The handbook contains all the theoretical material on the course of chemistry necessary for passing the exam. It includes all the content elements tested at the Unified State Examination in Chemistry and helps to summarize and systematize the knowledge and skills for the course of the secondary (complete) school. The theoretical material is presented in a concise, accessible form. Each section is accompanied by examples. test tasks, allowing you to test your knowledge and the degree of preparedness for the certification exam. Practical tasks correspond to the USE format. At the end of the manual, answers to tests are given that will help schoolchildren and applicants to test themselves and fill in the gaps. The manual is addressed to senior students, applicants and teachers.
Patterns of changes in the properties of elements and their compounds by periods and groups.
The modern formulation of the Periodic Law by D.I. Mendeleev:
- properties of the elements, as well as the simple and complex substances are in a periodic dependence on the charge of the nucleus of an atom, equal to the ordinal number of the element.
The Periodic System of Chemical Elements is a natural classification of chemical elements, which is a tabular expression of the Periodic Law of D.I. Mendeleev. It is a table consisting of periods (horizontal rows) and groups (vertical columns) of elements.
Group number A = Number of valence electrons: ns and np
Group number B = Number of valence electrons: ns and (n-1) d
In the short period version of the Periodic system - 8 groups. They are divided into subgroups A (main) and B (side).
In the long period version of the Periodic system - 18 groups. They are designated either in the same way as in the short-term version, or simply by numbers from 1 to 18 (for example, group IA or 1, VIIB or 17).
Period number = Number of energy levels filled with electrons = Designation of the last energy level (EL)
The modern Periodic system includes 7 periods. Each period begins with the element in whose atom an electron first appears at the corresponding energy level (hydrogen or alkaline element), and ends with the element in whose atom the level with the same number is completely filled (noble gas).
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Publication date: 08/10/2017 12:30 UTC
- USE 2020, Chemistry, 10 training options for examination papers to prepare for the unified state exam, Savinkina E.V., Zhiveinova O.G., 2019
- Chemistry, A complete guide to preparing for the exam, Lidin R.A.
- OGE, Chemistry in tables and diagrams, Reference manual, grades 8-9, Savinkina E.V., Loginova G.P., 2017
- USE-2019, Chemistry, 10 training options for examination papers to prepare for the unified state exam, Savinkina E.V., Zhiveinova O.G., 2019
The following tutorials and books:
- Nitrogen Handbook, Physical and chemical properties of gases and liquids, Production of process gases, Purification of process gases, Synthesis of ammonia, 1986
Handbook includes all theoretical material school course chemistry, which is necessary for passing the exam, - the final certification of students. This material is divided into 14 sections, the content of which corresponds to the topics tested at the USE - four content blocks: “Chemical element”, “Substance”, “Chemical reaction”, “Knowledge and application of substances and chemical reactions". For each section, training tasks from parts A and B are given - with a choice of answers and a short answer. Section 15 is completely devoted to solving the calculation problems included in the examination part C.
Test tasks are designed in such a way that by answering them, the student will be able to more rationally repeat the main provisions of the school chemistry course.
At the end of the manual, answers to tests are given that will help schoolchildren and applicants to test themselves and fill in the gaps.
For the convenience of working with this reference book, a table is provided that indicates the correspondence between the topics of the exam and sections of the book.
The manual is addressed to senior students, applicants and teachers.
1. Common elements. structure of atoms. Electronic shells. Orbitals
Chemical element- a certain type of atoms, denoted by a name and a symbol and characterized by a serial number and relative atomic mass.
In table. Table 1 lists common chemical elements, shows the symbols by which they are denoted (in brackets - pronunciation), serial numbers, relative atomic masses, characteristic oxidation states.
Zero the degree of oxidation of an element in its simple substance (substances) is not indicated in the table.
All atoms of one element have the same number of protons in the nucleus and the same number of electrons in the shell. Thus, in the element atom hydrogen H is 1 p+ in the core and on the periphery 1 e- ; in the element atom oxygen Oh located 8 p+ in the core and 8 e- in the shell; element atom aluminum Al contains 13 R+ in the core and 13 e- in the shell.
