This manual contains in a visual form a course of organic chemistry, studied in grades 10-11 of a comprehensive school. The manual can be used when studying, summarizing and repeating educational material, and can also be useful in organizing systematic repetition in preparation for final or entrance exams.
Theory of radicals (30 years of the XIX century. J. Berzelius, J. Liebig, J. Dumas)
a) organic substances contain radicals;
b) radicals are always constant, do not undergo changes, pass from one molecule to another;
c) radicals can exist in free form.
The concept of "radical" is firmly established in chemistry. The theory was subsequently rejected.
Theory of types (40-50s of the 19th century. C. Gerard, A. Kekule and others)
a) all organic substances - derivatives of the simplest inorganic substances - such as hydrogen, water, ammonia, etc.
b) the formulas do not express the internal structure of the molecule, but the methods of formation, the properties determine all the atoms of the molecule.
c) it is impossible to know the structure of matter, each substance has as many formulas as there are transformations.
The theory made it possible to classify organic substances, to predict and discover some, with special attention to chemical transformations, but could not predict, indicate the ways of synthesis of new substances.
Content
I. Theory of the chemical structure of organic compounds
1 The emergence of organic chemistry as a science (1807 J. Berzelius) 3
2. Organic and inorganic substances. Composition and some properties of organic substances 4
3. Pre-structural theories 5
4. Connection between the concepts of the theory of chemical structure 6
5. Prerequisites for the emergence of the theory of the chemical structure of organic substances 7
6. Theory of chemical structure. Basic provisions (1,2) 8
7. Theory of chemical structure. Basic provisions (3.4) 9
8. Theory of chemical structure. Key points (5) 10
9. Algorithm for searching for possible isomers of alkanes (isomerism of the carbon skeleton) 11
10. Classification of chemical compounds typical of organic compounds (according to the type of chemical transformations) 12
11. Classification of chemical compounds typical of organic compounds (according to the type of bond breaking) 13
12. Classification of hydrocarbons 14
II. Limit hydrocarbons
1. Methane. physical properties. Molecule structure 15
2. Sp3 hybridization 16
3. Alkanes 17
4. Isomers and homologues 18
5. Alkanes (unbranched structure) and alkyls 19
6. Nomenclature (rational) 20
7. Nomenclature (systematic) 21
8. Determination of the qualitative composition of organic compounds 22
9. Chemical properties of alkanes 23
10. Obtaining alkanes 24
11. Use of alkanes 25
12. Cycloalkanes (cycloparaffins, naphthenes) 26
III. Unsaturated hydrocarbons
1. Ethylene (ethene). The structure of the molecule. sp2 hybridization 27
2. Alkenes (olefins, ethylene hydrocarbons) 28
3. Properties of alkenes 29
4. Properties of alkenes 30
5. Use of alkenes 31
6. Obtaining alkenes 32
7. Diene hydrocarbons (alkadienes) 33
8. Chemical properties of alkadienes (with conjugated bonds) Preparation 34
9. General characteristics of rubbers. Their structure and properties 35
10. Acetylene (ethyne). Molecule structure sp-hybritization 36
11. Comparison of the structure of the solecule of ethane, ethylene and acetylene. Comparison of o and ts connections 37
12. Alkynes (acetylenic hydrocarbons) 38
13. Chemical properties of alkynes 39
14. Chemical properties of alkynes 40
15. Application of acetylene 41
16. Obtaining acetylene and its homologues 42
IV. aromatic hydrocarbons
1. Benzene. physical properties. Formula Kekule 43
