(1) the reaction of simple substance with oxygen;

1. Magnesium burns in oxygen: 2Mg+O2 ignites 2MgO.

2. Iron burns in oxygen: 3Fe+2O2 ignites Fe3O4.

3. Copper heating in oxygen: 2Cu+O2 heating 2CuO.

4. Aluminum burns in air: 4Al+3O2 ignites 2Al2O3.

5. Hydrogen burns in oxygen: 2H2+O2 ignites 2H2O.

6. Red phosphorus burns in air: 4P+5O2 ignites 2P2O5.

7. Sulfur powder burns in oxygen: S+O2 ignites SO2.

8. Complete combustion of carbon in oxygen: C+O2 ignites CO2.

9. Incomplete combustion of carbon in oxygen: 2C+O2 ignites 2CO.

10. Mercury burns in oxygen: 2Hg+O2 ignites 2HgO.

(2) the reaction of compounds with oxygen:

1 1. Carbon monoxide burns in oxygen: 2CO+O2 ignites 2CO2.

12. Methane burns in air: CH4+2O2 ignites CO2+2H2O.

13. Combustion of alcohol in air: C2H5OH+3O2 == Ignition == 2CO2+3H2O.

14. Combustion of acetylene in oxygen: 2C2H2+5O2 ignites 4CO2+2H2O (oxyacetylene flame).

2. Decomposition reaction:

15. Hydrogen peroxide catalyzed oxygen production: 2H2O2(MnO2 catalyzed) 2H2O+O2 =

16. Decomposition of water under direct current: 2H2O charged 2H2 =+O2 =

17. heating basic copper carbonate: Cu2(OH)2CO3 heating 2cuo+H2O+CO2 =

18. heating potassium chlorate (containing a small amount of manganese dioxide): 2kClO3 = 2kCl+3o2 =

19. heating potassium permanganate: 2KMnO4 heating k2mno4+MnO2+O2 =

20. Carbonic acid is unstable and decomposed: H2CO3 = H2O+CO2↑ =

2 1. high temperature calcined limestone: CaCO3, high temperature CaO+CO2↑ =

Three. Redox reaction:

22. Reduction of copper oxide by hydrogen: H2+ copper oxide heats copper +H2O.

23. Reduction of copper oxide with charcoal: 2Cu, high temperature 2Cu+CO2↑ =

24. Reduction of iron oxide by coke: 3C+ 2Fe2O3, high temperature 4Fe+3CO2↑ =

25. Reducing Fe3O4 with coke at high temperature: 2c+Fe3O4, 3Fe+2 CO2 =

26. Reduction of copper oxide by carbon monoxide: CO+ CuO heats Cu+CO2.

27. Reduction of iron oxide by carbon monoxide: 3CO+ Fe2O3, high temperature, 2Fe+3CO2.

28. Reduction of ferroferric oxide with carbon monoxide: 4CO+ Fe3O4, high temperature 3Fe+4CO2.

4. Relationship among simple substance, oxide, acid, alkali and salt

(1) elemental metal+acid salt+hydrogen (displacement reaction)

29. Zinc and dilute sulfuric acid Zn+H2SO4 = ZnSO4+H2 Write

30. Iron and dilute sulfuric acid Fe+H2SO4 = FeSO4+H2 Write

3 1. magnesium and dilute sulfuric acid mg+H2SO4 = mgso4+H2 =

32. Aluminum and dilute sulfuric acid 2Al +3H2SO4 = Al2(SO4)3 +3H2↑ 3+3H2+3H2 write 3+3H2

33. Zinc and dilute hydrochloric acid Zn+2HCl = = ZnCl2+H2 Write

34. Iron and dilute hydrochloric acid Fe+2HCl = = FeCl2+H2 Write

35. Magnesium and dilute hydrochloric acid Mg Mg+ 2HCl === MgCl2+H2↑ =

36. Aluminum and dilute hydrochloric acid 2Al+6HCl = = 2AlCl3+3H2 Write

(2) Simple metal+salt (solution)-another salt+another metal (displacement reaction)

37. The reaction between iron and copper sulfate solution: Fe+CuSO4 = FeSO4+Cu.

38. The reaction between zinc and copper sulfate solution: Zn+CuSO4 = ZnSO4+Cu.

39. The reaction between copper and mercury nitrate solution: Cu+Hg(NO3)2 = Cu(NO3)2+Hg.

(3) Alkaline oxide+acid salt+water

40. Reaction of iron oxide with dilute hydrochloric acid: Fe2O3+6HCl = 2FeCl3+3H2O.

4 1. Reaction of iron oxide with dilute sulfuric acid: Fe2O3+3H2SO4 =Fe2(SO4)3+3H2O.

