Large reference book on Chemistry EGE. Chemistry: Full Handbook for Preparing for EGE

The directory contains all theoretical Material at the rate of chemistry required for surchase EGE. It includes all the elements of the content being checked for the exam in chemistry, and helps to summarize and systematize the knowledge and skills for the course of the average (full) school. Theoretical material is set out in a brief, accessible form. Each section is accompanied by examples. test tasksallowing you to test your knowledge and degree of preparedness to the attestation exam. Practical tasks correspond to the format of the USE. At the end of the allowance, answers are answered to tests that will help schoolchildren and applicants check themselves and fill the existing gaps. The manual is addressed to senior schoolchildren, applicants and teachers.

The patterns of changing the properties of elements and their compounds in periods and groups.
Modern formulation of the Periodic Law D.I. Mendeleeva:
- the properties of the elements, as well as those formed by them simple and complex substances Are in periodic dependence on the charge of the atom kernel equal to the sequence number of the element.
Periodic system of chemical elements - natural classification Chemical elements, which is a table expression of the Periodic Law D.I. Mendeleeva. It is a table consisting of periods (horizontal series) and groups (vertical columns) of elements.
Group A \u003d number of valence electrons: NS and NP
Group number B \u003d number of valence electrons: NS and (N-1) D
In a short-range version of the periodic system - 8 groups. They are divided into subgroups A (main) and b (side).

In the long periodic variant of the periodic system - 18 groups. They are denoted or the same as in a short-period variant, or simply numbers from 1 to 18 (for example, a group Ia or 1, VIIB or 17).
Period number \u003d Energy levels filled with electrons \u003d designation of the last energy level (EU)
Modern periodic system includes 7 periods. Each period begins an element in the atom of which an electron appears in the corresponding energy level (hydrogen or an alkaline element), and the elements ended in the atom to the end the level with the same number (noble gas) is fully filled.

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Publication date: 08/10/2017 12:30 UTC

EGE 2020, Chemistry, 10 training options for examination work for preparation for a single state exam, Savinkina E.V., Zelaynova OG, 2019
Chemistry, full guide to prepare for EGE, Lidin R.A.
OGE, chemistry in tables and schemes, reference manual, 8-9 classes, Savinkina E.V., Loginova G.P., 2017
EGE-2019, chemistry, 10 training options for examination work for preparation for a single state exam, Savinkina E.V., Vynesova OG, 2019

The following textbooks and books:

Directory of Azotchik, Physico-chemical properties of gases and liquids, production of technological gases, cleaning of technological gases, ammonia synthesis, 1986

M.: 2017. - 256 p. M.: 2016. - 256 p.

The new reference book contains all theoretical material at the rate of chemistry necessary for the delivery of the USE. It includes all the elements of the content being checked by control and measuring materials, and helps to summarize and systematize knowledge and skills for the course of the average (full) school. Theoretical material is set forth in a brief and accessible form. Each topic is accompanied by examples of test tasks. Practical tasks comply with the format of the USE. At the end of the manual, answers are answered to tests. The manual is addressed to schoolchildren, applicants and teachers.

Format: PDF. ( 2017 , 256С.)

The size: 2 MB

Watch, download:drive.google

Format: PDF. ( 2016 , 256С.)