2. Electronic structure of benzene 44
3. Chemical properties of benzene 45
4. Chemical properties of benzene 46
5. Arenes (Aromatic hydrocarbons. Alkylbenzenes) 47
6. Toluene. Chemical properties. Mutual influence of atoms in a toluene molecule 48
7. Orientation rules in the benzene ring 49
8. The use of benzene. Getting arenas 50
9. Styrene. Naphthalene. Anthracene 51
10. Genetic relationship between groups of hydrocarbons 52
11. General information about hydrocarbon groups 53
12. General information about hydrocarbon groups 54
V. Alcohols and phenols
1. Limit monohydric alcohols 55
2. Chemical properties of alcohols 56
3. Ethanol (Ethyl alcohol) 57
4. Application of saturated monohydric alcohols 58
5. Methods for obtaining alcohols 59
6. Limit polyhydric alcohols 60
7. Ethers 61
8. Phenols 62
9. Chemical properties of phenol (by hydroxo group) 63
10. Chemical properties of phenol (on the benzene ring) 64
VI. Aldehydes and carboxylic acids
1. Aldehydes. Structure. Nomenclature. Isomerism 65
2. Formaldehyde. Receipt. Properties 66
3. Properties of aldehydes 67
4. Properties of aldehydes 60
5. Ketones G9
6. Preparation of aldehydes and ketones 70
7. Carboxylic acids. Homologous series 71
8. Some saturated monobasic acids 72
9. Carboxylic acids. Properties 73
10. Chemical properties of saturated monobasic carboxylic acids 74
11. Chemical properties of saturated monobasic carboxylic acids 15
12. Obtaining carboxylic acids 76
13.0 separate representatives of carboxylic acids. Classification 77
14. Separate representatives of carboxylic acids 78
VII. Complex ethers. Fats
1. Esters 79
2. Chemical properties of esters 80
3. Fats. Classification. Getting 81
4. Chemical properties of fats 82
5. Soaps 83
6. Synthetic detergents (CMC) 84
VIII. hydrocarbons
1. Carbohydrates. Compound. Classification 85
2. Glucose. Structure. Fructose 86
3. Glucose. Chemical properties 87
4. Glucose. Special properties. Application 88
5. Sucrose. Structure. Properties 89
6. Polysaccharides (CeH-mOsJn. Natural polymers 90
7. Starch and cellulose. Chemical properties 91
IX. Amines. Amino acids. Squirrels
1. Amines. Compound. Nomenclature. Isomerism 92
2. Amines. Chemical properties 93
3. Aniline. Structure. Properties 94
4. Amino acids. Nomenclature. Isomerism 95
5. Amino acids. Properties 96
6. Some amino acids of proteins 97
7. Obtaining and using amino acids 98
8. Proteins. Compound. Building 99
9. Protein structures 100
10. Chemical properties of proteins 101
11. Isomerism of classes of compounds 102
12. Genetic connection of organic substances 103
X Application
1. Qualitative reactions of organic compounds 104
2. Qualitative reactions of organic compounds 105
3. Periodic system of chemical elements 106
4. Symbols 107.
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Chemistry. (The whole school course in diagrams and tables) Barabbas N.E.
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The entire school course in chemistry is presented in the form of logical diagrams and informative tables. A visual, clear and schematic presentation of the material allows you to quickly assimilate a large amount of information, facilitate understanding of complex laws, concepts, definitions, generalize and systematize knowledge. The publication will help students effectively prepare for the exam in chemistry.
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Content
1. THEORETICAL FOUNDATIONS OF CHEMISTRY
1.1. Chemical element 8
1.1.1. Modern ideas about the structure of the atom. The structure of the electron shells of atoms
elements of the first four periods: s-, p- and d-elements. The electronic configuration of the atom. Ground and excited states of atoms 8
