№1
How many and what elementary particles form a 19F atom?
A) 9 neutrons and 9 electrons;
B) 9 neutrons, 10 protons and 19 electrons;
C) 9 protons and 19 electrons;
D) 19 protons and 19 electrons;
E) 9 protons, 10 neutrons and 9 electrons.
№2
The alkali metal atom forms an ion having the electronic configuration Is*2s22p63s23p6. This is the configuration
A) rubidium;
B) potassium;
C) sodium;
D) lithium;
E) cesium.

№3
What is the valency and oxidation state of nitrogen in nitric acid?
A) IV; +5;
B) III; -3;
C) V; +5;
D) IV; +4;
E) V; +3.
№4
In what century was the nucleus of the atom discovered by E. Rutherford?
A) in the 20th century;
B) in the 19th century;
C) in the 16th century;
D) in the 21st century;
E) in the XVIII century.

№5
Atoms are made up of...
A) protons and neutrons;
B) molecules;
C) atomic nuclei and electrons;
D) nucleons;
E) protons and electrons.

№6
The charge of an atom is...
A) zero;
B) the serial number of the element;
C) the number of electrons;
D) the charge of the nucleus;
E) the number of protons.

№7
Which of the sets of quantum numbers n, I, mi of an electron in an atom is allowed?
A) 3, 1, -1;
C) 3, 1.2;
C) 4, -2, 1;
0)7,0, 1;
E) -3,1,1.

№8
Which element has nine d-electrons at the third energy level?
A) K, Z=19;
B) Co, Z=27;
C) Cr, Z=24;
D) Cu, Z=29;
E) Ca, Z=20.

№9
Calculate the maximum possible number of electrons in the third energy level:
A) 8;
B) 14;
C) 18;
0) 32;
B) 24.

№10
Orbital quantum number L = 2. What is the maximum capacity of the corresponding energy sublevel?
A) 8;
B) 10;
C) 6;
D) 12;
E) 32.

№11
The orbital quantum number determines...
A) energy level;
B) magnetic properties;
C) forms of electron clouds;
D) orbital;
E) spin.
№12
How many electrons are there on 4d-noflypOBHe of a hafnium atom (Z=72)? A) 1;
B) 2;
C) 4;
0)10;
E) 8.

D) No. 13
Sublevels 3p, 3d, 4s, 4p in atoms are filled in the sequence...
A) Zp, 4s, 3d, 4p;
B) 3d, 3p, 4s, 4p;
C) 4s, 3p, 3d, 4p;
D) 3p, 3d, 4p, 4s;
E) Zp, 3d, 4s, 6p.

№14
The structure of the valence electron layer of an atom is expressed by the formula ... 5s25p4. What is the element's ordinal?
A) 48;
B) 36;
C) 52;
0)58;
E) 61;

№15
Which sublevel is filled in the atom with electrons after the 4p sublevel is filled? A)4d;
B) 3d;
C) 4s;
D)4f;
E)5s.

D) No. 16
The Periodic Law is a reflection of...
A) increase in the charge of the nucleus (elements);
B) depending on the serial number;
C) filling of electron shells;
D) increase atomic mass;
E) increase in atomic radii.

№17
What is the maximum number of electrons in a 33 orbital?
A) 1;
B) 2;
C) 6;
D)8;
E) 4;
№18
The main quantum number N takes the following values: A) -1/2,+1/2;
B) 0,1,2,3,4,5,...;
C) 1,2,3,4,5,6,7...;
D)-1,0,1,2,3,...;
E) -1, -2, -3, -4, ...

D) No. 19
What type of elements does Kurchatov iy (Z=104) belong to?
A) s-elements;
B) p-elements;
C) d-elements;
D) f-elements;

E) q-elements.
№20
The atom of which element in the unexcited state has an electronic configuration: 1 s2 2s2 2p6 3s2 Zrb 4s1?
A) Na(Z=ll);
B) K(Z=19);
C) Ca (Z=20);
D) Ba (Z=56);
E) Rb (Z=37).

№21
How many electrons are in the 4d sublevel of a molybdenum atom? A) 3;
B) 4;
C) 5;
D)6;
E) 2.

D) #22
Which pair of elements are d-elements?
A) Al, Mg;
B) Ti, Ge;
C) Ta, Mo;
D) Pb, Au;
E) Ba, Pt.

№23
Principal quantum number n=4. What are the values ​​of the orbital quantum number?
A) 1,2,3,4;
B) 0.1.2.3;
C) -4, -3, -2.0;
D) 1,2,3,4,5;
E) 0.1.2.3.4.

№24
Of the elements of the third period listed below, the most pronounced non-metallic properties are: A) aluminum;
B) silicon;
C) sulfur;
D) chlorine;
E) magnesium.

№25
Where are the metallic elements located on the Periodic Table?
A) elements of groups 1 and 2 of the main subgroups;
B) elements of group 7 of the main subgroup;
C) elements of the main subgroups from 4 to 7 groups;
D) elements of groups 1 and 2 of secondary subgroups;
E) elements of 1 and 2 periods.

№26
How many quantum numbers describe an electron orbital?
A)(n)
B) (n,l)
C) (n, l, ml, ms)
D) (l, m)
E)(n, l, ml)

№27
The principal quantum number describes....
A) the total energy of an electron;
B) molecular orbital;
C) orientation of the orbital in space;
D) number of electrons in an atom;
E) electron spin.

№28
How many electrons are in the 2p sublevel in the ground state of nitrogen (Z=7)?
A) 5;
B) 4;
C) 2;
0)3;
E) 6.

D) #29
What determines the valency of an atom?
A) period number;
B) group number;
C) the number of hydrogen atoms in the formation of a hydride;
D) (8 - N), where N is the group number in the table D.I. Mendeleev;
E) the number of unpaired ground state electrons and the same number in the excited state.

