Test for knowledge of inorganic chemistry. Alternative tests in inorganic chemistry. I. Complex substances and mixtures

Option #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. Number of electrons in the outer electron layer of a 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 = 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) occupies volume... l (n.s.)
1) 0,2 2) 5,6 3) 4,48 4) 28

A8. 16 g oxygen (0 2 ) are... mole

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

A9. The right side of the equation for the reaction between calcium hydroxide and
carbon dioxide with coefficients
1) CaC0 3 + 2H 2 0 2) CaC0 3 + H 2 0

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

A10. In connection K 2 Mn0 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) P 2) C1 3) F 4) S

A12. A covalent polar bond occurs in a substance

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

A13. Iron (I) sulfate reacts in solution with

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

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

3) MgO and C0 2 4) NO and HI

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

A16. Phosphorus is not used for

making matches
obtaining phosphorus(v) oxide in the production of phosphoric acid
formation of smoke screens during combustion
making inscriptions that glow in the dark

A17. Rate of reaction of Zn with H 2 S0 4 will decrease at

introduction of a catalyst
heating
diluting sulfuric acid with water
grinding zinc

A18. The main oxides are

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

5) CaO and BeO

A19. 6 moles of ions are formed upon complete dissociation of 2 moles

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 during a chemical reaction is...

Q2. 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 form (without numbers, commas or spaces). For example, GABV.

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

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

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

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

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 precipitate was formed.

AT 8. Oxygen can be obtained in the laboratory

decomposition of potassium permanganate B) distillation of liquid air
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 form without spaces or commas).

FINAL WORK FOR THE COURSE OF INORGANIC CHEMISTRY 9 CL.

Option No. 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. Number of electrons in the outer layer of a 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 acid is (in%)
1) 25 2) 30 3) 40 4) 75

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

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

A6. 4 g hydrogen (H 2 ) are... mole (n.s.)

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

A7. 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 connection NS10 4 chlorine oxidation state

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

A10. In a substance with the composition EO, the element E is

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

A11. A covalent nonpolar bond occurs in a substance

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

A12. Copper (P) sulfate reacts in solution with

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

A13. In the reaction equation between aluminum oxide and hydrogen bromide
acid, the ratio of the coefficients before the formulas of the reactants
substances are respectively equal
1)6:1 2) 1:6 3) 1:3 4)2:3

A14. Aluminum is not used

as a catalyst in the production of sulfuric acid
for the recovery of metals from oxides
for the production of electrical cables
for the production of aircraft alloys

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

A16. The main 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.s.) 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 moles of ions are formed upon complete dissociation of 1 mole

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)CaC0 3 4) NaCl

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

PART B

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

AT 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 D) Ba(OH) 2

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

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

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

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

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

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

AT 8. Sulfur(IV) oxide can be obtained

the action of dilute sulfuric acid on magnesium

B) burning sulfur

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 form without spaces or commas).

№1
How many and what elementary particles form the 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
An 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 are 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 did E. Rutherford discover the nucleus of the atom?
A) in the 20th century;
B) in the 19th century;
C) in the 16th century;
D) in the 21st century;
E) in the 18th 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) number of electrons;
D) nuclear charge;
E) 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;
B)3, 1,2;
C) 4, -2, 1;
0)7,0, 1;
E) -3,1,1.

№8
Which element has nine d electrons in its 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) shapes of electron clouds;
D) orbital;
E) spin.
№12
How many electrons are there on the 4d-noflypOBHe hafnium atom (Z=72)? A)1;
B) 2;
C) 4;
0)10;
E)8.

D) No. 13
Sublevels Zp, 3d, 4s, 4p in atoms are filled in the sequence...
A) Zr, 4s, 3d, 4p;
B) 3d, Zr, 4s, 4p;
C) 4s, Зр, 3d, 4р;
D) Зр, 3d, 4р, 4s;
E) Zr, 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 serial number?
A) 48;
B) 36;
C) 52;
0)58;
E)61;

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

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

№17
What is the maximum number of electrons in the 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 (Z=104) belong to?
A) s-elements;
B) p-elements;
C) d-elements;
D) f-elements;

E) q-elements.
№20
An atom of which element in an unexcited state has the electronic configuration: 1 s2 2s2 2p6 3s2 3рб 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 there in the 4d sublevel of a molybdenum atom? A)3;
B) 4;
C) 5;
D)6;
E)2.

D) No. 22
Which pair of elements are d-elements?
A) Al, Mg;
B) Ti, Ge;
C) Ta, Mo;
D) Pb, Au;
E) Ba, Pt.

№23
The main quantum number n=4. What values does the orbital quantum number take?
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 elements with metallic properties 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 group 4 to group 7;
D) elements of groups 1 and 2 of secondary subgroups;
E) elements of periods 1 and 2.

