1. komponenta

Lecture type	Total
Lectures	60
Seminar	30

* Load is given in academic hour (1 academic hour = 45 minutes)

1. Pure substances. Mixtures. Chemical and physical properties of substances (extensive and intensive). Physical and chemical changes. States of matter (phases of aggregation). Phase. Number and amount of entities. Law of mas conservation, Law of definite composition, law of mass conservation, Avogadro's constant, mole.
Chemical composition.
2. Atoms: Electron. Atomic nucleus. Nucleons. Isotopes. Atomic emission spectra. Atomic models. Electron motion: orbit vs. orbital. Electron configuration. Periodic table of elements.
3. Periodicity (Atomic size, ionization energy, electron affinity). Elemental substances (structures and properties). X-ray diffraction. Structures of metallic and molecular crystals. Allotropy.
4. Chemical Reactions: Writing and balansing chemical equations. Stoichiometric numbers (coefficients). Types of chemical reactions. Neutralization and precipitation reactions. Redox reactions. Standard reduction potentials and diagrams.
5. Stoichiometry of Chemical Reactions (basics), extent, degree of reaction
6. Chemical and Physical Properties of Elemental Substances. Elemental substances in redox reactions. Diagonal similarity. Oxides, oxocations and oxoanions of metals/nonmetals (nomenclature and formulas). Properties of oxides.
7. Gase:. Ideal gas laws for pure gases and gas mixtures.
8. hermodynamics: Internal energy, First Law of Thermodynamics. Work and heat.
Enthalpies of formation, combustion, and atomization. Reaction enthalpies.
Phase changes. Hess's law.
9. Ionic Bond: Ionic bond. Lattice energy. Ionic compounds in solid state (structures). Born-Haber cycle. Lattice enthalpy. Properties of ionic compounds.
Fajans's rules. Polymeric and layered structures.
10. Covalent Bond: Bond length. Bond dissociation. Bond enthalpies. Bond order. Diatomic and polyatomic molecules. Empirical and molecular formulas, Lewis structures. Hypovalent and hypervalent molecules. Radicals. Approximately localized sigma and pi bonds, conjugated bonds, delocalization. Electronegativity, bond polarity.
Hybridization. Molecular and ionic structures: VSEPR. LCP. Isomers. Using Lewis structures and bond enthalpies to calculate heats of reaction.

1. Chemistry, M. S. Silberberg, McGraw-Hill, NewYork.
2. General chemistry: principles and modern applications,, Ralph H. Petrucci et al, Pearson Canada Inc.
3. Chemistry, A. Burrows et al, Oxford University Press.

Mandatory course - Regular study - Chemistry