The size: 1.6 MB

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CONTENT
Preface 12.
The most important chemical concepts and laws 14
1. Theoretical Basics of Chemistry 18
1.1. Modern ideas On the structure of the atom 18
1.1.1. The structure of electronic shells of atoms of elements 18
Examples of tasks 24.
1.2. Periodic law and periodic system of chemical elements D.I. Mendeleev 25.
1.2.1. Patterns of changing the properties of elements and their compounds on periods and groups 25
Examples of tasks 28.
1.2.2. general characteristics IA-Sha-Group metals due to their position in the periodic system of chemical elements
DI. Mendeleev and the characteristics of the structure of their atoms 28
Examples of tasks 29.
1.2.3. Characteristics of transition elements (copper, zinc, chromium, iron) by their position in the periodic system of chemical elements D.I. Mendeleev
and the peculiarities of the structure of their atoms 30
Examples of tasks 30.
1.2.4. The overall characteristic of non-metals IVA-VIIA groups due to their position in the periodic system of chemical elements D.I. Mendeleev
and the characteristics of the structure of their atoms 31
Examples of tasks 31.
1.3. Chemical bond and structure of substance 32
1.3.1. Covalent chemical bond, its varieties and education mechanisms. Characteristics of covalent bond (polarity and communication energy). Ion connection.
Metal connection. Hydrogen bond 32.
Examples of tasks 36.
1.3.2. Electricity. The degree of oxidation and valence of chemical elements 37
Examples of tasks 39.
1.3.3. Molecular and non-elastic substances. Type of crystal lattice. The dependence of the properties of substances from their composition
and build 41.
Examples of tasks 43.
1.4. Chemical reaction 43.
1.4.1. Classification of chemical reactions in inorganic and organic chemistry 43
Examples of tasks 45.
1.4.2. The thermal effect of the chemical reaction. Thermochemical equations 46.
Job examples 48.
1.4.3. The rate of reaction, its dependence on various factors 48
Examples of tasks 50.
1.4.4. Reversible and irreversible chemical reactions. Chemical equilibrium. Displacement of chemical equilibrium under the action of various factors 50
For examples of tasks
1.4.5. Electrolytic dissociation electrolytes in aqueous solutions. Strong and weak electrolytes 53
Examples of tasks 54.
1.4.6. Ionic exchange reactions 54
Job examples 56.
1.4.7. Wednesday of aqueous solutions: sour, neutral, alkaline. Hydrolysis salts 57.
Examples of tasks 59.
1.4.8. Redox reactions. Corrosion of metals and ways to protect from it 60
Examples of tasks 64.
1.4.9. Electrolysis of melts and solutions (salts, alkalis, acids) 65
Job examples 66.
1.4.10. Ionic (rule V.V. Markovnikova) and radical mechanisms of reactions in organic chemistry 67
Job examples 69.
2. Inorganic Chemistry 71
2.1. Classification ne. organic substances. Nomenclature of inorganic substances (trivial and international) 71
Examples of tasks 75.
2.2. Characteristic chemical properties of simple substances - metals: alkaline, alkaline earth, aluminum; transition metals
(copper, zinc, chromium, iron) 76
Examples of tasks 79.
2.3. Characteristic chemical properties of simple substances - non-metals: hydrogen, halogen, oxygen, sulfur, nitrogen,
phosphorus, carbon, silicon 81
Examples of tasks 83.
2.4. Characteristic chemical properties of oxides: basic, amphoteric, acid 84
Job examples 86.
2.5. Characteristic chemical properties of bases and amphoteric hydroxides 87
Examples of tasks 88.
2.6. Characteristic chemical properties of acids 90
Examples of tasks 93.
2.7. Characteristic chemical properties of salts: medium, acidic, main; Complex (on the example of aluminum and zinc compounds) 94
Job examples 96
2.8. The relationship of various classes of inorganic substances 97
Examples of tasks 100.
3. Organic Chemistry 102
3.1. The theory of the structure of organic compounds: Homology and isomerism (structural and spatial).
Mutual influence of atoms in molecules 102
Examples of tasks 105.
3.2. Types of ties in organic substance molecules. Hybridization of carbon nuclear orbitals. Radical.
Functional group 106.
Examples of tasks 109.
3.3. Classification of organic substances. Nomenclature of organic substances (trivial and international) 109
Examples of tasks 115.