№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 main quantum number describes...
A) total electron energy;
B) molecular orbital;
C) orientation of the orbital in space;
D) the 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) No. 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 D.I. table. Mendeleev;
E) the number of unpaired electrons in the ground state and the same number in the excited state.

№30
From the thermodynamic functions given below, indicate the one that indicates the possibility of spontaneous occurrence of processes:
A) ∆G=0
B) ∆H C) ∆S>0;
D) ∆H>0
E)∆G No. 31
The first corollary of Hess's 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 a 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 substances;
D) the thermal effect of the reaction is equal to the difference in the heats of formation of the reaction products and starting substances;
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 which substance is the enthalpy of formation equal to zero?
A) CO2
B) CO
C)S
D)SO3
E) SO2

№34
What is meant by chemical bond?
A) the ability of atoms to combine with other atoms in certain proportions;
B) a 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 convergence 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 surrounding atoms.
№35
What is an ionic bond?

№36
What is a covalent bond called?
A) bond formed by electron pairs;
B) communication between ions due to electrostatic interaction;
C) a bond formed by a hydrogen ion when it is incorporated 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 lattice sites, held by rapidly moving electrons.
№37
What is a polar covalent bond?
A) bond formed by electron pairs;
B) communication between ions due to electrostatic interaction;
C) a bond formed by a hydrogen ion when it is incorporated 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 non-metal atoms, in which the electron cloud formed by a common pair of electrons turns out to be
asymmetrical and shifted towards the most electronegative atom of the element.
№38
What is a donor-acceptor bond called?
A) bond formed by electron pairs;
B) communication between ions due to electrostatic interaction;
C) a bond formed by a hydrogen ion when it is incorporated 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 lattice sites, held by rapidly moving electrons.
№39
In the oxides of elements of the third period of the periodic table presented below: Na2O, MgO, A12O3, SiO2, P2O5, SO3,
C12O7-in the period...
A) the main function increases;
B) acid function increases;
C) amphoteric function increases;
D) it is not possible to draw a conclusion regarding changes in the chemical nature of the 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) nonmetallic properties are reduced.

№43
What is the configuration of ground state valence electrons 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 valency 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 abstraction energy;
B) energy released when an electron is added;
C) half the 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) bond formed by electron pairs;
B) communication between ions due to electrostatic interaction;
C) this 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 lattice sites, held by rapidly moving electrons.
№48
Which of the following elements of the fourth period of the periodic table exhibits the same valence values in its hydrogen compound and in its higher oxide?
A) bromine;
B) germanium;
C) arsenic;
D) selenium;
E) iron,

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

CHEMISTRY , 1 COURSE, base 9 classes.

Teacher: Arkanova Elena Ivanovna

Conditions for completing the task: test tasks are completed in the classroom; time is allocated for answering questions of at least 2.5 academic hours (80 questions* 2 minutes). The tasks are completed on answer sheets.

Option 1

Note

Type A tasks

Eight electrons in the outer electron layer

a) S b) Si

c) O d) Ne

Number of orbitals at f-sublevel:

a) 1 b) 3

c) 5 d) 7.

3. Number of valence electrons on a chromium atom

a) 1 b) 2

at 4 d) 6.

4. Covalent nature of bonds in a series of compounds

LiF - BeF 2 - BF 3 - CF 4 - NF 3 - OF 2 - F 2:

d) does not change

5. An electron is...

a) a section of a circuit consisting of elements connected in series

b) charge of an atom of an element

6. It is unusual for substances with a metal crystal lattice:

a) low boiling point b) fragility

c) thermal conductivity d) plasticity

7. Does not undergo hydrolysis:

a) sodium acetate b) zinc chloride c) ethanol d) fat.

8. The reaction of magnesium with:

a) 1% HCl solution b) 5% HCl solution

c) 10% HCl solution d) 15% HCl solution.

9. The strongest acid is

a) silicon b) sulfur c) orthophosphoric d) chlorine

10. Provide a formula for determining the mass fraction of a substance

a) = m / V b) M = m /  .

