3 hours (180 minutes) are allotted to complete the examination paper in chemistry. The work consists of 3 parts and includes 43 tasks.
- Part 1 includes 28 tasks (A1-A28). Each question has 4 possible answers, of which only one is correct. Read each question carefully and analyze all possible answers.
- Part 2 consists of 10 tasks (B1-B10), to which you must give a short answer in the form of a number or sequence of numbers.
- Part 3 contains 5 most difficult tasks in general, inorganic and organic chemistry. Tasks C1-C5 require a full (detailed) answer.
All USE forms are filled in with bright black ink. The use of gel, capillary or fountain pens is allowed. When completing assignments, you can use a draft. Please note that entries in the draft will not be taken into account when evaluating the work.
We advise you to complete the tasks in the order in which they are given. To save time, skip the task that you can't complete right away and move on to the next one. If after completing all the work you have time left, you can return to the missed tasks.
When performing work, you can use the periodic system of chemical elements D.I. Mendeleev; table of solubility of salts, acids and bases in water; electrochemical series of metal voltages (they are attached to the text of the work), as well as a non-programmable calculator, which is issued during the exam.
The points you get for completed tasks are summed up. Try to complete as many tasks as possible and score the most points.
Part 1
When completing the tasks of this part in the answer sheet No. 1, under the number of the task you are performing (A1-A28), put the “×” sign in the box, the number of which corresponds to the number of the answer you have chosen.
A1 The particles contain the same number of electrons
1) Al 3+ and N 3-
2) Ca 2+ and Cl +5
3) S 0 and Cl -
4) N 3- and P 3-
A2 In the row of elements Na → Mg → Al → Si
1) the radii of atoms decrease
2) the number of protons in the nuclei of atoms decreases
3) the number of electron layers in atoms increases
4) the highest oxidation state of atoms decreases
A3 Are the following statements about metal compounds correct?
A. The oxidation state of beryllium in the higher oxide is +2.
B. The main properties of magnesium oxide are more pronounced than those of aluminum oxide.
1) only A is true
2) only B is true
3) both statements are correct
4) both judgments are wrong
A4 Chemical bond in the molecules of methane and calcium chloride, respectively
1) covalent polar and metallic
2) ionic and covalent polar
3) covalent non-polar and ionic
4) covalent polar and ionic
A5 The oxidation state of chlorine is +7 in the compound
1) Ca(ClO 2) 2
2) HClO 3
3) NH4Cl
4) HClO 4
A6 The molecular structure has
1) silicon(IV) oxide
2) barium nitrate
3) sodium chloride
4) carbon monoxide (II)
A7 Among the listed substances:
A) NaHCO 3
B) HCOOK
B) (NH 4) 2 SO 4
D) KHSO 3
E) Na 2 HPO 4
E) Na 3 PO 4
acid salts are
1) AGD
2) AVE
3) BDE
4) BDE
A8 Zinc reacts with solution
1) CuSO4
2) MgCl 2
3) Na 2 SO 4
4) CaCl2
A9 Which oxide reacts with HCl solution but does not react with NaOH solution?