42. The reaction between copper oxide and dilute hydrochloric acid: CuO+2HCl = CuCl2+H2O.

43. The reaction between copper oxide and dilute sulfuric acid: CuO+H2SO4 = CuSO4+H2O.

44. The reaction of magnesium oxide with dilute sulfuric acid: MgO+H2SO4 = magnesium sulfate +H2O.

45. The reaction of calcium oxide with dilute hydrochloric acid: CaO+2HCl = CaCl2+H2O.

(4) acidic oxide+alkaline salt+water

46. Sodium hydroxide will deteriorate when exposed to air: 2NaOH+CO2 = Na2CO3+H2O.

47. Sodium hydroxide absorbs sulfur dioxide gas: 2 NaOH+SO2 = Na2SO4+H2O.

48. Sodium hydroxide absorbs sulfur trioxide gas: 2NaOH+SO3 = Na2SO4+H2O.

49. The slaked lime deteriorates in air: Ca(OH)2+CO2 = CaCO3 ↓+ H2O.

50. The slaked lime absorbs sulfur dioxide: Ca(OH)2+SO2 = CaSO3 ↓+ H2O.

(5) acid+alkali-salt+water

5 1. Reaction of hydrochloric acid and sodium hydroxide: HCl+NaOH = = = NaCl+H2O.

52. Reaction of hydrochloric acid and potassium hydroxide: HCl+KOH = = = KCl+H2O.

53. The reaction between hydrochloric acid and copper hydroxide: 2HCl+Cu (OH) 2 = = CuCl2+2H2O.

54. The reaction between hydrochloric acid and calcium hydroxide: 2HCl+Ca (OH) 2 = = CaCl2+2H2O.

55. The reaction between hydrochloric acid and iron hydroxide: 3HCl+Fe (OH) 3 = = = FeCl 3+3H2O.

56. Aluminum hydroxide for the treatment of hyperacidity: 3HCl+Al (OH) 3 = = = AlCl3+3H2O.

57. The reaction between sulfuric acid and sodium hydroxide: H2SO4+2NaOH = = = Na2SO4+2H2O.

58. The reaction between sulfuric acid and potassium hydroxide: H2SO4+2koh = = = K2SO4+2h2o.

59. The reaction between sulfuric acid and copper hydroxide: H2SO4+Cu (OH) 2 = = CuSO4+2H2O.

60. The reaction between sulfuric acid and iron hydroxide: 3H2SO4+2Fe (OH) 3 = = Fe2 (SO4) 3+6H2O.

6 1. The reaction between nitric acid and sodium hydroxide: nitric acid+sodium hydroxide = = = sodium nitrite+H2O H2O.

(6) acid+salt-another acid+another salt

62. Calcium carbonate reacts with dilute hydrochloric acid: CaCO3+2hcl = = CaCl2+H2O+CO2 =

63. Sodium carbonate reacts with dilute hydrochloric acid: Na2CO3+2HCl = = 2NaCl+H2O+CO2 =

64. Magnesium carbonate reacts with dilute hydrochloric acid: MgCO3+2HCl = = MgCl2+H2O+CO2 =

65. Reaction between hydrochloric acid and silver nitrate solution: HCl+AgNO3 === AgCl↓+HNO3.

66. The reaction of sulfuric acid and sodium carbonate: Na2CO3+H2SO4 = = Na2SO4+H2O+CO2 =

67. The reaction between sulfuric acid and barium chloride solution: H2SO4+bacl2 = = = baso4 ↓+2hcl.

(7) alkali+salt-another alkali+another salt

68. Sodium hydroxide and copper sulfate: 2 NaOH+CuSO4 = = Cu (OH) 2 ↓+Na2SO4.

69. Sodium hydroxide and ferric chloride: 3 NaOH+FeCl 3 = = Fe (OH) 3 ↓+3 NaCl.

70. Sodium hydroxide and magnesium chloride: 2 NaOH+MgCl2 = = mg (OH) 2 ↓+2 NaCl.

7 1. Sodium hydroxide and copper chloride: 2 NaOH+CuCl2 = = Cu (OH) 2 ↓+2 NaCl.