Atoms of the same element can differ in the number of neutrons in the nucleus, such atoms are called isotopes. So, the element hydrogen H three isotopes: hydrogen-1 (special name and symbol protium 1 H) with 1 p+ in the core and 1 e- in the shell; hydrogen-2 (deuterium 2 H, or D) with 1 p+ and 1 P 0 in the core and 1 e- in the shell; hydrogen-3 (tritium 3 N, or T) with 1 p+ and 2 P 0 in the core and 1 e- in the shell. In the symbols 1 H, 2 H, and 3 H, the superscript indicates mass number is the sum of the numbers of protons and neutrons in the nucleus. Other examples:
Electronic formula atom of any chemical element in accordance with its location in the Periodic system of elements of D. I. Mendeleev, can be determined from Table. 2.
The electron shell of any atom is divided into energy levels(1, 2, 3rd, etc.), levels are divided into sublevels(marked with letters s, p, d, f). The sublevels are made up of atomic orbitals– areas of space where electrons are likely to stay. Orbitals are designated as 1s (orbital of the 1st level of the s-sublevel), 2 s, 2 R, 3 s, 3 p, 3d, 4 s… Number of orbitals in sublevels:
The filling of atomic orbitals with electrons occurs in accordance with three conditions:
1) minimum energy principle
Electrons fill the orbitals starting from the lower energy sublevel.
The sequence of increasing energy of sublevels:
1 s< 2 c< 2 p< 3 s< 3 p< 4 s≤ 3 d< 4 p< 5 s≤ 4 d< 5 p< 6 s…
2) prohibition rule (Pauli principle)
Each orbital can hold at most two electrons.
One electron in the orbital is called unpaired, two electrons - electron pair:
3) principle of maximum multiplicity (Hund's rule)
From the completed energy diagrams are derived electronic formulas element atoms. The number of electrons in the orbitals of a given sublevel is indicated in the superscript to the right of the letter (for example, 3 d 5 is 5 electrons per 3 d-sublevel); electrons of the 1st level go first, then the 2nd, 3rd, etc. Formulas can be complete and short, the latter contain in brackets the symbol of the corresponding noble gas, which conveys its formula, and, moreover, starting with Zn , the filled inner d-sublevel. Examples:
3 Li = 1s 2 2s 1 = [ 2 He]2s 1
8O=1s2 2s 2 2p 4= [ 2He] 2s 2 2p 4
13 Al = 1s 2 2s 2 2p 6 3s 2 3p 1= [ 10 Ne] 3s 2 3p 1
M.: 2017. - 256 p. M.: 2016. - 256 p.
New directory contains all the theoretical material on the course of chemistry necessary for passing the exam. It includes all elements of the content, checked by control and measuring materials, and helps to generalize and systematize knowledge and skills for the course of the secondary (complete) school. The theoretical material is presented in a concise and accessible form. Each topic is accompanied by examples of test tasks. Practical tasks correspond to the USE format. Answers to the tests are given at the end of the manual. The manual is addressed to schoolchildren, applicants and teachers.
Format: pdf ( 2017 , 256s.)
Size: 2 MB
Watch, download:drive.google
Format: pdf ( 2016 , 256s.)
Size: 1.6 MB
Watch, download:drive.google
CONTENT
Preface 12
MOST IMPORTANT CHEMICAL CONCEPTS AND LAWS 14
1. THEORETICAL FOUNDATIONS OF CHEMISTRY 18
1.1. Modern ideas about the structure of the atom 18
1.1.1. The structure of the electron shells of atoms of elements 18
Sample tasks 24
1.2. Periodic law and Periodic system of chemical elements D.I. Mendeleeva 25
1.2.1. Patterns of changes in the properties of elements and their compounds by periods and groups 25
Sample tasks 28
1.2.2. general characteristics metals of IA-IIIA-groups in connection with their position in the Periodic system of chemical elements
DI. Mendeleev and structural features of their atoms 28
Sample tasks 29
1.2.3. Characterization of transition elements (copper, zinc, chromium, iron) according to their position in the Periodic system of chemical elements D.I. Mendeleev
and features of the structure of their atoms 30
Sample tasks 30
1.2.4. General characteristics of non-metals of IVA-VIIA-groups in connection with their position in the Periodic system of chemical elements D.I. Mendeleev
and structural features of their atoms 31
Sample tasks 31
1.3. Chemical bond and structure of matter 32
1.3.1. covalent chemical bond, its varieties and mechanisms of formation. Characteristics of a covalent bond (polarity and bond energy). Ionic bond.
