Knowledge points of chemistry in senior one.

Chemistry knowledge points in senior one 1 1, Na:4Na+O2 = 2na 2 o in the air.

2. Sodium burns in air: 2Na+O2 ignites Na2O2.

3. The reaction between sodium and water: 2na+2h2o = 2nNaOH+H2 =

Ionic equation +-4 and sodium peroxide (Na2O2) react with water: 2Na2O2+2H2O = 4 NaOH+O2 =

+-6, sodium bicarbonate heating: sodium bicarbonate heating sodium carbonate +H2O+ carbon dioxide =

7. Treating hyperacidity with baking soda: nahco3+HCl = NaCl+H2O+CO2 ↑-+8, Na2CO3+2HCl=2NaCl+H2O+CO2↑ ionic equation CO2-+ Understand the essence (the step-by-step reaction process is as follows):

9. Introduce a small amount of carbon dioxide into sodium hydroxide: 2NaOH+ CO2= Na2CO3+H2O.

10, excess carbon dioxide is introduced into sodium hydroxide: 2NaOH+ CO2= Na2CO.

3+H2O and Na2CO3+H2O+ CO2= 2NaHCO3

Total reaction: NaOH+ CO2= NaHCO3.

1 1, the reaction equation of Al and NaOH solution: 2al+2nNaOH+2h2o = 2nalo2+3h2 = ionic equation 2Al+2OH-

12, reaction equation of Al and HCl solution: 2al+6HCl = 2alcl3+3H2 ↑+3+13, reaction equation of Al2O3 and dilute HCl: Al2O3+6HCl = 2AlCl3+3H2O ionic equation Al+3+.

14, the reaction equation of Al2O3 and NaOH solution: Al2O3+2NaOH = 2NALO2+H2O-

15, the ionic equation of the reaction of AlCl3 with a small amount of NaOH solution: Al3++3OH- = Al(OH)3↓

16, the reaction equation of Al(OH)3 with NaOH solution: Al (OH) 3+NaOH = NAALO2+2H2O-

17, ionic equation of AlCl3 reacting with excess NaOH solution: Al3++4OH- = AlO2-+2H2O.

Chemical equation for the reaction of 18 and Al(OH)3 with dilute HCl Al(OH)3+3HCl =AlCl3+ 3H2O ionic equation: Al(OH)+3+ 19, chemical equation for the reaction of AlCl3 with excess ammonia water: AlCl3+3H3. H2O = Al (OH) 3 ↓+3H4。

20. a small amount of carbon dioxide is introduced into naalo2: 2nalo2+CO2+3H2O = Na2CO3+2al (OH) 3↓

2 1, NaAlO2 is filled with enough carbon dioxide: naalo2+CO2+2h2o = nahco3+Al (OH) 3 ↓

22. Decomposition equation of Al (OH) 3 heating: 2Al(OH)3 heating Al2.

O3+3H2O

23. High temperature of iron and water vapor: 3Fe+4H2O(g) high temperature Fe3O4+4H2↑ =

24. the reaction of ferrous oxide with dilute hydrochloric acid: FeO+2HCl = FeCl2+H2O ionic equation: FeO+2H+2+.

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

27. The reaction between ferrous sulfate and sodium hydroxide solution: FeSO4+2NaOH = Fe(OH)2↓+ Na2SO4 ionic equation: Fe3+ —28, the equation of ferrous hydroxide exposed to air: 4Fe(OH)2+O2+2H2O = 4Fe(OH)3.

29. The chemical equation of the reaction between iron powder and ferric chloride solution: 2FeCl3+Fe = 3FeCl2 ionic equation: Fe+2Fe3+ 2+.

The chemical equation of the reaction between copper powder and ferric chloride solution: Cu+2FeCl3=2FeCl2+CuCl2.

30. Chemical reaction equation of introducing chlorine into ferrous chloride solution: 2FeCl2+Cl2 = 2FeCl3 ionic equation: 2Fe2+3+-

30. Chemical reaction equation of introducing chlorine into ferrous chloride solution: 2FeCl2+Cl2 = 2FeCl3 2+

3+- 3 1. Preparation of iron hydroxide colloid: FeCl3+3H2O heats 2Fe(OH)3 (colloid) +3HCl.