72. Calcium hydroxide and sodium carbonate: Ca (OH) 2+Na2CO3 = = CaCO3 ↓+2NaOH.

(8) salt+salt-two new salts

73. Sodium chloride solution and silver nitrate solution: NaCl+AgNO3 = = = AgCl ↓+Nano3.

74. Sodium sulfate and barium chloride: Na2SO4+bacl2 = = = baso4 ↓+2 NaCl.

Verb (short for verb) Other reactions:

75. Carbon dioxide is soluble in water: CO2+H2O === H2CO3.

76. Quicklime is soluble in water: CaO+H2O === Ca(OH)2.

77. Sodium oxide is soluble in water: Na2O+H2O = = = 2 NaOH.

78. Sulfur trioxide is soluble in water: SO3+H2O = = = H2SO4.

79. Copper sulfate crystal is decomposed by heat: CuSO4? Heating CuSO4+5H2O

80. Anhydrous copper sulfate as desiccant: CuSO4+5H2O = = = CuSO4? 5H2O

Summary of junior high school chemistry equation and its related knowledge points

1. Introduce carbon dioxide gas into clarified limewater (double decomposition reaction)

Calcium hydroxide+carbon dioxide = calcium carbonate ↓+H2O

Phenomenon: Lime water changes from clear to turbid.

Related knowledge: This reaction can be used to test the presence of carbon dioxide gas.

It is best not to use it for inspection. CaCO3+CO2+H2O=Ca(HCO3)2 precipitates disappear, and Ba(OH)2 solution can be used.

2. Magnesium belt burns in air (chemical reaction)

2 mg+oxygen = 2 mg oxygen

Phenomenon: magnesium burns violently in the air, releasing heat, giving off dazzling white light and generating white powder.

Related knowledge points: (1) In this reaction, magnesium changes from free state to bound state; (2) The color of the substance changes from silvery white to white. (3) Magnesium can be used as a flare; (4) The ignition point of magnesium bars is high, and the matches generate less heat, which can not reach the ignition point of magnesium and cannot be ignited with matches; (5) Magnesium is very active. In order to protect magnesium, a black protective film is coated on the surface of magnesium, and it should be polished with sandpaper before ignition.

3. Water is electrically decomposed (decomposition reaction)

2H2O =2H2↑ + O2↑

Phenomenon: After electrifying, bubbles appear on the electrode, and the gas volume ratio is about 1: 2.

Related knowledge points: (1) The anode produces oxygen and the cathode produces hydrogen; (2) The volume ratio of hydrogen and oxygen is 2: 1, and the mass ratio is1:8; (3) When electrolyzing water, a small amount of sodium hydroxide solution or dilute sulfuric acid is added in advance to enhance the conductivity of water; (4) the power supply is DC.

4. Reaction of quicklime with water (combination reaction)

Calcium oxide+H2O = calcium hydroxide

Phenomenon: White powder dissolves.

Related knowledge points: (1) The final solution name is calcium hydroxide solution, commonly known as clarified limewater; (2) Dropping colorless phenolphthalein will turn red; (3) Quicklime is calcium oxide, and hydrated lime is calcium hydroxide. (4) emitting a lot of heat

5. Making oxygen in the laboratory

(1) heating the mixture of potassium chlorate and manganese dioxide to produce oxygen (decomposition reaction)

2KClO3 =MnO2 (as catalyst) = 2kcl+3o2 =

Related knowledge points: (1) Manganese dioxide is used as a catalyst to accelerate the decomposition of potassium chlorate or the generation of oxygen; (2) The quality and chemical properties of manganese dioxide have not changed before and after the chemical reaction; (3) After the reaction is completed, the residual solid in the test tube is a mixture of potassium chloride and manganese dioxide, and the separation methods are: cleaning, drying and weighing.

② heating potassium permanganate to produce oxygen (decomposition reaction)

2k MnO 4 = k2mno 4+MnO 2+O2←

Related knowledge points: fortress cotton at the test tube mouth to prevent potassium permanganate powder from slipping and blocking the catheter.

(3) Hydrogen peroxide and manganese dioxide produce oxygen (decomposition reaction)

2H2O2=MnO2 (as catalyst) = 2h2o+O2 =

* * * Same knowledge point: (1) When collecting by upward exhaust method, the catheter should extend below the gas container and be placed directly above the table after collection; (2) At the end of the experiment, the catheter should be removed first, and the alcohol lamp should be removed, so as to avoid the backflow of water in the sink and the rupture of the test tube; (3) When heating, the test tube should be slightly inclined downward to avoid the backflow of condensed water and rupture the test tube; (4) collecting oxygen by a drainage gas collection method until bubbles are continuously and uniformly emitted; (5) Fill the bottle with a small piece of wood with sparks and put it in the bottle to check whether it is oxygen.