Metal connection. Hydrogen bond 32
Sample tasks 36
1.3.2. Electronegativity. The oxidation state and valency of chemical elements 37
Sample tasks 39
1.3.3. Substances of molecular and non-molecular structure. Type of crystal lattice. The dependence of the properties of substances on their composition
and buildings 41
Sample tasks 43
1.4. Chemical reaction 43
1.4.1. Classification of chemical reactions in inorganic and organic chemistry 43
Sample tasks 45
1.4.2. Thermal effect of a chemical reaction. Thermochemical equations 46
Sample tasks 48
1.4.3. Reaction rate, its dependence on various factors 48
Sample tasks 50
1.4.4. Reversible and irreversible chemical reactions. chemical balance. Shift in chemical equilibrium under the influence of various factors 50
Task examples
1.4.5. Electrolytic dissociation of electrolytes in aqueous solutions. Strong and weak electrolytes 53
Sample tasks 54
1.4.6. Ion exchange reactions 54
Sample tasks 56
1.4.7. Environment of aqueous solutions: acidic, neutral, alkaline. Salt hydrolysis 57
Sample tasks 59
1.4.8. Redox reactions. Corrosion of metals and methods of protection against it 60
Examples of tasks 64
1.4.9. Electrolysis of melts and solutions (salts, alkalis, acids) 65
Sample tasks 66
1.4.10. Ionic (V.V. Markovnikov's rule) and radical mechanisms of reactions in organic chemistry 67
Examples of tasks 69
2. INORGANIC CHEMISTRY 71
2.1. Classification is not organic matter. Nomenclature of inorganic substances (trivial and international) 71
Examples of tasks 75
2.2. characteristic Chemical properties simple substances - metals: alkali, 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, halogens, oxygen, sulfur, nitrogen,
phosphorus, carbon, silicon 81
Examples of tasks 83
2.4. Characteristic chemical properties of oxides: basic, amphoteric, acidic 84
Examples of tasks 86
2.5. Characteristic chemical properties of bases and amphoteric hydroxides 87
Examples of tasks 88
2.6. Characteristic chemical properties of acids 90
Sample tasks 93
2.7. Characteristic chemical properties of salts: medium, acidic, basic; complex (on the example of aluminum and zinc compounds) 94
Sample tasks 96
2.8. The relationship of different classes of inorganic substances 97
Job examples 100
3. ORGANIC CHEMISTRY 102
3.1. Theory of the structure of organic compounds: homology and isomerism (structural and spatial).
Mutual influence of atoms in molecules 102
Sample tasks 105
3.2. Types of bonds in molecules of organic substances. Hybridization of atomic orbitals of carbon. Radical.
Functional group 106
Sample tasks 109
3.3. Classification of organic substances. Nomenclature of organic substances (trivial and international) 109
Sample tasks 115
3.4. Characteristic chemical properties of hydrocarbons: alkanes, cycloalkanes, alkenes, dienes, alkynes, aromatic hydrocarbons(benzene and toluene) 116
Examples of tasks 121
3.5. Characteristic chemical properties of saturated monohydric and polyhydric alcohols, phenol 121
Job examples 124
3.6. Characteristic chemical properties of aldehydes, saturated carboxylic acids, esters 125
Examples of tasks 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
Sample 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 foundations of chemistry 145
4.1.1. Rules for working in the laboratory. Laboratory glassware and equipment. Safety rules when working with caustic, combustible and toxic substances,
household chemicals 145
Sample tasks 150
4.1.2. Scientific research methods chemical substances and transformations. Methods for separating mixtures and purifying substances 150
Examples of tasks 152
4.1.3. Determination of the nature of the environment of aqueous solutions of substances. Indicators 152
Job examples 153
4.1.4. Qualitative reactions for inorganic substances and ions 153
Job examples 156
4.1.5. Qualitative reactions of organic compounds 158
Job examples 159
4.1.6. The main methods for obtaining (in the laboratory) specific substances belonging to the studied classes of inorganic compounds 160
Job examples 165
4.1.7. The main methods for obtaining hydrocarbons (in the laboratory) 165
Examples of tasks 167
4.1.8. The main methods for obtaining oxygen-containing compounds (in the laboratory) 167
Examples of tasks 170
4.2. General representations on industrial methods for obtaining the most important substances 171
4.2.1. The concept of metallurgy: general methods for obtaining metals 171
Job examples 174
4.2.2. Are common scientific principles chemical production (on the example of industrial production of ammonia, sulfuric acid, methanol). chemical pollution