№30
From the following thermodynamic functions, indicate the one that indicates the possibility of spontaneous processes:
A) ∆G=0
B) ∆H C) ∆S>0;
D) ∆H>0
E)∆G #31
The first consequence of Hess' law is as follows:
A) the thermal effect of the reaction does not depend on the method of its implementation, but depends only on the initial and final states
substances;
B) the amount of energy released or absorbed by the system during the reaction is the thermal effect of the reaction;
C) the thermal effect of the reaction is equal to the difference between the sums of the heats of formation of the reaction products and starting materials;
D) the thermal effect of the reaction is equal to the difference between the heats of formation of the reaction products and starting materials;
E) the thermal effect of the reaction is equal to the sum of the heats of formation of the reaction products and starting materials.

№32
A) H2O2;
B) H2SO4
C) O2
D) H2O
E) NH3

№33
For what substance is the enthalpy of formation equal to zero?
A) CO2
B) CO
C) S
D) SO3
E) SO2

№34
What is meant by a chemical bond?
A) the ability of atoms to combine with other atoms in certain ratios;
B) set of particle interactions;
C) the order of connection of atoms in molecules;
D) interaction between electrons;
E) this is the attachment of other atoms to a given atom, accompanied by the approach of these atoms to several angstroms (10-10 m),
the release of energy and the regular orientation of these atoms relative to each other, taking into account the atoms of the environment.
№35
What is an ionic bond?

№36
What is called covalent bond?
A) a bond formed by electron pairs;
B) bonding between ions due to electrostatic interaction;
C) a bond formed by a hydrogen ion when it is introduced into a more electronegative atom;
D) a bond formed by a pair of electrons belonging to one atom and a vacant cell of another atom;
E) the connection between atoms and ions located at the lattice sites, held by rapidly moving electrons.
№37
What is a polar covalent bond?
A) a bond formed by electron pairs;
B) bonding between ions due to electrostatic interaction;
C) a bond formed by a hydrogen ion when it is introduced into a more electronegative atom;
D) a bond formed by a pair of electrons belonging to one atom and a vacant cell of another atom;
E) the bond between different atoms of non-metals, while the electron cloud formed by a common pair of electrons turns out to be
asymmetric and biased towards the most electronegative atom of the element.
№38
What is a donor-acceptor bond?
A) a bond formed by electron pairs;
B) bonding between ions due to electrostatic interaction;
C) a bond formed by a hydrogen ion when it is introduced into a more electronegative atom;
D) a bond formed by a pair of electrons belonging to one atom and a vacant cell of another atom;
E) the connection between atoms and ions located at the lattice sites, held by rapidly moving electrons.
№39
In the oxides of the elements of the third period of the periodic system presented below: Na2O, MgO, A12O3, SiO2, P2O5, SO3,
С12О7-in the period ...
A) the main function is increasing;
B) acid function increases;
C) amphoteric function increases;
D) it is not possible to draw a conclusion regarding the change in the chemical nature of oxides;
E) acid function decreases.
What formula can be used to determine the maximum number of electrons in a sublevel?
A) 21+1;
B) 2(21+1);
C)N2;
D) 2N2;
E) m+ 1.

№41
Which of the following elements has the lowest ionization potential?
A)Na,Z=ll;
B) Mg,Z=12;
C) K, Z=19;
D) Ca, Z=20;
E)Cs, Z=55.

E) No. 42
In the series N2O3, P2O3, As2O3, Sb2O3, Bi2O3:
A) metallic properties increase from N to Bi;
B) metallic properties decrease from N to Bi;
C) amphoteric properties decrease from Bi to N;
D) non-metallic properties increase from N to Bi;
E) non-metallic properties are reduced.

№43
What is the configuration of valence electrons in the ground state in a tungsten atom (Z=74)?
A)...5d16s2p3;
B) ... 5d55f "46s2;
C)...5d46s2;
D)...6s2p4;
E)...5d°6s2.
№44
Indicate the element that corresponds to the electronic configuration of the atom
A) potassium (Z= 19);
B) vanadium (Z=23);
C) calcium (Z=20);
D) scandium (Z=21);
E) chromium (Z=24).

№45
The highest valence among the listed metals has ...
A) Be (Z=4);
B) Mg(Z=12);
C) Al (Z=13);
D) Ti (Z=22);
E)Sc(Z=21)
E) No. 46
Electronegativity is...
A) electron detachment energy;
B) the energy released when an electron is attached;
C) half sum of ionization energy and electron affinity;
D) the ability to repel electron density;
E) the ability to donate valence electrons.

№47
What is a hydrogen bond?
A) a bond formed by electron pairs;
B) bonding between ions due to electrostatic interaction;
C) it is an intra- or intermolecular bond formed by a hydrogen ion and one of the electronegative atoms (fluorine,
oxygen, nitrogen)
D) a bond formed by a pair of electrons belonging to one atom and a vacant cell of another atom;
E) the connection between atoms and ions located at the lattice sites, held by rapidly moving electrons.
№48
Which of the given elements of the fourth period of the periodic system exhibits the same valency values ​​in its hydrogen compound and in the higher oxide?
A) bromine;
B) germanium;
C) arsenic;
D) selenium;
E) iron,

№49
How do the metallic properties of d-elements change in a period?
A) increase;
B) decrease;
C) complex addiction;
D) decrease and then increase;
E) increase and then decrease.
№50
The electronic configuration of the Zn2+ ion corresponds to the formula...
A)ls22s22p4;
C) Is22s22p63s23p6;
C)ls22s22p63s23p63d10;
D)ls22s22p63s23p63d104s2;
E)ls22s22p63s23p64s23d10.

