Lectures:
1.Basic terms. System composition, amount of substance, electronegativity, oxidation number.
2.Atom structure - atomic nucleus, radioactivity, mononuclear and binuclear reactions.
3.Atom structure – electron shell. Build-up principle, electron configuration.
4.Bonding types. Chemical bonding rise from the point of view of the quantum mechanics. Hybridization and molecule structure.
5.Periodic table. Metallic character, atomic radii, ionization energy, density, melting point.
6.States of matter. Phase diagram of one-component system. Ideal gas laws.
7.Gaseous mixtures. Real gases.
8.Dispersion systems. Solutions, Raoult’s law, Henry’s law. Atomic, metallic, ionic and molecular matters.
9.Classification of chemical reactions. Chemical kinetics. Factors influencing the chemical reaction rate.
10.Energetic changes at the chemical reactions. Internal energy, enthalpy, entropy, Gibbs energy.
11.Chemical equilibrium. The influence of temperature, pressure and concentration on the equilibrium mixture composition.
12.Electrolytic dissociation, ionic equations. Neutralization, precipitation reactions, hydrolysis, displacement of acids and bases.
13.Acid-base reactions. Acidity and basicity scale in aqueous solutions and ionic melts.
14.Oxidation-reduction reactions, electrode potential. Standard reduction potentials.
15.Stability of oxidation states. Frost diagrams.
16.Primary and secondary galvanic cells. Electrolysis of aqueous solutions and melts.
17.Chemistry of coordination compounds. Ligand types.
18.Theory of ligand field.
Computation exercises:
• Chemical nomenclature.
• Basic terms (amount of substance, multicomponent system composition).
• Calculations by the chemical formula.
• Ideal gas laws. Gaseous mixtures.
• Chemical equation and its evaluation.
• Solution preparation.
• Electrolytic dissociation, pH value determination.
• Oxidation-reduction reactions.
• Standard potentials and Frost diagrams.
• Rate of chemical reactions.
• Gibbs energy and equilibrium constant
1.Basic terms. System composition, amount of substance, electronegativity, oxidation number.
2.Atom structure - atomic nucleus, radioactivity, mononuclear and binuclear reactions.
3.Atom structure – electron shell. Build-up principle, electron configuration.
4.Bonding types. Chemical bonding rise from the point of view of the quantum mechanics. Hybridization and molecule structure.
5.Periodic table. Metallic character, atomic radii, ionization energy, density, melting point.
6.States of matter. Phase diagram of one-component system. Ideal gas laws.
7.Gaseous mixtures. Real gases.
8.Dispersion systems. Solutions, Raoult’s law, Henry’s law. Atomic, metallic, ionic and molecular matters.
9.Classification of chemical reactions. Chemical kinetics. Factors influencing the chemical reaction rate.
10.Energetic changes at the chemical reactions. Internal energy, enthalpy, entropy, Gibbs energy.
11.Chemical equilibrium. The influence of temperature, pressure and concentration on the equilibrium mixture composition.
12.Electrolytic dissociation, ionic equations. Neutralization, precipitation reactions, hydrolysis, displacement of acids and bases.
13.Acid-base reactions. Acidity and basicity scale in aqueous solutions and ionic melts.
14.Oxidation-reduction reactions, electrode potential. Standard reduction potentials.
15.Stability of oxidation states. Frost diagrams.
16.Primary and secondary galvanic cells. Electrolysis of aqueous solutions and melts.
17.Chemistry of coordination compounds. Ligand types.
18.Theory of ligand field.
Computation exercises:
• Chemical nomenclature.
• Basic terms (amount of substance, multicomponent system composition).
• Calculations by the chemical formula.
• Ideal gas laws. Gaseous mixtures.
• Chemical equation and its evaluation.
• Solution preparation.
• Electrolytic dissociation, pH value determination.
• Oxidation-reduction reactions.
• Standard potentials and Frost diagrams.
• Rate of chemical reactions.
• Gibbs energy and equilibrium constant