Fundamentals of General Chemistry. Terms and Problems in Tests. Part 1. Terms and Examples in Tasks

The Ministry of Science and Higher Education of the Russian Federation

Kazan National Research Technological University

T. Petrova, E. Starodubets

FUNDAMENTALS 

OF GENERAL CHEMISTRY

TERMS AND PROBLEMS IN TESTS

Part 1

Terms and Еxamples in Тasks

Study guide

Kazan

KNRTU Press

2020

UDC 54(075)
ВВC Г1я7

Published by the decision of the Editorial Review Board 
of the Kazan National Research Technological University

Reviewers:

Prof. A. Ulahovich

Assoc. Prof. S. Podyachev

Petrova T.
Fundamentals of General Chemistry. Terms and Problems in Tests : In 2 parts. 
Part 1. Terms and Examples in Tasks : Study guide / T. Petrova, E. Starodubets; 
The Ministry of Education and Science of the Russian Federation, Kazan National 
Research Technological University. – Kazan : KNRTU Press, 2020. – 100 p.

ISBN 978-5-7882-2838-9
ISBN 978-5-7882-2839-6 (р. 1)

The Part 1 of the study guide contains the dictionary of terms, task examples with 

detailed comments and tasks for self-control on the main topics of General Chemistry. 

The study guide is intended for the Russian speaking first-year students learning 

in the educational program in the area 18.03.01 "Chemical Technology", who study 
the discipline “General and Inorganic Chemistry” in English, also to attract students 
from foreign countries to study in the framework of international educational programs.

The study guide was prepared at the Department of Inorganic Chemistry.

ISBN 978-5-7882-2839-6 (р. 1)
© Petrova Т., Starodubets Е., 2020

ISBN 978-5-7882-2838-9
© Kazan National Research Technological 

University, 2020

UDC 54(075)
ВВC Г1я7

C O N T E N T S

1. АTOMIC STRUCTURE............................................................................5

1.1. Dictionary.............................................................................................5
1.2. Worked examples.................................................................................6
1.3. Tasks for self-control...........................................................................8
1.4. Задания для самоконтроля..............................................................11

2. PERIODIC CHANGES IN SOME PROPERTIES 
OF CHEMICAL ELEMENTS ATOMS .....................................................14

2.1. Dictionary...........................................................................................14
2.2. Worked examples...............................................................................15
2.3. Tasks for self-control.........................................................................16
2.4. Задания для самоконтроля..............................................................18

3. MOLECULAR ORBITAL (МО) THEORY...........................................21

3.1. Dictionary...........................................................................................21
3.2. Worked examples...............................................................................22
3.3. Tasks for self-control.........................................................................24
3.4. Задания для самоконтроля..............................................................27

4. VALENCE BOND THEORY .................................................................30

4.1. Dictionary...........................................................................................30
4.2. Worked examples...............................................................................33
4.3. Tasks for self-control.........................................................................35
4.4. Задания для самоконтроля..............................................................38

5. SOLUTIONS AND THEIR CONCENTRATIONS ...............................41

5.1. Dictionary...........................................................................................41
5.2. Worked examples...............................................................................41
5.3. Tasks for self-control.........................................................................46
5.4. Задания для самоконтроля..............................................................47

6. FUNDAMENTALS OF CHEMICAL THERMODYNAMICS.............48

6.1. Dictionary...........................................................................................48

6.2. Worked examples...............................................................................49
6.3. Tasks for self-control.........................................................................54
6.4. Задания для самоконтроля..............................................................56

7. СHEMICAL EQUILIBRIUM.................................................................59

7.1. Dictionary...........................................................................................59
7.2. Worked examples...............................................................................61
7.3. Tasks for self-control.........................................................................62
7.4. Задания для самоконтроля..............................................................64

8. KINETICS OF CHEMICAL REACTIONS AND CATALYSIS...........67

8.1. Dictionary...........................................................................................67
8.2. Worked examples...............................................................................68
8.3. Tasks for self-control.........................................................................70
8.4. Задания для самоконтроля..............................................................71

