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Section 1.
THEORETICAL FOUNDATIONS OF CHEMISTRY
1. Subject and tasks of chemistry.
– Physical and chemical phenomena.
– The place of chemistry among the natural sciences.
– Chemistry and ecology.
2. Fundamentals of atomic-molecular teaching.
– The concept of atom, element, substance.
– Relative atomic and relative molecular mass.
– A mole is a unit of quantity of a substance.
– Molar mass.
– Stoichiometry: law of conservation of mass of matter, constancy of composition. Relative gas density.
3. Chemical elements.
– Signs of chemical elements and chemical formulas.
– Simple substance, complex substance. Allotropy.
– Valency and oxidation state.
– Drawing up chemical formulas based on the valency of elements and atomic groups.
4. The structure of the atom.
– Atomic nucleus.
– Stable and unstable nuclei.
– Radioactive transformations, nuclear fission and nuclear fusion.
5. The dual nature of the electron.
– The structure of the electronic shells of atoms.
– Quantum numbers.
– Atomic orbitals.
– Electronic configurations of atoms in the ground and excited states.
6. Discovery of the periodic law by D.I. Mendeleev and the creation of the periodic system of chemical elements.
– Modern formulation of the periodic law.
– Structure of the periodic system: large and small periods, groups and subgroups.
– Dependence of the properties of elements and the compounds they form on the position of the element in the periodic table.
7. Types of chemical bonds:
– covalent (polar and non-polar),
– ionic,
– metallic,
– hydrogen.
– Mechanisms of formation and examples of compounds.
– Orbital hybridization model.
– Relationship between the electronic structure of molecules and their geometric
structure (using the example of compounds of elements of the second period).
8. Aggregate states of substances.
– The dependence of the transition of a substance from one state of aggregation to another on temperature and pressure.
– Gases.
– Laws of ideal gases. Mendeleev–Clapeyron equation.
– Avogadro’s law, molar volume.
– Liquids.
– Association of molecules in liquids.
– Solids.
– The main types of crystal lattices: cubic and hexagonal.
9. Classification of chemical reactions: reactions of connection, decomposition, substitution, exchange.
– Redox reactions.
– Determination of stoichiometric coefficients in the equations of redox reactions.
– Electrochemical voltage series of metals.
10. Thermal effects of chemical reactions.
– Thermochemical equations.
– Heat (enthalpy) of formation of chemical compounds.
– Hess’s law and consequences from it.
11. Rate of chemical reactions.
– Dependence of the reaction rate on the nature and concentration of reactants, temperature.
– Rate constant of a chemical reaction.
– Activation energy.
– Catalysis and catalysts.
12. Reversibility of chemical reactions.
– Chemical equilibrium and conditions for its displacement, Le Chatelier’s principle.
– Equilibrium constant, degree of conversion.
13. Solutions. Solubility of substances.
– The dependence of the solubility of substances on their nature, temperature and pressure.
– Ways to express the concentration of solutions (mass fraction, percentage concentration, molar concentration).
– Solid solutions.
– Alloys.
14. Strong and weak electrolytes.
– Electrolytic dissociation.
– Degree of dissociation.
– Ionic reaction equations.
– Properties of acids, salts and bases in the light of Arrhenius’s theory of electrolytic dissociation.
– Electrolysis of aqueous solutions and molten salts.
– Processes occurring at the cathode and anode.
Section 2.
INORGANIC CHEMISTRY
– Based on the periodic law, applicants should be able to give a comparative description of elements by groups and periods.
– Characteristics of an element include the electronic configuration of the atom;
possible valencies and oxidation states of the element in compounds; forms of simple substances and main types of compounds, their physical and chemical properties, laboratory and industrial methods of production; the prevalence of the element and its compounds in nature, the practical significance and areas of application of its compounds. When describing chemical properties, reactions involving inorganic and organic compounds (acid-base and redox transformations), as well as qualitative reactions, should be reflected.
1. The main classes of inorganic substances, their names (nomenclature), the genetic relationship between them.
2. Oxides and peroxides; types of oxides. Methods of preparation, properties of oxides and peroxides.
3. Bases, methods of preparation, properties. Alkalis, their preparation,
properties, application.
4. Acids, their classification, general properties, methods of preparation.
5. Salts, their composition, chemical properties, methods of production. Hydrolysis of salts.
6. Metals, their position in the periodic table. Physical and chemical properties. Main methods of obtaining. Metals and alloys in technology.
7. General characteristics of the main subgroup of group I of the periodic system of
chemical elements.
– Oxides, peroxides, hydroxides and salts of alkali metals. Potash fertilizers.
8. General characteristics of the elements of the main subgroup of group II of the periodic system of chemical elements.
– Calcium and its compounds. Water hardness and ways to eliminate it.
9. General characteristics of the elements of the main subgroup of group III of the periodic system of chemical elements.
– Aluminum. Amphotericity of aluminum oxide and hydroxide.
10. General characteristics of the elements of the main subgroup of group IV of the periodic system of chemical elements.
– Carbon, its allotropic modifications.
– Oxides of carbon (II) and (IV). Carbonic acid and its salts. Calcium and aluminum carbides.
11. Silicon.
– Silan.
– Magnesium silicide.
– Silicon(IV) oxide.
– Silicic acid and its salts.
12. General characteristics of the elements of the main subgroup of group V of the periodic system of chemical elements.
– Nitrogen.
