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GDZ control and measuring materials (kim) in chemistry Grade 8 Troegubova Vako
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St. Petersburg State Budgetary
Educational institution middle vocational education
"PETROVSKY COLLEGE"
PACKAGE OF TESTS
For technical specialties
Compiled by: Miftakhova N.I.
In the process of studying chemistry and in the course of doing test items students should know:
the most important chemical concepts:
1. substance, chemical element, atom, molecule,
2. relative atomic and molecular weight,
3. ion, allotropy, isotopes,
4. chemical bond, electronegativity, valency, oxidation state
5. mol, molar mass, molar volume gaseous substances,
6. substances of molecular and non-molecular structure,
7. solutions, electrolyte and non-electrolyte,
8. electrolytic dissociation,
9. oxidizer and reducer, oxidation and reduction,
10. thermal effect of the reaction, chemical reaction rate, catalysis, chemical equilibrium,
11. carbon skeleton, functional group, isomerism, homology;
basic laws of chemistry:
1. save masses of substances,
2. permanence composition of substances,
3. Periodic Law D.I. Mendeleev;
basic theories of chemistry
1. chemical bond,
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. basic, 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 reactions 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. Specify the number of the substitution equation.
a) 2H₂ + O → 2H₂Oc) 2H₂O → 2H₂ + O₂
b) 2Na + 2H₂O → 2NaOH + H₂ d) Fe + CuCl₂ → Cu + FeCl₂
6. Specify the equations of the exchange reaction.
a) H₂ + Cl₂ → HClc) 2NH₃ → N₂ + 3H₂
b) CuO + H₂SO₄ → CuSO₄ + H₂O d) NaOH + HCl → NaCl + HOH
7. What reaction is classified as a decomposition reaction?
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 lowered into a solution of copper chloride (2).
This is the reaction:
a) exchange c) substitution
b) hydration d) compounds
10. Mg oxide reacts with H₂SO₄
This is the reaction:
a) exchange c) substitution
b) compounds d) neutralization
11. From the list of reactions, select endothermic.
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 action of NaCl on AgKO₃
b) interaction of Cu with Cl₂
c) dissolution of Zn in acids
d) Decomposition of HNO₃
13. Replace the letters with the missing words.
Atoms, molecules or donating electrons are called (A). During the reaction they are (B). Atoms, molecules or ions that accept electrons. Called (B). During reactions, they (C)
14. The equation Fe⁺² + e → Fe⁺³ shows the process:
a) recovery c) dissolution
b) oxidation d) decomposition
15. In the equation oxidative reaction H₂S + K₂MnO₄ + H₂SO₄ → H₂O + S + MnSO₄ + K₂SO₄
a) 3.2.5 c) 2.2.5
b) 5.2.3 d) 5.2.4
16. A constant electric current was passed through a dilute solution of H₂SO₄.
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 the reaction of expansions:
a) 2C + O 2 → 2CO c) NH 4 Cl → NH 3 + HCl
b) Cu (OH) 2 → CuO + H 2 O d) H 2 + Cl 2 → 2HCl
2. Among the reaction equations, indicate the reactions of the compounds.
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. Specify the equations of the substitution reaction.
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. Exchange reaction equation
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 classified 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 referred to as an 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) substitutions
11. Exothermic reactions include the combustion of sulfur; interaction Fe with O 2 , burning N 2 ; reaction of Cl 2 with O 2; dissolution of H 2 SO 4 in water; decomposition (NH 4) 2 Cl 2 O 7. How many errors are in this judgment?
a) 2; b) 1; at 4; d) 3
12. The reaction of the interaction of NaCl with AqNO 3 and the oxidation reaction of CO on the basis of the direction of the reaction are attributed 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 of Mr in KMrO 4 is:
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 has the most active oxidizing agent (C), the weakest oxidizing properties are expressed in (D).