V)  = V / V m g)ω = A r: M r

11. Specify the molecular weight of Cl 2 O 7

a) 183 b) 105 c) 224 d) 97

12. Specify the mass fraction S VSO 2

a) 20.13% b) 17.5% c) 22.43% d) 97%

13. As the area of the reactant increases, the reaction rate

a) will increase b) will decrease

a) gram per liter c) mole

b) gram d) quantity n

A) K 2 MnO 4 : K +1 , Mn +4 , O -2 ;

b) Ba(ClO 3 ) 2 : Ba +2 , Cl +5 , O -2 ;

V)F 2 O: F -2 , O +2 ;

16. Give the equation for the oxidation reaction sodium sulfite to sulfate

sodium:

a) 5Nа 2 SO 3 + 2КМnО 4 + ЗН 2 SO 4 = 5Nа 2 SO 4 + К 2 SO 4 + 2МnSO 4 + ЗН 2 О.

b) Na 2 SO 3 + KMnO 4 = Na 2 O + K 2 O + MnSO 3

17. Determine the mass of 5 mol CO2:

A)176;

b)220g;

V)47;

18. Indicate which compound is a strong electrolyte:

a) Mg OH c) Zn SO 3

b) H 2 S d) Ba (NO 3 )2

19. Complete the reaction equation:Ca(H2 P.O.4 ) 2 + HCl =

a) CaCl 2 + 2H 3 PO 4;

b) Ca OH + 2H 3 PO 4 ;

c) Ca (OH)2 + 2H 3 PO 4 ;

20. Indicate how hydrolysis of Cr occurs 2 (SO 4 ) 3 :

A ) Cr 2 (SO 4 ) 3 + 2H 2 S = 2Cr(OH)SO 3

b) Cr 2 (SO 4 ) 3 + 2H 2 O = 2Cr(OH)SO 4

reaction scheme:

a) 2 Al + 6NaOH + 6H 2 O = 2Na 3

b ) 3Al + 9NaOH + 9H 2 O = 3Na 3

22. What is the nature of the reaction of an aqueous solution of nitric acid?

a) Alkaline, HN O 3 = NO 3 + + OH - ;

b) Sour, HN O 3 = H + + N O 3 - ;

23. Indicate what is formed in oxygen and air during the combustion of acetylene?

a) ammonia and carbon dioxide;

b) water and ethylene;

c) water and carbon dioxide;

24. Are reactions typical for most inorganic substances?

A) combustion;

b) connections;

V) decomposition;

25. In the transformation scheme FeCl 3 X 1 X 2 Fe (OH) 3

a) Fe 2 (SO 4 ) 3 and Fe 2 O 3

b) FePO 4 and Fe 3 O 4

c) Fe(NO 3) 3 and Fe 2 O 3

d) Fe(OH) 3 and Fe 2 (SO 4 ) 3

26. Indicate the type of hybridization of key carbon atoms in the molecule:

CH 2 CH CH 3

a) sp 3 b) sp c) sp 2

27. The angle between the axes of the carbon atom for sp-hybrid orbitals is equal to:

a) 109 28 b) 120 c) 180

28. In sp 2 -hybridization does not involve the orbitals of the second energy level of the atom

carbon in quantity:

a) one b) two c) three

29. The class of alkenes includes hydrocarbons with the general formula:

a) C n H 2n+2 b) C n H 2n c) C n H 2n-2

30. Compounds with a closed chain of carbon atoms in a molecule are called:

a) acyclic b) carbocyclic

31. All alcohols have a suffix in their name:

a) -en b) - ol c) -al

32. Isomers have the same:

a) number of atoms b) structure of molecules c) properties

33.Substances CH 3 CH 2 CH 2 CH 3 And CH 3 CH CH 3 are:

a) homologues b) isomers c) neither homologues nor isomers

34. Potassium permanganate solution discolors:

a) ethylene b) ethane c) 2-methylpropane d) 3,3-dimethylpentane.

CH 3 CH 2 OH CH 2 CH 2 + H 2 O , refers to

reactions:

a) substitution b) addition c) elimination.

36. The reaction whose equation is given above is the reaction:

a) dehydrogenation b) dehydration c) dehydrochlorination.

37. Alkanes correspond to the general formula:

38. Homologues are:

a) ethane and ethylene b) propane and ethane c) butane and isobutane d) methane and ethene

a) ethylene b) pentane c) 2-methylbutane d) hexene-1

40. Carbon atoms in the state of sp 3 hybridization are present in the molecule:

a) pentane b) ethylene c) 2-methylbutane d) n-heptane

41. The most typical type of reaction for alkenes:

a) elimination b) isomerization c) addition d) substitution

42. Alkanes are characterized by isomerism:

a) position of the functional group b) carbon skeleton

c) positions of the double bond d) geometric

43. The main part of natural gas is:

a) ethane b) propane c) hexane d) methane

44. Cracking of petroleum products is...

a) separation of oil hydrocarbons into fractions

b) conversion of saturated hydrocarbons of oil into aromatic ones

c) thermal decomposition of petroleum products, leading to the formation

hydrocarbons with fewer carbon atoms per molecule

d) conversion of aromatic hydrocarbons of oil into saturated ones

45. There are no multiple bonds in the hydrocarbon molecule:

a) cyclopropanab) butadiene-1,3 c) propine d) benzene

46. An aromatic ring is contained in a molecule:

a) hexane b) cyclohexane c) hexene d) 1,4-dimethylbenzene.

