A 3. Chemical bond.
1. Chemical bond in hydrogen chloride and barium chloride respectively
1) covalent polar and ionic 2) covalent nonpolar and ionic
3) ionic and covalent polar 4) ionic and covalent nonpolar
2.
Compounds with a covalent non-polar and ionic bond 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, ОF 2, 2) NH 4 C1, PC1 3, SiС1 4 3) KF, KS1, NH 4 F 4) CH 4, K 2 C0 3, C 2 H 2
6. The polarity of the E-H 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, RN 3 2) NH 3, NF 3, NC1 3 3) SO 2, CO 2, NO 2 4) BgC1 3, BgF 3, NBr
6. Bond strength increases in series
1) NH 3, RN 3 2) H 2, Br 2 3) CS 2, CO 2 4) HBg, HI
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 a row
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 a number of
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 according to the donor-acceptor mechanism
1) NH 3 2) H 2 O 3) H 3 O + 4) H 2 O 2
A. The more energy released when a bond is formed, the stronger the bond.
B. The more polar the bond, the easier it is to break ionicly.
1) only A is true 2) only B is true 3) both judgments are true 4) both are false
A. When some bonds are broken, energy is released.
B. The pi bond is less strong than the 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 false
16.
Bond strength increases in molecules in a row
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 to atoms:
a) different numbers of electrons
b) different numbers of protons
c) different numbers of neutrons
d) no difference
21
.In the KNO compound there are 3 chemical bonds:
a) all covalent b) all ionic
c) covalent and ionic
d) metallic and covalent
22
.In which series are the formulas of substances with ionic bonds 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 nonpolar 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 nonpolar 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 is 1) barium chloride 2) potassium oxide 3) ammonium chloride 4) ammonia
4. The molecular structure has
1) CO 2 2) KBr 3) MgSO 4 4) SiO 2
5
Substances have a molecular crystal lattice
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 .Have an atomic crystal lattice
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 .Has the highest melting point
1) lithium chloride 2) sodium chloride 3) potassium chloride 4) rubidium chloride
10 .Bromine is a volatile liquid with an unpleasant odor. Bromine crystal lattice
1) atomic 2) molecular 3) ionic 4) metallic
11 .Silicon oxide is refractory and insoluble. Its crystal lattice is 1) atomic 2) molecular 3) ionic 4) metallic
12 .Crystals are made up of molecules
1) sugar 2) salt 3) diamond 4) silver
13 . Crystals of 1) sugar 2) sodium hydroxide 3) graphite 4) copper are made up of oppositely charged ions
14 .A refractory and non-volatile substance is
1) C 6 H 6 2) BaCO 3 3) CO 2 4) O 3
15
. Evaluate the correctness of judgments A. If there is a strong bond between the particles in a 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 false
16
.Evaluate the correctness of judgments
A. If there is a strong connection between the particles in the crystal, then the substance easily evaporates
B. All gases have a molecular structure
1) only A is true 2) only B is true 3) both judgments are true 4) both are false
A. Among the substances of molecular structure there are gaseous, liquid and solid
under normal conditions
B . Substances with an atomic crystal lattice are solid under ordinary conditions
1) only A is true 2) only B is true 3) both judgments are true 4) both are false
Transcript
1 Tasks A4 in chemistry 1. The chemical bond in the molecules of methane and calcium chloride, respectively, covalent polar and metallic ionic and covalent polar covalent nonpolar and ionic covalent polar and ionic A covalent polar bond is formed in molecules between atoms of different nonmetals, ionic between atoms of metals and nonmetals. Let's determine the composition of substances using the formulas: in methane there is carbon and hydrogen, therefore the bond is covalent polar, in calcium chloride there is calcium and chlorine, which means the bond is ionic. Answer: Indicate a substance in which oxygen forms ionic bonds. ozone calcium oxide carbon dioxide water Calcium oxide is an ionic compound because ionic bonds are formed between metal and non-metal atoms. Answer: 2.
2 3. Compounds with a covalent nonpolar bond are arranged in a row: A covalent nonpolar bond is formed in simple substances between nonmetal atoms. 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) of 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). Among the proposed substances, oxygen in the -OH group is present only in alcohol molecules, therefore, among the proposed substances, a hydrogen bond is possible between alcohol molecules. The remaining substances belong to hydrocarbons and are not capable of forming hydrogen bonds. Answer: 3.
