Chemistry program for applicants to Moscow University State University consists of two sections. The first section presents the main theoretical concepts chemistry, which the applicant must master in order to be able to substantiate the chemical and physical properties of the substances listed in the second section, devoted to elements and their compounds.

The examination ticket can contain up to 10 tasks with differentiated assessment, covering all sections of the program for applicants. Examples exam tasks recent years placed in collections (see the list of recommended readings at the end of the program). During the exam, you can use calculators and reference tables, such as the Periodic Table chemical elements", "Solubility of bases, acids and salts in water", "A number of standard electrode potentials".

Part I. Fundamentals of theoretical chemistry

Chemistry subject. The place of chemistry in natural science. Mass and energy. Basic concepts of chemistry. Substance. Molecule. Atom. Electron. And he. Chemical element. Chemical formula. Relative atomic and molecular mass. Mol. Molar mass.

Chemical transformations. Law of conservation of mass and energy. Law of constancy of composition. Stoichiometry.

The structure of the atom. Atomic nucleus. Isotopes. Stable and unstable nuclei. Radioactive transformations, nuclear fission and nuclear fusion. Radioactive decay equation. Half life.

The dual nature of the electron. Structure electron shells atoms. Quantum numbers. Atomic orbitals. Electronic configurations atoms in the ground and excited states, Pauli's principle, Hund's rule.

Periodic law of D.I. Mendeleev and its justification from the point of view of the electronic structure of atoms. Periodic table of elements.

Chemical bond. Types chemical bonds: covalent, ionic, metallic, hydrogen. Mechanisms of education covalent bond: exchange and donor-acceptor. Energy of communication. Ionization potential, electron affinity, electronegativity. Polarity of connection, inductive effect. Multiple connections. Orbital hybridization model. Connection electronic structure molecules with their geometric structure (using the example of compounds of elements of the 2nd period). Delocalization of electrons in conjugated systems, mesomeric effect. The concept of molecular orbitals.

Valency and oxidation state. Structural formulas. Isomerism. Types of isomerism, structural and spatial isomerism.

Aggregate states of matter and transitions between them depending on temperature and pressure. Gases. Gas laws. Clayperon-Mendeleev equation. Avogadro's law, molar volume. Liquids. Association of molecules in liquids. Solids. Main types crystal lattices: cubic and hexagonal.

Classification and nomenclature chemical substances. Individual substances, mixtures, solutions. Simple substances, allotropy. Metals and non-metals. Complex substances. The main classes are not organic matter: oxides, bases, acids, salts. Complex connections. The main classes of organic substances: hydrocarbons, halogen-, oxygen- and nitrogen-containing substances. Carbo- and heterocycles. Polymers and macromolecules.

Chemical reactions and their classification. Types of chemical bond breaking. Homo- and heterolytic reactions. Redox reactions.

Thermal effects chemical reactions. Thermochemical equations. Heat of formation chemical compounds. Hess's law and its consequences.

Speed chemical reaction. Understanding the mechanisms of chemical reactions. Elementary stage of the reaction. Homogeneous and heterogeneous reactions. Speed ​​dependence homogeneous reactions on concentration (law of mass action). Rate constant of a chemical reaction, its dependence on temperature. Activation energy.

The phenomenon of catalysis. Catalysts. Examples of catalytic processes. An idea of ​​the mechanisms of homogeneous and heterogeneous catalysis.

Reversible reactions. Chemical balance. Equilibrium constant, degree of conversion. Bias chemical equilibrium under the influence of temperature and pressure (concentration). Le Chatelier's principle.

Dispersed systems. Colloidal systems. Solutions. The mechanism of solution formation. Solubility of substances and its dependence on temperature and the nature of the solvent. Ways to express the concentration of solutions: mass fraction, mole fraction, molar concentration, volume fraction. Difference physical properties solution on the properties of the solvent. Solid solutions. Alloys.

Electrolytes. Electrolyte solutions. Electrolytic dissociation acids, bases and salts. Acid-base interactions in solutions. Protic acids, Lewis acids. Amphoteric. Dissociation constant. Degree of dissociation. Ionic product of water. pH value. Hydrolysis of salts. Equilibrium between ions in solution and solid phase. Product of solubility. Formation of the simplest complexes in solutions. Coordination number. Stability constant of complexes. Ionic equations reactions.

Redox reactions in solutions. Determination of stoichiometric coefficients in the equations of redox reactions. Standard potentials for redox reactions. A range of standard electrode potentials. Electrolysis of solutions and melts. Faraday's laws of electrolysis.