1.1.2. Periodic law and Periodic system of chemical elements of D. I. Mendeleev.
Radii of atoms, their periodic changes in the system of chemical elements. Patterns of changes in the chemical properties of elements and their compounds by periods and groups 30
1.2. Chemical bond and structure of matter 33
1.2.1. Covalent chemical bond, its varieties (polar and non-polar), formation mechanisms. Characteristics of a covalent bond (bond length and energy). Ionic bond. Metal connection. Hydrogen bond 33
1.2.2. Electronegativity. The degree of oxidation and valence of chemical elements 40
1.2.3. Substances of molecular and non-molecular structure. Dependence of the properties of substances on the features of their crystal lattice 41
1.3. Inorganic Chemistry 45
1.3.1. Classification and nomenclature of inorganic substances 45
1.3.2. General characteristics of metals of the main subgroups of groups I-III in connection with their position in the Periodic system of chemical elements of D. I. Mendeleev and structural features of their atoms 46
1.3.3. Characteristics of transition elements - copper, zinc, chromium, iron - according to their position in the Periodic system of chemical elements of D.I. Mendeleev and the structural features of their atoms 47
1.3.4. General characteristics of non-metals of the main subgroups of groups IV-VII in connection with their position in the Periodic system of chemical elements of D.I. Mendeleev and structural features of their atoms 49
1.3.5. Characteristic chemical properties of simple substances - metals: alkali, alkaline earth, aluminum, transition metals (copper, zinc, chromium, iron) 53
1.3.6. Characteristic chemical properties of simple substances - non-metals: hydrogen, halogens, oxygen, sulfur, nitrogen, phosphorus, carbon, silicon 71
1.3.7. Characteristic chemical properties of oxides: basic, amphoteric, acidic 106
1.3.8. Characteristic chemical properties of bases and amphoteric hydroxides 109
1.3.9. Characteristic chemical properties of acids 113
1.3.10. Characteristic chemical properties of salts: medium, acidic, basic; complex (by the example of aluminum and zinc compounds). . . 118
1.4. Organic chemistry 128
1.4.1. Theory of the structure of organic compounds. Isomerism - structural and spatial. Homology and homology series 128
1.4.2. Types of bonds in molecules of organic substances. Hybridization of atomic orbitals of carbon. Radical. Functional group 133
1.4.3. Classification and nomenclature of organic compounds 135
1.4.4. Characteristic chemical properties of hydrocarbons: alkanes, cycloalkanes, alkenes, dienes, alkynes 138
1.4.5. Characteristic chemical properties of aromatic hydrocarbons: benzene and toluene 148
1.4.6. Characteristic chemical properties of saturated monohydric and polyhydric alcohols; phenol 152
1.4.7. Characteristic chemical properties of aldehydes, saturated carboxylic acids, esters 157
1.4.8. Characteristic chemical properties of nitrogen-containing organic compounds: amines and amino acids 163
1.4.9. Biologically important substances: fats, proteins, carbohydrates (monosaccharides, disaccharides, polysaccharides) 166
1.5. Chemical reaction 172
1.5.1. Classification of chemical reactions in inorganic and organic chemistry 172
1.5.2. Thermal effect of a chemical reaction. Thermochemical equations 174
1.5.3. Reaction rate, its dependence on various factors 175
1.5.4. Reversible and irreversible chemical reactions. chemical balance. Displacement of chemical equilibrium under the influence of various factors 177
1.5.5. Electrolytic dissociation of electrolytes in aqueous solutions. Strong and weak electrolytes 179
1.5.6. Ion exchange reactions 182
1.5.7. Salt hydrolysis. Environment of aqueous solutions: acidic, neutral, alkaline 183
1.5.8. Redox reactions. Corrosion of metals and methods of protection against it. . 185
1.5.9. Electrolysis of melts and solutions (salts, alkalis, acids) 188
1.5.10. Mechanisms of substitution and addition reactions in organic chemistry. Rule V. V. Markovnikov 189
1.5.11. Reactions confirming the relationship of different classes 191
2. METHODS OF KNOWLEDGE OF SUBSTANCES AND CHEMICAL REACTIONS
2.1. Experimental Foundations of Chemistry 193
2.1.1. Rules for working in the laboratory. Safety rules when working with caustic, combustible and toxic substances, household chemicals 193
2.1.2. Scientific methods for the study of chemicals and transformations. Methods for separating mixtures and purifying substances 195
2.1.3. Determination of the nature of the environment of aqueous solutions of substances. Indicators 196
2.1.4. Qualitative reactions to inorganic substances and ions. Identification of organic compounds 196
2.2. General methods for obtaining substances 203
2.2.1. General methods for obtaining metals. General scientific principles of chemical production (on the example of industrial production of ammonia, sulfuric acid, methanol) 204
2.2.2. Natural sources and processing of hydrocarbons 207
2.2.3. high molecular weight compounds. Reactions of polymerization and polycondensation. Polymers. Plastics, fibers, rubbers 209
2.2.4. Reactions characterizing the main properties and methods of obtaining 212
2.3. Calculations by chemical formulas and reaction equations 217
2.3.1. Calculation of the mass of a solute contained in a certain mass of a solution with a known mass fraction 224
2.3.2. Calculations: volume ratios of gases in chemical reactions 225
2.3.3. Calculation of the mass of a substance or volume of gases from a known amount of a substance, mass or volume of one of the substances participating in the reaction 226
2.3.4. Calculation of the thermal effect of a reaction 229
2.3.5. Calculation of the mass (volume, amount of substance) of the reaction products, if one of the substances is given in excess (has impurities) 231
2.3.6. Calculation 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 the dissolved substance 233
2.3.7. Finding the molecular formula of a substance. 234
2.3.8. Calculation of the mass or volume fraction of the yield of the reaction product from the theoretically possible 236
2.3.9. Calculation of the mass fraction (mass) of a chemical compound in a mixture 238
This reference manual contains the main material of the school chemistry course superimposed in a concise and accessible form: general chemistry, inorganic chemistry, organic chemistry. The manual is designed in the form of tables and diagrams. Recommended for schoolchildren, applicants and school teachers.