47. The polymerization reaction is possible for...

a) butadiene-1,3b) propane c) chloroethane d) benzene.

48. The reaction of addition of water to unsaturated hydrocarbons is called...

a) hydrogenation b) halogenation c) hydration d) hydrohalogenation.

49. A substance whose formula is CH 3 CH 2 OH belongs to...

a) monohydric alcoholsb) phenols

CH 3 CH CH CH CO, has a name:

CH 3 H

a) 4-methylpentanal b) 2-methylpentanal

c) 2-methylpentene-3-alg) hexanal

51. Formation of a bright blue complex with copper (II) hydroxide

a) aldehydes b) polyhydric alcohols c) phenols d) ketones

52. The “silver mirror” reaction gives:

a) ethanol b) ethanediol-1,2 c) propanetriol-1,2,3 d) ethanal .

53.Carboxylic acids include a substance whose formula...

a) CH 3 COOH b) CH 3 COOH c) CH 3 O CH 3 d) CH 3 COOCH 3

54. A substance whose formula CH 3 SOOS 2 H 5 has a name...

a) diethyl ether b) methyl acetate

c) ethyl acetate d) ethyl formic acid.

55. Soap is...

A ) sodium salt of higher carboxylic acid

b) glycerol ester

c) ester of a higher carboxylic acid

d) a mixture of higher carboxylic acids.

56. The basis for the production of margarine is the reaction:

a) hydrolysis of fats b) esterification

c) saponification of fats d) hydrogenation of liquid fats.

57. Is a polymer:

a) glucose b) cellulose c) sucrose d) fructose

58. The reaction of the “silver mirror” involves...

a) glucose b) fructose c) sucrose d) starch

59. The following reaction is not typical for glucose:

a) alcoholic fermentation b) hydrolysis c) oxidation d) reduction

60. The following statement is true...

a) As a result of polycondensation of amino acids, peptides are formed;

b) Synthetic carboxylic acids are obtained from amino acids;

c) Amino acids do not change the color of indicators;

d) Proteins are a mixture of amino acids linked together

intermolecular bonds.

Note

In questions from 61 to 65, establish a correspondence between the law, the electrical quantity and their concept. Fill out the provided response forms.

1. Periodic law of D.I. Mendeleev a) Under the influence of electric current, positively charged ions of the dissolved substance move to the cathode, negatively charged to the anode.

2. Theory of chemical structure

organic substances Butlerova A.M b)

3. Electrolytic theory

dissociation c) Carbon atoms connecting in a chain form a certain sequence in accordance with valence, on which their properties depend

4. Atomic-molecular science d) The properties of simple bodies and compounds of elements are periodically dependent on the magnitude of their atomic masses.

1 - … 2 - … 3 - … 4 -…

1)  = a) =m / 

2)  = b) =V / Vm

3) ω = c) = A r ∙ n/M r ;

4) M= d) =m / V

1 -…. 2 - …. 3 - …. 4 - ….

alkanes – a) C n H 2 n . 2G

alkenes and cycloalkanes – b) C n H 2 n + 1G

alkynes and alkadienes – c) C n H 2 n – 6

arenas – d) C n H 2 n – 2

monohaloalkanes – e) C n H 2 n

dihaloalkanes – e) C n H 2n+2

amino acids g) C n H 2 n (N.H. 2 ) COOH

scheme :

1) N A) 1s 2 2s 2 2p 6 3s 2 3p 2 ,

2) Si b) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 ,

3) F e V) 1 s 2 2 s 2 2 p 3 .

1 -…. 2 - … 3 - …

1) Li 2 O + S EO 3 A) K 2 CO 3,

2) CO 2 + K 2 ABOUTb) Sa(NABOUT 3 ) 2

3) N 2 O 5 + CaO V)Li 2 Se O 4,

1 -…. 2 - … 3- …

Note

In tasks 66 to 75, complete the phrase you started or insert words

66. Expressing a reaction using chemicals formulas are called...

67. The properties of elements and their compounds are in ...

depending on the nuclear charge

68. Thermal effect - the amount of heat that...

69. Chemical equilibrium is a state...

70. Hydrolysis is the process of exchange interaction between salt and water, accompanied by the formation...

71. A catalyst is a substance that accelerates a reaction, not…

72. Solvation is the process of interaction between molecules and ions of a dissolved substance...

73. Redox reactions consist of two processes: ... and ...

74. Electrolysis is the process of synthesis or decomposition of substances using...

Note

In type B tasks from 75 to 80, solve the problem and offer the correct answer

Type B tasks

75. Calculate the mass of oxygen that reacted with organic

substance weighing 33.3 g. As a result of the reaction,

the following substances:

I) carbon dioxide - (CO 2) weighing 52.8 g;

2) carbon monoxide – (CO) weighing 11.2 g;

3) soot (C) weighing 2.4 g;

4) water weighing 40.5 g.

