Saint Petersburg State Budgetary
Educational institution secondary vocational education
"PETROVSKY COLLEGE"
TEST PACKAGE
For specialties of a technical profile
Compiled by: N.I. Miftakhova
Explanatory note
In the process of studying chemistry and in the course of execution test items students should know:
the most important chemical concepts:
1.material, chemical element, atom, molecule,
2.the relative atomic and molecular weights,
3.ion, allotropy, isotopes,
4.chemical bond, electronegativity, valence, oxidation state
5.mole, molar mass, molar volume of gaseous substances,
6. substances of molecular and non-molecular structure,
7. solutions, electrolyte and non-electrolyte,
8.electrolytic dissociation,
9.oxidant and reductant, oxidation and reduction,
10.heat effect of reaction, rate of chemical reaction, catalysis, chemical equilibrium,
11. carbon skeleton, functional group, isomerism, homology;
basic laws of chemistry:
1.saving mass of substances,
2.constancy composition of substances,
3. Periodic law of DI Mendeleev;
basic theories of chemistry
1. chemical bond,
2.electrolytic dissociation,
3.structure of organic and inorganic compounds;
the most important substances and materials:
1. the most important metals and alloys;
2. sulfuric, hydrochloric, nitric and acetic acids;
3.noble gases, hydrogen, oxygen,
4.halogens, alkali metals;
5.base, acidic and amphoteric oxides and hydroxides, alkalis,
6.carbon dioxide and carbon monoxide, sulfur dioxide, ammonia, water,
7.natural gas, methane, ethane, ethylene, acetylene,
8.sodium chloride, sodium carbonate and bicarbonate, calcium carbonate and phosphate,
9.benzene, methanol and ethanol,
10.esters, fats, soaps,
11.monosaccharides (glucose), disaccharides (sucrose), polysaccharides (starch and cellulose),
12.aniline, amino acids, proteins,
13. artificial and synthetic fibers, rubbers, plastics.
Test on the topic "Types chemical reactions»
Option
1. Among the given reaction equations, indicate the reaction of the compound:
a) 2HgO → 2Hg + O₂ c) CaCO₃ → CaO + CO₂ e) CH₄ + 2O₂ → CO₂ + 2H₂
b) Fe + S → FeS d) 2H₂ + O₂ → 2H₂O₂
2. 2.Among the above reaction equations, the decomposition reaction ...