Final test for inorganic chemistry

The final test contains tasks on the main topics of the school chemistry course: “Structure of the atom”, “Periodic law and the periodic system of chemical elements of D.I. Mendeleev”, “Structure of matter”, “Chemical reactions”, “Basic patterns of chemical reactions”, “Solutions. Theory of electrolytic dissociation”, “Redox reactions”, “Classification of substances”, “Main classes of inorganic and organic compounds”.

Tasks are worth 1 point. The maximum score is 20.

Points received for correctly completed tasks are translated into traditional marks on a scale:

"5" - 18-20 points,

"4" - 15-17 points,

"3" - 12-14 points,

"2" - 11 points or less.

option 1

A1. The number of electrons that are contained in a carbon atom is: 1) 6; 2) 12; 3) 8

A2. The electronic formula of the atom is 1s 2 2s 2 2p 6 3s 2 3p 2 . The chemical sign of this element is: 1) C; 2) O; 3) Si

A3. The atomic radii of chemical elements in the series: chlorine, phosphorus, aluminum, sodium: 1) increase; 2) decrease; 3) do not change.

A4. chemical bond in a water molecule: 1) ionic; 2) covalent polar; 3) covalent non-polar.

A5. Formulas of acid oxides: 1) CO 2 and CaO; 2) CO 2 and SO 3; 3) K 2 O and Al 2 O 3

A6. Formula of hydrosulfide acid: 1) H 2 S; 2) H 2 SO 4; 3) H2SO3

A7. Exchange reactions include:

1) CaO + H 2 O Ca(OH) 2 ; 2) FROM u(OH) 2  CuO + H 2 O; 3) KOH + HNO 3  KNO 3 + H 2 O

A8. Electrolytes, during the dissociation of which metal cations are formed, and anions of the acid residue are called: 1) acids; 2) salts; 3) grounds.

A9. abbreviated ionic equation reactions H+ + OH -  H 2 O corresponds to the interaction in solution: 1) potassium hydroxide and hydrochloric acid; 2) copper hydroxide (II) and hydrochloric acid; 3) copper hydroxide (II) and silicic acid

A10. The precipitate is formed during the interaction in a solution of iron chloride (II) and: 1) hydrochloric acid; 2) potassium hydroxide; 3) copper (II) nitrate.

A11. The presence of an acid in a solution can be proved using: 1) litmus; 2) phenolphthalein; 3) alkalis.

A12. The coefficient in front of the reducing agent formula in the equation for the reaction of aluminum with oxygen is: 1) 5; 2) 8; 3) 4.

A13. The dissolution of chalk in hydrochloric acid will slow down with: 1) an increase in the concentration of acid; 2) grinding chalk; 3) acid dilution.

A14. Chemical equilibrium in the system FeO (t) + H 2 (g)<==>Fe (t) + H 2 O (l) + Q will shift towards the formation of reaction products with: 1) an increase in pressure; 2) temperature increase; 3) lowering the pressure.

A15. A solution of hydrochloric acid cannot interact: 1) with sodium hydroxide; 2) with carbon dioxide; 3) with calcium.

A16. Sulfur oxide (IV) reacts: 1) with water; 2) with carbonic acid; 3) with calcium.

A17. Phosphoric acid does not react: 1) with potassium hydroxide; 2) with magnesium; 3) with hydrogen.

A18. Carbonic acid reacts: 1) with calcium oxide; 2) with sodium nitrate; 3) with silicon oxide (IV)

A19. The sum of all coefficients in the equation for the reaction of calcium with phosphoric acid is: 1) 5; 2) 7; 3) 9.

A20. After evaporation to dryness of 40 g of the solution, 10 g of salt remained. The mass fraction of salt in the initial solution was equal to: 1) 5%, 2) 15%; 3) 25%.

option 2

A1. The number of neutrons contained in an oxygen atom is: 1) 6; 2) 12; 3) 8.

A2. The formula of the highest oxide of the element, the electronic formula of which is 1s 2 2s 2 2p 6 3s 2 3p 3: 1) N 2 O 5; 2) P 2 O 5 ; 3) B2O3.

A3. The most pronounced non-metallic properties are exhibited by: 1) phosphorus; 2) sulfur; 3) silicon.

A4. The formula of a substance with a covalent polar bond: 1) H 2 O; 2) O2; 3) CaCl2

A5. The formula of the base and acid, respectively: 1) Ca (OH) 2 and Be (OH) 2;

2) NaOH and KHSO 4 ; 3) Al(OH) 3 and HNO 3

A6. Sodium sulfite formula: 1) Na 2 SO 4; 2) Na 2 SO 3; 3) Na 2 S

A7. Substitution reactions include: 1)Ca + H 2 SO 4  CaSO 4 + H 2 ;

2) FROM u(OH) 2  CuO + H 2 O; 3) KOH + HNO 3  KNO 3 + H 2 O

A8. Electrolytes, during the dissociation of which metal cations and hydroxide ions are formed, are called: 1) salts; 2) acids; 3) grounds.

A9. Abbreviated ionic reaction equationBa 2+ + SO 4 2-  BaSO 4 corresponds to the interaction in solution: 1) barium carbonate and sodium sulfate; 2) barium nitrate and sulfuric acid; 3) barium hydroxide and sulfur oxide (VI).

A10. Water is formed by interaction in a solution of hydrochloric acid and: 1) calcium hydroxide; 2) calcium; 3) calcium silicate.

A11. The presence of alkali in a solution can be proved using: 1) litmus; 2) phenolphthalein; 3) acids.

A12. The coefficient in front of the oxidant formula in the equation for the reaction of aluminum with sulfur is: 1) 8; 2) 2; 3) 3.

A13. The dissolution of zinc in hydrochloric acid will be accelerated by: 1) increasing the concentration of acid; 2) when the reagents are cooled; 3) when adding water.

A14. Chemical equilibrium in the CO 2 (g) + C (t) system<==>2 CO (g) - Q will shift towards the formation of the reaction product with: 1) pressure increase; 2) temperature increase; 3) lowering the temperature

A15. A solution of hydrochloric acid can interact: 1) with copper; 2) with carbon dioxide; 3) with magnesium.