3 5. Each of the two substances has only covalent bonds: The molecules of substances in version 4 consist of non-metal atoms. Nonmetal atoms are connected through covalent bonds. Therefore this is the correct answer. Answer: A non-polar covalent bond is characteristic of each of two substances: water and diamond, hydrogen and chlorine, copper and nitrogen, bromine and methane. A covalent non-polar bond is formed in simple substances between non-metal atoms. In the second answer option, simple substances are given - non-metals, which means this is the correct answer. Answer: 2.
4 7. Covalent nonpolar bonds are characteristic of Covalent nonpolar bonds are formed in simple substances between nonmetal atoms. The simple substance is the non-metal iodine, which means this is the correct answer. 8. A covalent non-polar bond is characteristic of each of two substances: nitrogen and oxygen, water and ammonia, copper and nitrogen, bromine and methane. A covalent non-polar bond is formed in simple substances between non-metal atoms. Nitrogen and oxygen are simple non-metal substances, which means 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 shared electron pairs, formed between non-metal atoms. 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. Covalent bonds can be polar or non-polar. A non-polar bond is between identical atoms, a polar bond is between different atoms. (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 nonpolar bond has the formula A covalent nonpolar bond is a connection of atoms through shared electron pairs, formed between nonmetal atoms with the same electronegativity. The substance where a covalent nonpolar bond is formed is bromine. Answer: A hydrogen bond is formed between 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) of 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). 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 nonpolar ionic and covalent polar covalent nonpolar and covalent polar ionic and covalent nonpolar In the molecule of hydrogen chloride, atoms of different nonmetals have a covalent polar bond. Bromine is a simple non-metal substance, a covalent non-polar bond. 14. Both ionic and covalent bonds are involved in the formation of sodium chloride calcium carbide silicon oxide glucose 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 the anion) and covalent (between the 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 vinyl chloride ethylene glycol 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 contains a covalent nonpolar 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 contains a covalent nonpolar 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 the pair are formed only by covalent bonds. Covalent bonds are formed between non-metal atoms. Ionic bonds form between metals and non-metals. Also, an ionic bond occurs between ammonium ions, ions (for example) (and the like) and negative ones. Thus, only covalent bonds are formed by both substances of the pair Answer: 3.
10 19. A substance with an ionic type of bond is answered by 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 molecules of acetic acid, carbon dioxide, acetylene, hydrogen sulfide. A hydrogen bond is formed between the hydrogen atom of one molecule and the atom of an element with 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, the formation of which involves a hydrogen atom and an electronegative atom (oxygen, nitrogen, halogen). In the acetic acid molecule there is a group of COOH atoms where the electron density shifts, so the correct answer is acetic acid.
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1) covalent non-polar, ionic and covalent polar
2) ionic, covalent nonpolar and covalent polar
3) covalent polar, ionic and covalent nonpolar
4) ionic, covalent polar and covalent nonpolar
Nonmetallic properties of elements in the period with increasing nuclear charge of atoms
1) intensify; 2) change periodically; 3) weaken; 4) do not change
Carboxyl group is present in molecules
1) monohydric alcohols; 2) aldehydes; 3) polyhydric alcohols
4) carboxylic acids
5. The interaction of barium hydroxide with sulfuric acid is a reaction
1) accession; 2) exchange; 3) substitution; 4) hydration
The coefficient in front of the reducing agent formula in the reaction equation, the diagram of which
S + HNO 3 ® H 2 SO 4 + NO 2 + H 2 O, equal to
1) 1 2) 2 3) 3 4) 4
7.Lamp of a device for testing substances for electrical conductivity won't light up when immersing electrodes in
1) aqueous solution of sucrose; 2) aqueous solution of sodium chloride
3) formic acid (aqueous solution); 4) molten sodium hydroxide
8. The sum of all coefficients in the full and abbreviated ionic equations for 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)3; 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 heating alcohols in the presence of concentrated sulfuric acid, you can get
1) alcoholates; 2) ethers; 3) aldehydes; 4) carboxylic acids
Do not undergo hydrolysis
1) iron (III) sulfate; 2) alcohols; 3) ammonium chloride; 4) esters
Formula of organic substance A in the transformation scheme
+Cl 2 +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. The qualitative reaction to ammonium salts is
1) the effect of alkali; 2) the effect of another salt
3) the action of 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 glycerol
16. C greatest reaction occurs 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) + O 2 (g) Û 2NO 2 (g) + Q can be shifted towards the reaction product when
1) decrease in temperature; 2) increase in temperature;
3) decrease in pressure; 4) using a catalyst
Acetylene is obtained in the laboratory from
1) calcium carbide; 2) calcium carbonate; 3) carbon; 4) calcium hydroxide
In industry, acetic acid is produced
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 = CH 2 is
1) pentene-2 2) methylbutene-1 3) butene-1 4) methylbutane
Propanol-1 isomer formula
1) CH3-CH 2 -CH = O
2) СНз-СН 2 -О-СНз
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 equal to
1) 5.6g 2) 6.25g 3) 10.0g 4) 12.5g
23. The amount of barium nitrate formed by pouring solutions containing 3 moles of nitric acid and 4 moles of barium hydroxide is equal to
1) 3 2) 7 3) 2,5 4) 4
24. In the presence of a dewatering agent, 33.6 liters (no.) of ethylene were obtained from 92 g of ethanol. The product yield as a percentage of the theoretically possible was
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). For each task there are 4 possible answers, of which only one is correct. Read each task carefully and analyze all the options for the proposed answers.