a) 2HgO → 2Hg + O₂ c) MgCO₃ → MgO + CO₂
b) 2Mg + O₂ → 2MgO d) 4Al + 3O₂ → 2Al₂O₃
3. Which of the reaction equations are examples of endothermic processes?
a) H₂ + O₂ → 2H₂O + Q c) 2H₂O → 2H₂ + O₂ - Q
b) N₂ + 2H₂ → 2NH₃ + Q d) CaCO₃ → CaO + CO₂ - Q
4. Which of the p – th equations are examples of exothermic processes?
a) Hcl + NaOH → NaCl + H₂O + Q c) 2H₂O → 2H₂ + O₂ - Q
b) N₂ + 3H₂ → NH₃ + Q d) CaCO₃ → CaO + CO₂ - Q
5. Indicate the number of the equation of the p-ii substitution.
a) 2H₂ + O → 2H₂O c) 2H₂O → 2H₂ + O₂
b) 2Na + 2H₂O → 2NaOH + H₂ d) Fe + CuCl₂ → Cu + FeCl₂
6. Indicate the equations of the exchange reaction.
a) H₂ + Cl₂ → HCl c) 2NH₃ → N₂ + 3H₂
b) CuO + H₂SO₄ → CuSO₄ + H₂O d) NaOH + HCl → NaCl + HOH
7. What reaction is attributed to decomposition reactions?
a) Fe + O₂ → c) FeCO₃ →
b) Fe + HCl → d) FeO + C →
8. The equation Na₂CO₃ + 2HC → 2NaCl + Н₂O + CO₂ refers to the reaction:
a) neutralization c) exchange
b) oxidation - reduction d) decomposition
9. An iron nail was dipped into the copper chloride solution (2).
This is the reaction:
a) exchange c) Substitutions
b) hydration d) compounds
10. Mg oxide reacts with H₂SO₄
This is the reaction:
a) exchange c) substitution
b) compounds d) neutralization
11. Select endothermic from the list of reactions.
a) 2H₂O → 2H₂ + O₂ c) SO₂ + H₂O → H₂SO₃
b) 3H₂ + N₂ → 2NH₃ d) 2Fe + 3Cl₂ → 2FeCl₃
12. An example of reactions without changing the oxidation states of elements is:
a) the effect of NaCl on AgKO₃
b) interaction of Сu with Сl₂
c) dissolution of Zn in acids
d) Decomposition of HNO₃
13. Replace letters with missing words.
Atoms, molecules or donating electrons are called (A). During the reaction they are (B). Atoms, molecules, or ions that attach electrons. Name (B). During the reactions, they (C)
14. In the equation Fe⁺² + e → Fe⁺³ show the process:
a) recovery c) dissolution
b) oxidation d) decomposition
15. In the equation of the oxidative reaction H₂S + K₂MnO₄ + H₂SO₄ → H₂O + S + MnSO₄ + K₂SO₄ the coefficients of the starting materials are respectively equal:
a) 3.2.5 c) 2.2.5
b) 5.2.3 d) 5.2.4
16. A constant electric current was passed through the diluted H₂SO₄ solution.
The reaction takes place:
a) decomposition of H₂SO₄ c) reduction of S
b) oxidation of H₂ d) decomposition of water
Types of chemical reactions
Option
1. Among the given equations of reactions of decomposition reactions:
a) 2С + О 2 → 2CO c) NH 4 Cl → NH 3 + HCl
b) Cu (OH) 2 → CuO + H 2 O d) H 2 + Cl 2 → 2HCl
2. Indicate the reactions of the compounds among the reaction equations.
a) 2Cu + O 2 → 2CuO c) 2H 2 O → 2H 2 + O 2
b) Ca CO 3 → Ca O + CO 2 d) 4Na + O 2 → 2Na 2 O
3. Which of the reaction equations are examples of exoteric processes?
a) C + O 2 → CO 2 + Q c) 2HgO → 2Hg + O 2 - Q
b) CH 4 + 2O 2 → CO 2 + 2H 2 O + Q d) 2H 2 O → 2H 2 + O 2 - Q
4. Which of the reaction equations are examples of endothermic processes?
a) H 2 + O 2 → 2H 2 O + Q c) 2H 2 O → 2H 2 O → O 2 - Q
b) N 2 + 3H 2 → 2NH 3 + Q d) CaCO 3 - CO 2 - Q
5. Indicate the equations of the reaction of substitution.
a) Zn + 2HCl → ZnCl 2 + H 2 c) 2HӀ → H 2 + Ӏ 2
b) H 2 + Cl 2 → 2HCl d) N 2 + 3H 2 → 2 NH 3
6. Equation of exchange reaction
a) 2H 2 + O 2 → 2H 2 O c) Fe 2 O 3 + 3H 2 SO 4 → Fe 2 (SO 4) 3 + 3H 2 O
b) Ca + 2HOH → Ca (OH) 2 + H 2 d) H 2 + Cl 2 → 2HCl
7. What reaction is referred to as a compound reaction?
a) NH 3 + O 2 c) NH 3 →
b) NH 4 Cl + KOH → d) NH 3 + HCl →
8. What reaction is referred to as a substitution reaction?
a) Zn + HCl → c) ZnO + H 2 SO 4 →
b) Zn + HNO 3 → d) ZnCl 2 + AgNO 3 →
9. What reaction is attributed to the exchange reaction?
a) Na 2 O + H 2 O → c) Na 2 O + CO 2 →
b) Na 2 O + H 2 SO 4 → d) Na + H 2 J →
10. Na oxide reacts with CO 2. This is the reaction:
a) exchange c) decomposition
b) compounds d) substitution
11. Exothermic reactions include the combustion of sulfur; interaction Fe with O 2, combustion of N 2; the reaction of Cl 2 with O 2; dissolving H 2 SO 4 in water; decomposition of (NH 4) 2 Cl 2 O 7. How many mistakes are there in this judgment?
a) 2; b) 1; at 4; d) 3
12. The reaction of interaction of NaCl with AqNO 3 and the oxidation reaction of CO based on the direction of the reaction are referred to:
a) irreversible c) the first is irreversible, the second is reversible
b) reversible d) the first is reversible, the second is irreversible
13. An example of a redox reaction is:
a) decomposition of Ca CO 3 c) neutralization of HNO 3
b) decomposition of HNO 3 d) interaction of Ca CO 3 with HNO 3
14. The oxidation state Mr in KMrO 4 is equal to:
a) +7; b) -7; c) +6; d) +4
15. Oxidation occurs:
a) interaction with O 2
b) movement of an electron pair
c) electron attachment
d) recoil ẽ by an atom, molecule or ion
16. Instead of letters, insert the name of the chemical elements.
In period IV (A) is the most active oxidizing agent, and (B) is the most active reducing agent. The environment of the elements of group V I of the main subgroup is the most active oxidant (C), the most weak oxidizing properties are expressed in (D).