Periodic law.
The properties of chemical elements, as well as the forms and properties of compounds of elements, are in a periodic dependence on the charge of the nuclei of their atoms.
1. The serial number of the element is equal to the charge of the nucleus and the number of electrons.
2. Period number - the number of levels.
3. Group number - valency (maximum positive oxidation state).
4. The metallic properties of the elements increase from top to bottom and from right to left. These properties are exhibited by elements with a small number of valence electrons.
GENERAL CHEMISTRY
Basic concepts and laws of chemistry.
Atomic-molecular doctrine.
Moth. The molar mass of a substance.
Chemical reactions.,
The law of conservation of mass of matter.
The law of the constancy of the composition of matter.
gas laws.
Periodic law of D.I. Mendeleev.
The structure of the atom.
Model of the state of an electron in an atom.
Periodic law.
Chemical bond.
covalent bond.
Ionic bond.
polar molecules. non-polar molecules.
Metal connection.
Hydrogen bond.
Crystal cell. Types of crystal lattices.
Structural formulas.
The degree of oxidation.
Valence.
The rate of chemical reactions, chemical equilibrium.
Activation energy.
The concept of catalysis and catalysts.
Reversible and irreversible reactions.
chemical balance. Le Chatelier's principle.
Solutions. Theory of electrolytic dissociation.
Numerical expression of the composition of solutions.
Solubility of substances in water.
Thermal phenomena during dissolution.
Electrolytes and non-electrolytes.
Theory of electrolytic dissociation. Mechanism.
Dissociation of acids, bases and salts in aqueous solutions.
Degree of dissociation. Ion exchange reactions.
dissociation of water.
The most important classes of inorganic compounds.
Oxides.
Acids.
Hydroxides.
Salt.
Redox reactions.
Theory of redox reactions.
Drawing up equations of redox reactions.
Influence of the environment on the nature of the reactions.
Classification.
Electrolysis.
INORGANIC CHEMISTRY.
Hydrogen.
Hydrogen compounds.
alkali metals. I group. Main subgroup.
alkaline earth metals. IIA group. (Calcium).
Group III A elements (Aluminum).
Group IV A elements (Carbon, silicon).
Elements of the UA group (nitrogen, phosphorus).
Group VIA elements. Chalcogens (oxygen, sulfur).
Elements of group VIIA. Halogens (Chlorine).
Elements of secondary subgroups.
Chromium subgroup.
subgroup of iron.
ORGANIC CHEMISTRY.
Hydrocarbons.
Limit hydrocarbons.
unsaturated hydrocarbons.
aromatic hydrocarbons.
Oxygen-containing organic compounds.
Alcohols.
Phenols.
Aldehydes.g.
Polycondensation.
Ketones.
carboxylic acids.
Complex ethers.
Nitrogen-containing organic compounds.
Amines.
Aniline.
Amino acids.
Squirrels.