1) CO
2) SO3
3) P2O5
4) MgO
A10 Aluminum hydroxide reacts with each of two substances:
1) KOH and Na 2 SO 4
2) HCl and NaOH
3) CuO and KNO 3
4) Fe 2 O 3 and HNO 3
A11 Barium carbonate reacts with a solution of each of the two substances:
1) H 2 SO 4 and NaOH
2) NaCl and CuSO 4
3) HCl and CH 3 COOH
4) NaHCO 3 and HNO 3
A12 In the scheme of transformations
substances "X" and "Y" are respectively
1) Cl 2 and Cu (OH) 2
2) CuCl 2 (solution) and NaOH
3) Cl 2 and NaOH
4) HCl and H 2 O
A13 Butene-1 is a structural isomer
1) butane
2) cyclobutane
3) butina
4) butadiene
A14 Unlike propane, cyclopropane reacts
1) dehydrogenation
2) hydrogenation
3) combustion in oxygen
4) esterification
A15 Freshly precipitated copper(II) hydroxide reacts with
1) propanol
2) glycerin
3) ethyl alcohol
4) diethyl ether
A16 Formaldehyde does not react with
1) Ag 2 O (NH 3 solution)
2) O2
3) H2
4) CH 3 DOS 3
A17 Butanol-1 is formed as a result of the interaction
1) butanal with water
2) butene-1 with an aqueous solution of alkali
3) 1-chlorobutane with one alkali solution
4) 1,2-dichlorobutane with water
A18 In the transformation scheme HC ≡ CH → X → CH 3 COOH substance "X" is
1) CH 3 CHO
2) CH 3 - CO - CH 3
3) CH 3 - CH 2 OH
4) CH 3 - CH 3
A19 The interaction of carbon monoxide (IV) with water refers to the reactions
1) connections, irreversible
2) exchange, reversible
3) connections, reversible
4) exchange, irreversible
A20 The reaction rate of nitrogen with hydrogen will decrease when
1) temperature decrease
2) increase in nitrogen concentration
3) using a catalyst
4) increase in pressure
A21 Chemical equilibrium in the system
will shift towards the reaction products at
1) pressure increase
2) rise in temperature
3) pressure reduction
4) using a catalyst
A22 The largest amount of sulfate ions is formed in solution upon dissociation of 1 mol
1) sodium sulfate
2) copper(II) sulfate
3) aluminum sulfate
4) calcium sulfate
A23 Reduced ionic equation H + + OH - \u003d H 2 O corresponds to the interaction
1) H 2 SO 4 with NaOH
2) Cu(OH) 2 with HCl
3) H 2 SiO 3 with KOH
4) HCl with HNO 3
A24 Solutions of copper(II) chloride and
1) calcium chloride
2) sodium nitrate
3) aluminum sulfate
4) sodium acetate
A25 Sulfuric acid exhibits oxidizing properties in the reaction, the scheme of which is:
1) H 2 SO 4 + NH 3 → NH 4 HSO 4
2) H 2 SO 4 + KOH → K 2 SO 4 + H 2 O
3) H 2 SO 4 + P → H 3 PO 4 + SO 2
4) H 2 SO 4 + P 2 O 5 → HPO 3 + SO 3
A26 Are the following statements about the rules for handling substances correct?
A. Substances must not be tasted in the laboratory.
B. Mercury salts should be handled with extreme care due to their toxicity.
1) only A is true
2) only B is true
3) both statements are correct
4) both judgments are wrong
A27 A polymer having the formula
receive from
1) toluene
2) phenol
3) propylbenzene
4) styrene
A28 According to the thermochemical reaction equation
CaO (tv) + H 2 O (g) \u003d Ca (OH) 2 (tv) + 70 kJ
to obtain 15 kJ of heat, calcium oxide with a mass
1) 3 g
2) 6 g
3) 12 g
4) 56 g
Part 2
The answer to the tasks of this part (B1-B10) is a sequence of numbers or a number that should be written in the answer sheet No. 1 to the right of the number of the corresponding task, starting from the first cell. Write each number and comma in the decimal fraction entry in a separate box in accordance with the samples given in the form.
In tasks B1-B5, for each element of the first column, select the corresponding element of the second and write down the selected numbers in the table under the corresponding letters, and then transfer the resulting sequence of numbers to the answer form No. 1 without spaces, commas and other additional characters. (The numbers in the answer may be repeated.)
B1 Match the name of the compound with the general formula of the homologous series to which it belongs.
| A | B | IN | G |
The answer to tasks B6-B8 is a sequence of three digits that correspond to the numbers of the correct answers. Write these numbers in ascending order first in the text of the work, and then transfer them to the answer sheet No. 1 without spaces, commas and other additional characters.
B6 Interaction of 2-methylpropane and bromine at room temperature in the light
1) refers to substitution reactions
2) proceeds by a radical mechanism
3) leads to the predominant formation of 1-bromo-2-methylpropane
4) leads to the predominant formation of 2-bromo-2-methylpropane
5) proceeds with a break in the C - C bond
6) is a catalytic process
B7 Phenol reacts with
1) oxygen
2) benzene
3) sodium hydroxide
4) hydrogen chloride
5) sodium
6) carbon monoxide (IV)
Answer:___________________________
B8 Methylamine may interact with
1) propane
2) chloromethane
3) oxygen
4) sodium hydroxide
5) potassium chloride
6) sulfuric acid
Answer:___________________________
The answer to tasks B9-B10 is a number. Write this number in the text of the work, and then transfer it to the answer sheet No. 1 without indicating the units of measurement.
B9 Determine the mass of water that must be added to 20 g of a solution of acetic acid with a mass fraction of 70% to obtain a solution of acetic acid with a mass fraction of 5%. (Write down the number to the nearest integer.)