2 reacts with HF: SiO2+4HF=SiF4↑+2H2O 32, SiO2 reacts with NaOH solution: SiO2+2NaOH = Na2SiO3+H2O-2-33, SiO223-

34. the reaction between na2sio3 and hydrochloric acid: na2sio3+2hcl = 2nac+H2SO4 3 ↓

35.Na2SiO3 reacts with a small amount of carbon dioxide: Na2SiO3+CO2 +H2O = H2SiO3↓+ Na2CO3.

36.Na2SiO3 reacts with excess carbon dioxide: Na2SiO3+2CO2 +2H2O = H2SiO3↓+

sodium bicarbonate

37, chlorine and sodium reaction: Cl2+2Na ignition.

Reaction between chlorine and iron: 3Cl2+2Fe ignites 2FeCl3.

39. Reaction of chlorine and copper: Cl2+Cu ignites CuCl2.

40. Reaction of chlorine and hydrogen: Cl2+H2 ignites 2HCl.

4 1, chlorine becomes water: Cl2+H2O=HClO+HCl.

ionic equation

42. Absorb excess chlorine with sodium hydroxide solution: Cl2+2NaOH=NaCl+NaClO+H2O ionic equation-

43. Chlorine is introduced into lime milk to make bleaching powder concentrated solution: 2cl2+2ca (OH) 2 = CaCl2+Ca (clo) 2+2h2o Bleaching principle: Ca(ClO)2+H2O+ CO2=2 HClO+ CaCO3.

44, hypochlorous acid see photodegradation 2 hclo2 write

45. elemental sulfur reacts with oxygen at high temperature: 2 46. Sulfur dioxide is soluble in water: SO2+H2OH2SO3.

47. Sodium hydroxide and a small amount of sulfur dioxide: SO2 (small amount) +2 NaOH = Na2SO3+H2O-2-

48, sodium hydroxide and excess sulfur dioxide: SO2 (excess)+NaOH = nahso3-49, sulfur dioxide and sodium oxide: SO2+Na2O = Na2SO3.

50. Sodium carbonate and a small amount of sulfur dioxide: SO2 (small amount)+Na2CO3 = Na2SO3+CO2-51,sulfur dioxide and oxygen: 2SO2+O2 2SO3 (conditions: heating, catalyst).

52. Reaction of sulfur dioxide with oxidant chlorine: SO2+Cl2+2H2O = H2SO4+2HCl (Cl2 can be replaced by Br2 and I2) ionic equation: SO+2-★ SO2 can also undergo redox reaction with potassium permanganate and FeCl3.

53. The reaction of SO3 with water: SO3+H2O=H2SO4.

54.SO3 reacts with calcium hydroxide: SO3+ calcium hydroxide = calcium sulfate +H2O.

55.SO3 reacts with Cao: SO3+ Cao = calcium sulfate.

56. Nitrogen-oxygen combination: N2+O2 discharge 2NO

57.NO contact with air: 2NO+O2=2NO2.

58.NO2 is soluble in water: 3NO2+2H2O = 2HNO3+NO.

59. NO2 and O2 are mixed to form water: 4NO2+O2+2H2O = 4NO3.

60. NO and O2 are mixed to form water: 4NO+3O2+2H2O = 4NO3.

6 1, nitrogen-bound hydrogen (industrial synthetic ammonia): N2+3H22NH3.

Catalyst (high temperature, high pressure, catalyst)

Catalytic oxidation of ammonia: 4NH3+5 O2= heating 4NO+6H2O.

62. Ammonia and water: NH3+H2ONH3 ~ H2O

63, heating concentrated ammonia NH3﹒H2O heating NH3 write +H2O.