3.4. Characteristic chemical properties of hydrocarbons: alkanes, cycloalkanes, alkenes, dienes, alkins, aromatic hydrocarbons (benzene and toluene) 116
Examples of tasks 121.
3.5. Characteristic chemical properties of limit monatomic and polyhydric alcohols, phenol 121
Examples of tasks 124.
3.6. Characteristic chemical properties of aldehydes, limit carboxylic acids, esters of 125
Job examples 128.
3.7. Characteristic chemical properties of nitrogen-containing organic compounds: amines and amino acids 129
Examples of tasks 132.
3.8. Biologically important substances: fats, proteins, carbohydrates (monosaccharides, disaccharides, polysaccharides) 133
Examples of tasks 138.
3.9. The relationship of organic compounds 139
Examples of tasks 143.
4. Methods of knowledge in chemistry. Chemistry and life 145
4.1. Experimental Basics of Chemistry 145
4.1.1. Rules of work in the laboratory. Laboratory dishes and equipment. Safety rules when working with caustic, combustible and toxic substances,
Tools of household chemicals 145
Examples of tasks 150.
4.1.2. Scientific methods Research chemical substances and transformations. Methods for separating mixtures and purification of substances 150
Examples of tasks 152.
4.1.3. Determination of the nature of the aqueous solutions of substances. Indicators 152.
Examples of tasks 153.
4.1.4. Qualitative reactions on inorganic substances and ions 153
Job examples 156.
4.1.5. Quality reactions of organic compounds 158
Examples of tasks 159.
4.1.6. The main methods of obtaining (in the laboratory) of specific substances belonging to the studied classes inorganic connections 160
Examples of tasks 165.
4.1.7. Basic methods for producing hydrocarbons (in the laboratory) 165
Examples of tasks 167.
4.1.8. Basic ways to get oxygen-containing compounds (in the laboratory) 167
Job examples 170.
4.2. General ideas About industrial methods of obtaining essential substances 171
4.2.1. The concept of metallurgy: general methods Metals production 171.
Examples of tasks 174.
4.2.2. General scientific principles Chemical production (on an example of industrial production ammonia, sulfuric acid, methanol). Chemical pollution
Environment and its consequences 174
Examples of tasks 176.
4.2.3. Natural sources of hydrocarbons, their recycling 177
Examples of tasks 180.
4.2.4. High molecular compounds. Polymerization and polycondensation reactions 181
Examples of tasks 184.
4.3. Calculations by chemical formulas and reaction equations 184
4.3.1. Calculating the mass of the dissolved substance contained in a certain mass of the solution with a known mass fraction; Calculation of the mass fraction of substances in solution 184
Examples of tasks 186.
4.3.2. Calculations of volumetric gases in chemical reactions 186
Examples of tasks 187.
4.3.3. Calculations of the mass of a substance or gases on a known amount of substance, mass or volume of one
from those who participate in the reaction substances 187
Examples of tasks 188.
4.3.4. Calculations thermal Effect Reactions 189.
Examples of tasks 189.
4.3.5. Calculations of the mass (volume, amount of substance) of the reaction products, if one of the substances are given in excess (has impurities) 190
Examples of tasks 190.
4.3.6. Calculations of the mass (volume, amount of substance) of the reaction product, if one of the substances is given as a solution
With a certain mass fraction of a dissolved substance 191
Examples of tasks 191.
4.3.7. Finding the molecular formula of the substance 192
Examples of tasks 194.
4.3.8. Calculations of the mass or volume fraction of the reaction product output from theoretically possible 195
Examples of tasks 195.
4.3.9. Mass fractional calculations (mass) chemical compound In the mixture of 196.
Examples of tasks 196.
application
Chemistry elements 198.
Hydrogen 198.
IA Group elements 200
IIA-group elements 202
Elements of Sha-Group 204
IVA group elements 206
Elements of VA-Group 211
Elements of VTA-Group 218
Elements of VTIA-Group 223
Periodic system of chemical elements D.I. Mendeleev 230.
JUPAK: Periodic table of elements 232
The solubility of the bases, acids and salts in water 234
Valuation of some chemical elements 235
Acids and names of their salts 235
Atomic radii elements 236
Some of the most important physical constants 237
Consoles when making multiple
and dolle units 237
The prevalence of elements B. earth Kore 238
Answers to tasks 240

