C1020 General Chemistry

Faculty of Science
Autumn 2007
Extent and Intensity
4/0/0. 4 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).
Teacher(s)
prof. RNDr. Jiří Pinkas, Ph.D. (lecturer)
Guaranteed by
prof. RNDr. Jiří Pinkas, Ph.D.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: prof. RNDr. Jiří Pinkas, Ph.D.
Timetable
Mon 15:00–16:50 F1 6/1014, Mon 15:00–16:50 A,01026, Wed 10:00–11:50 A,01026, Wed 10:00–11:50 F1 6/1014
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
Course objectives
The important chemical principles and facts are covered, with considerable attention given to the quantitative aspects and to the techniques important to the further work in the field of chemistry and biochemistry. The course consists of a lecture, numerical exercises and problem classes.
Syllabus
  • 1. Principles of chemistry, matter, their properties and forms of matter existence, principal chemical laws, chemical formula, chemical materials, purity of compounds, mixtures, physical and chemical characteristcis of pure compounds.

    2. Atom symbolics, elemental particles, element, nuclide, isotope, isotone, isobare, mass of elements and molecules, mass unit u, mole, molar mass. Atomic nucleus, mass defect, stability of nuclei, radioactivity, radioactivity law, Fajans-Soddy rules, nuclear reactions.

    3. Physical differences between micro- and macro world, particle-wave character of microparticles, dualistic view on matter, Heisenberg principle of uncertainty. Bohr theory of hydrogen atom, emission spectrum of H.- atom, X-ray irradiation, Moseley law. Wave eguation, wave function, probalility of electron occurence, atomic orbital, quantum numbers, shapes of atomic orbitals, energy states and their degeneration, Aufbau principle of many electron atom, Pauli principle, Hund principle.

    4. Periodical law, primary and secondary periodicity. Properties of elements, ionization energy, electron affinity, electronegativity. Formation of ions, ions with 18 and 20 valence electrons, ionic radii, ionic crystals, methods of their study.

    5. Covalent nad donor-acceptor bonding, wave-mechanic model of chemical bond, overlap of atomic orbitals, overlap ingral, types of molecular orbitals (s, p, d), LCAO-MO, molecular diagrams of homo- and heteronuclear biatonic molecules. Polarity, ionic degree, bond order, length and energy of bond.

    6. Shape of molecules, hybridization, VSEPR method, delocalization of electron density, resonance, compounds with lack of electrons, weak interactions between molecules (van der Waals forces, H-bonding).

    7. Principles of coordination chemistry, central atom, ligand, coordination polyhedra, chelates, chelate effect, polynuclear complexes, clusters, structural isomery of complexes. Nomenclature of complex compounds. Donor-acceptor properties of ligands, principles of ligand field theory, octahedral, tetrahedral and tetragonal complexes, high- and low spin complexes, Jahn-Teller effect, spectral and magnetic properties of complexes. Complex equilibria, mechanisms of complexing reactions, trans-effect.

    8. State equation and simple laws for ideal gas, transport phenomena in gases, Graham law, real gas, critical state, liquefaction of gases, reduced van der Waals state equation, State equation for liguids, surface tension, viscosity.

    9. Common properties of solids, crystal lattice, Madelung constant, Born-Haber cycle, lattice energy, symmetryof molecules and ions. Band theory in electronic structure of solids, properties of metals, metallic bond, conductors, semiconductors, insulators. 10. Types and mechanism of chemical reactions, energy changes in course of chemical reactions, fundamental thermodynamical parameters (U,H,G,S) and laws, Hess law, thermodynamical conditions of spontaneous reaction course. Chemical equilibrium, equilibrium constant, influence of temperature and pressure, LeChatelier principle. Reaction kinetics, reaction velocity law, reaction molecularity and order. Arrhenius law, activation energy, reaction coordinate, homogenous and heterogenous catalysis.

    11. Equilibrium in polyphase system. Gibbs phase rule, definition of phase, component and degree of freedom. Solutions, solubility, concentration units, conductivity of solutions, electrolytical dissociation, solvation and association of ions, ionic strength, activity and activity coefficient. Pricipitation and solubility product, properties of diluted solutions, Raoult law, ebulioscopy and cryoscopy, distillation, rectification, sublimation, melting.

    12. Acid-base theories, solvotheory of acids and bases, superacid media, acidity and basicity of aqueous solutions, pH, hydrolysis of salts, buffers anf their capacity.

    13. Fundamentals of electrochemistry, Faraday law, coulometry, electrochemical potential, types of electrodes, standard electrode potentials, standard hydrogen electrode, Nernst and Nernst-Peters equations, galvanic cells.

    14. Absorption of elecrtomagnetic irradiation, function of spectrometer. Molecular spectra, IR and Raman spectrometry, electron spectrometry, luminiscence. Magnetic properties og compounds, magnetic moment of atom and nucleus, dia- and paramagnetism, ferro- and antiferromagnetism. X-ray structural analysis, mass spectrometry.
Literature
  • ZUMDAHL, Steven S. and Susan A. ZUMDAHL. Chemistry. 6th ed. Boston: Houghton Mifflin Company, 2003, xxiv, 1102. ISBN 0618221565. info
  • HILL, John W. General chemistry. 4th ed. Upper Saddle River, N.J.: Pearson Prentice Hall, 2005, xxvii, 107. ISBN 0131180037. 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
  • HÁLA, Jiří. Pomůcka ke studiu obecné chemie. 1. vyd. Brno: Masarykova univerzita, 1993, 85 s. ISBN 8021002891. info
  • VACÍK, Jiří. Obecná chemie. 1. vyd. Praha: Státní pedagogické nakladatelství, 1986, 303 s. info
Assessment methods (in Czech)
Výuka formou přednášky. Z kapacitních důvodů bude přednáška probíhat v aule a paralelně v učebně F1, do které bude výklad přenášen pomocí TV kamery. Zkouška je písemná a ústní.
Language of instruction
Czech
Follow-Up Courses
Further Comments
Study Materials
The course can also be completed outside the examination period.
The course is taught annually.
Listed among pre-requisites of other courses

Zobrazit další předměty

The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Autumn 1999, Autumn 2010 - only for the accreditation, Autumn 2000, Autumn 2001, Autumn 2002, Autumn 2003, Autumn 2005, Autumn 2009, Autumn 2010, Autumn 2011, Autumn 2011 - acreditation, Autumn 2012, Autumn 2013, Autumn 2014, Autumn 2015, Autumn 2016, autumn 2017, Autumn 2018, Autumn 2019, Autumn 2020, autumn 2021, Autumn 2022, Autumn 2023, Autumn 2024.
  • Enrolment Statistics (Autumn 2007, recent)
  • Permalink: https://is.muni.cz/course/sci/autumn2007/C1020