Chemical reactions.Option 1.
a) H 2 + N 2 → NH 3
b) CO + O 2 → CO 2
c) HNO 3 → NO 2 + H 2 O + O 2
d) Ca 3 N 2 + H 2 O → Ca (OH) 2 + NH 3
e) Ba + H 2 O → Ba (OH) 2 + H 2
a) Reaction of the compound: Ag + O 2 →
b) Reaction of the compound: P + Cl 2 →
c) Substitution reaction: Cr 2 O 3 + C →
d) Exchange reaction: A l 2 O 3 + HCI →
Option 2.
1. Place the coefficients, determine the type of reaction:
a) Mg + N 2 → Mg 3 N 2
b) C + Cr 2 O 3 → CO 2 + Cr
c) HNO 3 + CaO → Ca (NO 3) 2 + H 2 O
d) Na + H 2 O → NaOH + H 2
e) Ba O + H 2 SO 4 → BaSO 4 ↓ + H 2 O
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Compound reaction: Al + O 2 →
b)) Reaction of the compound: Mg + Cl 2 →
c) Substitution reaction: MnO 2 + H 2 →
d) Exchange reaction: A l 2 O 3 + H 2 SO 4 →
Option 3.
1. Place the coefficients, determine the type of reaction:
a) P + S → P 2 S 3
b) CuO + Al → Al 2 O 3 + Cu
c) HNO 3 + CaCO 3 → Ca (NO 3) 2 + H 2 O + CO 2
d) KClO 3 → KCl + O 2
e) KOH + H 3 PO 4 → K 3 PO 4 + H 2 O
2. Add the reaction equations, arrange the coefficients, name complex substances.
2 →
b)) Reaction of the compound: Al + S →
c) Substitution reaction: Cr 2 O 3 + C →
d) Decomposition reaction (electrolysis): H 2 O →
1) Zn + H₂SO₄ \u003d ZnSO₄ + H₂
2) Ba + 2H₂O \u003d Ba (OH) ₂ + H₂
3) Na₂O + 2HCI \u003d 2NaCI + H₂O
4) 2AI (OH) ₃ \u003d AI₂O₃ + 3H₂O
Option 4.
1. Place the coefficients, determine the type of reaction:
a) P 2 O 5 + H 2 O → H 3 PO 4
b) Cl 2 + Al → AlCl 3
c) NaNO 3 → NaNO 2 + O 2
d) KBr + Cl 2 → KCl + Br 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: B + O 2 →
d) The exchange reaction A l 2 O 3 + HCl →
3. With the release of gas, a reaction proceeds between:
1) sodium carbonate and magnesium nitrate
2) phosphoric acid and barium nitrate
3) ammonium chloride and calcium hydroxide
4) potassium chloride and silver nitrate
Option 5.
1. Place the coefficients, determine the type of reaction:
a) N 2 O 5 + H 2 O → HN O 3
b) Li + Cl 2 → LiCl
c) Cu (NO 3) → CuO + O 2 + NO 2
d) KOH + AlCl 3 → KCl + Al (OH) 3 ↓
e) Mg + H 3 PO 4 → Mg 3 (PO 4) 2 + H 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
2 →
d) Decomposition reaction: HgO →
3. Gas evolution occurs as a result of the reaction of sulfuric acid with
1) potassium hydroxide
2) sodium carbonate
3) potassium oxide
4) lead nitrate
Option 6.
1. Place the coefficients, determine the type of reaction:
a) P 2 O 5 + H 2 O → H 3 PO 4
b) Cl 2 + Al → AlCl 3
c) NaNO 3 → NaNO 2 + O 2
d) KBr + Cl 2 → KCl + Br 2
e) K 2 O + H 3 PO 4 → K 3 PO 4 + H 2 O
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: B + O 2 →
b)) Reaction of the compound: Al + N 2 →
c) Substitution reaction: FeO + Al →
d) Decomposition reaction (electrolysis): A l 2 O 3 →
3. Gas evolution occurs as a result of the reaction of sulfuric acid with ... Write the equation
1) SO₃ 2) HNO₃ 3) KCI 4) HBr
Option 7.