Answer: ___________ g.
B10 The mass of oxygen required to completely burn 67.2 L (N.O.) of hydrogen sulfide to SO 2 is __________ g. (Write the number to the nearest whole number.)
Don't forget to transfer all answers to the answer sheet No. 1.
Part 3
To write down the answers to the tasks of this part (C1-C5), use the answer sheet No. 2. First write down the number of the task (C1, C2, etc.), and then its full solution. Write your answers clearly and legibly.
C1 Using the electron balance method, write the equation for the reaction
C2 The salt obtained by dissolving iron in hot concentrated sulfuric acid was treated with an excess of sodium hydroxide solution. The brown precipitate formed was filtered off and dried. The resulting substance was fused with iron.
C3 Write the reaction equations that can be used to carry out the following transformations:
C4 To a solution of sodium hydroxide weighing 1200 g was added 490 g of a 40% solution of sulfuric acid. It took 143 g of crystalline soda Na 2 CO 3 ⋅10H 2 O to neutralize the resulting solution. Calculate the mass and mass fraction of sodium hydroxide in the initial solution.
C5 The interaction of 25.5 g of saturated monobasic carboxylic acid with an excess of sodium bicarbonate solution released 5.6 l (N.O.) of gas. Determine the molecular formula of the acid.
Chemistry Examination Grading System
PART 1
For the correct answer to each task of part 1, 1 point is put. If two or more answers are given (including correct), incorrect answer or no answer - 0 points.
| job number | Answer | job number | Answer | job number | Answer |
| A1 | 1 | A11 | 3 | A21 | 2 |
| A2 | 1 | A12 | 3 | A22 | 3 |
| A3 | 3 | A13 | 2 | A23 | 1 |
| A4 | 4 | A14 | 2 | A24 | 3 |
| A5 | 4 | A15 | 2 | A25 | 3 |
| A6 | 4 | A16 | 4 | A26 | 3 |
| A7 | 1 | A17 | 3 | A27 | 4 |
| A8 | 1 | A18 | 1 | A28 | 3 |
| A9 | 4 | A19 | 3 | ||
| A10 | 2 | A20 | 1 |
PART 2
A task with a short free answer is considered to be completed correctly if the sequence of digits (number) is correctly indicated.
For a complete correct answer in tasks B1-B8, 2 points are given, if one mistake is made - 1 point, for an incorrect answer (more than one mistake) or its absence - 0 points.
For the correct answer in tasks B9 and B10, 1 point is given, for an incorrect answer or its absence - 0 points.
job number | Answer |
PART 3
CRITERIA FOR VERIFICATION AND EVALUATION OF THE PERFORMANCE OF TASKS WITH A DETAILED ANSWER
For completing tasks, the following is assigned: C1, C5 - from 0 to 3 points; C2, C4 - from 0 to 4 points; C3 - from 0 to 5 points.
C1 Using the electron balance method, write the equation for the reaction
Na 2 SO 3 + ... + KOH → K 2 MnO 4 + ... + H 2 O
Determine the oxidizing agent and reducing agent.
Points |
|
Response elements: 2) it is indicated that sulfur in the +4 oxidation state is a reducing agent, and manganese in the +7 oxidation state (or potassium permanganate due to manganese in the +7 oxidation state) is an oxidizing agent; | |
The answer contains an error in only one of the elements | |
There are two errors in the response. | |
Maximum score |
C2 The salt obtained by dissolving iron in hot concentrated sulfuric acid was treated with an excess of sodium hydroxide solution.
The brown precipitate formed was filtered off and dried. The resulting substance was fused with iron.
Write the equations of the described reactions.
Points |
|
Response elements:
| |
Correctly written 4 reaction equations | |
Correctly written 3 reaction equations | |
Correctly written 2 reaction equations | |
| Correctly written 1 reaction equation | 1 |
All elements of the answer are written incorrectly | |
Maximum score |
C3 Write the reaction equations that can be used to carry out the following transformations:
Points |
|
Response elements:
| |
The answer is correct and complete, includes all the above elements | 5 |
| Correctly written 4 reaction equations | 4 |
| Correctly written 3 reaction equations | 3 |
| Correctly written 2 reaction equations | 2 |
| Correctly written one reaction equation | 1 |
| 0 | |
| Maximum score |
C4 To a solution of sodium hydroxide weighing 1200 g was added 490 g of a 40% solution of sulfuric acid. It took 143 g of crystalline soda Na 2 CO 3 ⋅10H 2 O to neutralize the resulting solution. Calculate the mass and mass fraction of sodium hydroxide in the initial solution.