A16. Sulphuric acid reacts: 1) with water; 2) with calcium oxide; 3) with carbon dioxide.

A17. Phosphorus oxide (V) does not react: 1) with copper hydroxide (II); 2) with water; 3) with potassium hydroxide.

A18. Silicic acid is formed by the interaction of: 1) silicon with water; 2) silicon oxide (IV) with water; 3) sodium silicate with hydrochloric acid.

A19. In the equation for the reaction of iron with chlorine to form iron (III) chloride, the coefficient in front of the salt formula is: 1) 1; 2) 2; 3) 3.

A20. 20 grams of salt are dissolved in 30 grams of water. The mass fraction of salt in the solution is: 1) 40%; 2) 50%; 3) 60%.

option 3

A1. The number of protons that are contained in the nitrogen atom is: 1) 14; 2) 7; 3) 5.

A2. The electronic formula of the external energy level of the carbon atom:

1) 2s 2 2p 6 3s 2 ; 2) 2s 2 2p 6 3s 2 3p 2 ; 3) 2s 2 2p 2 .

A3. The most pronounced metallic properties are exhibited by: 1) magnesium;

2) calcium; 3) barium.

A4. Chemical bond in an oxygen molecule: 1) ionic; 2) covalent polar;

3) covalent non-polar.

A5. Formulas of basic oxides: 1) CO 2 and SO 3; 2) K 2 O and CaO; 3) CO 2 and Al 2 O 3.

A6. The formula of iron hydroxide (III): 1) Fe (OH) 2; 2) Fe (OH) 3; 3) Fe 2 O 3.

A7. Connection reactions include: 1)KOH + HNO 3  KNO 3 + H 2 O;

2) FROM u(OH) 2  CuO + H 2 O; 3) CaO + H 2 O Ca(OH) 2

A8. When a substance dissociates into aqueous solution ions K + , H + and CO 3 2- were formed. This substance is: 1) an acid salt; 2) medium salt; 3) alkali.

A9. Reduced ionic reaction equation 2H + + SiO 3 2-  H 2 SiO 3 corresponds to the interaction in solution: 1) carbonic acid and aluminum silicate; 2) hydrochloric acid and potassium silicate; 3) silicic acid and calcium carbonate.

A10. Gas is formed by interaction in a solution of sulfuric acid and:

1) zinc; 2) zinc oxide; 3) zinc hydroxide

A11. The presence of carbon dioxide can be proved using: 1) phenolphthalein;

2) lime water; 3) hydrochloric acid.

A12. The coefficient in front of the reducing agent formula in the equation for the reaction of aluminum with sulfuric acid is: 1) 4; 2) 6; 3) 2.

A13. The dissolution of magnesium in hydrochloric acid will be accelerated by:

1) adding a catalyst; 2) adding water; 3) adding an inhibitor.

A14. Chemical equilibrium in system 2SO 2(d) + O 2(d)  2 SO 3(d) + Qwill shift towards the formation of the reaction product with: 1) an increase in temperature; 2) lowering the temperature; 3) lowering the pressure.

A15. A solution of hydrochloric acid can interact with: 1) sulfuric acid; 2) carbon monoxide; 3) sodium.

A16. Sulfur oxide (VI) reacts with: 1) hydrogen; 2) potassium hydroxide; 3) nitrogen.

A17. Nitric acid reacts with: 1) nitrogen; 2) water; 3) sodium.

A18. When carbon dioxide is passed through lime water, the following occurs: 1) clouding of the solution; 2) gas formation; 3) color change.

A19. The sum of all coefficients in the equation for the reaction of potassium with water is: 1) 3; 2) 5; 3) 7.

A20. To prepare 400 grams of a 2% salt solution, you need to take salt, the mass of which is: 1) 6 g; 2) 8 g 3) 10 g.

ANSWERS

option 1

option 2

option 3

A1

A2

A3

A4

A5

A6

A7

A8

A9

A10

A11

A12

A13

A14

A15

A16

A17

A18

A19

A20

List of used literature

Gabrielyan O.S. Chemistry: textbook. for stud. prof. textbook institutions / O.S. Gabrielyan, I.G. Ostroumov. - M., 2005.

Gabrielyan O.S. Chemistry in tests, tasks, exercises: textbook. allowance for students. avg. prof. educational institutions/ O.S. Gabrielyan, G.G. Lysova - M., 2006.

Erokhin Yu.M., Frolov V.I. Collection of tasks and exercises in chemistry (with didactic material): studies. allowance for students sredn. prof. manager - M., 2004.

There are only 26 Voros in the tests. Given a question and a correct answer.

School curriculum tests in chemistry

	liquid metal? (Mercury)
	What are substances that are made up of atoms of the same type called? (simple)
	Color of phenolphthalein in alkalis? (Crimson)
	A gas that supports combustion? (Oxygen)
	What is the name of the smallest particle of a substance that determines its properties? (Molecule)
	The volume of one mole of gas? (22.4l)
	Who discovered the law of conservation of mass of matter? (Lomonosov)
	The gas that is used to cut and weld metals? (Oxygen)
	The smallest indivisible particle of elements? (Atom)
	The most common element on earth? (Oxygen)
	What are salts of sulfuric acid called? (sulphates)
	Who discovered the periodic law? (Mendeleev)
	What gas is the most abundant in the Earth's atmosphere? (Nitrogen)
	Which acid is saltier, sulfuric acid or carbonic acid? (sulphuric)
	What is the composition of a water molecule (water formula)? (H2O)
	What is the valency of oxygen? (2)
	What is the formula for nitric acid? ( HNO-3)
	The lightest gas? (Hydrogen)
	What is the name of the number that is written in front of the formulas? (Coefficient)
	Specify acid-free acid: sulfuric, hydrochloric, nitric. (salt)
	Substances that change the rate of chemical reactions? (Catalysts)
	How many states of aggregation does water have? (Three)
	A unit of measure for the amount of a substance? (Moth)
	At what temperature does pure water boil? (100)
	The gas needed for breathing? (Oxygen)
	formula for oxygen? (O-2)

Chemistry test

I. Expand the essence of the periodic law of D. I. Mendeleev in the light of the theory of the structure of the atom.

1. Specify the name of the element forming amphoteric compounds:

c) sodium.