- Part 2 consists of 10 tasks (B1-B10), to which you must give a short answer in the form of a number or a sequence of numbers.
- Part 3 contains 5 of the most difficult tasks in general, inorganic and organic chemistry. Tasks C1-C5 require a complete (detailed) answer.
All Unified State Exam forms are filled out in bright black ink. You can use gel, capillary or fountain pens. When completing assignments, you can use a draft. Please note that entries in the draft will not be taken into account when assessing the work.
We advise you to complete the tasks in the order in which they are given. To save time, skip a task that you cannot complete immediately and move on to the next one. If you have time left after completing all the work, 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 given during the exam.
The points you receive 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 answer form No. 1, under the number of the task you are performing (A1-A28), put the “×” sign in the box whose number corresponds to the number of the answer you have chosen.
A1 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 a row of elements Na → Mg → Al → Si
1) atomic radii decrease
2) the number of protons in the nuclei of atoms decreases
3) the number of electronic 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 correct
2) only B is correct
3) both judgments are correct
4) both judgments are incorrect
A4 Chemical bond in methane and calcium chloride molecules, respectively
1) covalent polar and metallic
2) ionic and covalent polar
3) covalent nonpolar 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
D) Na 2 HPO 4
E) Na 3 PO 4
acid salts are
1) AGD
2) ABE
3) BDE
4) BDE
A8 Zinc interacts with solution
1) CuSO 4
2) MgCl 2
3) Na 2 SO 4
4) CaCl2
A9 Which oxide reacts with a solution of HCl, but does not react with a solution of NaOH?
1) CO
2) SO 3
3) P 2 O 5
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 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 transformation scheme
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 OCH 3
A17 Butanol-1 is formed as a result of interaction
1) butanal with water
2) butene-1 with aqueous alkali solution
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 is a reaction
1) connections, irreversible
2) exchange, reversible
3) connections, reversible
4) exchange, irreversible
A20 The rate of reaction of nitrogen with hydrogen will decrease when
1) decreasing temperature
2) increasing nitrogen concentration
3) using a catalyst
4) increasing pressure
A21 Chemical equilibrium in the system
will shift towards the reaction products when
1) increasing pressure
2) increasing temperature
3) decrease in pressure
4) using a catalyst
A22 The largest amount of sulfate ions is formed in solution during dissociation of 1 mol
1) sodium sulfate
2) copper(II) sulfate
3) aluminum sulfate
4) calcium sulfate
A23 Abbreviated ionic equation H + + OH - = 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 a 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 judgments about the rules for handling substances correct?
A. It is prohibited to taste substances in the laboratory.
B. Mercury salts should be handled with extreme caution due to their toxicity.
1) only A is correct
2) only B is correct
3) both judgments are correct
4) both judgments are incorrect
A27 Polymer having the formula
get from
1) toluene
2) phenol
3) propylbenzene
4) styrene
A28 According to the thermochemical reaction equation
CaO (tv) + H 2 O (l) = Ca(OH) 2 (tv) + 70 kJ
to obtain 15 kJ of heat you will need calcium oxide weighing
1) 3 g
2) 6 g
3) 12 g
4) 56 g
Part 2
The answer to the tasks in this part (B1-B10) is a sequence of numbers or a number that should be written down in answer form No. 1 to the right of the number of the corresponding task, starting from the first cell. Write each digit and comma in the decimal fraction 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 answer form No. 1 without spaces, commas and other additional symbols. (The numbers in the answer may be repeated.)