Part II. Elements and their connections.

Inorganic chemistry

Applicants must, based on the Periodic Law, give comparative characteristics elements in groups and periods. Characteristics of elements include: electronic configurations 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; prevalence of the element and its compounds in nature, practical significance and applications of the compounds. When describing chemical properties, reactions involving inorganic and organic compounds(acid-base and redox transformations), as well as qualitative reactions.

Hydrogen. Isotopes of hydrogen. Hydrogen compounds with metals and non-metals. Water. Hydrogen peroxide.

Halogens. Hydrogen halides. Halides. Oxygen-containing compounds chlorine

Oxygen. Oxides and peroxides. Ozone.

Sulfur. Hydrogen sulfide, sulfides, polysulfides. Sulfur oxides (IV) and (VI). Sulfurous and sulfuric acids and their salts. Esters of sulfuric acid. Sodium thiosulfate.

Nitrogen. Ammonia, ammonium salts, metal amides, nitrides. Nitrogen oxides. Nitrous and nitric acids and their salts. Ethers nitric acid.

Phosphorus. Phosphine, phosphides. Phosphorus (III) and (V) oxides. Phosphorus halides. Ortho-, meta- and diphosphoric acids. Orthophosphates. Esters of phosphoric acid.

Carbon. Carbon isotopes. The simplest hydrocarbons: methane, ethylene, acetylene. Calcium, aluminum and iron carbides. Oxides of carbon (II) and (IV). Transition metal carbonyls. Carbonic acid and its salts.

Silicon. Silan. Magnesium silicide. Silicon(IV) oxide. Silicic acids, silicates.

Bor. Boron trifluoride. Ortho- and tetraboric acids. Sodium tetraborate.

Noble gases. Examples of compounds of krypton and xenon.

Alkali metals. Oxides, peroxides, hydroxides and salts alkali metals.

Alkaline earth metals, beryllium, magnesium: their oxides, hydroxides and salts. Introduction to organomagnesium compounds (Grignard reagent).

Aluminum. Aluminum oxide, hydroxide and salts. Complex aluminum compounds. Ideas about aluminosilicates.

Copper, silver. Copper (I) and (II) oxides, silver (I) oxide. Copper(II) hydroxide. Silver and copper salts. Complex compounds of silver and copper.

Zinc, mercury. Zinc and mercury oxides. Zinc hydroxide and its salts.

Chromium. Chromium (II), (III) and (VI) oxides. Hydroxides and salts of chromium (II) and (III). Chromates and dichromates (VI). Complex compounds of chromium (III).

Manganese. Manganese (II) and (IV) oxides. Manganese(II) hydroxide and salts. Potassium manganate and permanganate.

Iron, cobalt, nickel. Oxides of iron (II), (II)-(III) and (III). Hydroxides and salts of iron (II) and (III). Ferrates (III) and (VI). Complex iron compounds. Salts and complex compounds of cobalt (II) and nickel (II).

Organic chemistry

Characteristics of each class of organic compounds include: features of the electronic and spatial structure of the 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 chemical properties, it is necessary to take into account reactions involving both a radical and a functional group.

Structural theory as the basis of organic chemistry. Carbon skeleton. Functional group. Homologous series. Isomerism: structural and spatial. Introduction to optical isomerism. Mutual influence of atoms in a molecule. Classification organic reactions on the mechanism and charge of active particles.

Alkanes and cycloalkanes. Conformers.

Alkenes and cycloalkenes. Conjugated dienes.

Alkynes. Acid properties alkynes

Aromatic hydrocarbons (arenes). Benzene and its homologues. Styrene Reactions aromatic system and a hydrocarbon radical. Orienting effect of substituents on the benzene ring (orientants of the first and second kind). The concept of condensed aromatic hydrocarbons.

Halogen derivatives of hydrocarbons: alkyl-, aryl-, and vinyl halides. Substitution and elimination reactions.

Simple and polyhydric alcohols. Primary, secondary and tertiary alcohols. Phenols. Ethers.

Carbonyl compounds: aldehydes and ketones. Saturated, unsaturated and aromatic aldehydes. The concept of keto-enol tautomerism.

Carboxylic acids. Saturated, unsaturated and aromatic acids. Mono and dicarboxylic acids. Carboxylic acid derivatives: salts, anhydrides, acid halides, esters, amides. Fats.

Nitro compounds: nitromethane, nitrobenzene.

