Chemical formula junior Daquan .

 Sulfuric acid, hydrochloric acid H2SO4 sulfurous acid H2SO3 hydrogen sulfide H2S HCl HNO3 nitric acid H2CO3 carbonic acid chemical formula junior common substances hydrogen oxygen nitrogen phosphorus sulfur chlorine gas (non-metallic elemental) H2 C N2 O2 PS Cl2 Calcium potassium sodium zinc, copper and barium magnesium aluminum W mercury (metal simple substance) Na Mg Al K Ga Fe Zn Cu Ba W Hg water nitrogen dioxide, carbon monoxide, carbon dioxide, sodium oxide of phosphorus pentoxide silica H2O CO CO2 P2O5 Na2O NO2 SiO2 MgO sulfur trioxide copper oxide nitric oxide barium oxide cuprous oxide SO2 SO3 NO MgO CuO BaO Cu2O ferrous oxide iron oxide (iron red) iron oxide of aluminum oxide of tungsten trioxide FeO Fe2O3 Fe3O4 Al2O3 WO3 silver oxide lead oxide manganese dioxide (common oxides ) Ag2O PbO MnO2 potassium chloride sodium chloride (salt) calcium chloride, magnesium chloride, aluminum chloride, barium chloride, copper chloride KCl NaCl MgCl2 CaCl2 CuCl2 ZnCl2 BaCl2 AlCl3 ferrous chloride, ferric chloride, silver chloride (chloride / hydrochloride) FeCl2 FeCl3 AgCl hydrochloric acid nitric acid phosphoric acid hydrogen bromide hydrogen carbonate (a common acid) H2SO4 HCl HNO3 H3PO4 H2S HBr H2CO3 Calcium sulfate copper sulfate barium sulfate, ferrous sulfate, potassium magnesium sulfate CuSO4 BaSO4 CaSO4 KSO4 MgSO4 FeSO4 Fe2 (SO4) 3 Sodium aluminum sulfate potassium sulfate potassium sodium nitrate silver nitrate Al2 (SO4) 3 NaHSO4 KHSO4 NaSO3 NaNO3 KNO3 AgNO3 magnesium nitrate cupric nitrate sodium nitrite, sodium carbonate, calcium carbonate, calcium nitrate magnesium carbonate MgNO3 Cu (NO3 ) 2 Ca (NO3) 2 NaNO3 Na2CO3 CaCO3 MgCO3 potassium carbonate (common salt) K2CO3 sodium hydroxide calcium hydroxide potassium hydroxide barium hydroxide magnesium hydroxide aluminum hydroxide, cupric hydroxide NaOH Ca (OH) 2 Ba (OH) 2 Mg (OH) 2 Cu (OH) 2 KOH Al (OH) 3 hydroxide, ferrous hydroxide (common base) Fe (OH) 3 Fe (OH) 2 methanol, ethanol, methane, acetylene, acetic acid (common organic compounds) CH4 C2H2 CH3OH C2H5OH CH3COOH basic copper carbonate gypsum plaster alum copperas Cu2 (OH) 2CO3 CaSO4 • 2H2O 2 CaSO4 • H2O KAl (SO4) 2 • 12H2O FeSO4 • 7H2O crystal blue vitriol sodium carbonate (common crystalline hydrate) CuSO4 • 5H2O Na2CO3 urea ammonium nitrate ammonium sulfate ammonium bicarbonate • 10H2O potassium dihydrogen phosphate (common fertilizer) CO (NH2) 2 NH4NO3 (NH4) 2SO4 NH4HCO3 KH2PO4 precipitation: red-brown flocculent precipitate -------- Fe (OH) 3 light green precipitate ------------ Fe (OH) 2 blue flocculent precipitate ---------- Cu (OH) 2 white precipitate -------- ------ CaCO3, BaCO3, AgCl, BaSO4, (which BaSO4, AgCl is insoluble in HNO3 white precipitate, CaCO3 BaCO3 precipitate was dissolved in HNO3 white), Mg (OH) 2. pale yellow precipitate (solution )---- S slightly soluble in water ------------ Ca (OH) 2, CaSO4 summary of a junior high school chemistry equations, the nature of oxygen: (1) elemental reaction with oxygen: (compound reaction) 1. magnesium burns in air: 2Mg + O2 lit 2MgO 2. iron burning in oxygen: 3Fe + 2O2 light Fe3O4 3. copper heat in the air: 2Cu + O2 heating 2CuO 4. aluminum burns in air: 4Al + 3O2 light 2Al2O3 5. hydrogen combustion in air: 2H2 + O2 lit 2H2O 6. of red phosphorus burns in air (the air component of the experimental): 