1. Place the coefficients, determine the type of reaction:
a) K 2 O + H 2 O → KOH
b) Li + N 2 → Li 3 N
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: Ba + N 2 →
b)) Reaction of the compound: K + Cl 2 →
c) Substitution reaction: Fe 2 O 3 + Mg →
d) Decomposition reaction (electrolysis): HgO →
3.K exchange reactions the interaction between
1) sodium oxide and carbon dioxide
2) iron chloride (||) and chlorine
3) hydrochloric acid and magnesium hydroxide
4) phosphoric acid and zinc
Option 8.
1. Place the coefficients, determine the type of reaction:
a) K 2 O + P 2 O 5 → K 3 PO 4
b) Li + N 2 → Li 3 N
c) AgNO 3 → Ag + O 2 + NO 2
d) KOH + CuSO 4 → K 2 SO 4 + Cu (OH) 2 ↓
e) Mg + HCl → MgCl 2 + H 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: N 2 + O 2 →
b)) Reaction of the compound: S + Cl 2 →
c) Exchange reaction: Fe 2 O 3 + H 2 SO 4 →
d) Decomposition reaction (electrolysis): NaCl →
3. What equation corresponds to the exchange reaction
1) CuO + H₂SO₄ \u003d CuSO₄ + H₂O
2) CaO + H₂O \u003d Ca (OH) ₂
3) Zn + 2HCI \u003d ZnCI₂ + H₂
4) 2Cr (OH) ₃ \u003d Cr₂O₃ + H₂O
Option 9.
1. Place the coefficients, determine the type of reaction:
a) K 2 O + H 2 O → KOH
b) А l + S → Al 2 S 3
d) NaOH + FeSO 4 → K 2 SO 4 + Fe (OH) 2 ↓
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: Ba + Br 2 →
b)) Reaction of the compound: Fe + Cl 2 →
c) Exchange reaction: Fe 2 O 3 + HNO 3 →
d) Decomposition reaction (electrolysis) KCl →
3. Which equation corresponds to the exchange reaction
1) Zn + H₂SO₄ \u003d ZnSO₄ + H₂
2) Ba + 2H₂O \u003d Ba (OH) ₂ + H₂
3) Na₂O + 2HCI \u003d 2NaCI + H₂O
4) 2AI (OH) ₃ \u003d AI₂O₃ + 3H₂O
Option 10.
1. Place the coefficients, determine the type of reaction:
a) NO 2 + H 2 O + O 2 → HNO 3
b) A l 2 O 3 + SO 3 → Al 2 (SO 4) 3
c) Fe (OH) 3 → Fe 2 O 3 + H 2 O
d) NaOH + H 3 PO 4 → Na 3 PO 4 + H 2 O
e) ZnO + HCl → ZnCl 2 + H 2 O
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: K + Br 2 →
b)) Reaction of the compound: P + Cl 2 →
c) Exchange reaction: FeO + HNO 3 →
d) Decomposition reaction (electrolysis) LiCl →
3.With the release of gas, a reaction occurs between
1) potassium silicate and calcium hydroxide
2) calcium carbonate and hydrochloric acid
3) zinc nitrate and barium oxide
4) potassium sulfate and magnesium chloride
Option 11.
1. Place the coefficients, determine the type of reaction:
a) SO 2 + O 2 → SO 3
b) P + S → P 2 S 3
e) Zn + HCl → ZnCl 2 + H 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
2 →
3. Gas is released when the solutions interact. Write the equations.
1) potassium chloride and sulfuric acid
2) calcium carbonate and nitric acid
3) sulfuric acid and barium hydroxide
4) sodium phosphate and of hydrochloric acid
Option 12.
1. Place the coefficients, determine the type of reaction:
a) H 2 + O 2 → H 2 O
b) Сl 2 + O 2 → Cl 2 O 7
c) CuOH → Cu 2 O + H 2 O
d) Ba (OH) 2 + HPO 3 → Ba (PO 3) 2 + H 2 O
e) Fe + HCl → FeCl 2 + H 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: Н 2 + N 2 →
b)) Substitution reaction: К + НОН →
c) Exchange reaction: CuO + H 2 SO 4 →
d) Decomposition reaction (electrolysis) BaF 2 →
3. Exchange reactions include the interaction between. Write equations.
1) potassium oxide and water
2) chlorine and oxygen
3) nitric acid and barium hydroxide
4) sulfuric acid and magnesium
Option 13.