76. Determine the formula of a chemical compound if mass

the shares of its constituent elements are equal: H - 2.04%, S - 32.65%,

O - 65.31%.

77. What is the volume of oxygen released from one mole?

each of the substances: KClO 3, KMn O 4, KN O 3, Hg O according to the data below

reactions?

2 KClO 3 = 2KSl+ ZO 2 ,

2KMnABOUT 4 = K 2 MnABOUT 4 + MnABOUT 2 + O 2 ,

2KNO 3 = 2KNABOUT 2 + O 2 ,

2HgO = 2Hg + O 2.

1) AlWITHl 3 + CON (izb.) →

2) AlWITHl 3 + NN 3(izb.)+ N 2 About →

3) Al( NABOUT 3 ) 3 + NA 2 S+ N 2 About →

4) Na[Al(HE) 4 ] + CO 2 →

the following transformations:

M g → MgS O 4 → Mg (N O 3) 2 → Mg O → (CH 3 COO) 2 Mg.

80. Write the structural formula of 2,2,5,5-tetramethylhexane.

Write the formula of its isomer

Option 2

Note

In tasks 1 to 60, indicate the only correct answer

1. The electronic configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 has an atom of the element

a) K b) Ca c) Ba d) Na.

2. Number of orbitals at the d-sublevel:

a) 1 b) 3 c) 5 d) 7.

3. Number of valence electrons in a strontium atom

a) 1 b) 2 c) 3 d) 10.

4. Ionic nature of bonds in a series of compounds

Li 2 O - Na 2 O - K 2 O - Rb 2 O

a) decreases; b) increases;

c) first increases, then decreases; d) does not change

5. An electron orbital is...

a) the section of the path that the elements of matter connected together take

b) the conventional path along which an electron moves around the nucleus of an element

V ) negatively charged particle

6. What changes when the sequence of atoms in a molecule changes:

a) quantity and volume of the substance,
b) quantitative composition and density of the substance,
c) molecular mass and geometric shape.
d) Chemical structure and properties

7. Which aqueous solution is alkaline?:

a) sodium acetate b) copper (II) nitrate

c) potassium chloride d) aluminum sulfate.

8. The reaction will proceed at the highest speed at room temperature:

a) zinc with sulfuric acid

b) sodium with phenol

c) iron with oxygen

d) solutions of copper (II) sulfate and potassium hydroxide.

9. Of the listed metals, the most fusible is

a) copper b) mercury c) tin d) sodium.

10. Provide the formula to determinemolar mass of a substance

A) = m / V b) M = m /  . V) = V / V m G) ω = A r: M r

11. Specify the mass fraction S VSO 2

a) 20.13% b) 17.5% c) 22.43% G) 97%

12. Specify the molecular weight of Cl 2 O 7

a) 183b) 105 c) 224 d) 97

13. As the density of the reactant increases, the reaction rate

a) will increase b) will decrease

b) will not change d) will become equal to zero

14. Specify the units of measurement for molar mass

a) gram per liter c) mole

b) gram d) quantity n

15. Indicate where the oxidation states are correctly placed

A ) Ca(NO 2 ) 2 :Ca +2 , N +2 , O -2 ;

b) H 2 SiF 2 : H +1 , Si +3 , F -1 ;

V) Cr 2 (SO 4) 3: Cr +3, S +6, O -2.

16. State the reaction equation for the oxidation of iron (II) disulfide with concentrated nitric acid.

a) FeS 2 + 18H N O 3 (conc) = F e (N O 3) 3 + 2H 2 SO 4 + 15NO 2 + 7H 2 O.

b) F e (SO 4) 3 + HN O 3 (conc) = F e (N O 3) 3 + H 2 SO 4 + NO 2 + H 2 O.