2. Designate the element that is part of the main subgroup:

a) calcium

b) iron

3. Determine the number of electrons that can be contained in f - sublevel of the electron shell:

4. Establish a correspondence between the number of electrons in the external energy level and the name of the chemical element:

a) 1, 1. potassium,

b) 2, 2. chlorine,

c) 3, 3. phosphorus,

d) 5. 4. aluminum,

5. Set the sequence of increasing charge of the nucleus of elements:

b) sodium

c) rubidium,

d) actinium.

6. Set the correspondence between the element symbol and its name:

a) Al, 1. magnesium,

b) Na, 2. nitrogen (nitrogen),

c) N, 3. mercury,

d) Hg. 4. aluminum,

5. sodium.

7. Designate the elements that can show valency II:

a) sodium

b) calcium,

c) aluminum.

d) magnesium

e) purple,

d) iron.

8. Designate the element of the second group:

b) carbon (carbon),

c) aluminum

9. Determine the molecular weight of the CaCo3 compound:

10. Choose a characteristic of the composition of a molecule of a simple substance:

a) is made up of one type of atom

b) consists of atoms of different types,

c) contains only two atoms.

d) contains only one atom.

11. Indicate the number of protons in the nucleus of an atom at number 20:

II Methane. Describe the structure of molecules, properties and applications.

1. Designate the valency of carbon in organic compounds:

at four,

2. Designate the homological difference in the homologous series of alkanes:

3. Specify the molecular formula of methane:

4. Specify the possible combustion products of methane:

a) oxygen

c) carbon dioxide

5. Specify the properties characteristic of methane:

a) gaseous

b) liquid

c) explosiveness,

d) lighter than air

e) good solubility in water.

6. Indicate possible products during the decomposition of methane:

a) molecular hydrogen

b) atomic hydrogen,

7. A characteristic reaction for methane is:

a) substitutions

b) joining,

c) exchange.

d) polymerization.

8. According to the structure of molecules, methane is:

a) an alkyne

b) alkene,

c) an alkane

d) cyclans.

9. Specify the general molecular formula of the homologous series of alkanes:

b) Сu H2n - 2bb

d) Сu H2n - 4.

10. Designate the compounds with which methane reacts:

11. Methane is used as a raw material in the processes:

a) oxidation,

b) recovery,

c) polymerization,

d) synthesis of new substances,

Option number 1

PART A

Choose the correct answer.

A1. Only complex substances are in the series:

1) iron and hydrogen chloride, 2) copper sulfate and copper oxide,

3) hydrogen sulfide and graphite, 4) graphite and diamond.

A2. The substance KNS0 3 is

1) salt 2) acid 3) base 4) oxide.

A3. The number of electrons in the outer electron layer of the silicon atom
1) 3 2) 14 3) 28 4) 4

A4. A precipitate is formed when hydrochloric acid is added to the solution.
acids:

1) barium hydroxide 2) silver nitrate

3) potassium nitrate 4) potassium carbonate

A5. Equation Mg + H 2 S0 4 \u003d H 2 + MgS0 4

Corresponds to the reaction of 1) connection, 2) substitution, 3) decomposition, 4) exchange.

A6. 500 g of solution contains 15 g of calcium nitrate, while the mass
the proportion of salt is (in%)
1) 3 2) 10 3) 20 4) 30

A7. 0.2 mol of carbon monoxide (P) (CO) occupy a volume ... l (n.o.)
1) 0,2 2) 5,6 3) 4,48 4) 28

A8. 16 g oxygen (0 2 ) make up ... mole

1) 0,5 2) 1 3) 16 4) 6,02-10 23

A9. The right side of the reaction equation between calcium hydroxide and
carbon dioxide with coefficients
1) CaCO 3 + 2H 2 0 2) CaCO 3 + H 2 0

3) CaC0 3 + H 2 4) CaO + H 2 C0 3

A10. In connection K 2 Мn0 4 oxidation state of manganese

1)+2. 2)+3 3)+6 4)+7

A11. In a substance of composition E 2 0 7 element E is

1) R 2) C1 3) F 4) S

A12. A covalent polar bond is carried out in a substance

1) S 8 2) K 5 S 3) K 4) H 2 S0 4

A13. Iron sulfate (P) reacts in solution with

1) Cu 2) Si 3) Ag 4) Mg

A14. Calcium oxide reacts with each of the substances
1) KOH and HC1 2)S0 2 and H 2 0

3) MgO and C0 2 4) NO and HI

A15. In the equation for the reaction between aluminum and hydrogen bromide
substances, respectively, is equal to
1)1:3 2) 3: 1 3) 2: 3 4) 1: 6

A16. Phosphorus is not used for

1. making matches
2. production of phosphorus(v) oxide in the production of phosphoric acid
3. formation of smoke screens during combustion
4. making inscriptions that glow in the dark

A17. Reaction rate of Zn with H 2 S0 4 will decrease at

1. the introduction of a catalyst
2. heating
3. dilution of sulfuric acid with water
4. grinding zinc

A18. Basic oxides are

3) Li 2 0 and H 2 0 4) C0 2 and Si0 2

5) CaO and BeO

A19. 6 mol of ions are formed with complete dissociation of 2 mol

l)Fe(N0 3 ) 2 2)FeS0 4 3) Fe(N0 3 ) 3 4) Fe 2 (S0 4 ) 3

1) 1,12 2) 11,2 3) 22,4 4)44,8

PART B

IN 1. A particle that accepts electrons in a chemical reaction is...