The new directory includes the entire theoretical material of the school course in chemistry necessary for the preparation and delivery of a single state exam.
The content of the book is based on control and measuring materials that determine the volume educational materialwhich is checked by state final certification.
The theoretical material of the directory is set out in a brief and accessible form. The clarity of the presentation and clarity of the educational material will allow to effectively prepare for the exam.
Each section of the book corresponds to the four substantive blocks verifiable for the exam: " Theoretical basis Chemistry "- Periodic law and a periodic system of chemical elements D.I. Mendeleev, chemical bond and structure of substance, chemical reaction; " Inorganic chemistry», « Organic chemistry"," Methods of cognition of chemistry. Chemistry and Life "- Experimental Fundamentals of Chemistry, General Representations on Industrial Methods of obtaining essential substances.

R. A. Lidin

Chemistry: Full Handbook for Preparing for EGE

Preface

Test tasks are compiled in such a way that, responding to them, the student will be able to more rationally repeat the main positions of the school course of chemistry.

At the end of the allowance, answers are answered to tests that will help schoolchildren and applicants check themselves and fill the existing gaps.

For the convenience of working with this directory, a table is provided, where the correspondence between the subject of the exam and the sections of the book is indicated.

The manual is addressed to senior schoolchildren, applicants and teachers.

1. Common items. The structure of atoms. Electronic shells. Orbital

Chemical element- a certain type of atoms, denoted by the title and symbol and characterized by a sequence number and relative atomic mass.

In tab. 1 listed common chemical elements, the characters they are designated (in brackets - pronunciation), sequence numbers, relative atomic masses, characteristic degrees of oxidation.

Zero The degree of oxidation of the element in its simple substance (substances) in the table is not specified.

All atoms of one element have the same number of protons in the kernel and the number of electrons in the shell. So, in the element atom hydrogen N is 1. p + in the kernel and peripherals 1 e.-; In an element atom oxygen Oh is 8. p + in the kernel and 8 e.- in the shell; Atom element aluminum Al contains 13. r+ in the kernel and 13 e.- In the shell.

Atoms of one element may differ in the number of neutrons in the nucleus, such atoms are called isotopes. So, the element hydrogen H Three isotope: hydrogen-1 (special name and symbol details 1H) with 1 p + in the kernel and 1 e.- in the shell; hydrogen-2. (deuterium 2N, or D) with 1 p + and 1 p0 in the kernel and 1 e.- in the shell; hydrogen-3. (tritium 3H, or T) with 1 p + and 2 p0 in the kernel and 1 e.- In the shell. In the characters 1H, 2N and 3N, the upper index indicates mass number- The sum of the numbers of protons and neutrons in the kernel. Other examples:

Electronic formula The atom of any chemical element in accordance with its location in the periodic system of elements D. I. Mendeleev can be determined by table. 2.

The electronic shell of any atom is divided into energy levels (1, 2, 3rd, etc.), levels are divided into sill (denoted by letters s, P, D, F). Sloves consist of out atomic orbitals - areas of space, where the electron presence is likely. The orbitals are designated as 1s (orbital of the level of the S-sub-line), 2 s., 2r, 3s., 3r, 3D, 4s.... Number of orbitals in sublevels:

Filling atomic orbitals by electrons occurs in accordance with three conditions:

1) the principle of minimum energy

Electrons are filled with orbital, starting with a slight energy.

The sequence of increasing energy of sublevels:

1s. < 2c. < 2p. < 3s. < 3p. < 4s. ≤ 3d. < 4p. < 5s. ≤ 4d. < 5p. < 6s.…

2) Prohibition rule (Pauli principle)

Each orbital can accommodate no more than two electrons.

One electron in orbitals is called unpaired, two electrons - electronic couple:

3) the principle of maximum multipleness (Hinda rule)

Within the subproduction, the electrons first fill out all the orbital half, and then - completely.