Points |
|
Response elements: It is also possible to calculate on the basis of the reaction equations for the formation of NaHSO 4 and its subsequent interaction with Na 2 CO 3 . The final answer will not change; 2) the total amount of sulfuric acid was calculated, as well as the amount 3) the amount of sulfuric acid that reacted with sodium hydroxide and the mass of sodium hydroxide in the initial solution were calculated: n (H 2 SO 4) \u003d 2 - 0.5 \u003d 1.5 mol 4) the mass fraction of sodium hydroxide in the initial solution was calculated: | |
The answer is correct and complete, includes all the above elements | 4 |
| The response contains an error in one of the above elements. | 3 |
| Response contains errors in two of the above elements | 2 |
| The answer contains errors in three of the above elements. | 1 |
| All elements of the answer are written incorrectly | 0 |
| Maximum score | 4 |
* Note.
C5 When 25.5 g of saturated monobasic carboxylic acid reacted with an excess of sodium bicarbonate solution, 5.6 l (N.O.) of gas was released. Determine the molecular formula of the acid.
| Points | |
response elements. С n H 2n+1 COOH + NaHCO 3 = СnH 2n+1 COONa + H 2 O + CO 2 2) The molar mass of the acid is calculated: 3) The molecular formula of the acid is established: Molecular formula - C 4 H 9 COOH | |
| The answer is correct and complete, includes all the above elements | 3 |
| The first and second elements of the answer are written correctly | 2 |
| The first or second element of the answer is written correctly | 1 |
| All elements of the answer are written incorrectly | 0 |
| Maximum score | 3 |
* Note. In the case when the answer contains an error in the calculations in one of the elements (second, third or fourth), which led to an incorrect answer, the mark for completing the task is reduced by only 1 point.
A 3. Chemical bond.
1. Chemical bonding in hydrogen chloride and barium chloride, respectively
1) covalent polar and ionic 2) covalent non-polar and ionic
3) ionic and covalent polar 4) ionic and covalent non-polar
2.
Compounds with covalent non-polar and ionic bonds are respectively
1) barium sulfate and methanol 2) hydrogen sulfide and methane
2) water and acetylene 4) nitrogen and calcium fluoride
3.
Chemical bond in methane and calcium chloride molecules, respectively
1) hydrogen and ionic 2) ionic and covalent polar
3) covalent non-polar and ionic 4) covalent polar and ionic
4. Substances with only covalent polar bonds are listed in the series:
1) CaF 2, Na 2 S, N 2 2) P 4, FeC1 3, NH 3 3) SiF 4, HF, H 2 S 4) Na 3 P, LiH, S0 2
5. Substances with an ionic type of bond are
1) SF 6, NH 4 F, OF 2, 2) NH 4 C1, PC1 3, SiC1 4 3) KF, KS1, NH 4 F 4) CH 4, K 2 C0 3, C 2 H 2
6. The polarity of the E-N bond increases in the series
1) H 2 S, HC1 2) HF , H 2 O 3) NH 3, C 2 H 6 4) H 2 S, H 2 Se
7. The bond length increases in the series
1) PC1 3, RVg 3, PH 3 2) NH 3, NF 3, NC1 3 3) SO 2, CO 2, NO 2 4) BrC1 3, BrF 3, HBg
6. Bond strength increases in a row
1) NH 3, PH 3 2) H 2, Br 2 3) CS 2, CO 2 4) HBr, NI
9.
The ionic nature of the bond is most pronounced in the compound
1) BeO 2) K 2 O 3) MgO 4) B 2 O 3
10. The number of σ-bonds is the same in molecules in the series
1) H 2 S, CO 2, NH 3 2) H 2 O, SO 2, SO 3 3) PF 3, NH 3, HC1 4) C 2 H 2, SO 3, NH 3
11 .The number of π-bonds in the molecule increases V row
1) CO 2, SO 2, C 2 H 2 2) C 2 H 2, NO 2, NO 3) NO, N 2, SO 3 4) HC1O 4, H 2 CO 3, C 2 H 2
12.