environment and its consequences 174
Job examples 176
4.2.3. natural springs hydrocarbons, their processing 177
Job examples 180
4.2.4. high molecular weight compounds. Polymerization and polycondensation reactions 181
Job examples 184
4.3. Calculations by chemical formulas and reaction equations 184
4.3.1. Calculation of the mass of a solute contained in a certain mass of a solution with a known mass fraction; calculation of the mass fraction of a substance in a solution 184
Job examples 186
4.3.2. Calculations of volume ratios of gases in chemical reactions 186
Examples of tasks 187
4.3.3. Calculations 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 involved in the reaction 187
Examples of tasks 188
4.3.4. Calculations of the thermal effect of a reaction 189
Sample tasks 189
4.3.5. Calculations of the mass (volume, amount of substance) of the reaction products, if one of the substances is given in excess (has impurities) 190
Sample 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 the dissolved substance 191
Sample tasks 191
4.3.7. Finding the molecular formula of a substance 192
Job examples 194
4.3.8. Calculations of the mass or volume fraction of the yield of the reaction product from the theoretically possible 195
Job examples 195
4.3.9. Calculations of the mass fraction (mass) of a chemical compound in a mixture 196
Examples of tasks 196
Application
CHEMISTRY OF THE ELEMENTS 198
Hydrogen 198
Elements of IA-Group 200
Elements of IIA-group 202
Elements of the SHA-group 204
Elements of IVA group 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
IUPAC: Periodic Table of the Elements 232
Solubility of bases, acids and salts in water 234
Valency of some chemical elements 235
Acids and names of their salts 235
Atomic radii of elements 236
Some of the most important physical constants 237
Prefixes in the formation of multiples
and submultiple units 237
The prevalence of elements in earth's crust 238
Answers to tasks 240
The new handbook includes all the theoretical material of the school course in chemistry, which is necessary for preparing and passing the unified state exam.
The content of the book is based on control and measuring materials that determine the volume educational material, which is checked by the state final certification.
The theoretical material of the handbook is presented in a concise and accessible form. The clarity of presentation and clarity of the educational material will allow you to effectively prepare for the exam.
Each section of the book corresponds to four content blocks that are tested on the exam: Theoretical basis Chemistry” - Periodic law and Periodic system of chemical elements D.I. Mendeleev, chemical bond and structure of matter, chemical reaction; "Inorganic Chemistry", "Organic Chemistry", "Methods of learning chemistry. Chemistry and Life” - experimental foundations of chemistry, general ideas about industrial methods for obtaining the most important substances.
R. A. Lidin
Chemistry: A complete guide to preparing for the exam
Foreword
The handbook includes all the theoretical material of the school chemistry course required to pass the Unified State Examination, the final assessment of students. This material is divided into 14 sections, the content of which corresponds to the topics tested at the USE - four content blocks: “Chemical Element”, “Substance”, “Chemical Reaction”, “Knowledge and Application of Substances and Chemical Reactions”. For each section, training tasks from parts A and B are given - with a choice of answers and a short answer. Section 15 is completely devoted to solving the calculation problems included in the examination part C.
Test tasks are designed in such a way that by answering them, the student will be able to more rationally repeat the main provisions of the school chemistry course.
At the end of the manual, answers to tests are given that will help schoolchildren and applicants to test themselves and fill in the gaps.
For the convenience of working with this reference book, a table is provided that indicates the correspondence between the topics of the exam and sections of the book.
The manual is addressed to senior students, applicants and teachers.
1. Common elements. structure of atoms. Electronic shells. Orbitals
Chemical element- a certain type of atoms, denoted by a name and a symbol and characterized by a serial number and relative atomic mass.
In table. Table 1 lists common chemical elements, shows the symbols by which they are denoted (in brackets - pronunciation), serial numbers, relative atomic masses, characteristic oxidation states.