B1 Establish a correspondence between the name of the compound and 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 numbers that correspond to the numbers of the correct answers. Write down these numbers in ascending order first in the text of the work, and then transfer them to answer form No. 1 without spaces, commas and other additional characters.
B6 Reaction of 2-methylpropane and bromine at room temperature in the light
1) refers to substitution reactions
2) proceeds through a radical mechanism
3) leads to the preferential formation of 1-bromo-2-methylpropane
4) leads to the preferential formation of 2-bromo-2-methylpropane
5) proceeds with the rupture of 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 can 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 answer form No. 1 without indicating the units of measurement.
Q9 Determine the mass of water that must be added to 20 g of acetic acid solution with a mass fraction of 70% to obtain a solution of acetic acid with a mass fraction of 5%. (Write the number to the nearest whole number.)
Answer: ___________ g.
Q10 The mass of oxygen required for the complete combustion of 67.2 liters (n.s.) of hydrogen sulfide to SO 2 is equal to __________ g. (Write the number to the nearest whole number.)
Do not forget to transfer all answers to answer form No. 1.
Part 3
To record answers to the tasks of this part (C1-C5), use answer form No. 2. First write down the task number (C1, C2, etc.), and then its complete solution. Write down your answers clearly and legibly.
C1 Using the electronic balance method, create a reaction equation
C2 The salt obtained by dissolving iron in hot concentrated sulfuric acid was treated with an excess of sodium hydroxide solution. The brown precipitate that formed was filtered and calcined. The resulting substance was fused with iron.
C3 Write 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. To neutralize the resulting solution, 143 g of crystalline soda Na 2 CO 3 ⋅10H 2 O was required. Calculate the mass and mass fraction of sodium hydroxide in the original solution.
C5 When 25.5 g of saturated monobasic carboxylic acid reacted with an excess of sodium bicarbonate solution, 5.6 l (n.s.) of gas was released. Determine the molecular formula of the acid.
Evaluation system for examination work in chemistry
PART 1
For the correct answer to each task in Part 1, 1 point is given. If two or more answers are indicated (including the correct one), an incorrect answer or no answer - 0 points.
| Job No. | Answer | Job No. | Answer | Job No. | 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 completed correctly if the sequence of numbers (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 error) 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 No. | Answer |
PART 3
CRITERIA FOR CHECKING AND EVALUATING COMPLETION OF TASKS WITH DETAILED ANSWER
For completing tasks the following is given: 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, create an equation for the reaction
Na 2 SO 3 + … + KOH → K 2 MnO 4 + … + H 2 O
Identify the oxidizing agent and the reducing agent.
Points |
|
Response elements: 2) it is indicated that sulfur in the oxidation state +4 is a reducing agent, and manganese in the oxidation state +7 (or potassium permanganate due to manganese in the oxidation state +7) is an oxidizing agent; | |
There was an error in only one of the elements in the answer. | |
There were errors in two elements in the answer | |
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 that formed was filtered and calcined. The resulting substance was fused with iron.
Write the equations for the reactions described.
Points |
|
Response elements:
| |
4 reaction equations written correctly | |
3 reaction equations written correctly | |
2 reaction equations written correctly | |
| 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 elements mentioned above | 5 |
| 4 reaction equations written correctly | 4 |
| 3 reaction equations written correctly | 3 |
| 2 reaction equations written correctly | 2 |
| One reaction equation written correctly | 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. To neutralize the resulting solution, 143 g of crystalline soda Na 2 CO 3 ⋅10H 2 O was required. Calculate the mass and mass fraction of sodium hydroxide in the original solution.
Points |
|
Response elements: Calculation is also possible based on the reaction equations for the formation of NaHSO 4 and its subsequent interaction with Na 2 CO 3. The final answer won't change; 2) the total amount of sulfuric acid is 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 original solution were calculated: n(H 2 SO 4) = 2 − 0.5 = 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 elements mentioned above | 4 |
| There was an error in one of the above elements in the answer. | 3 |
| The answer 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.s.) of gas was released. Determine the molecular formula of the acid.
| Points | |
Elements of the response. C 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 has been established: Molecular Formula - C 4 H 9 COOH | |
| The answer is correct and complete, includes all the elements mentioned above | 3 |
| The first and second elements of the answer are written correctly | 2 |
| The first or second elements of the answer are written correctly | 1 |
| All elements of the answer are written incorrectly | 0 |
| Maximum score | 3 |
*Note. If the answer contains an error in calculations in one of the elements (second, third or fourth), which led to an incorrect answer, the score for completing the task is reduced by only 1 point.