The bond is formed by the donor-acceptor mechanism
1) NH 3 2) H 2 O 3) H 3 O + 4) H 2 O 2
A. The more energy is released during the formation of a bond, the stronger the bond.
B. The more polar the bond, the easier it is broken by the ionic type.
1) only A is true 2) only B is true 3) both judgments are true 4) both are wrong
A. When some bonds are broken, energy is released.
B. A pi bond is less strong than a sigma bond.
A. When a chemical bond is formed, energy is always released.
B. Double bond energy less than a single bond.
1) only A is true 2) only B is true 3) both judgments are true 4) both are wrong
16.
Bond strength increases in molecules in the series
1) chlorine-oxygen-nitrogen 2) oxygen-nitrogen-chlorine
3) oxygen-chlorine-nitrogen 4) chlorine-nitrogen-oxygen
17. Hydrogen bonds form between molecules
1) hydrogen 2) formaldehyde 3) acetic acid 4) hydrogen sulfide
18
.The ability of atoms to accept electrons increases in the series:
a) Br,S,Te b) C,Si,Pb c) Cl,Br,I d) N,O,F
19
.Due to the covalent polar bond, the following substances are formed:
a) H 2 S, Cl 2, H 2 O b) CO, SO 2, N 2 O 5 c) NaCl, F 2, NO d) HCl, NH 3, KI
20
.Ions compared with atoms:
a) different number of electrons
b) different number of protons
c) different number of neutrons
d) no difference
21
.In the KNO 3 compound, the chemical bonds are:
a) all covalent b) all ionic
c) covalent and ionic
d) metallic and covalent
22
.In what series are the formulas of substances with an ionic bond written?
a) HBr, KOH, CaBr 2
b) CaCl 2 , NaOH, K 2 SO 4
c) H 2 SO 4, K 2 SO 4, Al (OH) 3
d) K 2 O, NaF, SO 3
23
.The most electronegative element is:
a) boron b) sulfur c) oxygen d) nitrogen
24
A substance with an ionic bond has the formula: a) F 2 b) HF c) CaF 2 d) OF 2
25
.A chemical bond is formed between the atoms of chemical elements with serial numbers 11 and 7:
a) covalent non-polar b) covalent polar c) ionic d) metallic
26
.A substance with a metallic bond has the formula:
a) BaCl 2 b) PCl 3 c) Cl 2 d) Ba
27
.Chemical bond in potassium oxide
a) covalent polar b) covalent non-polar c) ionic d) metallic.
A 5. Substances of molecular and non-molecular structure.
1 .All substances of molecular structure are characterized
1) high melting point 2) electrical conductivity
3) consistency of composition 4) hardness
2 .Silicon crystal lattice
3 . The molecular structure has 1) barium chloride 2) potassium oxide 3) ammonium chloride 4) ammonia
4. The molecular structure has
1) CO 2 2) KVg 3) MgSO 4 4) SiO 2
5
.Molecular crystal lattice have substances
1) graphite and diamond 2) silicon and iodine
3) chlorine and carbon monoxide (4) 4) potassium chloride and barium oxide
6
.Allotropic modifications are
1) sulfur and selenium 2) graphite and diamond
3) oxygen-17 and oxygen-18 4) nitrogen and ammonia
7 .Atomic crystal lattice have
1) silicon oxide (4) and carbon monoxide (4) 2) chlorine and iodine 3) graphite and silicon 4) potassium chloride and sodium fluoride
8 .Substance of non-molecular structure
1) CO 2) MgO 3) CO 2 4) SO 3
9 .The highest melting point has
1) lithium chloride 2) sodium chloride 3) potassium chloride 4) rubidium chloride
10 .Bromine is a volatile liquid with an unpleasant odor. Crystal lattice of bromine
1) atomic 2) molecular 3) ionic 4) metallic
11 .Silicon oxide is refractory, insoluble. Its crystal lattice is 1) atomic 2) molecular 3) ionic 4) metallic
12 .Crystals are made of molecules
1) sugar 2) salt 3) diamond 4) silver
13 . Oppositely charged ions consist of crystals of 1) sugar 2) sodium hydroxide 3) graphite 4) copper
14 .Refractory and non-volatile substance is
1) C 6 H 6 2) VaCO 3 3) CO 2 4) O 3
15
. Evaluate the correctness of judgments A. If there is a strong bond between the particles in the crystal, then the substance is refractory
B. All solids have a non-molecular structure
1) only A is true 2) only B is true 3) both judgments are true 4) both are wrong
16
.Assess the correctness of judgments
A. If there is a strong bond between the particles in a crystal, then the substance evaporates easily
B. All gases have a molecular structure
1) only A is true 2) only B is true 3) both judgments are correct 4) both are incorrect
A. Among the substances of the molecular structure there are gaseous, liquid and solid
under normal conditions
B . Substances with an atomic crystal lattice are solid under normal conditions
1) only A is true 2) only B is true 3) both judgments are correct 4) both are incorrect
transcript
1 Tasks A4 in chemistry 1. Chemical bond in the molecules of methane and calcium chloride, respectively, covalent polar and metallic ionic and covalent polar covalent non-polar and ionic covalent polar and ionic Covalent polar bond is formed in molecules between atoms of different non-metals, ionic between atoms of metals and non-metals. Let us determine the composition of substances according to the formulas: in methane, carbon and hydrogen, therefore, the bond is covalent polar, in calcium chloride, calcium and chlorine, which means the bond is ionic. Answer: Indicate the substance in which oxygen forms ionic bonds. ozone calcium oxide carbon dioxide water Calcium oxide is an ionic compound because an ionic bond is formed between metal and non-metal atoms. Answer: 2.