Zero the degree of oxidation of an element in its simple substance (substances) is not indicated in the table.
All atoms of one element have the same number of protons in the nucleus and the same number of electrons in the shell. Thus, in the element atom hydrogen H is 1 p+ in the core and on the periphery 1 e-; in the element atom oxygen Oh located 8 p+ in the core and 8 e- in the shell; element atom aluminum Al contains 13 R+ in the core and 13 e- in the shell.
Atoms of the same element can differ in the number of neutrons in the nucleus, such atoms are called isotopes. So, the element hydrogen H three isotopes: hydrogen-1 (special name and symbol protium 1H) with 1 p+ in the core and 1 e- in the shell; hydrogen-2 (deuterium 2H, or D) with 1 p+ and 1 P 0 in the core and 1 e- in the shell; hydrogen-3 (tritium 3H, or T) with 1 p+ and 2 P 0 in the core and 1 e- in the shell. In the symbols 1H, 2H, and 3H, the superscript indicates mass number is the sum of the numbers of protons and neutrons in the nucleus. Other examples:
Electronic formula an atom of any chemical element in accordance with its location in the Periodic system of elements of D. I. Mendeleev can be determined from Table. 2.
The electron shell of any atom is divided into energy levels(1, 2, 3rd, etc.), levels are divided into sublevels(marked with letters s, p, d, f). The sublevels are made up of atomic orbitals– areas of space where electrons are likely to stay. Orbitals are designated as 1s (orbital of the 1st level of the s-sublevel), 2 s, 2R, 3s, 3p, 3d, 4s… Number of orbitals in sublevels:
The filling of atomic orbitals with electrons occurs in accordance with three conditions:
1) minimum energy principle
Electrons fill the orbitals starting from the lower energy sublevel.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 hold at most two electrons.One electron in the orbital is called unpaired, two electrons - electron pair:
3) principle of maximum multiplicity (Hund's rule)
Within a sublevel, electrons first fill all the orbitals by half, and then completely.Each electron has its own characteristic - spin (conventionally represented by an up or down arrow). The spins of the electrons add up as vectors, the sum of the spins given number electrons at the sublevel should be maximum(multiplicity):
Filling of levels, sublevels and orbitals of atoms of elements from H with electrons (Z= 1) to Kr (Z= 36) shown in energy diagram(the numbers correspond to the filling sequence and coincide with the serial numbers of the elements):
From the completed energy diagrams are derived electronic formulas element atoms. The number of electrons in the orbitals of a given sublevel is indicated in the superscript to the right of the letter (for example, 3 d 5 is 5 electrons per 3 d-sublevel); electrons of the 1st level go first, then the 2nd, 3rd, etc. Formulas can be complete and short, the latter contain in brackets the symbol of the corresponding noble gas, which conveys its formula, and, moreover, starting with Zn , the filled inner d-sublevel. Examples:
3Li = 1s22s1 = 2s1
8O=1s2 2s22p4 = 2s22p4
13Al = 1s22s22p6 3s23p1 = 3s23p1
17Cl = 1s22s22p6 3s23p5 = 3s23p5
2OCa = 1s22s22p63s23p 4s2 = 4s2
21Sc = 1s22s22p63s23p6 3d14s2 = 3d14s2
25Mn = 1s22s22p63s23p6 3d54s2 = 3d54s2
26Fe = 1s22s22p63s23p6 3d64s2 = 3d64s2
3OZn = 1s22s22p63s23p63d10 4s2 = 4s2
33As = 1s22s22p63s23p63d10 4s24p3 = 4s24p3
36Kr = 1s22s22p63s23p63d10 4s24p6 = 4s24p6
Electrons outside brackets are called valence. They are involved in the formation of chemical bonds.
The exception is:
24Cr = 1s22s22p63s23p6 3d54s1 = Зd54s1(not 3d44s2!),
29Cu = 1s22s22p63s23p6 3d104s1 = 3d104s1(not 3d94s2!).