64. Ammonia and concentrated hydrochloric acid smoke in the air: NH3+HCl=NH4Cl.

65. Thermal decomposition of ammonium bicarbonate: NH4HCO3 is heated by 3 =+CO2 =+H2O.

66. Ammonium chloride is decomposed by heating: NH4Cl heats NH3 =+HCl =

67, the laboratory with solid and solid mixed heating ammonia:

2NH4Cl+Ca(OH)2 2 +2NH3↑+2H2O

68. Mixed heating of metallic copper and concentrated sulfuric acid: Cu+2H2SO4 (concentrated) 4+SO2 =+2H2O.

69. A small amount of iron: 2Fe+6H2SO4 (concentrated) heating Fe2 (SO4) 3+3SO2 =+6H2O.

Iron excess: Fe+2H2SO4+SO2 =+2H2O.

70. Mixed heating of charcoal and concentrated sulfuric acid: C+2H2SO4 (concentrated) 2 =+2SO2 =+2H2O.

7 1. The reaction between copper and concentrated nitric acid: Cu+4hno3 = Cu (NO3) 2+2no2 =+2h2o+-2+72. Reaction of copper with dilute nitric acid: 3cu+8HNO3 = 3cu (NO3) 2+2no ↑+4h2o+-2+heating.

Senior one chemistry 2 knowledge points 1. Test of sulfate ion: bacl2+Na2SO4 = baso4 ↓+2nNaCl.

2. Test of carbonate ion: CaCl2+Na2CO3 = CaCO3↓+2NaCl.

3. The reaction between sodium carbonate and hydrochloric acid: Na2CO3+2HCl = 2NaCl+H2O+CO2 =

4, charcoal reduction of copper oxide writing

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

6. The reaction between calcium chloride and sodium carbonate solution: CaCl2+Na2CO3 = CaCO3↓+ 2NaCl.

7. Sodium burns in air: sodium reacts with oxygen: 4Na+O2 = 2Na2O.

8. The reaction between sodium peroxide and water: 2Na2O2+2H2O = 4NaOH+O2 =

9. The reaction between sodium peroxide and carbon dioxide: 2Na2O2+2CO2 = 2Na2CO3+O2.

10, the reaction of sodium and water: 2na+2h2o = 2nNaOH+H2 =

1 1. Reaction of iron with water vapor: 3fe+4h2o (g) = f3o4+4h2 =

12. the reaction of aluminum with sodium hydroxide solution: 2al+2Al+2NaOH+2H2O = 2NaAlO2+3H2↑ = =

13. The reaction between calcium oxide and water: CaO+H2O = Ca(OH)2.

14. The reaction between iron oxide and hydrochloric acid: Fe2O3+6HCl = 2FeCl3+3H2O.

15. The reaction between alumina and hydrochloric acid: Al2O3+6HCl = 2AlCl3+3H2O.

16. The reaction between alumina and sodium hydroxide solution: Al2O3+2NaOH = 2NALO2+H2O-

17. The reaction of ferric chloride with sodium hydroxide solution: FeCl3+3NaOH = Fe(OH)3↓+ 3NaCl.

18. The reaction between ferrous sulfate and sodium hydroxide solution: FeSO4+2NaOH = Fe(OH)2↓+ Na2SO4.

19, ferrous hydroxide is oxidized to ferric hydroxide: 4Fe(OH)2+2H2O+O2 = 4Fe(OH)3.

20. Thermal decomposition of iron hydroxide: =

2 1. Aluminum hydroxide prepared in laboratory: Al2 (SO4) 3+6HNH3? H2O = 2Al(OH)3↓ + 3(NH3)2SO4

22. The reaction between aluminum hydroxide and hydrochloric acid: Al(OH)3+3HCl = AlCl3+3H2O.

23. The reaction between aluminum hydroxide and sodium hydroxide solution: Al(OH)3+NaOH = NaAlO2+2H2O.

24. Thermal decomposition of aluminum hydroxide: 25. The reaction between ferric chloride solution and iron powder: 2FeCl3+Fe = 3FeCl2.

26. Introduce chlorine into ferrous chloride: 2FeCl2+Cl2 = 2FeCl3.

27. Reaction of silicon dioxide with hydrofluoric acid: SiO2+4HF = SiF4+2H2O Reaction of silicon with hydrofluoric acid: Si+4hf = SiF4+2H2 =

28. High temperature reaction between silica and calcium oxide: 29. The reaction between silica and sodium hydroxide solution: silica+sodium hydroxide = silica +H2O.