1. Place the coefficients, determine the type of reaction:
a) H 2 + N 2 → NH 3
b) C + Ca → CaC 2
c) KClO 3 → KCl + O 2
d) Mg Cl 2 + AgNO 3 → Mg (NO 3) 2 + AgCl ↓
e) Al + H 2 SO 4 → Al 2 (SO 4) 3 + H 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) The reaction of the compound: F 2 + B →
b)) Substitution reaction: Ca + HOH →
c) Exchange reaction: Ba (NO 3) 2 + Na 2 SO 4 →
d) Decomposition reaction (electrolysis) CaO →
3. The precipitate is not formed when mixing solutions
1) sodium carbonate and sulfuric acid
2) sodium sulfate and barium nitrate
3) calcium carbonate and hydrochloric acid
4) potassium sulfite and barium chloride
Option 14.
1. Place the coefficients, determine the type of reaction:
a) H 2 + F 2 → HF
b) C + Na → Na 4 C
c) KMnO 4 → K 2 MnO 4 + MnO 2 + O 2
d) Mg (OH) 2 + HNO 3 → Mg (NO 3) 2 + H 2 O
e) Al + HBr → AlBr 3 + H 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: Н 2 + Cl 2 →
b)) Substitution reaction: Ba + HOH →
c) Exchange reaction: BaCl 2 + H 2 SO 4 →
d) Decomposition reaction (electrolysis) BaO →
3. Which equation corresponds to the exchange reaction
1) Zn + H₂SO₄ \u003d ZnSO₄ + H₂
2) Ba + 2H₂O \u003d Ba (OH) ₂ + H₂
3) Na₂O + 2HCI \u003d 2NaCI + H₂O
4) 2AI (OH) ₃ \u003d AI₂O₃ + 3H₂O
Option 15.
1. Place the coefficients, determine the type of reaction:
a) SO 2 + O 2 → SO 3
b) P + S → P 2 S 3
c) Cr (OH) 3 → Cr 2 O 3 + H 2 O
d) Ba (OH) 2 + H 3 PO 4 → Ba 3 (PO 4) 2 + H 2 O
e) Zn + HCl → ZnCl 2 + H 2
2. Add the reaction equations, arrange the coefficients, name complex substances.
a) Reaction of the compound: Mg O + SiO 2 →
b)) Reaction of the compound: P + O 2 →
c) Exchange reaction: CuO + HNO 3 →
d) Decomposition reaction (electrolysis) LiF →
3. Gas is released when the solutions interact. Write the equations.
1) potassium chloride and sulfuric acid
2) calcium carbonate and nitric acid
3) sulfuric acid and barium hydroxide
4) sodium phosphate and hydrochloric acid
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Types chemical equations... (9kl)