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transcript
1 E.V. Savinkina G.P. Loginova CHEMISTRY IN TABLES AND SCHEMES Reference manual classes Publishing house AST Moscow
2 UDC 373:54 BBC 24ya721 С13 С13 Savinkina, Elena Vladimirovna. Chemistry in tables and diagrams: a reference guide: classes / E.V. Savinkina, G.P. Loginova. Moscow: AST Publishing House, (1) p. ISBN (LLC "Publishing house AST") (New school curriculum) ISBN (LLC "Publishing house AST") (Preparation for the unified state exam) The reference book presents a school chemistry course in the form of accessible diagrams and tables. Visual, simple and convenient presentation of the material contributes to its better assimilation and memorization. The book will provide effective assistance in the study of new and repetition of topics covered, as well as in preparing for the unified state exam in the course of chemistry. Chemistry teachers can use it in the classroom as reference charts. UDC 373:54 LBC 24ya721 ISBN (LLC AST Publishing House) (New school curriculum) ISBN (LLC AST Publishing House) (Preparation for the unified state exam) Savinkina E.V., Loginova G.P. AST Publishing House LLC
3 CONTENTS Foreword THEORETICAL FOUNDATIONS OF CHEMISTRY Structure of the atom Table 1. Atom Table 2. Fundamentals of the quantum theory of atomic structure Table 3. Energy levels and sublevels Scheme 1. Orbital shapes Table 4. Rules for filling atomic orbitals (in the ground state of the atom) Scheme 2. Sequence filling AO with electrons Table 5. Blocks of elements Table 6. Electronic configurations of neutral atoms in the ground state for elements of the first four periods Periodic law D.I. Mendeleev Table 7. Numbers of periods and groups Table 8. Patterns of changes in properties in groups Table 9. Patterns of changes in properties in periods Table 10. Changes in the composition and properties of hydrogen compounds, higher oxides and hydroxides of elements of the 3rd period of the periodic system
4 4 Chemical bond Table 11. Types of chemical bond Table 12. Description of covalent bond Table 13. Mechanisms of covalent bond formation Table 14. Multiple bonds Scheme 3. Orbital overlap Table 15. Formulas of molecules Table 16. Chemical bond parameters Table 17. Valency. Oxidation state Table 18. Determination of the oxidation state Table 19. Types of crystal lattices Classification of chemical reactions Table 20. Classification by changes in the composition of substances Table 21. Classification by the state of aggregation of substances Table 22. Classification by the basis of reversibility Table 23. Classification by thermal effect Chemical reaction rate Table 24. Basic quantities Table 25. Reaction rate versus concentration Table 26. Change in the rate of a chemical reaction Chemical equilibrium Table 27. Le Chatelier principle Table 28. Shift in chemical equilibrium Electrolytic dissociation Table 29. Dissociation products
5 Table 30. Some strong acids and bases Table 31. Degree of dissociation Exchange reactions in solution Table 32. Berthollet rules Table 33. Molecular and ionic equations Hydrolysis Table 34. Hydrolysis of inorganic substances Table 35. Reversible hydrolysis of salts Table 36. Medium in acidic solutions salts Redox reactions Table 37. Functions of an oxidizing agent and a reducing agent Table 38. Oxidized and reduced forms of certain substances Table 39. Types of redox reactions Table 40. Electrochemical series of voltages of metals Table 41. A number of non-metals Table 42. Examples of oxidizing and reducing agents Table 43. Method electronic balance Table 44. Corrosion retardation Electrolysis Table 45. Electrodes Table 46. Electrolysis of melts Table 47. Electrolysis of solutions Reaction mechanisms in organic chemistry Table 48. Main reaction mechanisms
6 Table 49. Substitution reaction mechanism Table 50. Markovnikov's rule INORGANIC CHEMISTRY Classes of inorganic substances Table 51. Inorganic substances Table 52. Simple substances Table 53. The position of non-metals in the periodic system of elements Table 54. Complex substances Table 55. Ortho- and metaforms of hydroxides Table 56. Trivial names of some oxygen-containing acids and their anions Table 57. Classification of hydroxides and oxides Table 58. Classification of salts Scheme 4. General classification of inorganic substances Metals Table 59. Reactions of metals Non-metals Table 60. Reactions of non-metals Oxides Table 61. Reactions of basic oxides Table 62 Reactions of acid oxides Table 63. Reactions of amphoteric oxides Bases and amphoteric hydroxides Table 64. Reactions of bases Table 65. Reactions of amphoteric hydroxides