30. Introduce carbon dioxide into the sodium silicate solution: Na2SiO3+CO2+H2O = Na2CO3+H2SiO3↓

3 1. The reaction between sodium silicate and hydrochloric acid: Na2SiO3+2HCl = 2NaCl+H2SiO3↓

32. Reaction of chlorine with metallic iron: 33. Reaction of chlorine with copper: 34. Reaction of chlorine with metallic sodium;

35. Reaction between chlorine and water: Cl2+H2O = HCl+HClO.

36. Photolysis of hypochlorous acid: =

37. Chlorine reacts with sodium hydroxide solution: Cl2+2NaOH = NaCl+NaClO+H2O.

38. The reaction of chlorine with hydrated lime: 2cl2+2ca (OH) 2 = CaCl2+Ca (clo) 2+2h2o.

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

40. Bleaching powder is exposed to air for a long time: Ca(ClO)2+H2O+CO2 = CaCO3↓+2HClO.

4 1. The reaction of sulfur dioxide with water: SO2+H2O ≈ H2SO3.

42. Nitrogen reacts with oxygen under discharge: 43. Nitric oxide reacts with oxygen: 2NO+O2 = 2NO2.

44. The reaction between nitrogen dioxide and water: 3NO2+H2O = 2HNO3+NO.

45. Sulfur dioxide reacts with oxygen under the action of catalyst: 2SO2+46, and sulfur trioxide reacts with water: SO3+H2O = H2SO4.

47. The reaction between concentrated sulfuric acid and copper: Cu+2H2SO4 (concentrated +2H2O+SO2 =-

48. The reaction between concentrated sulfuric acid and charcoal: C+2H2SO4 (concentration = =+2SO2 =+2H2O)

49. The reaction between concentrated nitric acid and copper: Cu+4NO3 (concentrated) = Cu (NO3) 2+2H2O+2NO2 =

50. Reaction of dilute nitric acid with copper: 3Cu+8HNO3 (dilute+4h2o+2no =

5 1. Ammonia is decomposed by heating: =+H2O.

52. Reaction between ammonia and hydrogen chloride: NH3+HCl = NH4Cl.

53. Thermal decomposition of ammonium chloride: =+HCl =

54. Decomposition of ammonium bicarbonate by heating: =+H2O =+CO2 =

55. The reaction between ammonium nitrate and sodium hydroxide: NH4NO3+↑+NaNO3+H2O.

56. Laboratory preparation of ammonia: 2nh4cl++2h2o+2nh3 =

57. Reaction between chlorine and hydrogen: 58. The reaction between ammonium sulfate and sodium hydroxide: (NH4) 2SO4+=+Na2SO4+2H2O.

59、SO2 + CaO = CaSO3

60、SO2 + 2NaOH = Na2SO3 + H2O

6 1, SO2+calcium hydroxide = CaSO3↓+H2O

62、SO2 + Cl2 + 2H2O = 2HCl + H2SO4

63、SO2 + 2H2S = 3S + 2H2O

64. Recovery of NO and NO2: NO2+NO+2NaOH = 2NaNO2+H2O.

65、Si + 2F 2 = SiF4

66、Si + 2NaOH + H2O = NaSiO3 +2H2↑

67. Laboratory method of making simple silicon: preparing crude silicon: SiO2+2C high-temperature electric furnace Si+2CO (quartz sand) (coke) (crude silicon).

Transformation from crude silicon to pure silicon: Si (crude) (pure) +4HCl

Non-metallic elements (fluorine, chlorine, oxygen, sulfur, N2, phosphorus, carbon, silicon)

1, oxidizability:

F2 + H2 = 2HF

F2 +Xe (excess) =XeF2

2F2 (excess) +Xe=XeF4

NF2 +2M=2MFn (for most metals) 2F2 +2H2O=4HF+O2.

2 F2+2 NaOH = 2 NaF+OF2+H2O F2+2 NaCl = 2 NaF+Cl2

F2 +2NaBr=2NaF+Br2

F2+2NaI =2NaF+I2

F2 +Cl2 (equal volume) =2ClF 3F2 (excess)+Cl2 = 2clf2f2f2 (excess) +I2 = 2f7.