Types chemical equations. (9kl)
1. What equation corresponds to the neutralization reaction?
1) HCl + KOH = KCl + H 2 O
2) H 2 + Cl 2 \u003d 2HCl
3) HCl + AgNO 3 = AgCl + HNO 3
4) 2HCl + Zn = ZnCl 2 + H 2
2. Reaction whose equation
3MgCl 2 + 2K 3 PO 4 = Mg 3 (PO 4) 2 + KCl
is a reaction
1) exchange 3) connections
2) decompositions 4) substitutions
3. What equation corresponds to the exchange reaction?
1) MgO + CO 2 = MgCO 3
2) FeCl 3 + 3NaOH = 3NaCl + Fe(OH) 3
3) 2NaI + Br 2 = 2NaCl + I 2
4) 2AgBr \u003d 2Ag + Br 2
4. What equation corresponds to the substitution reaction?
1) MgCO 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. What equation corresponds to the redox reaction?
1) CaCO 3 \u003d CO 2 + CaO
2) Zn + H 2 SO 4 \u003d ZnSO 4 + H 2
3) BaCl 2 + Na 2 SO 4 = BaSO 4 + 2NaCl
4) Na 2 CO 3 + H 2 O + CO 2 \u003d 2NaHCO 3
6. Which of the equations not applicable to oxidative recovery reactions?
1) 2Al + 6H 2 O \u003d 2Al (OH) 3 + 3H 2
2) 2CO + O 2 \u003d 2CO 2
3) 2KOH + CO 2 = K 2 CO 3 + H 2 O
4) 2H 2 S + 3O 2 \u003d 2SO 2 + 2H 2 O
7. What equation corresponds to the decomposition reaction?
1) Fe + H 2 SO 4 \u003d FeSO 4 + H 2
2) 2HNO 3 + Fe(OH) 2 = 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) substitutions 3) expansions
2) connections 4) exchange
9. Which of the entries corresponds to the compound reaction equation?
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 degree of oxidation, a 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
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) Combination reaction: Ag + O 2 →
b) Connection reaction: P + Cl 2 →
c) Substitution reaction: Cr 2 O 3 + C →
d) Exchange reaction: A l 2 O 3 + HCI →
Option 2.
1. Arrange 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) Combination reaction: Al + O 2 →
b)) Connection reaction: 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. Arrange 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 reaction equations, arrange coefficients, name complex substances.
2 →
b)) Combination reaction: Al +S →
c) Substitution reaction: Cr 2 O 3 + C →
d) Decomposition reaction (electrolysis): H 2 O →
1) Zn + H₂SO₄ = ZnSO₄ + H₂
2) Ba + 2H₂O = Ba(OH)₂ + H₂
3) Na₂O + 2HCI = 2NaCI + H₂O
4) 2AI(OH)₃ = AI₂O₃ + 3H₂O
Option 4.
1. Arrange the coefficients, determine the type of reaction:
a) P 2 O 5 + H 2 O → H 3 RO 4
b) Cl 2 + Al → AlCl 3
c) NaNO 3 → NaNO 2 + O 2
d) KBr + Cl 2 → KCl + Br 2
2. Add reaction equations, arrange coefficients, name complex substances.
a) Combination reaction: B + O 2 →
d) 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. Arrange 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 reaction equations, arrange 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. Arrange the coefficients, determine the type of reaction:
a) P 2 O 5 + H 2 O → H 3 RO 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 reaction equations, arrange coefficients, name complex substances.
a) Combination reaction: B + O 2 →
b)) Connection reaction: 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 an equation
1) SO₃ 2) HNO₃ 3) KCI 4) HBr
Option 7.