2 3. Compounds with a covalent non-polar bond are arranged in a row: A covalent non-polar bond is formed in simple substances between atoms of non-metals. 4. Hydrogen bonding is characteristic of alkanes arenes alcohols alkynes An intermolecular hydrogen bond is formed between a hydrogen atom covalently bonded to an atom with high electronegativity (F, O and N), one molecule and an atom of an element with high electronegativity (F, O, N, Cl) another molecule. For example, a hydrogen bond is formed between the hydrogen atom of one hydrogen fluoride molecule and the fluorine atom of another hydrogen fluoride molecule (indicated by a dotted line). hydrocarbons and are not capable of forming hydrogen bonds. Answer: 3.
3 5. Each of the two substances has only covalent bonds: Molecules of substances in variant 4 consist of non-metal atoms. Atoms of non-metals are connected through covalent bonds. Therefore, this is the correct answer. Answer: A non-polar covalent bond is characteristic of each of the two substances: water and diamond, hydrogen and copper chloride and nitrogen, bromine and methane. A covalent non-polar bond is formed in simple substances between non-metal atoms. In the second variant of answers, simple substances, non-metals, are given, which means that this is the correct answer. Answer: 2.
4 7. A covalent non-polar bond is characteristic of a Covalent non-polar bond is formed in simple substances between atoms of non-metals. A simple substance is non-metal iodine, so this is the correct answer. 8. A covalent non-polar bond is characteristic of each of the two substances: nitrogen and oxygen of water and ammonia, copper and nitrogen of bromine and methane. A covalent non-polar bond is formed in simple substances between atoms of non-metals. Nitrogen and oxygen are simple non-metal substances, so this is the correct answer.
5 9. Substances with a covalent polar bond are in the series: A covalent bond is a connection of atoms through common electron pairs, formed between atoms of non-metals. An ionic bond is a bond between ions, formed by the interaction of metal and non-metal atoms. In the first option, the molecules consist only of non-metal atoms, so this is the correct answer. A covalent bond can be polar or non-polar. A non-polar bond is between like atoms, a polar bond is between different ones. (More precisely, a non-polar covalent bond between atoms with the same electronegativity, a polar one between atoms with different electronegativity) 10. A substance with an ionic bond is an Ionic bond is a bond between ions, formed by the interaction of metal and non-metal atoms. The ionic compound is calcium fluoride.
6 11. A substance with a covalent non-polar bond has the formula A covalent non-polar bond is a combination of atoms through common electron pairs, formed between atoms of non-metals with the same electronegativity. The substance where a covalent non-polar bond is formed is bromine. Answer: A hydrogen bond is formed between the molecules of ethane benzene hydrogen ethanol An intermolecular hydrogen bond is formed between a hydrogen atom covalently bonded to an atom with high electronegativity (F, O and N), one molecule and an atom of an element with high electronegativity (F, O, N, Cl ) of another molecule. For example, a hydrogen bond is formed between the hydrogen atom of one hydrogen fluoride molecule and the fluorine atom of another hydrogen fluoride molecule (indicated by a dotted line) Among the proposed substances, a hydrogen bond is possible between ethanol molecules Answer: 4.