17. Determine the mass of 9 molS ABOUT2 :

A)176;

b)220g;

V)576;

18. Indicate which compound is not a strong electrolyte:

a) HJ c) KOH

b) H 2 S d) Ba (NO 3 )2

19. Specify the missing substance:P2 O5 +...= Ca3 (P.O.4 ) 2 + H2 O

A) Ca N;

b)Ca OH;

V) Ca(OH) 2 ;

20. Indicate how hydrolysis occurs R2 S3 :

A) P 2 S 3 + 6H 2 O = 2H 3 PO 3 + 3H 2 S

b) R 2 SABOUT 3 + 6H = 2H 3 P.O. 3 + 3H 2 SABOUT 3

21. Indicate, correctly adjusted by the electronic balance method,

reaction scheme:

a) 3Na + 2H 2 O = 4 NaOH + H 2

b) 2Na + H 2 O = 2NaOH + H 2

22. What is the nature of the reaction of an ammonia aqueous solution?

A) Alkaline, NH 3 + H 2 O = NH 4 + + OH - ;

b)Sour, N.H. 3 +H 2 O=NH 3 + +OH - +H - ; ;

23. Indicate the correct empirical formula of the substance, consisting of:

Na - 32.8%, Al - 12.9%, F - 54.3%.

A) Na 2 Al3 F;

b) Na 3 AlF;

V) NaAlF;

24. Are reactions typical for most organic substances?

A)combustion;

b) connections;

V) decomposition;

25. In the transformation scheme Al (OH) 3
Y
Al(OH)3

substances “X 1” and “X 2” can be, respectively:

a) K 2 SO 4 and KOH

b) NaCl and HCl

c) Na 2 SO 4 and H 2 SO 4

d) HNO 3 and NaOH

26.Type of hybridization of carbon atoms in a molecule CH 3 CH 2 CH 2 CH 3

a) sp 2 b) sp 3 c) sp

27. The angle between the axes of the carbon atom for sp 3 - hybrid orbitals is equal to:

a) 109, 28 b) 120 c) 180

28. Orbitals of the second energy do not participate in sp-hybridization

level of carbon atom in quantity:

a) one b) two c) three

29. The class of alcohols includes substances with a functional group...

a) CO b) -OH c) SONON

30. Compounds with an open chain of atoms in a molecule are called:

a) acyclic

b) carbocyclic

31. All alcohols have a suffix in their name...

a) -en b) -ol c) -al

32.Isomers differ from each other...

a) number of atoms

b) molecular structure and properties

33.Substances CH 3 CH 2 CH 3 And CH 3 CH 2 CHCH 3 are:

a) homologues b) isomers c) neither homologues nor isomers.

34. A solution of potassium permanganate does not discolor the substance with the formula...

a) CH 3 CH 3 b) CH 2 CH CH 3

c) H 3 CH CH CH 3 d) CH 2 CH 2

35. Reaction whose equation is CH 3 CHCH 2 + H 2 CH 3 CH 2 CH 3 , refers

to reactions:

a) substitution b) addition c) elimination.

36. The reaction whose equation is given above is the reaction...

a) hydrogenation b) halogenation c) polymerization

37. Alkenes correspond to the general formula:

a) Сn Н 2n b) Сn Н 2n+2 c) Сn Н 2n-2 d) Сn Н 2n - 6

38. Homologues are:

a) methane and chloromethane b) propene and ethene

c) ethylene and butane d) 2-methylbutane and butane.

39. Hydrocarbons do not have isomers:

a) butene-1 b) propane c) n-heptane d) 2-methylpentene-2

40. ¶- there is no bond in the molecule...

a) propene b) 2-methylhexane c) 2-methylhexene-2 d) ethylene.

41. The most typical type of reaction for alkanes...

a) elimination b) isomerization

c) accession d) substitution

42. Alkenes are characterized by isomerism...

a) positions of the functional group

b) carbon skeleton

c) positions of the double bond, geometric

43. Oil in its composition is...

a) simple substance

b) a complex substance of the alkene class

c) a mixture of hydrocarbons, the basis of which is linear and linear alkanes

branched structure

d) a mixture of alkenes.

44.Oil distillation is carried out in order to obtain...

a) only methane and benzene

b) only gasoline and methane

c) various petroleum products

d) only aromatic hydrocarbons.

45.Butadiene contains...

a) one double bond

b) two double bonds

c) one triple bond

d) two triple bonds.

46. Weak acidic properties are exhibited by:

a) alkenes b) alkynes c) alkadienes d) arenes.

47. Reaction of addition of hydrogen to unsaturated hydrocarbons

called:

a) hydrogenation b) halogenation

c) hydration d) hydrohalogenation.

48. The process of producing rubber from rubber is called:

a) polymerization b) vulcanization

c) rectification d) hydration.

49. A substance whose formula CH 3 COOH, refers to…

a) monohydric alcohols b) phenols

c) aldehydes d) polyhydric alcohols

50. A substance whose formula is CH 3 CH CH 2 CH CH 3, has a name

OH C 2 H 5

a) 2-ethylpentanol-5 b) 4-ethylpentanol-2

c) 3-methylhexanol-5 d) 4-methylhexanol-2

51. Formation of a violet complex compound with iron(III) chloride

is a qualitative response to...

a) phenolb) aldehyde c) monohydric alcohol d) polyhydric alcohol.