B2. Establish a correspondence between the class of inorganic compounds and the formula of the substance. In strict accordance with the sequence of numbers in the left column, write down the letters of the selected answers from the right column. Transfer the resulting sequence LETTERS in the answer sheet (without numbers, commas and gaps). For example, GABV.

VZ. 12 protons and 12 neutrons contains the nucleus of an atom of a chemical element...

AT 4. The number of electrons in a copper atom is...

AT 5. Arrange the elements in order of strengthening of metallic properties, writing down the numbers of substances without spaces and commas l) Ga 2) C 3) Si 4) Ge

AT 6. Arrange the substances in ascending order of the oxidation state of bromine atoms, writing down the numbers of the substances without spaces and commas

1. Br 2 2)NaBr0 3 3)NaBr 4) NaBrO

AT 7. When pouring solutions containing 2 mol of calcium nitrate and 3 mol of potassium carbonate, ... g of a precipitate was formed.

AT 8. Oxygen can be obtained in the laboratory

1. decomposition of potassium permanganate B) distillation of liquid air
2. decomposition of sodium nitrate D) decomposition of magnesium oxide E) decomposition of marble

Answer: .

(Write down the corresponding letters in alphabetical order and transfer them to the answer sheet without gaps or commas).

FINAL WORK FOR THE COURSE OF INORGANIC CHEMISTRY 9 CL.

Option number 2

PART A

Choose the correct answer.

A1. Both complex and simple substances are in the series:

1) nitrogen and chlorine, 2) ammonia and diamond, 3) hydrogen sulfide and carbon dioxide, 4) hydrogen bromide and water.

A2. The substance KNS0 3 is

1) salt 2) acid 3) base 4) oxide

A3. The number of electrons in the outer layer of the sulfur atom
1) 4 2) 6 3) 16 4) 32

A4. 1000 g of solution contains 250 g of sulfuric acid, while
the mass fraction of the acid is (in%)
1) 25 2) 30 3) 40 4) 75

A5. 0.1 mol of neon (Ne) occupy a volume ... l (n.o.s.)

1) 0,1 2) 2,24 3) 22,4 4) 20

A6. 4 g hydrogen (H 2 ) make up ... mole (n.o.)

1) 0,5 2) 2 3) 12,04-10 23 4) 4

A7. The right side of the reaction equation between magnesium and sulfuric acid with coefficients

1) MgS0 4 + H 2 0 2) MgS0 4 + H 2

3) MgS0 4 + 2H 2 0 4) MgS0 3 + H 2

A8. Number of moles of NaOH required to react with 1 mole of FeCl 2 , equals

1)1 2)2 3)3 4)4

A9. In the HC10 compound 4 oxidation state of chlorine

1) +2 2) +3 3) +6 4) +7

A10. In the substance of the EO composition, the element E is

1) Na 2) Be 3) B 4) F

A11. A covalent non-polar bond is carried out in a substance

1) R 4 2) R 2 0 5 3) Ca 4) Ca 3 R 2

A12. Copper sulfate (P) reacts in solution with

1) Ag 2) Hg " 3) Zn 4) S

A13. In the equation for the reaction between aluminum oxide and hydrobromide
acid ratio of the coefficients in front of the formulas of the reactants
substances, respectively, is equal to
1)6:1 2) 1:6 3) 1:3 4)2:3

A14. Aluminum is not used

1. as a catalyst in the production of sulfuric acid
2. for the recovery of metals from oxides
3. for the manufacture of electrical cables
4. for the manufacture of aviation alloys

A15. In the reaction 2NaI + Br 2 \u003d 2NaBr + I 2
the number of electrons accepted by one atom of the oxidizing agent is
1) 1 2) 2 3) 3 4) 4

A16. Basic oxides are

1) A1 2 0 3 and C0 2 2) BaO and Cu 2 0

3) Li 2 0 and H 2 0 4) C0 2 and Si0 2

A17. The amount of phosphorus substance that can react with 11.2 liters (n.o.) of oxygen according to the equation

4P + 50 2 = 2P 2 0 5 ,
is ... mole
1) 0,4 2) 12,4 3) 8,96 4) 4

A18. 5 mol of ions are formed with complete dissociation of 1 mol

l)Fe(N0 3 ) 2 2)A1 2 (S0 4 ) 3 3) Fe(N0 3 ) 3 4) MgS0 4

A19. Not found in nature

1) A1 2 0 3 2) A1 3) CaCO 3 4) NaCl

A20. When mixing solutions containing 1 mol of sodium carbonate and
1 mol of hydrochloric acid, gas will be released with a volume of ... l (n.o.)
1) 1,12 2) 11,2 3)22,4 4) 44,8

PART B

IN 1. Substances that decay into ions in solutions or melts are ...

IN 2. Establish a correspondence between the class of inorganic compounds and the formula of the substance. In strict accordance with the sequence of numbers in the left column, write down the letters of the selected answers from the right column. Transfer the resulting sequence E) Va (OH) 2

AT 3. 17 protons and 18 neutrons contains the nucleus of an atom of a chemical element ...

AT 4. The number of electrons in a calcium atom is...

AT 5. Arrange the elements in order of strengthening of non-metallic properties, writing down the numbers of substances without spaces and commas: 1) As 2) S 3) Se 4) Ge

AT 6. Arrange the substances in ascending order of oxidation state
phosphorus atoms, writing down the numbers of substances without spaces and commas

1) R 4 2) Mg 3 P 2 3) PCl 5 4) R 2 0 3

AT 7. When pouring solutions containing 2 mol of iron (II) chloride and 1 mol of sodium sulfide, ... g of a precipitate was formed.