Cl2 +H2 =2HCl

3Cl2 +2P=2PCl3

Cl2 +PCl3 =PCl5

Cl2 +2Na=2NaCl

3Cl2 +2Fe=2FeCl3

Cl2 +2FeCl2 =2FeCl3 Cl2+Cu=CuCl2

2cl 2+2 nabr = 2 NaCl+br2cl 2+2 nai = 2 NaCl+I2

5Cl2+I2+6H2O=2HIO3+ 10HCl

Knowledge points of chemistry in senior one 3. Chapter 1: From experimental chemistry.

I. Separation, Purification and Identification of Common Substances

1. General physical method-separation according to the difference of physical properties of substances.

Crystallization is the process of separating crystals from solution by solute, which can be used to separate and purify the mixture of several soluble solids. The principle of crystallization is to reduce the solubility of each component in a certain solvent by evaporation or lowering the temperature, so as to precipitate crystals. When the evaporating dish is heated to evaporate the solution, the solution should be constantly stirred with a glass rod to prevent the droplets from splashing due to local high temperature. When more solids appear in the evaporating dish, stop heating, for example, the mixture of NaCl and KNO3 is separated by crystallization.

Two. Distillation distillation is a method to purify or separate liquid mixtures with different boiling points. The process of separating various mixed liquids by distillation principle is called fractionation.

Attention during operation:

① Put a small amount of broken porcelain pieces in the distillation bottle to prevent the liquid from boiling.

(2) The position of the mercury ball of the thermometer should be on the same horizontal line with the lower edge at the bottom of the branch pipe.

③ The liquid in the distillation bottle should not exceed 2/3 of its volume and should not be less than 1/3.

(4) The cooling water in the condenser tube enters from the lower mouth and is discharged from the upper mouth.

⑤ The heating temperature should not exceed the boiling point of the substance with the highest boiling point in the mixture, such as the fractionation of petroleum.

Three. Liquid separation and extraction liquid separation are two methods to separate two liquids which are immiscible and have different densities. Extraction is a method of extracting solute from a solution composed of it and another solvent by using the solubility difference of solute in immiscible solvents. The selected extractant should meet the following requirements: immiscible with the solvent in the stock solution; Solute is much more soluble than the original solvent, and the solvent is volatile. In the process of extraction, attention should be paid to:

(1) Pour the solution to be extracted and the extraction solvent into the separatory funnel from the upper opening in sequence, the amount of which should not exceed 2/3 of the volume of the funnel, plug the plug and vibrate.

(2) When vibrating, hold the neck of the upper mouth of the funnel with your right hand, press the plug with the root of your index finger, hold the cock with your left hand, control the piston with your fingers, invert the funnel and vibrate hard.

(3) Then, the separation funnel is allowed to stand, and the liquid is separated after layering, and the lower liquid is discharged from the funnel mouth and the upper liquid is poured out from the upper mouth. For example, using carbon tetrachloride to extract bromine from bromine water. Four. Sublimation Sublimation refers to the process that a solid substance directly changes into a gas state without going through a liquid state after absorbing heat. Using the sublimation characteristics of some substances, this substance is separated from other substances that do not sublimate when heated.

For example, heating to sublimate iodine separates the mixture of I2 and SiO2.

2. Chemical separation and purification of substances

The separation of substances can generally be carried out by chemical methods first, and then according to the mixture

Separate the features by an appropriate separation method (see Basic Operation of Chemistry).

When separating and purifying substances by chemical methods, attention should be paid to:

(1) It is best not to introduce new impurities;

(2) The quality of the purified substance cannot be lost or reduced.

③ The experimental operation should be simple, not complicated. When removing impurities from the solution by chemical methods, it is necessary to add excessive separation reagents to make the separated substances or ions as clean as possible. In the multi-step separation process,

The added reagent should be able to remove irrelevant substances or ions added before.

For inorganic solutions, the following methods are usually used for separation and purification:

(1) Generation precipitation method (2) Generation gas method (3) Redox method (4) Mutual transformation between normal salt and acid salt method (5) Removal of impurities by amphoteric substances (6) Ion exchange method.