52. Thanks to Kucherov’s reaction, you can get:

a) ethanal b) ethanol c) glycerol d) phenol.

53.Esters include a substance whose formula is:

a) CH 3 COOH

b) CH 3 CH

c) CH 3 O CH 3

d) CH 3 COOSH 3

54. Liquid fats differ from solid fats in that they contain...

a) free hydroxyl groups

b) residues of aromatic carboxylic acids

c) esters of higher carboxylic acids and ethylene glycol

d) residues of unsaturated carboxylic acids.

55. A substance whose formula CH 3 CH 3 CCH 2 COCH 3 OH has a name:

a) 3-methylbutanoic acid b) 2,2-dimethylbutanoic acid

c) 3,3-dimethylbutanoic acidd) hexanoic acid

56. Esters are obtained using the reaction:

a) hydration b) esterification c) polymerization d) saponification.

57. According to its chemical properties, glucose is...

a) polyhydric alcohol b) aldehyde

c) aldehyde alcohol d) acid

58. Blue staining with iodine solution gives:

a) glucose b) starch c) cellulose d) sucrose

59. The following statements are incorrect:

a) amino acids are highly soluble in water;

b) amino acids are obtained industrially using the Zinin reaction;

c) amino acids exhibit amphoteric properties;

d) amino acids enter into esterification reactions.

60.Aniline, in contrast to phenol:

a) reacts with bromine

b) poorly soluble in water

c) reacts with hydrochloric acid

d) burns.

Note

In tasks 61 to 65, match and fill out the proposed answer form

61. Establish a correspondence between the law, theory and their formulation:

1. Law of conservation of mass of matter a) Under the influence of electric current, positively charged ions of the dissolved substance move towards the cathode, negatively charged ones move towards the anode.

2. Avogadro's Law

b) Bodies consist of molecules and atoms that are in continuous motion, subject to the forces of repulsion and attraction.

3. Electrolytic theory

dissociation V)NA = 6,02 . 10 23 particles of matter. Equal volumes of any gas contain an equal number of molecules.

4. Atomic-molecular science d)The mass of substances entering into a chemical reaction is equal to the mass of substances formed as a result of the reaction

1 - … 2 - … 3 - … 4 -…

62. Establish a correspondence between a quantity and its formula

1)  = a) =m / 

2)  = b) =V / Vm

3) ω = c) =A r ∙ n/M r ;

4) M= d) =m / V

1 -…. 2 - …. 3 - …. 4 - ….

63. Establish a correspondence between a substance and its formula

phenols – a) C n H 2 n – 7 OH

alcohols – b) R 1 – NH – R 2

carboxylic acids – c) C n H 2 n + 1 N.H. 2 , R – NH 2

esters – d) C n H 2 n + 1 COOHR –COOH

primary amines – e) C n H 2 n + 1 OH, R–COH

secondary amines – e) R 1 –COOR 2

7. tertiary amines g) R 1 – N–R 2

R 3

1 -…. 2 - … 3 - … 4 - … 5- … 6- … 7- …

64. Establish a correspondence between a substance and its electronic graphic

scheme:

1) TOr A) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 3p 6 5s 2 4d 10 5p 4 ,

2) Those b) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 3p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 4 .

3) WV)1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 3 p 6 ,

1 -…. 2 - … 3 - …

65. Establish a correspondence between a chemical reaction and the reaction product:

1) CO 2 + NN 3 + N 2 ABOUTA)2 NaNSABOUT 3 .

2) SABOUT 2 + Na 2 SABOUT 3 + N 2 ABOUTb)NN 4 NSO 3 .

3) SABOUT 3 + N 2 ABOUTV)N 2 SABOUT 4 .

1 -…. 2 - … 3- …

Note

In tasks 66 to 74, finish the phrase you started.

66. If two elements form several chemical compounds with each other, then the masses of one of the elements are related to each other as small integers - this is the law...

67. The properties of substances are determined by their... and...

68. Thermal effect - the amount of heat that...

69 . Chemical equilibrium is a state...

70. Hydrolysis is a process of exchange interaction between salt and water, accompanied by the formation of...

71 . A catalyst is a substance that accelerates a reaction, not...

72. Oxidation of aldehydes with an ammonia solution of silver oxide...

73. The general name for monohydric alcohols is...

74. The reaction of formation of esters as a result of interaction

alcohols with acids...

Note

In tasks type B from 75 to 80 solve the problem and indicate the correct answer

Tasks type B

1. Calculate the mass fractions of hydrogen and oxygen in peroxide

hydrogen H 2 O 2 .