7 13. In the molecules of hydrogen chloride and bromine, the chemical bond is, respectively, covalent polar and covalent non-polar ionic and covalent polar covalent non-polar and covalent polar ionic and covalent non-polar In the molecule of hydrogen chloride, atoms of different non-metals have a covalent polar bond. Bromine is a simple substance non-metal bond covalent non-polar. 14. Both ionic and covalent bonds are involved in the formation of sodium chloride, calcium carbide, glucose silicon oxide. Sodium chloride is a compound with an ionic type of bond, silicon oxide is covalent, glucose is covalent. Only in the case of calcium carbide () are there both ionic (between the cation and anion) and covalent (between carbon atoms in the anion) bonds in the compound. Answer: 2.
8 15. A substance in which a covalent bond is formed by a donor-acceptor mechanism ammonium nitrate ethylene glycol chloride calcium carbide Ammonium ion (in this case contained in ammonium nitrate) is a typical example of a particle in which a covalent bond is formed by a donor-acceptor mechanism. 16. Which molecule has a covalent non-polar bond? H 2 O 2 H 2 O SF 2 CaF 2 In the hydrogen peroxide molecule there is a bond between oxygen atoms, which is covalent non-polar.
9 17. Which molecule has a covalent non-polar bond? C 2 H 6 CH 4 NO 2 HCl Only in the ethane molecule (C 2 H 6) there is a carbon-carbon bond, which is covalent non-polar. 18. Both substances of a pair are formed only by covalent bonds. Covalent bonds are formed between atoms of non-metals. Ionic bonds form between metals and nonmetals. Also, an ionic bond occurs between ammonium ions, ions (for example,) (and the like) and negative ones. Thus, both substances of the pair are formed only by covalent bonds. Answer: 3.
10 19. A substance with an ionic type of bond corresponds to the formula Ionic bond is a bond between ions, formed by the interaction of metal and non-metal atoms, therefore the correct answer is rubidium fluoride. Answer: Hydrogen bonds are formed between the molecules of acetic acid carbon dioxide acetylene hydrogen sulfide acid A hydrogen bond is formed between the hydrogen atom of one molecule and the atom of an element with a high electronegativity of another molecule, such elements can be: O, N, F, Cl. For a hydrogen bond, it is necessary to have polar covalent bonds in the molecule, in the formation of which a hydrogen atom and an electronegative atom (oxygen, nitrogen, halogen) participate. In the acetic acid molecule there is a group of COOH atoms where the electron density shift occurs, so the correct answer is acetic acid.
1. From the proposed list, select two compounds in which there is an ionic chemical bond. 2. A hydrogen bond is formed between the hydrogen molecules of methanol toluene methanal methanic acid
Tasks for preparation 1. From the proposed list, select two compounds in which there is an ionic chemical bond. 2. From the proposed list, select two compounds in which between molecules
Test in chemistry 2 11th grade structure of matter answers >>> Test in chemistry 2 11th grade structure of matter answers Test in chemistry 2 11th grade structure of matter answers Test
1. What type of chemical bond is in barium oxide? covalent non-polar metallic covalent polar ionic 2. What type of chemical bond is in chlorine(vii) oxide? covalent polar ionic covalent
Postponed tasks (114) The ionic nature of the bond is most pronounced in the compound 1) CCl 4 2) SiO 2 3) CaBr 2 4) NH 3 In substances formed by combining identical atoms, the chemical bond 2) covalent
3. Chemical bond An ionic chemical bond is a bond formed due to the electrostatic attraction of cations to anions. A covalent chemical bond is a bond formed between atoms by
Test "Classification of chemical bonds" 1. A covalent non-polar bond is formed between a chlorine atom and an atom of 1) potassium 2) hydrogen 3) chlorine 4) carbon 2. A covalent non-polar bond is formed between
Tasks A6 in chemistry 1. The molecular structure has 1) silicon oxide (iv) 2) barium nitrate 3) sodium chloride 4) carbon monoxide (ii) The structure of a substance is understood from what particles of molecules, ions, atoms it is built