1. Which equation corresponds to the neutralization reaction?
1) HCl + KOH \u003d KCl + H 2 O
2) H 2 + Cl 2 \u003d 2HCl
3) HCl + AgNO 3 \u003d AgCl + HNO 3
4) 2HCl + Zn \u003d ZnCl 2 + H 2
2. Reaction, the equation of which
3MgCl 2 + 2K 3 PO 4 \u003d Mg 3 (PO 4) 2 + KCl
is a reaction
1) exchange 3) connections
2) decomposition 4) substitution
3. Which equation corresponds to the exchange reaction?
1) MgO + CO 2 \u003d MgCO 3
2) FeCl 3 + 3NaOH \u003d 3NaCl + Fe (OH) 3
3) 2NaI + Br 2 \u003d 2NaCl + I 2
4) 2AgBr \u003d 2Ag + Br 2
4. Which equation corresponds to the substitution reaction?
1) MgСO 3 \u003d CO 2 + MgO
2) Na 2 CO 3 + CO 2 + H 2 O \u003d 2NaHCO 3
3) NaCl + AgNO 3 \u003d NaNO 3 + AgCl
4) 2Na + 2H 2 O \u003d 2NaOH + H 2
5. Which equation corresponds to the redox reaction?
1) СaСO 3 \u003d CO 2 + CaO
2) Zn + H 2 SO 4 \u003d ZnSO 4 + H 2
3) BaCl 2 + Na 2 SO 4 \u003d BaSO 4 + 2NaCl
4) Na 2 CO 3 + H 2 O + CO 2 \u003d 2NaHCO 3
6. Which of the equations not applicable to oxidatively - reductive reactions?
1) 2Al + 6H 2 O \u003d 2Al (OH) 3 + 3H 2
2) 2CO + O 2 \u003d 2CO 2
3) 2KOH + CO 2 \u003d K 2 CO 3 + H 2 O
4) 2H 2 S + 3O 2 \u003d 2SO 2 + 2H 2 O
7. Which equation corresponds to the decomposition reaction?
1) Fe + H 2 SO 4 \u003d FeSO 4 + H 2
2) 2HNO 3 + Fe (OH) 2 \u003d Fe (NO 3) 2 + 2H 2 O
3) 2H 2 SO 4 + C \u003d CO 2 + 2SO 2 + 2H 2 O
4) 4Fe (NO 3) 2 \u003d 2Fe 2 O 3 + 8NO 2 + O 2
8. The interaction of potassium with water refers to reactions
1) substitution 3) decomposition
2) connections 4) exchange
9. Which of the entries corresponds to the reaction equation of the compound?
1) 2CO 2 + Ca (OH) 2 \u003d Ca (HCO 3) 2
2) 2HCl + Na 2 O \u003d 2NaBr + H 2 O
3) H 2 SO 4 + Pb \u003d PbSO 4 + H 2
4) 2NO 2 + H 2 O \u003d HNO 3 + HNO 2
10. Without changing the oxidation state, the reaction proceeds, the scheme of which
1) Ca + H 2 O --- Ca (OH) 2 + H 2
2) HCl + Na 2 CO 3 ---- NaCl + H 2 O + CO 2
3) H 2 SO 4 + H 2 S --- SO 2 + H 2 O
4) HNO 3 + FeO --- Fe (NO 3) 3 + NO 2 + H 2 O
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Lesson type:generalization and systematization of knowledge and skills.
Didactic goal: to summarize and systematize the knowledge of students obtained during the study of the topic.
Tasks:
- Educational:
- to repeat and consolidate knowledge about the types of chemical reactions in terms of the number and composition of the initial and forming substances in standard and non-standard situations, the signs characterizing the course of chemical reactions, the ability to apply the law of conservation of the mass of substances.
- develop the ability to compare, classify, generalize facts and concepts.
- Developing:
- develop general educational abilities and skills (planning an answer, reasoning logically, applying your knowledge in practice).
- develop independence, will, the ability to overcome difficulties in learning, logical thinking
- Educational:
- foster collectivism, the ability to work in pairs, reflect on their own activities.
Psychological goal: creating a comfortable microclimate for each student.
Teaching methods:reproductive, explanatory and illustrative, partially exploratory.
Forms of training: frontal, individual, steam room, individualized.
Equipment and reagents: a piece of chalk in a mortar, copper wire, alcohol lamp, holder, test tubes, test tube rack, solutions: NaOH, СuСl 2, Fe, tables: "Solubility of hydroxides and salts in water", " Periodic system chemical elements of DI Mendeleev ”,“ Classification of chemical reactions in inorganic chemistry ”, tests, reference schemes, didactic cards.
Lesson plan
- Organizational moment.
- Goal setting and motivation.
- Updating.
- Systematization.
- Application teaching material in familiar and new learning situations.
- Checking the level of training.
- Homework information.
- Reflection.
- Completion of the lesson with grading and commentary.
DURING THE CLASSES
I. Organizational moment
II. Goal setting and motivation
The purpose of the lesson is set before the students in an accessible form, the significance of this topic is motivated in the further study of the chemistry course.
Teacher: So we learned how to write chemical sentences in the form of chemical equations. As in the Russian language, sentences are exclamatory, interrogative and incentive, chemical reactions are compounds, decomposition, substitution, exchange.
Today in the lesson we will once again repeat and bring knowledge into the system, about the types of chemical reactions based on the basic concepts.
What are they useful for?
For studying chemical properties substances that are characterized by chemical equations.
Solve computational problems using equations, because you have already made sure that if the equation is incorrectly drawn up, the coefficients are not correctly placed, the problem will be solved incorrectly.
III. Updating
Teacher: First, let's remember the basic concepts and conduct a chemical warm-up.
Working with the class by a frontal conversation on chemical warm-up issues (There is didactic material on each student table.