9. HYDROLYSIS ........................................................................................74

9.1. Dictionary...........................................................................................74
9.2. Worked examples...............................................................................75
9.3. Tasks for self-control.........................................................................78
9.4. Задания для самоконтроля..............................................................80

10. OXIDATION – REDUCTION REACTIONS ......................................83

10.1. Dictionary.........................................................................................83
10.2. Worked examples ............................................................................84
10.3. Tasks for self-control.......................................................................88
10.4. Задания для самоконтроля............................................................91

TASKS FOR SELF-CONTROL. KEYS.....................................................94
BIBLIOGRAPHY........................................................................................98

1 .  А T O M I C  S T R U C T U R E

1 . 1 .  D i c t i o n a r y

English
Russian

Atomic orbital
Атомная орбиталь

Atomic spectrum
Атомный спектр

Aufbau principle
Принцип наименьшей энергии

Boundary surface 
Граничная поверхность

Core electrons
Внутренние электроны

Degenerate orbitals
Вырожденные орбитали

Effective nuclear charge
Эффективный заряд ядра

Electromagnetic radiation
Электромагнитное излучение

Electron
Электрон

Electronic structure
Электронная структура

Excited state
Возбужденное состояние

Frequency
Частота

Ground state
Основное состояние

Ground state electronic 
configuration

Электронная конфигурация основного состояния

Ground state valence electronic 
configuration 

Валентная электронная конфигурация основного состояния

Heisenberg’s uncertainty principle
Принцип неопределенности Гейзенберга

Hydrogen-like species
Водородоподобные частицы

Hund’s rule
Правило Хунда

Magnetic quantum number
Магнитное квантовое число

Magnetic spin quantum
number

Магнитное спиновое квантовое 
число

Many-electron species
Многоэлектронные частицы

Neutron
Нейтрон

Nucleus
Ядро

Orbital (s orbital, p orbital, d orbital, f orbital)

Орбиталь (s-орбиталь, p-орбиталь, 
d-орбиталь, f-орбиталь)

Orbital quantum number
Орбитальное квантовое число

English
Russian

Pauli exclusion principle
Принцип запрета Паули

Planck constant
Постоянная Планка

Principal quantum number
Главное квантовое число

Proton
Протон

Quantum
Квант

Schrӧdinger wave equation
Волновое уравнение Шредингера

Spherical symmetry
Сферическая симметрия

Valence electrons
Валентные электроны

Velocity
Скорость

Wavefunction
Волновая функция

Wavelength
Длина волны

Wave–particle duality
Корпускулярно-волновой дуализм 

1 . 2 .  W o r k e d  e x a m p l e s

Example 1. Write down sets of quantum numbers that describe an electron 
in an atomic orbital with n = 1.
Answer

For n = 1, the allowed values of l are integers between 

0 and (n – 1).

Therefore, for n = 1, the only allowed value of l is 0. 

Magnetic quantum number ml has integral values between 

+l…0…–l.

For l = 0, the only allowed value of ml is 0. Therefore, for n = 1 there is one 
atomic orbital with the set of quantum numbers: 

n = 1; l = 0; ml = 0.

This orbital can contain up to two electrons. Therefore, each electron in this
atomic orbital is defined by a set of four quantum numbers:

n = 1; l = 0; ml = 0; ms = +1/2

or

n = 1; l = 0; ml = 0; ms = −1/2.

Example 2. Determine the ground state electronic configuration of sodium atom.
Answer

The atomic number of sodium is 11, and there are eleven electrons 

to be accommodated in atomic orbitals in the ground state of the atom. 
The usual order of filling of atomic orbitals (lowest energy first) is:

1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 5d  4f <

< 6p < 7s < 6d  5f…

The lowest energy orbital is the 

1s (n = 1; l = 0; ml = 0).

The maximum number of electrons in the 1s orbital is two.

The next lowest energy orbital is the 

2s (n = 2; l = 0; ml = 0).

The maximum number of electrons in the 2s orbital is two

The next lowest energy orbitals are the three degenerate

2p orbitals (n = 2; l = 1, ml = −1; 0; +1).

The maximum number of electrons in the 2p orbitals is six, two spin-paired 
electrons per orbital.