– Ammonia, its industrial synthesis.
– Ammonium salts.
– Nitrides.
– Nitrogen oxides.
– Nitric and nitrous acids and their salts.
– Nitrogen fertilizers.
13. Phosphorus, its allotropic modifications.
– Phosphine, phosphides. Phosphorus (V) oxide, ortho-, meta- and diphosphoric acids and their salts.
– Phosphorus fertilizers.
14. General characteristics of the elements of the main subgroup of group VI of the periodic system of chemical elements.
– Oxygen, its allotropic modifications, properties of ozone.
– Oxides and peroxides.
15. Water, structure of water. Physical, chemical properties.
– Hydrogen peroxide.
– Crystal hydrates.
16. Sulfur.
– Hydrogen sulfide.
– Sulfides.
– Sulfur oxides (IV) and (VI), preparation, properties.
– Sulfuric and sulfurous acids, their properties; salts of sulfuric and sulfurous acids. Production of sulfuric acid.
17. Hydrogen, its interaction with metals, non-metals, oxides, organic compounds.
18. General characteristics of the elements of the main subgroup of group VII of the periodic system of chemical elements.
– Hydrogen halides.
– Halides. Oxygen-containing chlorine compounds.
19. General characteristics of transition metals.
20. Iron, its oxides and hydroxides, the dependence of their properties on the degree of oxidation of iron.
– Chemical reactions underlying the production of iron and steel. The role of iron and its alloys in technology.
Section 3.
ORGANIC CHEMISTRY
The characteristics of each class of organic compounds include features of the electronic and spatial structure of compounds of this class, patterns of changes in physical and chemical properties in the homologous series, nomenclature, types of isomerism, main types of chemical reactions and their mechanisms. Characteristics of specific compounds include physical and chemical properties, laboratory and industrial methods of preparation, and areas of application. When describing the chemical properties of compounds, it is necessary to take into account reactions involving both a radical and a functional group.
1. Theory of the chemical structure of organic compounds by A.M. Butlerov.
– Dependence of the properties of substances on their structure.
– Types of isomerism.
– The nature of chemical bonds in molecules of organic compounds, homo- and heterolytic methods of breaking bonds.
– The concept of free radicals.
2. Saturated hydrocarbons (alkanes and cycloalkanes), their electronic and spatial structure (sp3 hybridization).
– Nomenclature, isomerism.
3. Ethylene hydrocarbons (alkenes), their electronic and spatial structure (sp 2 – hybridization, s- and p-bonds).
– Nomenclature, isomerism.
– Markovnikov’s rule.
– Cycloalkenes.
– Conjugated diene hydrocarbons, features of their chemical properties.
4. Acetylene hydrocarbons (alkynes), their electronic and spatial structure (sp-hybridization, s- and p-bonds).
– Nomenclature. Acidic properties of alkynes.
– Kucherov’s reaction.
5. Aromatic hydrocarbons (arenes).
– Benzene, electronic and spatial structure (sp2 hybridization).
– Benzene homologues.
– The concept of the mutual influence of atoms using the example of toluene (reaction of an aromatic system and a hydrocarbon radical).
6. Natural sources of hydrocarbons: oil, natural and associated petroleum gases,
coal.
– Oil distillation.
– Cracking.
– Products obtained from petroleum, their application.
7. Alcohols. Primary, secondary and tertiary alcohols.
– Nomenclature, structure, chemical properties of monohydric alcohols.
– Polyhydric alcohols, nomenclature, special properties (ethylene glycol, glycerin).
8. Phenol, its structure, mutual influence of atoms in the molecule.
– Chemical properties of phenol, comparison with the properties of aliphatic alcohols.
9. Aldehydes and ketones.
– Nomenclature, structure, physical and chemical properties.
– Features of the carbonyl group. Formic and acetaldehydes, preparation, application.
10. Carboxylic acids.
– Nomenclature, structure, physical and chemical properties.
– Mutual influence of the carboxyl group and hydrocarbon radical.
– Saturated, unsaturated and aromatic acids.
– Examples of acids: formic (its features), acetic, stearic, oleic, benzoic.
11. Esters.
– Structure, chemical properties.
– Esterification reaction. Fats, their role in nature, chemical processing of fats (hydrolysis, hydrogenation).
12. Carbohydrates. Monosaccharides: ribose, deoxyribose, glucose, fructose.
– Their structure, physical and chemical properties, role in nature.
– Cyclic forms of monosaccharides.
– Polysaccharides: starch and cellulose.
– The meaning of carbohydrates in nature.
13. Amines.
– Aliphatic and aromatic amines.
– Mutual influence of atoms using the example of aniline.
– Primary, secondary and tertiary amines.
14. Amino acids and hydroxy acids.
– Structure, chemical properties, isomerism.
– Examples of hydroxy acids: lactic, tartaric, salicylic. a-Amino acids are the structural units of proteins.
– Peptides.
– Structure, biological role of proteins.
15. Pyrrole.
– Pyridine.
– Pyrimidine and purine bases that are part of nucleic acids.
– Understanding the structure of nucleic acids.
16. Polymerization and polycondensation reactions.
– General concepts of the chemistry of macromolecular compounds (HMCs): monomer, polymer, elementary unit, degree of polymerization (polycondensation).
– Examples of different types of HMCs.