I. Chemical warm-up
1. What is a chemical phenomenon, how does it differ from a physical one?
2. What are the signs of chemical reactions known to you?
3. Give the definition of a chemical reaction.
4. What are the conditions for the course of chemical reactions?
5. What reactions relate to:
and) compound reactions,
b) decomposition reactions,
c) exchange reactions,
d) substitution reactions.
IV. Systematization
Teacher: We continue our warm-up.
II. Differentiated work by types of chemical reactions and selection of coefficients.
Teacher: Now let's check how you know how to distinguish chemical reactions from each other. In task number 2 you have written down the schemes of chemical reactions. From the proposed list, select reactions and arrange the coefficients: the first option is in compound reactions, the second is decomposition, the third is substitution, and the fourth is exchange.
Students work independently for 3 minutes. The correctness of the execution is checked through the recording on the computer. At this stage, the ability to read equations is consolidated.
Evaluation criteria: no errors - score "5"; one mistake - score "4"; two mistakes - score "3"; more than three mistakes - fail.
III. Working with chemical equations
From the list of chemical reaction schemes, select:
Option 1 - compound reactions,
Option 2 - decomposition reactions,
Option 3 - exchange reactions,
Option 4 - substitution reactions.
1. HgO ––\u003e Hg + O 2 2. Сu (OH) 2 + HCl ––\u003e H 2 O + CuCl 2
3. Al + O 2 ––\u003e Al 2 O 3 4. KBr + Cl 2 ––\u003e KCl + Br 2
5. Zn + HCl ––\u003e ZnCl 2 + H 2 6. Ca + O 2 ––\u003e CaO
7. СuCl 2 + NaOH ––\u003e Cu (OH) 2 + NaCl 8. H 2 O ––\u003e H 2 + O 2
1. What was the basis for determining the type of reaction?
2. Why do we call the above record a diagram?
3. What do we equalize in the reaction equation?
4. On the basis of what law do we place the coefficients?
5. Arrange the coefficients in the above reaction schemes.
Teacher: You all know the expression: "Theory is tested by practice."
Student experiment
Purpose: consolidate knowledge about physical and chemical phenomena.
Tasks:
- Develop the ability to compare and classify natural phenomena.
- Develop skills and abilities to reason logically, plan an answer.
№1. Grind chalk in a mortar. Explain what this phenomenon is and why you think so.
(A student at the blackboard grinds chalk in a mortar and concludes that a physical phenomenon has occurred, since no new substance was formed).
№2. Anneal the copper wire
Comment on your observations and determine the type of phenomenon.
Before the experiment, the safety rules for working with an alcohol lamp are repeated.
(The 2nd student ignites a copper wire over the flame of an alcohol lamp, observes the formation of plaque and concludes that a chemical reaction has occurred, since a new substance has formed).
Since this is a chemical phenomenon, write down the equation for the reaction of burning copper. Remember! When burning, copper exhibits the highest oxidation state. Determine the type and products of the chemical reaction. Arrange the odds.
Based on the experiments, output:Now we have seen in practice and saw how a physical phenomenon differs from a chemical one. Here we observed one of the types of chemical reaction - the reaction of the compound.
V. Application of teaching material in familiar and new learning situations
Experimental work:
Purpose: consolidate knowledge of chemical reactions.
Tasks:
- To repeat and consolidate knowledge about the types of chemical reactions in terms of the amount and composition of the starting substances and reaction products
- Develop independence, logical thinking;
- To foster collectivism, the ability to work in pairs.
1. Exchange reaction between copper (II) chloride and sodium hydroxide.
The screen shows the scheme: NaOH + CuCl 2 ––\u003e
Students are asked to determine the products of interaction between sodium hydroxide and copper (II) chloride.
Teacher:Write down according to the scheme the reaction equation of the interaction between sodium hydroxide and copper (II) chloride. (Students write down reaction equations).
–
What substances react? (Difficult)
–
What type of reaction? (Exchange)
- What products will be formed? (Copper (II) hydroxide and sodium chloride).
Find these substances in the solubility table, what can you say about them? (Copper (II) hydroxide is an insoluble base, therefore, precipitates, we put in the equation around this formula)
The predicted result is compared with the real one when performing a laboratory experiment.
- We have predicted the result of this reaction. Let's make sure by doing an experiment in practice.
Held laboratory work pupils under the guidance of a teacher.
On the basis of all this, a conclusion is made about the type of reaction performed and the sign of its course.