There are usually three kinds of tests for substances: identification, identification and inference. Their similarities are: according to the special properties and characteristic reactions of substances, appropriate reagents and methods are selected to accurately observe the obvious phenomena in the reaction, such as color change, precipitation formation and dissolution, gas generation and odor, flame color and so on.

(1)H can make purple litmus test solution or orange methyl orange test solution turn red.

(2) When Na+ and K+ are tested by flame reaction, their flames are yellow and light purple respectively (through the cobalt glass slide). 2+

(3)Ba can make dilute sulfuric acid or soluble sulfate solution produce white BaSO4 precipitate, which is insoluble in dilute nitric acid.

(4)Mg2+ can react with NaOH solution to generate white Mg(OH)2 precipitate, which can be dissolved in NH4Cl solution. 3+

(5)Al can react with a proper amount of NaOH solution to produce white Al(OH)3 flocculent precipitate, which can be dissolved in hydrochloric acid or excessive NaOH solution. +

(6)Ag can react with dilute hydrochloric acid or soluble hydrochloric acid to generate white AgCl precipitate, which is insoluble in dilute HNO3 and soluble in ammonia to generate [Ag (NH3) 2]+4+.

(7)NH ammonium salt (or concentrated solution) reacts with NaOH concentrated solution and is heated to release NH3 gas with pungent smell, so that the wet red sapphire blue test paper is blue. 2+

(8)Fe can react with a small amount of NaOH solution to generate white Fe(OH)2 precipitate, which quickly turns gray-green and finally turns red-brown Fe(OH)3 precipitate. Or adding KSCN solution to ferrous salt solution does not appear red, but immediately appears red after adding a small amount of fresh chlorine water. 2 Fe2 ++ Cl2 = 2 E3 ++ 2cl-(9)Fe3+ can react with KSCN solution to generate blood-red Fe(SCN)3 solution, and can react with NaOH solution to generate reddish-brown Fe(OH)3 precipitate.

The blue aqueous solution of (10)Cu2+ (concentrated CuCl2 solution is green) can react with NaOH solution to generate blue Cu(OH)2 precipitate, which can be transformed into black CuO precipitate after heating. The solution containing Cu2+ can react with Fe and Zn sheets to form copper on metal sheets.

③ Detection of several important anions

(1)OH- can turn colorless phenolphthalein, purple litmus and orange methyl orange into red, blue and yellow respectively.

(2)Cl- can react with silver nitrate to generate white AgCl precipitate, which is insoluble in dilute nitric acid and soluble in ammonia water to generate [Ag(NH3)2]+.

(3)Br- can react with silver nitrate to generate pale yellow AgBr precipitate, which is insoluble in dilute nitric acid.

(4)I- can react with silver nitrate to generate yellow AgI precipitate, which is insoluble in dilute nitric acid; It can also react with chlorine water to generate I2, which turns the starch solution blue.

(5)SO42- can react with the solution containing Ba2+ to generate white BaSO4 precipitate, which is insoluble in nitric acid.

(6)SO32- concentrated solution can react with strong acid to generate colorless and pungent SO2 gas, which can make magenta solution fade. It can react with BaCl2 solution to generate white BaSO3 precipitate, and dissolve in hydrochloric acid to generate colorless and pungent SO2 gas. 2-

(7)S can react with Pb(NO3)2 solution to produce black PbS precipitate.

(8)Co32- can react with BaCl2 solution to generate white BaCO3 precipitate, and dissolve in nitric acid (or hydrochloric acid) to generate colorless and odorless CO2 gas, which can make clear limewater turbid.

(9)HCO 3- Boil the salt solution containing HCO 3- to release colorless and odorless CO2 gas, which can make clear limewater turbid or add dilute MgSO4 solution to HCO 3- hydrochloric acid solution without any phenomenon. When heated and boiled, white precipitated magnesium carbonate is produced and carbon dioxide gas is released at the same time. 3-

The neutral solution of (10)PO4 containing phosphate can react with AgNO3 to generate yellow Ag3PO4 precipitate, which is soluble in nitric acid.