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WORKING PROGRAM OF THE SUBJECT "CHEMISTRY", GRADE 9
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WORKING PROGRAM IN CHEMISTRY ABSTRACT CLASS: 8-9
Requirements for the level of training of graduates: The student must know: the most important chemical concepts: substance, chemical element, atom, molecule, atomic and molecular mass, ion, allotropy, isotopes,
1) covalent non-polar, ionic and covalent polar
2) ionic, covalent non-polar and covalent polar
3) covalent polar, ionic and covalent non-polar
4) ionic, covalent polar and covalent non-polar
Non-metallic properties of elements in a period with an increase in the charge of the nucleus of atoms
1) are amplified; 2) change periodically; 3) weaken; 4) do not change
The carboxyl group is present in the molecules
1) monohydric alcohols; 2) aldehydes; 3) polyhydric alcohols
4) carboxylic acids
5. The interaction of barium hydroxide with sulfuric acid is the reaction
1) connections; 2) exchange; 3) replacement; 4) hydration
The coefficient in front of the reducing agent formula in the reaction equation, the scheme of which
S + HNO 3 ® H 2 SO 4 + NO 2 + H 2 O is
1) 1 2) 2 3) 3 4) 4
7. Light bulb of the device for testing substances for electrical conductivity will not light up when the electrodes are immersed in
1) an aqueous solution of sucrose; 2) aqueous sodium chloride solution
3) formic acid (vodv. Solution); 4) sodium hydroxide melt
8. The sum of all coefficients in the full and reduced ionic equations of the reaction between nitric acid and barium hydroxide is equal to
1 ) 10 and 3 2) 12 and 3 3) 10 and 4 4) 12 and 4
Abbreviated ionic reaction equation
Zn 2+ + 2OH - = Zn(OH) 2 ¯ corresponds to the interaction of substances
1) ZnSO 4 (solution) and Fe (OH) s; 2) ZnSO 4 (solution) and Ba (OH) 2 (solution)
3) ZnCl 2 (solution) and NaOH (solution); 4) ZnO and H 2 O
10. Nitric acid does not react With
l) FeO 2) CaCO3 3) SiO 2 4) Cu
11. When alcohols are heated in the presence of concentrated sulfuric acid, you can get
1) alcoholates; 2) ethers; 3) aldehydes; 4) carboxylic acids
Not subject to hydrolysis
1) iron sulfate (III); 2) alcohols; 3) ammonium chloride; 4) esters
The formula of organic matter A in the transformation scheme
+Cl2 +NaOH
C 2 H 6 ® X ® A
1) C 2 H 5 OH; 2) C 2 H 5 Ona; 3) C 2 H 5 Cl; 4) C 2 H 6
14. A qualitative reaction to ammonium salts is
1) the action of alkali; 2) the action of another salt
3) the action of the acid; 4) decomposition of nitrates
15. The "silver mirror" reaction is characteristic of both substances
1) acetic acid and acetaldehyde; 2) formic acid and formaldehyde
3) glucose and glycerol; 4) sucrose and glycerin
16. C greatest reaction proceeds at room temperature
1) zinc with dilute sulfuric acid; 2) magnesium with hydrochloric acid
3) iron with oxygen; 4) sodium carbonate (solution) with hydrochloric acid
Chemical equilibrium in the system
2NO (g) + О 2 (g) Û 2NO 2 (g) + Q can be shifted towards the reaction product at
1) lowering the temperature; 2) temperature increase;
3) pressure drop; 4) using a catalyst
Acetylene is produced in the laboratory from
1) calcium carbide; 2) calcium carbonate; 3) carbon; 4) calcium hydroxide
In industry, acetic acid is obtained
1) catalytic oxidation of butane
2) the interaction of sodium acetate with sulfuric acid
3) hydrolysis of esters
4) hydrolysis of ethers
20. The homologue of CH3-CH 2 -CH 2 -CH \u003d CH 2 is
1) pentene-2 2) methylbutene-1 3) butene-1 4) methylbutane
Propanol-1 isomer formula
1) CH3-CH 2 -CH \u003d O
2) CH3-CH2 -O-CH3
3) CH3-CH 2 -CH 2 OH
22. The mass of alkali that must be dissolved in 50 g of water to prepare a 10% solution is
1) 5.6g 2) 6.25g 3) 10.0g 4) 12.5g
23. The amount of barium nitrate substance formed by draining solutions containing 3 mol of nitric acid and 4 mol of barium hydroxide is
1) 3 2) 7 3) 2,5 4) 4
24. In the presence of a dewatering agent, 33.6 liters (N.O.) of ethylene were obtained from 92 g of ethanol. The yield of the product as a percentage of the theoretically possible amounted to