1. Arrange the coefficients, determine the type of reaction:
a) K 2 O + H 2 O → KOH
b) Li + N 2 → Li 3 N
2. Add reaction equations, arrange coefficients, name complex substances.
a) Combination reaction: Ba + N 2 →
b)) Connection reaction: K + Cl 2 →
c) Substitution reaction: Fe 2 O 3 + Mg →
d) Decomposition reaction (electrolysis): HgO →
3.K exchange reactions refers to 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. Arrange 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 reaction equations, arrange coefficients, name complex substances.
a) Coupling reaction: N 2 + O 2 →
b)) Connection reaction: 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 = CuSO₄ + H₂O
2) CaO + H₂O = Ca(OH)₂
3) Zn + 2HCI = ZnCI₂ + H₂
4) 2Cr(OH)₃ = Cr₂O₃ + H₂O
Option 9.
1. Arrange the coefficients, determine the type of reaction:
a) K 2 O + H 2 O → KOH
b) A l + S → Al 2 S 3
d) NaOH + FeSO 4 → K 2 SO 4 + Fe (OH) 2 ↓
2. Add reaction equations, arrange coefficients, name complex substances.
a) Combination reaction: Ba + Br 2 →
b)) Connection reaction: 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 = ZnSO₄ + H₂
2) Ba + 2H₂O = Ba(OH)₂ + H₂
3) Na₂O + 2HCI = 2NaCI + H₂O
4) 2AI(OH)₃ = AI₂O₃ + 3H₂O
Option 10.
1. Arrange 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 reaction equations, arrange coefficients, name complex substances.
a) Combination reaction: K + Br 2 →
b)) Connection reaction: P + Cl 2 →
c) Exchange reaction: FeO + HNO 3 →
d) Decomposition reaction (electrolysis) LiCl →
3. With the release of gas, a reaction proceeds 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. Arrange 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 reaction equations, arrange coefficients, name complex substances.
2 →
3. Gas is released during the interaction of solutions. Write 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. Arrange the coefficients, determine the type of reaction:
a) H 2 + O 2 → H 2 O
b) Cl 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 reaction equations, arrange coefficients, name complex substances.
a) Connection reaction: H 2 + N 2 →
b)) Substitution reaction: K + HOH →
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. Arrange 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 reaction equations, arrange coefficients, name complex substances.
a) Connection reaction: 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. Precipitation does not form 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. Arrange 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 reaction equations, arrange coefficients, name complex substances.
a) Connection reaction: H 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 = ZnSO₄ + H₂
2) Ba + 2H₂O = Ba(OH)₂ + H₂
3) Na₂O + 2HCI = 2NaCI + H₂O
4) 2AI(OH)₃ = AI₂O₃ + 3H₂O
Option 15.
1. Arrange 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 reaction equations, arrange coefficients, name complex substances.
a) Connection reaction: Mg O + SiO 2 →
b)) Connection reaction: P + O 2 →
c) Exchange reaction: CuO + HNO 3 →
d) Decomposition reaction (electrolysis) LiF →
3. Gas is released during the interaction of solutions. Write 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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Lesson type: generalization and systematization of knowledge and skills.
Didactic goal: generalize and systematize the knowledge of students obtained in the study of the topic.
Tasks:
- Educational:
- repeat and consolidate knowledge about the types of chemical reactions in terms of the quantity 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 mass of substances.
- develop the ability to compare, classify, generalize facts and concepts.
- Developing:
- develop general educational skills and abilities (planning a response, reasoning logically, applying your knowledge in practice).
- develop independence, will, ability to overcome difficulties in learning, logical thinking
- Educational:
- to cultivate collectivism, the ability to work in pairs, to reflect on one's own activities.
Psychological goal: creating a comfortable microclimate for each student.
Teaching methods: reproductive, explanatory and illustrative, partially exploratory.
Forms of study: frontal, individual, steam room, individualized.
Equipment and reagents: piece of chalk in a mortar, copper wire, spirit lamp, holder, test tubes, test tube stand, solutions: NaOH, CuCl 2 , Fe, tables: “Solubility of hydroxides and salts in water”, “ Periodic system chemical elements D. I. Mendeleeva”, “Classification of chemical reactions in inorganic chemistry”, tests, reference schemes, didactic flashcards.