7 acids complex salts (hydroxocomplexes) Table 72. Decomposition of nitrates (depending on the position of metals in a series of voltages) Table 73. Decomposition of ammonium salts Interrelation of classes of inorganic substances Table 74. Transformations of inorganic substances ORGANIC CHEMISTRY Structure of organic substances Table 75. Theory of the structure of organic substances A. M. Butlerov Table 76. Types of organic compounds Table 77. Carbon-carbon bonds Table 78. Carbon atom Table 79. Types of hybridization Table 80. Composition of organic molecules Table 81. Classes of organic compounds .. 73 Table 82. Isomers Table 83. Mutual influence of atoms in molecules
8 8 Nomenclature of organic substances Table 84. Components of the names of organic compounds Table 85. Names of carbon chains Table 86. Designation of the degree of saturation of bonds Table 87. Names of characteristic groups of organic compounds Table 88. Names of some aromatic compounds Table 89. Names of some hydrocarbon radicals Table 90 Numerical prefixes (indicate the number of identical structural elements) Table 91. Composition of the name of the substance Hydrocarbons Table 92. Classification of hydrocarbons Table 93. Reactions of saturated hydrocarbons Table 94. Reactions of unsaturated hydrocarbons Table 95. Reactions of aromatic hydrocarbons Table 96. Reactions of haloalkanes Oxygen-containing organic compounds Table 97 Alcohols and phenols Table 98. Reactions of alcohols and phenols Table 99. Carbonyl compounds Table 100. Reactions of aldehydes and ketones Table 101. Carboxylic acids Table 102. Reactions of carboxylic acids Nitrogen-containing org Anic compounds Table 103. Amines Table 104. Reactions of amines
9 Table 105. Names of some natural amino acids Table 106. Properties of amino acids Biologically important substances Scheme 5. Fats Table 107. Carboxylic acids that make up fats Table 108. Carbohydrates Table 109. Structure levels of protein molecules Table 110. Chemical properties of proteins Table 111. Color reactions of proteins Interrelation of organic compounds Table 112. Catalysts used in organic chemistry Scheme 6. Genetic relationship of organic compounds COGNITIVE METHODS IN CHEMISTRY Working with substances and chemical equipment Table 113. Basic rules for working in a chemical laboratory Table 114. Chemical utensils and equipment Table 115 Table 116. Rules for the use of substances in everyday life Scientific methods for studying chemicals and transformations Table 117. Research methods Table 118. Methods for separating mixtures
10 Table 119. Coloring of indicators Table 120. Qualitative reactions to cations Table 121. Qualitative reactions to anions Table 122. Detection of gases Table 123. Recognition of organic compounds Methods for obtaining substances Table 124. Methods for obtaining simple substances Table 125. Methods for obtaining oxides Table 126. Methods for obtaining bases and amphoteric hydroxides Table 127. Methods for obtaining acids Table 128. Methods for obtaining salts Table 129. Methods for obtaining saturated hydrocarbons Table 130. Methods for obtaining alkenes Table 131. Methods for obtaining alkynes (acetylene) Table 132. Methods for obtaining arenes (benzene) Table 133. Methods for the production of monohydric alcohols Table 134. Methods for the production of polyhydric alcohols Table 135. Methods for the production of phenols Table 136. Methods for the production of aldehydes and ketones Table 137. Methods for the production of carboxylic acids Industrial production of substances Table 138. Methods for the production of metals Table 139. Metallurgical m Methods Scheme 7. Domain process
11 Table 140. Some industrial processes Table 141. Products of fractional distillation of oil Table 142. Chemical processing of oil Table 143. Obtaining high-molecular compounds (polymers) Table 144. Classification of polymers Table 145. Polymers based on ethylene and its derivatives Calculations by chemical formulas and equations reactions Table 146. Relationships between quantities in solution Table 147. Preparation of solutions Table 148. The most important quantities for calculations Table 149. Relationships between quantities Normal physical conditions Table 150. Stoichiometric laws Table 151. Calculations by reaction equations Table 152. Finding the molecular formula of a substance APPENDICES Table 1. Periodic system of elements of D.I. Mendeleev Table 2. Chemical elements: serial number, atomic mass (rounded), electronegativity Table 3. Solubility of inorganic compounds in water
12 FOREWORD To help schoolchildren and teachers, a manual is offered, which is a generalized presentation in visual tables and diagrams of all the basic rules, laws, formulas and calculations in the course of organic and inorganic chemistry. All major sections of chemistry studied in the classroom are included. This is the structure of the atom, the periodic law of D. I. Mendeleev, the structure of the periodic system of chemical elements, types of chemical bonds, substances and mixtures, classes of inorganic compounds, classification of chemical reactions, the rate of chemical reactions and chemical equilibrium, reaction mechanisms in organic chemistry, metals and non-metals and their properties, chemical properties of complex substances, the relationship of classes of inorganic substances, organic substances and their structure, the composition of organic molecules, isomers, the nomenclature of organic substances, hydrocarbons, their classification and properties, nitrogen-containing organic compounds, biologically important substances, the structure and properties of protein molecules , carbohydrates, the relationship of organic compounds. In addition, the manual describes the basic rules and methods of work in a chemical laboratory, gives the characteristics of chemical
