborate protocols containing the description of the principle of the method and all calculations including the calculation of theoretical yield which will be compared with the practical yield obtained.
Learning outcomes
After completing the course student will:
-know basic chemical glassware,equipment and apparatus;
-be able to perform basic laboratory operations independently;
-know inorganic compound nomenclature and basic chemical clculations;
-understand the basic principles of general chemistry;
-know basic chemistry of elements
Syllabus
  • Lectures:
    General Chemistry.
    Role of the chemistry in the spectrum of naturae sciences. History of chemistry. Milestone discoveries in chemical history. Mass, discreetness of particles. Elements, symbols, periodic table, molecule, chemical formula, chemical equation. Structure and electron formula, octet rule, hypervalence, resonance, oxidation state, formal charge. Electronegativity. Definition of element, nuclide, isotope. Atomic number, atomic mass, molecular mass, amount of mass, mol. Atom, nucleus, elemental particles of mass. Moseley rule. Radioactivity, natural and artificial radionuclides, nuclear reactions, decay families.
    Quantum and wave theory, wave and particle, interference and difraction. Schrödinger equation. Planetar atom model, electron shell, Bohr model of hydrogen atom, line and continual spectra, therms, hydrogen spectrum. Structure of electron shell, quantum nombers, Pauli rule, Hund rule, stable valence shell configuration, excited state, electron configuration writing. Mendelejev periodic rule. Ionization potential, electron affinity, electronegativity. Atomic orbitals.
    Chemical bond, forms of bonding, bonding energy. Covalent bond. Valence bonding theory, simple and multiple bonds. VSEPR. Hybridization.
    Molecule orbitals theory (MO) - linear combination of atomic orbitals (LCAO), energetic diagram. MO for: H2, N2, O2 and O3. Delocalized bonds, polarised bond. System of bonds in ethene, ethyne, benzene and allene.
    Hydrogen bonds, other weak interactions. Ionization, basic ion properties, ionic bond. Crystals. Metalic bond. Electron conductivity. Donor-acceptor bond, ions of transition metals, coordinational reactions, sorts of ligands and their properties. Coordination bonding theory. Structure, magnetic properties.
    Chemical ballance, basic thermodynamical and thermochemical laws, state equations. Entalpy, entropy, free energy, spontaneousness of processes. Floating ballance principle. Basics of chemical kinetics. Speed and order of reaction. Activation energy. Arrhenius equation. Catalysis. Radical reactions. Photochemical reactions. State definitions. State of matter, dispersion systems. Solubility, solutions, concentration, diffusion, osmosis.
    Base and acid theories, protolytic reactions, neutralisation, salts, strenght of acid and base, pH, indicators, salts hydrolysis, buffers. Lewis theory, electrophiles and nucleophiles. Coagulation. Factor of solubility. Reduction-oxidation reactions. Ballancing of red-ox equations. Electrode processes. Electrochemical potential.
    Inorganic chemistry.
    Chemistry of hydrogen, water. Alkalic metals, metals of alkaline earths.
    P elements, Halogens, Noble gases. Transition elements.
    Inorganic compounds important in biosystems and pharmacy.
    Seminars
    - Nomenclature of inorganic compounds
    - Solutions concentration calculations
    - Chemical equations, stoichometry, Acidobasic equilibria
    electron configuration, shape of molecules, Lewis formulas
    Practical class
    - Introduction to laboratory work
    - Distillation and extraction
    - Synthesis of trihydrogen boric acid.
    - Synthesis of disodium tetrahydroxo pentaoxoborate.
    - Synthesis of lead iodide.
    - Benzoic acid purification
    - Preparation od copper and ferrous sulphate pentahydrate.
    - Preparation of ferric oxide
    - Coordination compounds, hydroxides - test tube reactions

Literature
    required literature
  • Krätsmár-Šmogrovič, J. a kol. Všeobecná a anorganická chémia. Ostrava, 2007. info
    recommended literature
  • Galamboš M. a kol. Názvoslovie anorganických látok.Princípy a príklady. Bratislava, UKO, 2009. ISBN 978-80-223-2. info
  • Sirotek, V., Karlíček, J. Chemické výpočty a názvosloví anorganických látek. Plzeň, ZČU, 2005. URL info
  • Flemr, V., Holečková, E. Úlohy z názvosloví a chemických výpočtů v anorganické chemii. Praha, VŠCHT, 2001. ISBN 978-80-7080-435-3. info
  • Ulická, Ľ., Ulický, L. Príklady zo všeobecnej a anorganickej chémie. 2. vyd. Bratislava, 1987. info
    not specified
  • Greenwood N.N., Earnshaw A. Chemistry of the Elements. Amsterdam, Elsevier, 2010. ISBN 9780750633659. info
  • Polák, R., Zahradník, R. Obecná chemie: stručný úvod. Praha, Academia, 2000. ISBN 80-200-0794-6. info
  • Klikorka, Jiří - Hájek, Bohumil - Votinský, Jiří. Obecná a anorganická chemie. Praha, 1989. info
Teaching methods
seminars (nomenclature and calculations), laboartory courses, lectures
Assessment methods
To obtain credits, it is necessary to meet the following conditions: compulsory participation in seminars and laboratory courses, the obligation to prepare protocols from all practical tasks. Success in continuous tests in nomenclature and calculations at least 60%. Completion of the written part of the exam in nomenclature and calculations to at least 60%. Completion of an oral exam in general chemistry and an oral exam in inorganic chemistry.
Language of instruction
Czech
Further comments (probably available only in Czech)
Study Materials
The course can also be completed outside the examination period.
Teacher's information
Course evaluation.
The course consists of lectures and exercises. 8 credits can be obtained for the course under the following conditions:
1. successfull completion of seminars and exercises
Attendance at all seminars and exercises is compulsory.
Absence from seminars and exercises must be documented by a reliable medical certificate.
In case of another reason for absence, the student will replace the exercise in the last week.
Protocols are handed in from the exercises, which are either accepted by the teachers after checking, or returned for completion. Acceptance of all protocols is a condition for admission to the exam.
Part of the exercises are continuous tests on terminology, calculations and formulas. The condition for admission to the exam is an average of at least 60% success in all tests. In the last week of the semester, the student takes a final test on nomenclature, calculations and equations. The test result makes up a third of the final grade. The condition for admission to the exam is at least 60% success rate. The final test can be repeated a maximum of two times (three attempts in total) during the correction dates in the first and second week of January. No further correction dates will be listed!
Evaluation of the final test:
A( 1 ) 92-100%
B( 1-) 84-91%
C( 2 ) 76-83%
D( 2-) 68-75%
E( 3 ) 60-67%
F <60 %
2. successful completion of the exam
The exam is oral and is divided into General Chemistry and Inorganic Chemistry, from which the student chooses one question at random. The final grade is the average of the final test and both oral parts. If one of the parts is graded as F, the exam result is F.
The course is also listed under the following terms Autumn 2020, Autumn 2021, Autumn 2022, Autumn 2023.
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