2. Decomposition of copper (II) hydroxide.
Teacher: Now take a test tube in which copper (II) hydroxide was obtained, fix it in a test tube holder, heat it up. Not forgetting about safety precautions:
1. First, warm up the entire tube, and then heat the solution.
2. Heating is carried out in the upper part of the flame, since it is this flame that has the highest temperature.
Students conduct an experiment “decomposition of copper (II) hydroxide”, observe the changes taking place.
- What changes do you observe? (The appearance of a black precipitate, and water drops on the walls of the test tube)
One student on the blackboard, and the rest in notebooks write down the reaction equation
Cu (OH) 2 ––\u003e CuO + H 2 O
Output: Thus, a decomposition reaction took place, since two new complex substances were formed from one complex substance.
3. Interaction of copper (II) chloride with iron
Teacher: It remains for us to consider one more type of chemical reaction. Let's lay experience. In a test tube with a steel nail, add a solution of copper (II) chloride. We will see what changes are taking place later, but for now we will write down the reaction equation.
While the reaction is going on, students write the equation in a didactic notebook.
CuCl 2 + Fe ––\u003e Fe Cl 2 + Cu, its type is determined.
Now look, have there been changes or changes in the test tube in our experience? (The steel nail is covered with a red coating - copper, and the solution has changed from blue to green).
- What conclusion can be drawn?
Pupils draw a conclusion on the basis of observations.
Students do general conclusion on the classification of chemical reactions by the number of starting and resulting substances. For those who find it difficult to draw a conclusion on their own, a reference scheme is proposed
Classification of chemical reactions according to the number and composition of the starting and forming substances
Vi. Checking the level of training
Exercise 1.Work on options I, II
Determine the type of each chemical reaction.
From the letters that indicate the correct answers, you will get:
Option I- the name of the French chemist, who formulated in 1789, independently of Lomonosov, the law of conservation of the mass of substances.
Option II - the name of the scientist, one of the founders of the atomic-molecular doctrine.
Option I.
From the letters that indicate the correct answers, you will get the name of the French chemist, who formulated in 1789 independently of Lomonosov, the law of conservation of the mass of substances.
| Chemical reaction scheme | Reaction exchange |
Reaction |
Reaction |
Reaction |
| 2Na + S ––\u003e Na 2 S | TO | L | E | TO |
| 2Al + 3H 2 SO 4 ––\u003e Al 2 (SO 4) 3 + 3H 2 | P | Sh | F | AND |
| 2H 2 O ––\u003e 2H 2 + O 2 | R | IN | IN | Z |
| Na 2 O + H 2 O ––\u003e 2NaOH | E | Have | L | AND |
| Mg (OH) 2 + 2HNO 3 ––\u003e Mg (NO 3) 2 + 2H 2 O | AND | B | ABOUT | R |
| Zn + 2HCl ––\u003e ZnCl 2 + H 2 | H | D | Have | Z |
| 2NO + O 2 ––\u003e 2NO 2 | I | B | F | FROM |
| 2NaOH + H 2 SO 4 ––\u003e Na 2 SO 4 + 2H 2 O | E | D | X | T |
Option II.
Determine the type of each chemical reaction.
From the letters that indicate the correct answers, you will get the name of the scientist, one of the founders of the atomic-molecular doctrine.
| Chemical reaction scheme | Reaction exchange |
Reaction |
Reaction |
Reaction |
| H 2 O 2 ––\u003e H 2 + O 2 | ||||
| 2KNO 3 ––\u003e 2KNO 2 + O 2 | ||||
| Zn + 2HCl ––\u003e ZnCl 2 + H 2 | ||||
| 2NaOH + ZnCl 2 ––\u003e Zn (OH) 2 + 2NaCl | ||||
| 2H 2 O + 2Na ––\u003e 2NaOH + H 2 | ||||
| 4Al + 3O 2 ––\u003e 2Al 2 O 3 | ||||
| 2Cu + O 2 ––\u003e 2CuO | ||||
| Fe 2 O 3 + 3H 2 ––\u003e 2Fe + 3H 2 O (g) | ||||
| BaCl 2 + H 2 SO 4 ––\u003e BaSO 4 + 2HCl |
Working time: 3 minutes.
Evaluation criteria: no errors - offset;
there are mistakes - fail.
Task 2.Differentiated independent work on tests, two levels.
Time: 7 minutes;
Evaluation criteria: no errors - "5"; one error - "4"; two errors - "3"; more than three mistakes - fail.