4P + 5O2 light 2P2O5 7. sulfur burns in air: S + O2 lit SO2 8. combustion of carbon in oxygen: C + O2 ignite CO2 9. Carbon incomplete combustion in oxygen: 2C + O2 lit 2CO (2) compounds with oxygen reaction: 10. monoxide burning in oxygen: 2CO + O2 lit 2CO2 11. Methane burns in air: CH4 + 2O2 ignite CO2 + 2H2O 12. alcohol burns in air: C2H5OH + 3O2 light 2CO2 + 3H2O (3) the source of oxygen: 13. Meaning ear of glass composition of the air heating experiments 2HgO Hg + O2 ↑ 14. Heating potassium permanganate: 2KMnO4 heating K2MnO4 + MnO2 + O2 ↑ (laboratory system of oxygen principle 1) 15. Hydrogen peroxide manganese dioxide as a catalyst in the decomposition reaction under the conditions: H2O2 MnO22H2O + O2 ↑ (laboratory system the principle of oxygen 2) Second, the nature of water: 16. The role of water in the DC decomposition (of the composition of the water test): 2H2O power 2H2 ↑ + O2 ↑ 17. Lime dissolved in water: CaO + H2O == Ca (OH) 2 18. Carbon dioxide is soluble in water: H2O + CO2 == H2CO3 Third, conservation of mass: 19. Magnesium burns in air: 2Mg + O2 lit 2MgO 20. Iron and copper sulfate solution reaction: Fe + CuSO4 === FeSO4 + Cu 21. Hydrogen reduction of copper oxide: H2 + CuO heating Cu + H2O 22. Magnesium reduction of copper oxide: Mg + CuO four heating Cu + MgO, carbon and carbon oxides: (1) the chemical properties of carbon-23. Full combustion of carbon in oxygen : C + O2 ignite CO2 24. Charcoal reduction of copper oxide: C + 2CuO temperature 2Cu + CO2 ↑ 25. Coke reduction of iron oxide: 3C + 2Fe2O3 temperature 4Fe + 3CO2 ↑ (2) coal stove in the place of three reactions: (a few combination reaction) 26. Coal stove in the bottom: C + O2 ignite CO2 27. Coal stove in the middle: CO2 + C temperature 2CO 28. Coal stove in the upper part of the blue flame produces: 2CO + O2 lit 2CO2 (3) the system of law and nature of carbon dioxide: 29. Marble and dilute hydrochloric acid (laboratory system for carbon dioxide): CaCO3 + 2HCl == CaCl2 + H2O + CO2 ↑ 30. Unstable carbonate decomposition: H2CO3 == H2O + CO2 ↑ 31. Carbon dioxide is soluble in water: H2O + CO2 == H2CO3 32. Calcination of limestone (industrial manufacturing carbon dioxide): CaCO3 hot CaO + CO2 ↑ 33. Lime water and carbon dioxide reaction (to identify carbon dioxide): Ca (OH) 2 + CO2 === CaCO3 ↓ + H2O (4) the nature of carbon monoxide: 34. Reduction of copper oxide carbon monoxide: CO + CuO heating Cu + CO2 35. Flammability of carbon monoxide: 2CO + O2 2CO2 other light reaction: 36. Sodium carbonate and dilute hydrochloric acid (the principle of fire extinguishers): Na2CO3 + 2HCl == 2NaCl + H2O + CO2 ↑ V. fuel and its use: 37. Methane burns in air: CH4 + 2O2 light CO2 + 2H2O 38. Alcohol burns in air: C2H5OH + 3O2 light 2CO2 + 3H2O 39. The combustion of hydrogen in the air: 2H2 + O2 2H2O six light metal (1) metal and oxygen reaction: 40. Magnesium burns in air: 2Mg + O2 lit 2MgO 41. Iron burning in oxygen: 3Fe + 2O2 light Fe3O4 42. Copper heat in the air: 2Cu + O2 heating 2CuO 43. Aluminum oxide film formed in the air: 4Al + 3O2 = 2Al2O3 (2) metal + acid ---- elemental ---- salt + hydrogen (replacement reaction) 44. zinc and dilute sulfuric acid Zn + H2SO4 = ZnSO4 + H2 ↑ 45. iron and sulfuric acid Fe + H2SO4 = FeSO4 + H2 ↑ 46. magnesium and sulfuric acid Mg + H2SO4 = MgSO4 + H2 ↑ 47. aluminum and sulfuric acid 2Al +3 H2SO4 = Al2 (SO4) 