13 courts and equipment, examples of calculations based on formulas and equations of reactions, as well as examples of qualitative reactions are offered. The appendix to the manual contains the periodic table of elements of D. I. Mendeleev, a table of the solubility of inorganic compounds in water. A brief and concise presentation of the material will help students independently or with the help of a teacher to repeat the school chemistry course and successfully prepare for the unified state exam in grade 11. The structure of the manual corresponds to the structure of the codifier of content elements in chemistry for compiling control measuring materials for the exam and corresponds to the logic of studying and repeating the school chemistry course. The manual adopted the following abbreviations: conc. concentrated solution, n. y. under normal conditions, razb. very dilute solution, pract. practical, razb. dilute solution, theor. theoretical.
14 THEORETICAL FOUNDATIONS OF CHEMISTRY STRUCTURE OF THE ATOM Atom Table 1 Electrons (e) Nucleus protons (p +) neutrons (n 0) Mass number (A) the total number of protons and neutrons in the atomic nucleus electrons in an atom A \u003d N (n 0) + N (p +) Z \u003d N (p +) \u003d N (e) uncertainty principle) 14
15 Energy levels and sublevels Table 3 Energy levels (EL) Energy sublevels (EPL) Number of electrons 1 1s 2 2 2s 2p 3 3s 3p 3d 4 4s 4p 4d 4f , which has a certain energy, is the largest. Orbital shapes Scheme 1 s-orbital p-orbital 15
Unified state exam in CHEMISTRY qualifier of content elements and requirements for the level of training of graduates of educational organizations for conducting a unified state exam in chemistry
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CHEMISTRY, class Unified State Exam in CHEMISTRY
Moscow City Education Department A.A. NIKOLAEV" WORKING PROGRAM
Analysis of the HSC Subject Chemistry. Parallel 8 grades Control topic: “Initial chemical concepts” Date: November 2014 8А/1 18 5 8 5 0 100% 72% 4.0 8B/1 15 0 8 6 1 93% 53% 3.5 8В/1 21 1 11 8 1 95%
ANALYTICAL REPORT OF THE SUBJECT COMMISSION ON THE RESULTS OF THE USE IN CHEMISTRY 1 The report was prepared by A.N. Levkin, Deputy Chairman of the Subject Commission in Chemistry 2
Explanatory note The work program was compiled on the basis of the Federal component of the state Standard of secondary (complete) general education in chemistry (basic level), the program was used
PROGRAM of entrance examination in chemistry for foreign citizens applying for undergraduate and specialist programs The program is intended for applicants in the following areas:
Atomic-molecular doctrine. Molecules. Atoms. Chemical element, simple substance, complex substance. Signs of chemical elements and chemical formulas. Calculation of the mass fraction of a chemical element in a substance
Annex 10 to Order 311/1 dated August 28, 2015 "On approval of the basic general education programs of basic general education (FSES), basic general education, secondary general education" Working
Chemistry 1. Initial chemical concepts. The subject of chemistry. bodies and substances. Basic methods of cognition: observation, measurement, description, experiment. Physical and chemical phenomena. Safety regulations
1 Explanatory note This program was developed on the basis of the Exemplary programs of basic general education in chemistry (basic level), corresponding to the federal component of the state standard
Calendar-thematic planning Subject: Chemistry Class: 11 Hours per week: 2 Total hours per year: 68 I trimester. Total weeks: 10.6, total hours: 22. Sec. Theme of the lesson Topic 1. Structure of the atom and periodic
PROGRAM IN CHEMISTRY The program is based on the mandatory minimum content of secondary (complete) general education and consists of three sections. The first section is devoted to the theoretical foundations of chemistry. AT
2 Specification of control measuring materials for the unified state exam in CHEMISTRY in 2016 Unified state exam in CHEMISTRY Specification of control measuring instruments
PROGRAM OF ENTRANCE EXAMS IN CHEMISTRY TO SARATOV STATE MEDICAL UNIVERSITY IN 2009 1. Subject of chemistry, its tasks. The place of chemistry among the natural sciences, the relationship of sciences with chemistry.