Examples of Part A assignments
1. Name, not related to hydrogen isotopes
1) deuterium
2) oxonium
2. The formula for the valence sublevels of a metal atom is
3. The number of unpaired electrons in the ground state of an iron atom is
4. In the excited state of the aluminum atom, the number of unpaired electrons is
5. Electronic formula 3d94s0 corresponds to the cation
6. The electronic formula of the E2-3s23p6 anion corresponds to the element
7. The total number of electrons in the Mg2+ cation and F- anion is
2. Periodic law. Periodic system. Electronegativity. Oxidation states
The modern formulation of the Periodic Law, discovered by D. I. Mendeleev in 1869:
The properties of the elements are in a periodic dependence on the ordinal number.The periodically recurring nature of the change in the composition of the electron shell of the atoms of the elements explains the periodic change in the properties of the elements when moving through the periods and groups of the Periodic system.
Hello.
Please tell me the recommended textbooks for admission to medical university in biology and chemistry?
Before starting to prepare for next year's exams, I would like to decide on the textbooks. I graduated from school a long time ago, I have to prepare from scratch.
Based on what they write on the forums, the tutorials below are most cited.
CHEMISTRY:
1). "The Beginnings of Chemistry. A modern course for applicants to universities. Kuzmenko N.E., Eremin V.V., Popkov V.A.
2). "Manual in chemistry for applicants to universities." Khomchenko G.P.
3). "Chemistry. 8-11 grades.” Rudzitis G.E., Feldman F.G.
4). "Chemistry tutor" Alexander Egorov
5). "Collection of tasks and exercises in chemistry." Kuzmenko N.E., Eremin V.V.
6). “Manual in chemistry for applicants to universities. Questions, exercises, tasks. Samples of exam tickets. Puzakov S.A., Popkov V.A.
7). "Problem solving in chemistry." Belavin I.Yu.
8). "Problem in chemistry. Grade 11." Lyovkin A.N., Kuznetsova N.E.
BIOLOGY:
1). " General biology: Grades 10-11: Textbook for educational institutions." Profile level: At 2 pm Ed. Shumny V.K., Dymshits G.M.
2). "Biology full course" In 3 volumes (Anatomy, Botany, Zoology). Bilich G.L., Kryzhanovsky V.A.
3). "Biology. For applicants to universities "Vladimir Yarygin
4). "Biology. General biology" V. B. Zakharov, S. G. Mamontov, N. I. Sonin, E. T. Zakharova
5). "Biology. In 2 volumes Edited by N. V. Chebyshev
6). "Human Anatomy: Textbook: in two books" Sapin M.R., Bilich G.L.
7). "Biology. Anatomy and physiology of man. 8th grade. Deep Learning." Sapin M.R., Sivoglazov V.I., Bryksina Z.G.
8). "Biology for applicants to universities" R. G. Zayats, V. E. Butvilovsky, V. V. Davydov, I. V. Rachkovskaya
9). “Fundamentals of Biology. Full course general educational high school» A. A. Kamensky, N. A. Sokolova, M. A. Valovaya
10). "Biology. Manual for preparatory departments of medical institutes "N. E. Kovalev, L. D. Shevchuk, O. I. Shchurenko
eleven). “Preparing for the exam in biology” A. G. Lebedev
12). "Biology. Handbook for high school students and university applicants. A complete course of preparation for the final exams "T. L. Bogdanova, E. A. Solodova
Tell me, if it's not difficult, what textbooks are better to buy in order to enter?!
I am very worried that I will waste time on unnecessary books and thereby simply not prepare properly. Help advice. Please!
Sincerely, Alexander Strokin.
Unsubscribe about chemistry.
1 and 5 almost completely repeat each other, but very good. Take 1 - the theory is described in more detail there, the tasks are the same as in 5.
As far as I know, level 2 tasks are not very difficult, easier than level 1.
3 - an ordinary school textbook. If you can handle the theory level of 1, then you can probably do without it.
4 - did not meet. Books with such a name are scary :)
6 - the level is about the same as in 1. A good book.
7 - did not meet.
8 - tasks are simple, but there are a lot of the same type. Good for getting hands on at the level of the school curriculum.
I hope my answer is helpful. Good luck!
Alexander Sergeevich, thanks for the answer! Tell me, what are the best chemistry problem books to buy? Separate for high school or specifically for the exam?
Please write YOUR RECOMMENDED LIST OF TEXTBOOKS IN CHEMISTRY AND PROBLEM (EXERCISES) IN CHEMISTRY. So that I can finally decide. I will be very grateful to you.