AT 8. Sulfur(IV) oxide can be obtained

1. action of dilute sulfuric acid on magnesium

B) burning sulfur

1. burning hydrogen sulfide in excess air

D) the action of concentrated sulfuric acid on copper

D) the action of dilute sulfuric acid on sodium sulfide

Answer: .

(Write down the corresponding letters in alphabetical order and transfer them to the answer sheet without gaps or commas).

I. Complex substances and mixtures

1. The composition is heterogeneous.
2. Consists of different substances.
3. Do not have permanent properties.
4. Have permanent properties.
5. Retain the properties of the original components.
6. Do not retain the properties of the original components.
7. Can be separated by physical methods.
8. Cannot be separated by physical methods.
9. The original components are present in certain proportions.
10. The initial components are present in arbitrary ratios.
11. Rock granite is composed of quartz, mica and feldspar.
12. An iron sulfide molecule consists of iron and sulfur atoms.
13. There are homogeneous and heterogeneous.
14. Composition is expressed by a chemical formula.

Complex Substances

II. Atom and molecule

1. The smallest particle of a chemical element.
2. The smallest particle of a substance that retains its properties.
3. There are forces of mutual attraction and repulsion.
4. During physical phenomena they are preserved, during chemical phenomena they are destroyed.
5. Particles differ in size and properties.
6. Are in continuous motion.
7. Have a chemical symbol.
8. Have a chemical formula.
9. They have quantitative characteristics: mass, relative mass, valence, oxidation state.
10. Can connect with each other.
11. During chemical reactions, they are not destroyed, but regrouped.
Key "+" if "yes", key "-" if "no".

Job number
Molecule

III. Simple substance and chemical element

1. A set of atoms of the same type.
2. Consists of atoms of the same kind.
3. In chemical reactions, it cannot decompose to form several other substances.
4. Oxygen is a gas that is slightly soluble in water.
5. Fish breathe oxygen dissolved in water.
6. Iron is a metal that is attracted to a magnet.
7. Iron is part of iron sulfide.
8. An oxygen molecule consists of two oxygen atoms.
9. Currently known 114 various kinds atoms.
10. Oxygen is part of the water.
Key "+" if "yes", key "-" if "no".

Job number
simple substance
Chemical element

IV. Coefficient and index

1. Shows the number of atoms in a molecule.
2. Number in front of a chemical formula or symbol of a chemical element.
3. In the molecules of most simple gaseous substances, it is equal to 2.
4. Put in accordance with the valence in the formula of a complex substance.
5. Set when the number of atoms in the left and right parts chemical equation.
6. 7H, 5O.
7. There are two hydrogen atoms and one oxygen in a water molecule.
8. In the chemical formulas of metals, it is equal to 1.
9. In an iron sulfide molecule, the sum is 2.
10.5FeS.
Key "+" if "yes", key "-" if "no".

Job number
Coefficient

V. Simple matter and compound matter

1. Molecules are made up of atoms of the same kind.
2. Molecules are made up of different types of atoms.
3. Do not decompose during chemical reactions with the formation of other substances.
4. Decompose during chemical reactions with the formation of other substances.
5. Constant physical properties: melting point, boiling point, color, density, etc.
6. Destroyed by chemical reactions, but preserved by physical phenomena.
7. The composition is constant.
8. The composition varies within fairly wide limits.
9. Does not have permanent properties.
10. A molecule consists of two oxygen atoms and one hydrogen atom.
11. Can exist in three states of aggregation: gaseous, liquid, solid.
Key "+" if "yes", key "-" if "no".

Job number
simple substance
complex substance

VI. Chemical phenomena and physical phenomena

1. Molecules are saved.
2. Molecules are destroyed.
3. Change in the state of aggregation.
4. They change color and smell, heat is released, a precipitate forms.
5. Atoms are not destroyed, but rearranged.
6. Can be expressed using a chemical equation.
7. Melting glass when water freezes.
8. Combustion of fuel, decay of organic matter.
9. Chalk grinding.
10. Rusting of iron, souring of milk.
11. Isolation of copper on an iron nail in a solution of copper chloride.
12. Burning alcohol.
Key "+" if "yes", key "-" if "no".

chemical phenomena

physical phenomena

VII. Types of chemical reactions

1. The original substance is one complex.
2. Initial substance - two or more simple ones.
3. Initial substance - one simple and one complex.
4. Reaction products - two or more simple substances.
5. Reaction products - two or more complex substances.
6. Reaction products are one complex substance.
7. Reaction products - a simple and complex substance.
8. Reaction products - two or more simple or complex substances.
9. Reaction products - two complex substances.
10. Reaction products are two simple substances.
11. Decomposition of malachite.
12. Burning sulfur.
13. Interaction of zinc with hydrochloric acid.
Key "+" if "yes", key "-" if "no".

Connection reaction

decomposition reaction

substitution reaction

Exchange reaction

VIII. Hydrogen and oxygen

1. Dissolves in water.
2. Poorly soluble in water.
3. Light gas.
4. Heavy gas.
5. Combustible gas.
6. Gas supporting combustion.
7. Burns in chlorine.
8. Is a reducing agent.
9. When mixed with oxygen, forms an explosive mixture.
10. Collect by displacement of air.
11. Collected in a vessel turned upside down.
12. Collected in a vessel placed on the bottom.
13. Harvested by displacing water.
14. Interact with copper oxide when heated.
15. Used as an environmentally friendly fuel.
16. Used in rocket engines.
Key "+" if "yes", key "-" if "no".

Oxygen

IX. Metals and non-metals

1. Simple substances with a metallic luster, good conductors of heat and electricity, malleable.
2. Simple substances - solid, liquid or gaseous, mostly do not have a metallic luster, they do not conduct electric current well.
3. The highest valency for oxygen is I-II.
4. Higher oxides have basic properties.
5. Form volatile hydrogen compounds.
6. The highest valency for oxygen is IV-VII.
7. Higher oxides have acidic properties.
8. Do not form volatile hydrogen compounds.
9. Form hydroxides with basic properties.
10. Form hydroxides with acidic properties.
Key "+" if "yes", key "-" if "no".