EXAMINATION TICKETS OF THE STATE FINAL CERTIFICATION IN CHEMISTRY UNDER THE PROGRAMS OF BASIC GENERAL EDUCATION Ticket 1 1. The periodic system of chemical elements of D. I. Mendeleev and the structure of atoms:
Lesson planning in chemistry, Grade 11, (1 hour per week, 34 hours in total), O. S. Gabrielyan's teaching materials Lesson topic Elements of content Requirements for the level of students' preparation Experiment Homework Date
The structure of the work program: 1. Explanatory note to the work program 2. Calendar and thematic planning for grades 10-11 3. Requirements for the level of mastering students' knowledge 4. Forms of knowledge assessment
Test programs in chemistry Subject and tasks of chemistry. The place of chemistry among the natural sciences. Atomic-molecular doctrine. Molecules. Atoms. The constancy of the composition of matter. relative atomic and relative
Unified state exam in CHEMISTRY PROJECT CHEMISTRY, grade 11 2 Specification of control measuring materials for the unified state exam in CHEMISTRY in 2017 Specification of control
2 Planned results of mastering the subject As a result of studying chemistry, the student must know / understand: chemical symbols: signs of chemical elements, formulas of chemicals and equations of chemical
PROGRAM OF ENTRANCE TEST ON THE SUBJECT "CHEMISTRY" At the exam in chemistry entering the university must: - show knowledge of the basic theoretical provisions; - be able to apply theoretical
INTRODUCTION TEST PROGRAM IN CHEMISTRY The program is based on the mandatory minimum content of secondary (complete) general education and consists of three sections. The first section is devoted to theoretical
The work program of the elective course "Chemistry" for grade 11 for the 2016-2017 academic year author: teacher of biology and chemistry Kolosnitsyna S.V. s.zubovo 2016 Explanatory note The elective course "Chemistry" is intended
CHEMISTRY Theory of the structure of matter Atom. Composition of atomic nuclei. Chemical element. The constancy of the composition of matter. Relative atomic and relative molecular weight. The law of conservation of mass, its meaning
Thematic planning for 2015-2016 academic year chemistry Grade 10 Textbook O.S. Lesson Gabrielyan Date Title of the section, topic of the lesson (indicating the number of hours) Formed knowledge, skills. Ways of activity
Unified State Examination in CHEMISTRY
PROGRAM OF ENTRANCE TESTS IN CHEMISTRY FOR APPLICANTS TO URF IN 2014 Preparing for the exam, applicants must show knowledge of the basic theoretical principles of chemistry as one of the most important natural sciences.
PROGRAM IN CHEMISTRY GENERAL INSTRUCTIONS At the exam in chemistry, applicants to the academy must show: 1) a clear knowledge of the basic laws of chemistry and the provisions of the theory of the structure of matter, on which all modern
STANDARD OF BASIC GENERAL EDUCATION IN CHEMISTRY The study of chemistry at the level of basic general education is aimed at achieving the following goals: mastering the most important knowledge about basic concepts and laws
The list of content elements checked at the entrance exam in CHEMISTRY
PROGRAM OF ENTRANCE TESTS IN CHEMISTRY TO PSU IN 2016 CONTENT OF THE PROGRAM IN CHEMISTRY for entrants Section 1. THEORETICAL FOUNDATIONS OF CHEMISTRY Modern ideas about the structure
Explanatory note for grade 0. The program is different in accordance with the Federal component of the state educational standard of secondary general education and based on the program for general education
2 Explanatory note The program was developed on the basis of the mandatory minimum content of secondary (complete) general education in chemistry. Content of the program 1. Subject and tasks of chemistry. physical phenomena
Entering the university must show knowledge of the basic theoretical provisions of chemistry as one of the most important natural sciences that underlie the scientific understanding of nature. The candidate must be able to apply