6. Charcoal burns in the air (chemical reaction)

Complete combustion: C+O2= CO2

Incomplete combustion: 2C+O2= 2CO

Phenomenon: there is red light in the air; Oxygen gives off white light, gives off heat, and produces colorless gas, which makes clear limewater turbid.

Related knowledge points: The products after the reaction can be tested with clear limewater.

7. Sulfur burns in air (or oxygen) (combination reaction)

Sulfur+oxygen = sulfur dioxide

Phenomenon: a faint light blue flame is emitted in the air, and a bright blue-purple flame is emitted in oxygen, resulting in colorless irritating gas.

Related knowledge points: (1) The daubed product can be tested by purple litmus (purple turns red); (2) Put a small amount of water or alkaline solution (NaOH) at the bottom of the gas container in advance to absorb the generated sulfur dioxide to prevent air pollution.

8. Iron wire burns in oxygen (combination reaction)

3Fe + 2O2 =Fe3O4

Phenomenon: the iron wire burns violently in oxygen, sparks radiate, releases heat, and produces black solids.

Related knowledge points: (1) The spiral coil is to increase the contact area with oxygen; (2) Hanging a lighted match under the wire is to ignite the wire; (3) When the match is about to burn out and extend into the container, it is too early, the match consumes oxygen, and the iron wire cannot burn completely; Too late to ignite; (4) Put a small amount of fine sand at the bottom of the gas container in advance to prevent scalding products from splashing and cracking the bottom of the bottle.

9. Red phosphorus burns in oxygen (combination reaction)

4P + 5O2=2P2O5

Phenomenon: produce a lot of white smoke and emit heat.

Related knowledge points: Red phosphorus can be used to determine the oxygen content in the air.

10. Hydrogen burns in air (combination reaction)

2H2 + O2 =2H2O

Phenomenon: produce light blue flame, release heat and produce water droplets.

Related knowledge points: (1) Hydrogen is a common reducing agent; (2) Before ignition, be sure to check its purity.

1 1. Reduction of copper oxide with charcoal (displacement reaction)

C + 2CuO =2Cu + CO2

Phenomenon: Black powder gradually turns into bright red substance, releasing heat.

Related knowledge points: (1) put charcoal powder and copper oxide in the test tube to make the heating area large and the reaction fast; (2) introducing a conduit into clarified limewater, and checking whether CO2 has been generated; (3) add a net cover on the alcohol lamp to concentrate the flame and raise the temperature; (4) First, withdraw the airway to prevent the lime water from flowing back and the test tube from breaking; (5) after the test tube is cooled, the powder is poured out to prevent the hot copper-oxygen reaction from generating CuO；; (6)C is the reducing agent and CuO is the oxidizing agent.

12. reduction of copper oxide by hydrogen (displacement reaction)

H2+CuO= copper+H2O

Phenomenon: the black powder gradually turns into a bright red substance, and water drops are produced at the mouth of the test tube.

Related knowledge points: (1) At the beginning of the experiment, hydrogen should be introduced for a period of time to drive out the air in the test tube; (2) After the experiment, the alcohol lamp should be removed first, and then the hydrogen conduit should be removed to prevent the newly generated copper from combining with oxygen in the air to generate copper oxide.

13. Laboratory preparation of carbon dioxide gas (metathesis reaction)

Marble (limestone) reacts with dilute hydrochloric acid.

Calcium carbonate+hydrochloric acid = calcium chloride+H2O+carbon dioxide

Phenomenon: white solid dissolves, producing a large number of bubbles.

Related knowledge: (1) Calcium carbonate is a white insoluble solid. Using its solubility in hydrochloric acid, calcium carbonate mixed in substances can be removed by hydrochloric acid; (2) concentrated hydrochloric acid cannot be used, because concentrated hydrochloric acid is volatile, releasing HCl gas mixed with CO2. Impurities of CO2; (3) Dilute sulfuric acid cannot be used, because calcium carbonate and sulfuric acid reflect that CaSO4 is slightly soluble in water and covers the solid surface, which stops the reaction; (4) Calcium carbonate powder cannot be used because the contact area of reactants is large and the reaction speed is too fast.

14. industrial preparation of carbon dioxide gas (decomposition reaction)

Calcined limestone at high temperature

CaCO3= CaO + CO2↑

Related knowledge points: CaO is commonly known as quicklime.