Job number
non-metals

X. Group and period

(In a group, changes are considered from top to bottom, in a period - from left to right)
1. Non-metallic properties are enhanced.
2. Non-metallic properties weaken.
3. Metal properties are enhanced.
4. Metallic properties weaken.
5. Items contain the same number electrons in the outer electronic level.
6. The elements contain the same number of electronic levels.
7. The number of electronic levels is increasing.
8. The radius of atoms decreases.
9. The radius of atoms increases.
10. Gradual increase in the number of electrons at the outer level.
11. The same structure of the external electronic level.
12. The attraction of external electrons to the nucleus increases.
Key "+" if "yes", key "-" if "no".

XI. alkali metals. (lithium, sodium, potassium, rubidium, cesium)

1. Silver-white metal.
2. Metals with density less than 1.
3. Metals with a density greater than 1.
4. The lightest metal.
5. The heaviest metal.
6. Metal with a melting point below the temperature of the human body.
7. Metals that form basic oxides during oxidation.
8. Metals with an oxygen valency equal to 1.
9. Metals that catch fire at ordinary temperatures.
10. Metals that ignite only when heated.
11. Metals interacting with water to form alkali.
12. The most active metal.
Key "+" if "yes", key "-" if "no".

XII. Halogens (fluorine, chlorine, bromine, iodine)

1. Gaseous substance.
2. Liquid substance.
3. Solid.
4. Boiling point below 0o C.
5. Boiling point above 0o C.
6. Halogen dark gray.
7. Halogen red - brown.
8. Reacts with hydrogen to form volatile hydrogen compounds.
9. Reacts with metals to form salts.
10. Hydrogen valency is 1.
11. Oxygen valency is 7.
12. Possible valency 1. 3. 5. 7.
Key "+" if "yes", key "-" if "no".

XIII. Chlorine and hydrogen chloride

1. colorless gas
2. Yellow-green gas.
3. A gas with a pungent odor that smokes in moist air.
4. A gas with a pungent and suffocating odour.
5. It dissolves well in water.
6. It is poorly soluble in water.
7. The oxidation state of chlorine is 0.
8. The oxidation state of chlorine is -1.
9. In a molecule, there are polar covalent bonds between atoms.
10. In a molecule, there are covalent non-polar bonds between atoms.
11. Reacts with hydrogen in the light.
12. Reacts with metals under normal conditions.
13. Used to produce hydrochloric acid.
14. Store and transport in steel cylinders.
15. The gas is 2.5 times heavier than air.
16. The gas is slightly heavier than air.

Key "+" if "yes", key "-" if "no".

Hydrogen chloride

XIV. nitrogen and ammonia

1. Gaseous under normal conditions.
2. Has no smell.
3. Has a pungent odor.
4. has no color.
5. It is slightly soluble in water.
6. Let's well dissolve in water.
7. Easy to liquefy.
8. The oxidation state of nitrogen is - 3.
9. The oxidation state of nitrogen is 0.
10. In a molecule between atoms there are covalent polar bonds.
11. In a molecule between atoms there are covalent non-polar bonds.
12. Does not burn in air.
13. Reacts with hydrogen in the presence of a catalyst.
14. Burns in oxygen.
15. Interacts with water.
16. Interacts with acids to form salts.
Key "+" if "yes", key "-" if "no".

XV. Carbon monoxide (II) and carbon monoxide (IV)

1. Gas, practically insoluble in water.
2. Gas, visibly, soluble in water.
3. Gaseous under normal conditions.
4. Has no smell.
5. Doesn't liquefy.
6. Easy to liquefy and solidify.
7. Toxic gas.
8. Non-poisonous gas.
9. The oxidation state of carbon is +2.
10. The oxidation state of carbon is +4.
11. Flammable.
12. Off.
13. In a molecule between atoms there are covalent polar bonds.
14. Gas is lighter than air.
15. Gas is heavier than air.
16. Non-salt-forming oxide.
17. Acid oxide.
18. Reacts with metal oxides to form carbon monoxide (IV).
19. Turbidity is observed when passing through lime water.
Key "+" if "yes", key "-" if "no".

Carbon monoxide (IV)

XVI. Carbon monoxide (IV) and silicon oxide (IV)

1. Colorless gas, 1.5 times heavier than air.
2. Solid crystalline substance.
3. Substance with a molecular crystal lattice.
4. Substance with an atomic crystal lattice.
5. Dissolves in water.
6. Practically insoluble in water.
7. Is an acidic oxide.
8. Has no smell.
9. Easy to liquefy and harden.
10. The oxidation state of an element is +4.
11. Has low temperature melting.
12. Has a high melting point.
13. Reacts with basic oxides.
14. Reacts with alkalis.
15. Does not enter into chemical reaction with water.
16. At elevated temperatures, it displaces other, more volatile acidic oxides from salts.
Key "+" if "yes", key "-" if "no".

Carbon monoxide (IV)

XVII. Hydrochloric acid and sulfuric acid

1. Oily, viscous liquid.
2. Colorless liquid.
3. In moist air it "smokes".
4. Possesses hygroscopicity.
5. Concentrated. Irritating to the respiratory tract and mucous membranes.
6. At normal temperature, it is non-volatile and odorless.
7. Carbonizes sugar, paper, wood, fibers.
8. Forms hydrates when dissolved in water.
9. Used for drying gases.
10. Can be stored in iron containers and transported in steel tanks.
11. Stored and transported in rubberized tanks and barrels.
12. Used in batteries
Key "+" if "yes", key "-" if "no".

Hydrochloric acid