Each electron has its own characteristic - spin (conditionally depicted up or down arrow). The spins of electrons fold as the vectors, the sum of the spins of this number of electrons on the paragraph should be maximum (Multipleness):

Filling with electrons levels, sublevels and orbitals of atoms of elements from H (Z \u003d 1) to kr (Z \u003d 36) shown on energy diagram (The numbers respond to the fill sequence and coincide with the sequence numbers of the elements):

From the filled energy diagrams are derived electronic formulas Atoms of elements. The number of electrons in orbitals of this sublayer is indicated in the upper index to the right of the letter (for example, 3 d.5 is 5 electrons on s d.-provine); First there are electron levels of level 1, then the 2nd, 3rd, etc. The formulas can be complete and briefs, the latter contain a symbol of the corresponding noble gas in brackets than its formula is transmitted, and, above, starting with Zn filled with internal D-supel. Examples:

3Li \u003d 1S22S1 \u003d 2S1

8O \u003d 1s2 2s22p4. = 2s22p4.

13Al \u003d 1s22S22p6. 3S23P1 = 3S23P1

17Cl \u003d 1S22S22P6. 3S23p5 = 3S23p5

2Os \u003d 1S22S22P63S23P. 4S2. = 4S2.

21Sc \u003d 1S22S22P63S23P6. 3D14S2. = 3D14S2.

25mn \u003d 1S22S22P63S23P6. 3D54S2. = 3D54S2.

26Fe \u003d 1S22S22P63S23P6. 3D64S2. = 3D64S2.

3Ozn \u003d 1S22S22P63S23P63D10 4S2. = 4S2.

33as \u003d 1S22S22P63S23P63D10 4S24P3. = 4S24P3.

36Kr \u003d 1S22S22P63S23P63D10. 4S24P6. = 4S24P6.

Electrons made by brackets are called valentines. They are participating in the formation of chemical ties.

The exception is:

24Cr \u003d 1S22S22P63S23P6. 3D54S1 = ZD54S1 (and not 3D44S2!)

29CU \u003d 1S22S22P63S23P6. 3D104S1 = 3D104S1 (not 3D94S2!).

Examples of assignments of part a

1. name, do not relate To hydrogen isotopes, is

1) deuterium

2) Oxonius

2. The formula for valence pins of the metal atom is

3. The number of unpaired electrons is basically the state of the iron atom equals

4. In the excited state of the aluminum atom, the number of unpaired electrons is equal

5. The 3D94S0 electronic formula meets the cation

6. Electronic formula Anion E2- 3S23P6 meets the element

7. The total number of electrons in the MG2 + cation and anion is equal to

2. Periodic law. Periodic system. Electricity. Oxidation degree

Modern formulation of a periodic law, open by D. I. Mendeleev in 1869:

Properties of elements are in periodic dependence on the sequence number.

The periodically repeated nature of the change in the composition of the electronic shell of the atoms of elements explains the periodic change in the properties of the elements when moving through periods and groups of the periodic system.

Title: Chemistry. Full guide to prepare for the exam.

The directory includes the entire theoretical material of the school chemistry school, necessary for the delivery of the USE, the total certification of students. This material is distributed over 14 sections, the content of which corresponds to the themes verifiable for the exam, - four intensive blocks: "chemical element", "substance", "chemical reaction", "Cognition and use of substances and chemical reactions". For each section there are training tasks from parts A and B - with a choice of response and a brief answer. Section 15 is fully dedicated to solving the calculated tasks included in the examination part of C.
Test tasks are compiled in such a way that, responding to them, the student will be able to more rationally repeat the main positions of the school course of chemistry.
At the end of the allowance, answers are answered to tests that will help schoolchildren and applicants check themselves and fill the existing gaps.
For the convenience of working with this directory, a table is provided, where the correspondence between the subject of the exam and the sections of the book is indicated.
The manual is addressed to senior schoolchildren, applicants and teachers.