3 +3 H2 ↑ 48. zinc and dilute hydrochloric acid Zn + 2HCl == ZnCl2 + H2 ↑ 49. iron and dilute hydrochloric acid Fe + 2HCl == FeCl2 + H2 ↑ 50. magnesium and dilute hydrochloric acid Mg + 2HCl == MgCl2 + H2 ↑ 51. Aluminium and dilute hydrochloric acid 2Al + 6HCl == 2AlCl3 + 3 H2 ↑ (3) elemental metal + salt (solution) ------- new metal + new salt 52. Iron and copper sulfate solution reaction: Fe + CuSO4 == FeSO4 + Cu 53. zinc and copper sulfate solution reaction: Zn + CuSO4 == ZnSO4 + Cu 54. copper and mercury nitrate solution reaction: Cu + Hg (NO3) 2 == Cu (NO3) 2 + Hg (3) iron The smelting principle: 55.3CO + 2Fe2O3 seven 4Fe + 3CO2 ↑ temperature, acid, alkali, salt 1, the chemical properties acid (1) -------- acid + metal salt + hydrogen (see above) (2 ) -------- acid + metal oxide salt + water 56. ferric oxide and hydrochloric acid reaction: Fe2O3 + 6HCl == 2FeCl3 + 3H2O 57. ferric oxide and sulfuric acid reaction: Fe2O3 + 3H2SO4 == Fe2 ( SO4) 3 + 3H2O 58. oxide copper and dilute hydrochloric acid: CuO + 2HCl == CuCl2 + H2O 59. oxide copper and dilute sulfuric acid reaction: CuO + H2SO4 == CuSO4 + H2O (3) acid + base ----- --- salt + water (neutralization reaction) 60. Hydrochloric acid and caustic soda from the reaction: HCl + NaOH == NaCl + H2O 61. Hydrochloric acid and calcium hydroxide reaction: 2HCl + Ca (OH) 2 == CaCl2 + 2H2O 62. Hyperacidity drug treatment of aluminum hydroxide: 3HCl + Al ( OH) 3 == AlCl3 + 3H2O 63. sulfuric acid and caustic soda reaction: H2SO4 + 2NaOH == Na2SO4 + 2H2O (4) acid + acid + salt -------- Another alternative salt 64. Marble and dilute hydrochloric acid reaction: CaCO3 + 2HCl == CaCl2 + H2O + CO2 ↑ 65. Dilute hydrochloric acid and sodium carbonate: Na2CO3 + 2HCl == 2NaCl + H2O + CO2 ↑ 66. Sodium bicarbonate and dilute hydrochloric acid: NaHCO3 + HCl == NaCl + H2O + CO2 ↑ 67. Sulfuric acid and barium chloride solution reaction: H2SO4 + BaCl2 == BaSO4 ↓ + 2HCl 2, alkali chemical properties (1) Base + non- -------- salt, metal oxide + water 68. Caustic exposure to the air deterioration: 2NaOH + CO2 == Na2CO3 + H2O 69. Caustic soda to absorb sulfur dioxide gas: 2NaOH + SO2 == Na2SO3 + H2O 70. Caustic sodium absorption of sulfur trioxide gas: 2NaOH + SO3 == Na2SO4 + H2O 71. On the deterioration in air lime: Ca (OH) 2 + CO2 == CaCO3 ↓ + H2O 72. Hydrated lime to absorb sulfur dioxide: Ca (OH) 2 + SO2 == CaSO3 ↓ + H2O (2) ----- alkaline + acid --- salt + water (neutralization reaction equation above) (3) another base + base + salt -------- another salt 73. calcium hydroxide and sodium carbonate: Ca (OH ) 2 + Na2CO3 == CaCO3 ↓ + 2NaOH 3, the chemical properties of salt (1) salt (solution) + metal elemental ------- Another alternative metal + salt 74. iron and copper sulfate solution reaction : Fe + CuSO4 == FeSO4 + Cu (2) -------- acid, another salt + acid + salt, the other 75. Dilute hydrochloric acid and sodium carbonate: Na2CO3 + 2HCl == 2NaCl + H2O + CO2 ↑ sodium bicarbonate and dilute hydrochloric acid: NaHCO3 + HCl == NaCl + H2O + CO2 ↑ (3) salt + alkali ------- - Another alternative base + salt 76. calcium hydroxide and sodium carbonate: Ca (OH) 2 + Na2CO3 == CaCO3 ↓ + 2NaOH (4) salt + salt two new salt ----- 77. Sodium chloride solution and silver nitrate solution: NaCl + AgNO3 == AgCl ↓ + NaNO3 78. Sodium sulfate and barium chloride: Na2SO4 + BaCl2 == BaSO4 ↓ + 2NaCl.