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).
doc. RNDr. Pavel Kubáček, CSc. (lecturer)
Guaranteed by
doc. RNDr. Pavel Kubáček, CSc.
Department of Chemistry - Chemistry Section - Faculty of Science
Mon 18:00–19:50 A,01026, Wed 10:00–11:50 A,01026
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.
  • 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.
  • 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
Assessment methods
23(24) non-obligatory lectures with 10 running optional homeworks. Final written examination (test on the computer).
Language of instruction
Follow-Up Courses
Further Comments
The course is taught once in two years.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 2004, Autumn 2006.
  • Enrolment Statistics (recent)
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