The chemical element is a certain type of atoms, denoted by the title and symbol and characterized by the sequence number and the relative atomic mass.
In tab. 1 lists common chemical elements, the characters that they are designated (in brackets - pronunciation), sequence numbers, relative atomic masses, characteristic degrees of oxidation.
The zero degree of element oxidation in its simple substance (substances) in the table is not specified.
The electronic shell of any atom is divided into energy levels (1, 2, 3 th, etc.), the levels are divided into subcloves (denoted by letters S, P, D, F). Subjects consist of atomic orbitals - areas of space, where the electron stay is likely. Orbitals are designated as 1s (orbital level S subeter), 2S, 2P, 3S, 3P, 3D, 4S ...

Content
Preface
1. Common items. The structure of atoms. Electronic shells. Orbital
2. Periodic law. Periodic system. Electricity. Oxidation degree
3. Molecules. Chemical bond. Structure of substances
4. Classification and interconnection of inorganic substances
5. Metals of the main subgroups of I-III groups
5.1. Sodium
5.2. Potassium
5.3. Calcium
5.4. Hardness of water
5.5. Aluminum
6. Transitional metals of the 4th period. Properties, methods of obtaining. General properties Metals
6.1. Chromium
6.2. Manganese
6.3. Iron
6.4. General properties of metals. Corrosion
7. Nonmetals of the main subgroups of IV-VII groups
7.1. Hydrogen
7.2. Halogens
7.2.1. Chlorine. Chloroorod
7.2.2. Chlorida
7.2.3. Hypochlorites. Chlorate
7.2.4. Bromides. Iodidi.
7.3. Hallcohele
7.3.1. Oxygen
7.3.2. Sulfur. Hydrogen sulfide. Sulfida
7.3.3. Sulphur dioxide. Sulfites
7.3.4. Sulfuric acid. Sulfates
7.4. Non-metals VA groups
7.4.1. Nitrogen. Ammonia
7.4.2. Nitrogen oxides. Nitric acid
7.4.3. Nitrit. Nitrate
7.4.4. Phosphorus
7.5. Non-metals IVA groups
7.5.1. Carbon in free form
7.5.2. Carbon oxides
7.5.3. Carbonates
7.5.4. Silicon
8. Theory of structure, manifold, classification and nomenclature of organic compounds. Types of chemical reactions
9. Hydrocarbons. Homology and isomeria. Chemical properties and methods of getting
9.1. Alkana. Cycloalkanes
9.2. Alkenes. Alkadien
9.3. Alkina
9.4. Arena
10. Oxygen-containing organic compounds
10.1. Alcohols. Simple ethers. Phenols
10.2. Aldehydes and Ketones
10.3. Carboxylic acids. Esters. Fat.
10.4. Carbohydrates
11. Nitrogen-containing organic compounds
11.1. Nitro compound. Amines
11.2. Amino acids. Proteins
12. Chemical reactions. Speed, energy and reversibility
12.1. Reaction speed
12.2. Energy reactions
12.3. Reversible reactions
13. Aqueous solutions. Solubility and dissociation of substances. Ion exchange. Hydrolysis of salts
13.1. Solubility of substances in water
13.2. Electrolytic dissociation
13.3. Dissociation of water. Wednesday solutions
13.4. Ion exchange reactions
13.5. Hydrolysis of salts
14. Redox reactions. Electrolysis
14.1. Oxidifiers and reducing agents
14.2. Selection of coefficients by electronic balance
14.3. A number of voltage metals
14.4. Electrolysis melt and solution
15. Decision of settlement tasks
15.1. Mass fraction of solutes. Dilution, concentration and mixing of solutions
15.2. Volumetric ratio of gases
15.3. Mass of a substance (gas volume) according to the number of other reagent (product)
15.4. Thermal reaction effect
15.5. Mass (volume, amount of substance) product on the reagent in excess or impurities
15.6. Mass (volume, amount of substance) of a reagent product with a known mass fraction in solution
15.7. Finding the molecular formula of the organic compound
Answers

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