15. Carbon monoxide burns in air (combination reaction)

2CO + O2 =2CO2

Phenomenon: blue flame is produced.

Related knowledge points: (1) Carbon monoxide is a common reducing agent; (2) Before ignition, be sure to check its purity.

16. reduction of copper oxide with carbon monoxide

CO + CuO= Cu + CO2

Phenomenon: the black powder gradually turns into bright red powder, and the gas produced makes the lime water turbid.

Related knowledge points: carbon monoxide is a reducing agent and copper oxide is an oxidizing agent.

17. Methane burns in air.

CH4 + 2O2 =CO2 + 2H2O

Phenomenon: The flame is bright and light blue.

Related knowledge points: methane is the main component of natural gas (or biogas) and a good fuel.

18. industrial production of hydrochloric acid (combination reaction)

H2+Cl2= 2HCl

Related knowledge: This reaction shows that oxygen is not necessary for combustion under special conditions.

19. Hydrogen production in laboratory (displacement reaction)

Zinc+sulfuric acid = zinc sulfate +H2

Related knowledge points: (1) Hydrogen is a common reducing agent; (2) Before ignition, be sure to check its purity.

20. Charcoal and carbon dioxide produce carbon monoxide (combined reaction).

Carbon+carbon dioxide = carbon dioxide

Related knowledge points: (1) Carbon monoxide is a common reducing agent; (2) Before ignition, be sure to check its purity.

2 1. Water and carbon dioxide produce carbonic acid (combination reaction)

CO2 + H2O= H2CO3

Phenomenon: Carbonic acid forms, which can turn purple litmus solution red.

22. Unstable decomposition of carbonic acid (decomposition reaction)

H2CO3 =H2O + CO2↑

Related knowledge points: (1) Carbonic acid is an unstable acid, which is easily decomposed when heated; (2) In the process of decomposition, carbon dioxide escapes from the solution and turns the red litmus solution into purple.

23. The reaction principle of fire extinguisher

Al2(SO4)3+6 nah co 3 = = 3 na 2 so 4+2Al(OH)3↓+6 CO2↓

Fire extinguishing principle: when putting out a fire, a large amount of carbon dioxide and foam can be sprayed out, which can be attached to combustible materials to isolate them from the air and achieve the purpose of fire extinguishing.

24. Reaction between metal and water (displacement reaction)

①2K+ 2H2O = KOH + H2↑

②3Fe + 4H2O= Fe3O4 + 4H2↑

25. Reaction between water and nonmetal (displacement reaction)

C+H2O= CO+ H2 ↑

26. Reaction of water with oxides (combination reaction)

①SO3 +H2O =H2SO4

②Na2O +H2O =2NaOH

27. Ammonium bicarbonate is decomposed by heat (decomposition reaction)

NH4HCO3= NH3↑ + H2O + CO2↑

28. Use hydrochloric acid to remove rust (double decomposition reaction)

Fe2O3 + 6HCl =2FeCl3 + 3H2O

29. Insert the iron wire into the copper sulfate solution (displacement reaction)

Iron+copper sulfate = ferrous sulfate+copper

Phenomenon: the solution changes from blue to light green, and red solid is produced on the iron surface.

30. Dropping sodium hydroxide solution into copper sulfate solution (double decomposition reaction)

cuso 4+2 NaOH = Cu(OH)2←+na2so 4

Phenomenon: blue precipitate is produced.

3 1. Sulfur dioxide reacts with caustic soda solution.

SO2+2NaOH=Na2SO3+H2O

32. Low alcohol

C2H5OH+2O2=2CO2+3H2O

33. The sodium chloride solution reacts with silver nitrate solution to generate insoluble precipitate (double decomposition reaction)

Sodium chloride+silver nitrate = sodium nitrite+silver chloride ↓

34. Dilute sulfuric acid solution reacts with barium nitrate solution to generate insoluble precipitate.

Sulfuric acid+barium nitrate = barium sulfate ↓+nitric acid

35. Mixed heating of ammonium chloride solid and calcium hydroxide solid (double decomposition reaction)

2 NH4Cl+Ca(OH)2 = 2 NH3 ↑+ 2H2O+CaCl 2

36. Reaction of sodium carbonate with hydrochloric acid (double decomposition reaction)

Na2CO3+HCl=NaCl+CO2+H2O

Phenomenon: Solids dissolve, resulting in bubbles.

Related knowledge points: sodium carbonate is commonly known as soda ash.