Unfortunately, I posted this question on many forums, but no answers yet from anyone. I do not know what to do. Time goes by, I'm afraid not to be in time and I'm marking time.
Zero level! I totally forgot everything. Today I was looking through trial assignments for the USE for 2012, 2011, 2010. in chemistry and biology, so I don't know anything at all. Really felt like a fool! At 5% I only remember the answers. And in biology and chemistry - the same story - zero!
Finished school in 2002. And apparently, upon admission to a university, I will be able to take either the Unified State Examination at the university, or simply Exams, which the same university conducts on its own. One of two, in short. Here I am completely confused. What is the best way to prepare? What is better to take upon admission - the Unified State Examination or the Exam from the university? Is it better to "sharpen" brains under the Unified State Examination or just solve problems and that's it? WHAT TO DO?!
The exam is more understandable and clearly structured, the internal exam is a thing in itself.
But if you forgot everything, then preparing yourself for these subjects is problematic, you need someone to help you, guide you, check the solutions, answer the questions that have arisen, clarify the incorrectness, explain the approaches to the tasks. It is useless to solve chemical problems according to the model, they are very simple, logical, but this logic must be felt.
And I would not leave less than a year to prepare.
Let's say my course of preparation for the exam is divided into 35 big serious topics. So consider))
Alexander, since the level is completely zero, in chemistry I would highly recommend the textbook by E. E. Minchenkov for grades 8 and 9.
http://www.labirint.ru/books/280907/
http://www.labirint.ru/books/280910/
It is very well written. Remember the very basics for the summer, both theories and calculations.
Two years ago, when my adult student after the medical school passed the internal exam in the second medical school, it was almost the same exam, only truncated. There were even tasks from the USE task bank. Now, I don't know.
If you need a textbook, then, of course, Kuzmenko, Eremin.
Puzakov's and especially Belavin's tasks for the exam are too high level, waste your time.
Although Puzakov is good, but for other purposes. If you are going to take a profile exam - then yes, take Puzakov, but even better - collections of Competition Problems of Moscow State University.
For the exam, Doronkin's manuals (for parts A and B, and separately part C) and Asanova are best suited. Of course, they have typos and incorrectness, but they are optimal for work.
http://www.labirint.ru/books/351705/ - part C in full
http://www.labirint.ru/books/350553/ - thematic tests, part A and B
http://www.labirint.ru/books/269618/ - organics on topics in the USE structure, a very useful book
http://www.labirint.ru/books/238816/ - general chemistry, also tests and tasks, according to the structure of the exam.
Biology
1) If we talk about textbooks, then you can take:
in botany - Gulenkova, Elenevsky "Biology: botany grade 6"
in zoology - Nikishov, Sharova "Biology: animals 7-8 (or 7th grade)"
in anatomy - Batuev "Biological: man 8 (or 9th grade)"
in General Biology - "General Biology" in two volumes, ed. Borodin
2) Benefits - No. 12 from your list or D.A. Solovkov "Unified State Examination in Biology: practical training"
There is also a manual "Biology. A school course in 100 hours" (E.A. Solodova, T.L. Bogdanova). It was made directly to prepare for the exam. To get a grip on tests in all sections of the school course - collections of tests for grades 6.7.8 and 9 (E.A. Solodova. Test tasks.)
Dear topic starter, my advice to you is to take Yegorov's book "Tutor in Chemistry" and read from the very beginning, USE level this book completely overlaps, is written intelligibly, with examples and tests, to work out the material, use FIPI tests, of which there are a lot of sales, and there are these collections on the net.
With all due respect to the textbook of Kuzmenko and Eremin, it is redundant for the Unified State Examination, especially when you start reading it, you will see that the authors are put on unnecessary for USE topics. Kuzmenko and Eremin's textbook is indispensable if you enter chemical universities, where you have to take an internal exam in chemistry. If you enter a medical university and, judging by the senior post, the top starter has very little time left and a very weak level, then Kuzmenko-Eremin will not save him, but only sink him. You have to be realistic about your strengths.
A small addition about Egorov. Take exactly the book that was written about in paragraph 4. He also published another one, with the word "ege" in the title. They like to offer it in stores instead of the first one, but many necessary topics are missing there.
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