2. The reaction proceeds according to the equation: ZBa 2 + + 2PO 4 3- = Ba 3 (PO 4) 2 ↓

Write two different equations in molecular form,

corresponding to this reaction.

3 . Give examples of salt formation: a) from two simple

substances; b) from two complex substances; c) from simple and

complex substance.

4 . Write complete equations for the following reactions:

1) FeSO 4 + KClO 3 + N 2 SO 4 → ...

2) FeSO 4 + KClO 3 + KON → ...

3) I 2 + INA(HE) 2 → ...

4) HFr+ KBrO 3 + N 2 SO 4 → ...

5 . Write the reaction equations that allow you to carry out

the following transformations: N aCl → N a → N aH → N aOH → N aHS O 3 .

6 . Write the structural formulas of 2.2-dimethylpentane and

2.3-dimethylpentane.

Outcome Indicators mastering the discipline "Chemistry"

Assessing students' knowledge and skills within a discipline section

Excellent rating

91-100% correct answers

163 - 179

points

Rated "good"

76-90% correct answers

136 - 162 points

Rating "satisfactory"

61-75% correct answers

109 – 135 points

Rating "unsatisfactory"

60% or less correct answers

108 points or less

Number of options:

Test tasks consist of 2 options of 80 questions each.

lead time test task:

- 160 min

Scores are announced on the day of the event.

Answer form

(evaluation paper)

Student _________________ group _________ option___ 1

question

answer

question

answer

question

answer

question

answer

question

answer

question

answer

question

answer

question

answer

Total for the test

GRADE

Student ______________

(signature)

Checked ____________/

Answer form

(evaluation paper)

Student _________________ group _________ option ___2

For questions 1 to 60, indicate the only correct answer.

question

answer

question

answer

question

answer

question

answer

In tasks 61 to 65, match and fill out the form provided.

question

answer

question

answer

question

answer

question

answer

Total for the test

GRADE

Student ______________

(signature)

Checked ____________/

Final test in 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 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”.

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

Points received for correctly completed tasks are converted into traditional marks on the 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 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. Chemical symbol of this element: 1) C; 2) O; 3) Si

A3. The radii of atoms 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 nonpolar.

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) H 2 SO 3

A7. Exchange reactions include:

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

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

A9. Abbreviated ionic equation for the reaction 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 by the interaction in a solution of iron (II) chloride and: 1) hydrochloric acid; 2) potassium hydroxide; 3) copper (II) nitrate.

A11. The presence of acid in a solution can be proven 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) increasing acid concentration; 2) grinding chalk; 3) diluting the acid.

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

A15. A solution of hydrochloric acid cannot react: 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 equal to: 1) 5; 2) 7; 3) 9.

A20. After evaporating 40 g of solution to dryness, 10 g of salt remained. The mass fraction of salt in the original 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 an 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) B 2 O 3 .

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

A4. Formula of a substance with a covalent polar bond: 1) H 2 O; 2) O 2; 3) CaCl 2

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. Formula of sodium sulfite: 1) Na 2 SO 4; 2) Na 2 SO 3; 3) Na2S

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

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

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

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 the 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 proven using: 1) litmus; 2) phenolphthalein; 3) acids.

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

A13. The dissolution of zinc in hydrochloric acid will accelerate with: 1) increasing acid concentration; 2) when cooling the reagents; 3) when adding water.

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

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

A16. Sulfuric 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 equal to: 1) 1; 2) 2; 3) 3.

A20. 20 grams of salt were 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 contained in a nitrogen atom is: 1) 14; 2) 7; 3) 5.

A2. Electronic formula for the outer energy level of a 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 nonpolar.

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

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

A7. The reactions of the compound include: 1)KOH + HNO 3  KNO 3 + H 2 O;

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

A8. During the dissociation of the substance in an aqueous solution, K +, H + and CO 3 2- ions were formed. This substance is: 1) an acidic salt; 2) medium salt; 3) alkali.

A9. Abbreviated ionic equation for reaction 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. The gas is formed by the interaction in a solution of sulfuric acid and:

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

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

2) lime water; 3) hydrochloric acid.

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

A13. The dissolution of magnesium in hydrochloric acid will accelerate when:

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

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

A15. A solution of hydrochloric acid can react 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 equal to: 1) 3; 2) 5; 3) 7.

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

ANSWERS

option 1

option 2

option 3

A10

A11

A12

A13

A14

A15

A16

A17

A18

A19

A20

List of used literature

Gabrielyan O.S. Chemistry: textbook. for students prof. textbook establishments / O.S. Gabrielyan, I.G. Ostroumov. – M., 2005.

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

Erokhin Yu.M., Frolov V.I. Collection of problems and exercises in chemistry (with didactic material): textbook. allowance for students average. prof. manager – M., 2004.