Amines. Aliphatic and aromatic amines. Primary, secondary and tertiary amines. Basicity of amines. Quaternary ammonium salts and bases.

Halogenated acids. Hydroxy acids: lactic, tartaric and salicylic acids. Amino acids: glycine, alanine, cysteine, serine, phenylalanine, tyrosine, lysine, glutamic acid. Peptides. Understanding the structure of proteins.

Carbohydrates. Monosaccharides: ribose, deoxyribose, glucose, fructose. Cyclic forms monosaccharides. The concept of spatial isomers of carbohydrates. Disaccharides: cellobiose, maltose, sucrose. Polysaccharides: starch, cellulose.

Pyrrole. Pyridine. Pyrimidine and purine bases included in the composition nucleic acids. Understanding the structure of nucleic acids.

Polymerization and polycondensation reactions. Individual types high molecular weight compounds: polyethylene, polypropylene, polystyrene, polyvinyl chloride, polytetrafluoroethylene, rubbers, copolymers, phenol-formaldehyde resins, artificial and synthetic fibers.

• Kuzmenko N.E., Eremin V.V., Popkov V.A. The beginning of chemistry. Modern course for those entering universities. - M.: Exam, 1998-2006.
• Kuzmenko N.E., Eremin V.V., Popkov V.A. Chemistry for high school students and those entering universities. - M.: Bustard, 1995-2000; Peace and Education, 2004.
• Kuzmenko N.E., Eremin V.V. 2500 problems in chemistry for schoolchildren and applicants. - M.: Peace and Education, 2004.
• Chemistry. Formulas for success entrance exams/Ed. N.E. Kuzmenko and V.I. Terenina. - M.: Moscow University Publishing House, 2006.
• Chemistry: Reference materials/ Ed. Yu.D. Tretyakova. - M.: Astrel, 2002.
• Eremina E.A., Ryzhova O.N. Quick reference in chemistry for schoolchildren. - M.: Peace and Education, 2002-2006.
• Chemistry. Big reference book for schoolchildren and those entering universities. - M.: Bustard, 1999-2001.
• Kuzmenko N.E., Eremin V.V., Churanov S.S. Collection of competitive problems in chemistry. - M.: Exam, 2001, 2002, 2205.
• Fremantle M. Chemistry in action. In 2 parts - M.: Mir, 1991, 1998.
• Eremin V.V., Drozdov A.A., Kuzmenko N.E., Lunin V.V. Chemistry textbook for grades 8-9 secondary schools. - M.: Peace and Education, 2004-2006.

Biology is a set of sciences about living nature. Its name comes from Greek words"bios" - life and "logos" - teaching.

The subject of biology studies the structure and functions of living beings, their origin, development and distribution, natural communities, their relationships with each other and environment. All organisms that make up living nature - plants, animals and humans, are considered by biology in their historical development, movement, change and complication.

The proposed tests include questions on general biology, botany, zoology, anatomy, physiology and human hygiene, basics of genetics, ecology and biosphere, used in passing the Unified State Exam and on entrance exams to medical universities.

The biology test consists of

from 10 questions randomly selected from the database,

compiled based on the source

Bogdanova T.L. Biology. Assignments and exercises. A guide for applicants to universities. M., graduate School, 1991

When completing the test, mark what you think are the correct answers to the questions presented and click the “Finish” button at the bottom of the page. The test is considered passed if 100% correct answers are submitted within 10 minutes.

Taking the test is completely free,

does not require registration, sending SMS, phone number, etc.

Thanks, comments and wishes are accepted on the forum

Chemistry program for applicants to the Russian National research university consists of four sections. The first section presents the basic theoretical concepts of chemistry that an applicant must master. The second and third sections contain factual material on inorganic and organic chemistry, respectively. The fourth section provides the main types of calculations that an applicant must be able to perform. At the end of the program there is a list of basic literature that an applicant can use in preparation for the tests.

Part 1. general chemistry

Subject and tasks of chemistry. Chemical and physical phenomena. The relationship of chemistry with others natural disciplines. Chemistry and medicine.

Basic provisions of atomic-molecular teaching. Substances with molecular and non-molecular structure. Atoms, molecules, ions.

Relative atomic and relative molecular mass. Mol. Amount of substance. Molar mass.

Chemical transformations. Law of conservation of mass and energy. The law of constancy of the composition of matter. Stoichiometry.

Avogadro's law and consequences from it. Molar volume of gas. Normal conditions. Absolute and relative density gas Average molar mass gas mixture. Volume ratios of gases during chemical reactions. Clayperon-Mendeleev equation.