Lesson Plan
- Organizational moment.
- Goal setting and motivation.
- Actualization.
- Systematization.
- Application educational material in familiar and new learning situations.
- Checking the level of training.
- Information about homework.
- Reflection.
- Completion of the lesson with grading and commenting.
DURING THE CLASSES
I. Organizing moment
II. Goal setting and motivation
The goal of the lesson is set in front of students in an accessible form, the importance of this topic is motivated in the further study of the course of chemistry.
Teacher: So we have learned to write chemical sentences in the form of chemical equations. As in Russian sentences are exclamatory, interrogative and incentive, chemical reactions are compounds, decompositions, substitutions, exchanges.
Today in the lesson we will repeat once again and bring into the system knowledge about the types of chemical reactions based on the basic concepts.
What are they good for?
For studying chemical properties substances that are characterized by chemical equations.
Solve calculation problems using equations, because you have already made sure that if the equation is written incorrectly, the coefficients are not correctly placed, the task will be solved incorrectly.
III. Update
Teacher: To begin with, let's recall the basic concepts and conduct a chemical warm-up.
Working with the class through a frontal conversation on chemical warm-up (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. Indicate the signs of chemical reactions known to you?
3. Define a chemical reaction.
4. What are the conditions for the flow of chemical reactions?
5. What reactions are related to:
a) compound reactions,
b) decomposition reactions,
c) exchange reactions,
d) substitution reactions.
IV. Systematization
Teacher: We continue our workout.
II. Differentiated work on the types of chemical reactions and the selection of coefficients.
Teacher: And now let's check how you can distinguish chemical reactions from each other. In task number 2, you have written down the schemes of chemical reactions. From the proposed list, select the reactions, and arrange the coefficients: the first option is in the compound reactions, the second is decomposition, the third is substitution, the fourth is exchange.
Students work independently for 3 minutes. The correctness of the execution is checked by 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 errors - score "3"; more than three errors - a failure.
III. Working with chemical equations
From the list of chemical reaction schemes, select:
1 option- compound reactions,
Option 2- decomposition reactions,
3 option- exchange reactions,
4 option- substitution reactions.
1. HgO ––> Hg + O 2 2. Сu(OH) 2 + HCl ––> H 2 O + CuCl 2
3. Al + O 2 ––> Al 2 O 3 4. KBr + Cl 2 ––> KCl + Br 2
5. Zn + HCl ––> ZnCl 2 + H 2 6. Ca + O 2 ––> CaO
7. СuCl 2 + NaOH -–> Cu (OH) 2 + NaCl 8. H 2 O -–> H 2 + O 2
1. On what basis was the type of reaction determined?
2. Why do we call the given entry a scheme?
3. What do we equalize in the reaction equation?
4. Based on 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
Target: consolidate knowledge of physical and chemical phenomena.
Tasks:
- Develop the ability to compare and classify natural phenomena.
- Develop skills and abilities to reason logically, plan a response.
№1. Grind chalk in a mortar. Explain what it is and why you think so.
(The student at the blackboard grinds chalk in a mortar and concludes what happened physical phenomenon, since no new substance was formed).
№2. Burn 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 burns 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 been formed).
Since this is a chemical phenomenon, write down the equation for the combustion reaction of copper. Remember! When burning, copper exhibits the highest degree of oxidation. Determine the type and products of the chemical reaction. Set the ratios.
Based on the experiments done conclusion: 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 connection.
V. Application of educational material in familiar and new learning situations
Experimental work:
Target: consolidate knowledge of chemical reactions.
Tasks:
- Repeat and consolidate knowledge about the types of chemical reactions in terms of the quantity and composition of the starting materials and reaction products;
- Develop independence, logical thinking;
- Cultivate teamwork, the ability to work in pairs.