The next lowest energy orbital is the

3s (n = 3; l = 0; ml = 0).

The maximum number of electrons in the 3s orbital is two, but only one 
remain to be accommodated (the sodium atom has eleven electrons; four 

electrons occupy the 1s and 2s orbitals and six electrons occupy the 2p orbitals).

Therefore, the ground state electronic configuration of Na is:

1s22s22p63s1.

1 . 3 .  T a s k s f o r  s e l f - c o n t r o l

1. No two electrons in the same atom may have the same set of n, l, ml
and ms quantum numbers. This is:
A) Heisenberg’s uncertainty principle; 
B) Aufbau principle; 
C) Pauli exclusion principle; 
D) Hund’s rule.

2. For a microparticle it is impossible to determine exactly and simultaneously: 
A) both the momentum and energy;
B) both the energy and velocity;  

С) both the momentum and time;
D) both the momentum and posi
tion.

3. The Louis de Broglie hypothesis is:
A) energy of electromagnetic radiation is emitted or absorbed only in discrete amounts (in quanta);
B) it is impossible to describe the microparticles motion by the laws 
of Newtonian mechanics; 
C) light is an electromagnetic wave;
D) all microparticles exhibit wave properties.

4. The behavior of electron as a microparticle is based on the following 
provisions (see below). Specify the wrong ones:
A) uncertainty in determining of position and momentum;
B) quantum nature of energy changes;
C) at any chosen distance from the nucleus, the probability of finding 
the electron is the same in all directions;
D) electron could exhibit the properties of both a particle and a wave.

5. What does the uncertainty principle in quantum mechanics mean?
А) all microparticles exhibit both particle and wave properties; 
B) the relationship between the errors in determining of the coordinate 
and momentum of a particle;
С) the energy of electromagnetic radiation is quantized;
D) the relationship between the coordinate and momentum of the microparticle.

6. The equation that relates the energy of a quantum and the frequency 
of the radiation is called:
А) Schrӧdinger wave equation;
В) the Planck equation;
С) the Arrhenius equation;
D) the de Broglie relationship.

7. The largest number of energy levels has an atom of:
А) Li;
B) Na;

C) K;
D) Rb.

8. Atoms that have the same number of valence electrons are:
А) Cl and Mn;
B) Al and Si;

C) P and Cr;
D) Ca and Sc.

9. The atom with the smallest number of energy levels is:
А) С;
В) Si;

С) Ge;
D) Sn.

10. What are the allowed types of orbitals if the value of the principal quantum number is equal to1? 
А) s orbital;
B) s and p orbitals;

C) s and d orbitals;
D) p and d orbitals.

11. Maximum possible number of electrons in a 2р and a 4d atomic orbitals 
is:
А) 2 and 4;
B) 2 and 6;

C) 6 and 10;
D) 3 and 5.

12. In the outer (highest energy) energy level in the ground state the chromium atom has:
A) 2 electrons; 
B) 6 electrons;

C) 4 electrons;  
D) 1 electron.

13. The number of electrons in the ion Mn2+ is:
А) 25;
B) 27;
C) 23;
D) 21.

14. The number of valence electrons in the ion Zn2+ is:
А) 10;
B) 2;
C) 0;
D) 12.

15. The ground state valence electronic configuration 5s25p5 has an atom
of:
А) Tc;
B) I;

C) Br;
D) Nb.

16. The ground state valence electronic configuration 4d55s2 has an atom
of:
А) Cd;
B) Sr;

C) Tc;
D) Mo.

17. The atomic number of the element with а 4d25s2 ground state valence 
electronic configuration is:
А) 40; 
B) 30;

C) 28;
D) 16.

18. The ground state electronic configuration of the ion F─ is:
А)1s22s2; 
B) 1s22s22p5; 
C) 1s22s22p6; 
D) 1s22s22p4.

19. The atom with a ground state valence electronic configuration ns2np3 is:
А) oxygen; 
B) antimony;
C) vanadium; 
D) fluorine.

20. The atom with a ground state valence electronic configuration 5d66s2 is:
A) barium; 
B) rhenium; 
C) osmium; 
D) radon.