Chemical element. The structure of the nuclei of atoms of chemical elements. Isotopes. Stable and unstable nuclei. Radioactive transformations, nuclear fission and nuclear fusion. Half life.

Simple substance compound. Phenomena of allotropy and isomerism. Signs of chemical elements and chemical formulas. Valence and oxidation state of an atom.

The structure of the electronic shells of atoms. Energy levels and sublevels, atomic orbitals. Quantum numbers. Paired and unpaired electrons. Basic patterns of electron placement in atoms of elements of small and large periods. Electronic configurations of atoms in the ground and excited states, Pauli's principle, Hund's rule. s-, p-, d- and f-elements.

Discovery by D.I. Mendeleev periodic law and creation periodic table elements. Modern formulation periodic law. Reasons for the periodicity of the properties of elements. The meaning of the periodic law. Periods, groups and subgroups in the periodic table. Relationship between the properties of elements and their compounds with their position in the periodic table. Metals and non-metals.

Types of chemical bonds: covalent (polar and non-polar), ionic, metallic, hydrogen (intermolecular and intramolecular). - and -Bonds. Mechanisms of covalent bond formation (using unpaired electrons and donor-acceptor type). Energy of communication. Ionization potential, electron affinity, electronegativity. Valence possibilities atom.

Orbital hybridization model. Relationship between the electronic structure of molecules and their geometric structure (using the example of compounds of elements of the 2nd period).

Crystalline and amorphous substances. Main types of crystal lattices.

Classification of chemical reactions according to various signs: by the change in the oxidation states of atoms, by the number and composition of the initial and resulting substances, by the type of rupture of covalent bonds (by mechanism), by the thermal effect, by the sign of reversibility.

Redox reactions. Reduction and oxidation processes. Reducing agents and oxidizing agents.

Thermal effect of a chemical reaction. Heat of formation and heat of combustion of a substance. Thermochemical reaction equations. Thermal effects during dissolution various substances in water.

The rate of chemical reactions. Homogeneous and heterogeneous reactions. Dependence of the reaction rate on the nature of the reactants, concentration, temperature, contact surface. Kinetic equation of reaction, rate constant. Catalysis and catalysts. Homogeneous and heterogeneous catalysis. Inhibitors. Enzymes as biocatalysts.

Chemical balance. Equilibrium constant, degree of conversion. Shift in the position of chemical equilibrium under the influence various factors: concentrations of reactants, pressure, temperature. Le Chatelier's principle.

Solutions. Solutions concentrated and diluted, saturated and unsaturated. The dependence of the solubility of substances on their nature, pressure and temperature. Processes that occur when various substances are dissolved in water. Solubility coefficient. Methods of expressing the composition of a solution (mass fraction, molar concentration). Colloidal systems, reasons for their stability. Coagulation. Coarsely dispersed systems (suspensions and emulsions).

Electrolytic dissociation. Degree of dissociation. Strong and weak electrolytes. Ionic reaction equations. Conditions for the occurrence of chemical reactions in electrolyte solutions. Properties of acids, bases and salts in the light of the theory of electrolytic dissociation.

Part 2. Inorganic chemistry

Main classes of inorganic substances.

Oxides, classification of oxides. Methods for producing oxides. Their physical and chemical properties.

Bases, their classification, methods of preparation and chemical properties. Alkalis. Amphoteric hydroxides.

Acids, their classification, methods of preparation, physical and chemical properties.

Salts, their classification, nomenclature, methods of preparation and chemical properties. Hydrolysis of salts. Crystal hydrates.

Metals, their position in the periodic table. General physical and chemical properties of metals. Electrochemical voltage series of metals. Alloys. Corrosion of metals and its prevention. The main methods of obtaining metals.

Alkali metals, their general characteristics. Occurrence in nature, methods of production, physical and chemical properties. Important Connections alkali metals, their application. Sodium and potassium hydroxides, their preparation, properties and applications. Potash fertilizers.

General characteristics of elements main subgroup Group II of the periodic table, their oxides and hydroxides. Calcium, its occurrence in nature, production, physical and chemical properties. The most important calcium compounds, their preparation, properties and applications. Water hardness and ways to eliminate it.

Aluminum. Occurrence in nature, production, physical and chemical properties, application. Aluminum oxide, hydroxide and salts. Complex aluminum compounds. Ideas about aluminosilicates.