1. Exchange reaction between copper (II) chloride and sodium hydroxide.
The scheme is written on the screen: NaOH + CuCl 2 ––>
Students are tasked with determining the products of the interaction between sodium hydroxide and copper (II) chloride.
Teacher: Write down according to the scheme the equation of the reaction of interaction between sodium hydroxide and copper (II) chloride. (Students write down the reaction equations).
–
What substances are reacting? (Complicated)
–
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, it precipitates, in the equation we put around this formula)
The predicted result is compared with the real one when performing a laboratory experiment.
- We predicted the result of this reaction. Let's make sure by experimenting in practice.
Held laboratory work students under the guidance of a teacher.
Based on all this, a conclusion is made about the type of reaction carried out and the sign of its occurrence.
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, and heat it up. Don't forget about safety:
1. First, heat the entire test tube, and then heat the solution.
2. Heating is carried out in the upper part of the flame, since it is it 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 drops of water on the walls of the test tube)
One student on the board, and the rest in notebooks write the reaction equation
Cu(OH) 2 ––> CuO + H 2 O
Conclusion: 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 put in the experience. Pour a solution of copper (II) chloride into a test tube with a steel nail. What changes occur, we will see later, but for now we will write the reaction equation.
While the reaction is proceeding, the students write the equation in a didactic notebook.
CuCl 2 + Fe ––> Fe Cl 2 + Cu, its type is determined.
And now look, have there been any changes in the test tube in the experiment laid down by us? (The steel nail is covered with a red coating - copper, and the solution has changed from blue to green).
– What conclusion can be drawn?
Students draw conclusions based on their observations.
Students do general conclusion on the classification of chemical reactions according to the number of initial and formed substances. For those who find it difficult to independently draw a conclusion, a reference scheme is offered.
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:
I option- the name of the French chemist who formulated in 1789, independently of Lomonosov, the law of conservation of mass of substances.
II option- the name of a scientist, one of the founders of the atomic and molecular theory.
I option.
From the letters that indicate the correct answers, you will get the name of a French chemist who, independently of Lomonosov, formulated in 1789 the law of conservation of mass of substances.
| Scheme of a chemical reaction | Reaction exchange |
Reaction |
Reaction |
Reaction |
| 2Na + S ––> Na 2 S | To | L | E | To |
| 2Al + 3H 2 SO 4 ––> Al 2 (SO 4) 3 + 3H 2 | P | W | F | BUT |
| 2H 2 O -–> 2H 2 + O 2 | R | AT | AT | Z |
| Na 2 O + H 2 O -–> 2NaOH | E | At | L | And |
| Mg(OH) 2 + 2HNO 3 ––> Mg(NO 3) 2 + 2H 2 O | BUT | B | O | R |
| Zn + 2HCl ––> ZnCl 2 + H 2 | H | G | At | Z |
| 2NO + O 2 ––> 2NO 2 | I | b | F | With |
| 2NaOH + H 2 SO 4 ––> Na 2 SO 4 + 2H 2 O | E | D | X | T |
II option.
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 and molecular theory.
| Scheme of a chemical reaction | Reaction exchange |
Reaction |
Reaction |
Reaction |
| H 2 O 2 ––> H 2 + O 2 | ||||
| 2KNO 3 ––> 2KNO 2 + O 2 | ||||
| Zn + 2HCl ––> ZnCl 2 + H 2 | ||||
| 2NaOH+ ZnCl 2 ––> Zn(OH) 2 + 2NaCl | ||||
| 2H 2 O + 2Na -–> 2NaOH + H 2 | ||||
| 4Al + 3O 2 ––> 2Al 2 O 3 | ||||
| 2Cu + O 2 ––> 2CuO | ||||
| Fe 2 O 3 + 3H 2 ––> 2Fe + 3H 2 O (g) | ||||
| BaCl 2 + H 2 SO 4 ––> 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 mistake - "4"; two errors - "3"; more than three errors - a failure.