Side subgroup metals VIII group(iron, nickel, platinum). Their electronic structure. Iron, its occurrence in nature, production, physical and chemical properties, application. Oxides, hydroxides and salts of iron, their preparation and properties. Nickel and platinum, their physical and chemical properties, application.

Metals of secondary subgroups (copper, zinc, titanium, chromium, manganese). Their electronic structure, occurrence in nature, preparation, physical and chemical properties. Oxides, hydroxides and salts of these elements.

Hydrogen, its general characteristics, occurrence in nature. Isotopes of hydrogen. Methods for producing hydrogen in the laboratory and in industry, physical and chemical properties, application.

Halogens, their general characteristics. Halogen compounds in nature. Production of halogens. Application of halogens and their compounds. Chlorine. Production of chlorine in the laboratory and in industry. Its physical and chemical properties. Preparation, properties and applications of hydrogen chloride, of hydrochloric acid and its salts. Connections with positive powers oxidation of chlorine.

General characteristics of the elements of the main subgroup of group VI of the periodic system. Sulfur, its occurrence in nature, production, allotropy, physical and chemical properties, application. Sulfur oxides, their preparation and properties. Hydrogen sulfide and sulfides, their preparation and properties. Sulfuric acid, its electronic structure, preparation, physical and chemical properties, application. Salts of sulfuric acid. Sulfurous acid and its salts.

Oxygen. Its presence in nature. Allotropy of oxygen. Preparation and properties of ozone. Oxygen production in the laboratory and in industry. Its physical and chemical properties. The role of oxygen in nature, its use.

Water. The structure of the water molecule and hydronium ion. Physical and chemical properties of water. Hydrogen and metal peroxides, their preparation and properties.

General characteristics of the elements of the main subgroup of group V of the periodic table. Phosphorus, its occurrence in nature, its production. Allotropy of phosphorus, physical and chemical properties, application. Phosphides and phosphine. Phosphorus(III) and (V) oxides. Phosphorus halides. Ortho-, meta- and diphosphoric acids. Their preparation and chemical properties. Salts of phosphoric acid. Phosphorus fertilizers.

Nitrogen, its general characteristics, occurrence in nature, production. Electronic structure of the nitrogen molecule. Physical and chemical properties of nitrogen. Nitrides. Ammonia, the structure of its molecule, preparation, physical and chemical properties, application. Nitrogen oxides and nitric acid. The structure of the nitric acid molecule, its preparation and chemical properties, application. Properties of nitric acid salts. Nitrogen fertilizers.

General characteristics of the elements of the main subgroup of group IV of the periodic table of elements. Silicon, its occurrence in nature, production, physical and chemical properties, application. Silicon(IV) oxide and silicic acid, their chemical properties. Silicic acid salts.

Carbon. Its general characteristic is being in nature. Allotropy of carbon. Production of carbon, its physical and chemical properties, application. Carbon oxides and carbonic acid. Their preparation and properties. Salts carbonic acid, their preparation, properties and application.

Qualitative reactions to inorganic substances and ions.

Part 3. Organic chemistry

Theory chemical structure organic compounds by A.M. Butlerov. Dependence of the properties of organic compounds on their structure. Types of isomerism. Electronic nature of chemical bonds in organic compounds. Types of covalent bond cleavage in reactions of organic compounds. Free radicals.

Homologous series saturated hydrocarbons(alkanes). Their electronic structure, isomerism, nomenclature. Conformations. Methods for obtaining alkanes, their physical and chemical properties, application.

Cycloalkanes, their structure, isomerism, nomenclature. Methods of preparation and chemical properties of cycloalkanes.

Ethylene hydrocarbons (alkenes). Their electronic structure, isomerism, nomenclature. Geometric isomerism. Preparation, physical and chemical properties of alkenes. Markovnikov's rule. Application of alkenes.

Alkadienes. Electronic structures, isomerism, nomenclature. Preparation, chemical properties and use of alkadienes.

Alkynes. Electronic structure, isomerism, nomenclature. Acidic properties of alkynes. Methods of preparation, physical and chemical properties of alkynes. Application.

Aromatic hydrocarbons (arenes). Electronic structure of the benzene molecule. Isomerism and nomenclature of benzene homologues. Preparation of benzene and its homologues. Chemical properties aromatic hydrocarbons. Orienting effect of substituents on the benzene ring. Mutual influence of atoms in a molecule using the example of toluene. Styrene Application of aromatic hydrocarbons.

Halogen derivatives of various classes of hydrocarbons. Their methods of preparation and chemical properties.

Natural sources of hydrocarbons: oil, natural and associated gas, coal. Processes occurring during their processing.

Alcohols. Their classification, isomerism, nomenclature. Electronic structure of the molecule ethyl alcohol. Homological limit series monohydric alcohols, methods of their preparation, physical and chemical properties, application. Polyhydric alcohols, methods of their preparation, chemical properties and application.

Phenols. Electronic structure of phenol. Methods for producing phenol, its physical and chemical properties. Mutual influence of atoms in a phenol molecule. Comparison of the properties of phenol with the properties of alcohols. Application of phenol.

Ethers, their structure and methods of preparation.

Carbonyl compounds. Aldehydes and ketones. Electronic structure of the carbonyl group. Isomerism and nomenclature of aldehydes, their methods of preparation, physical and chemical properties. Application.

Carboxylic acids. Electronic structure of the carboxyl group. Dependence of the strength of carboxylic acids on the structure of the organic radical. Nomenclature and isomerism of monobasic carboxylic acids. Methods for producing carboxylic acids, their physical and chemical properties. Application. Unsaturated carboxylic acids (acrylic, methacrylic). Oxalic acid.

Esters, their structure and nomenclature. Receipt esters, their physical and chemical properties, application. Fats as representatives of esters, their role in nature, fat processing. Carboxylic acids that are part of fats (stearic, palmitic, oleic, linoleic and linolenic). Soaps and other cleaning products.

Nitro compounds. Nitromethane and nitrobenzene.

Carbohydrates. Classification of carbohydrates. Monosaccharides (glucose, fructose, ribose and deoxyribose), their structure. Cyclic forms of monosaccharides. Physical and chemical properties of glucose, its application. Disaccharides: cellobiose, maltose and sucrose, their structure and properties. Polysaccharides (starch and cellulose). Their structure, location in nature, biological role, chemical properties and applications. Dextrins.

Amines, their electronic structure, isomerism, nomenclature. Preparation of amines, physical and chemical properties. Amines as organic bases. Comparison of the basic properties of various amines and ammonia. Manifestation of the mutual influence of atoms in the aniline molecule.

Hydroxy acids. Lactic acid. Optical isomerism.

Amino acids. Their isomerism and nomenclature. Preparation, physical and chemical properties of amino acids. a-Amino acids that make up proteins (glycine, alanine, valine, phenylalanine, tyrosine, serine, cysteine, glutamic acid, lysine, tryptophan). Peptides. Primary, secondary and tertiary structure of protein. Properties of proteins.

General concepts of the chemistry of high-molecular compounds: monomer, polymer, structural link, degree of polymerization, stereoregularity of the polymer. Polymerization and polycondensation reactions. Polymers obtained by polymerization reaction (polyethylene, polypropylene, polyvinyl chloride, polymethyl methacrylate). Rubbers. Natural and synthetic rubbers. Vulcanization of rubbers. Polymers obtained by polycondensation reaction. Phenol-formaldehyde resins. Synthetic fibers nylon and lavsan. Artificial fibers (silk acetate). Biopolymers.

Qualitative reactions to various classes of organic substances.

Part 4. Basic types of calculations that an applicant must master

Calculation molar mass substance based on its formula or relative and absolute density(for gases).

Calculation of the amount of a substance based on its mass or volume (for gases).

Bringing the volume of gas to normal conditions.

Definition mass fractions elements in a substance, based on its formula.

Determination of the formula of a substance based on elemental analysis data.

Calculation of solution composition (mass fractions of dissolved substances or their molar concentrations)

Stoichiometric calculations using equations of chemical reactions in moles (in volumes for reactions involving gases)

Finding coefficients in the equations of redox reactions using the electronic balance method.

The simplest thermochemical calculations.

Determination of the rate of a chemical reaction by the change in the amount of a substance over a certain time interval, according to kinetic equation reactions, recalculation of the reaction rate when temperature changes (according to the Van't Hoff equation).

Modern school books in chemistry for classes with in-depth study chemistry.

Kuzmenko N.E., Eremin V.V., Popkov V.A. The beginning of chemistry. Modern course for applicants to universities. - M.: Exam, 1998-2012.

Slesarev V.I. and others. Chemistry simulator. Khimizdat. St. Petersburg 2003.

Chemistry. A large reference book for schoolchildren and those entering universities. - M.: Bustard, 1999-2001.

Belavin I.Yu. Solving problems in chemistry. RGMU. M. 2009.