Chemistry good into, seek junior second semester chemistry all knowledge points

1, red solid: copper, iron oxide

2, green solid: basic copper carbonate

3, blue solid: copper hydroxide, copper sulfate crystals

4, purple-black solid: potassium permanganate

5, yellowish solid: sulfur

6, colorless solids: ice, dry ice, diamond

7, silvery white solid Silver, iron, magnesium, aluminum, mercury and other metals

8, black solids: iron powder, charcoal, copper oxide, manganese dioxide, ferric oxide, (carbon black, activated charcoal)

9, reddish-brown solids: ferric hydroxide

10, white solids: sodium chloride, sodium carbonate, sodium hydroxide, calcium hydroxide, calcium carbonate, calcium oxide, copper sulfate, phosphorus pentoxide, magnesium oxide < /p>

(ii), the color of the liquid

11, colorless liquid: water, hydrogen peroxide

12, blue solution: copper sulfate solution, copper chloride solution, copper nitrate solution

13, light green solution: ferrous sulfate solution, ferrous chloride solution, ferrous nitrate solution

14, yellow solution: ferrous sulfate solution, ferric chloride solution, ferrous nitrate solution

14. Ferrous nitrate solution

15, purplish red solution: potassium permanganate solution

16, purple solution: litmus solution

(C), the color of gases

17, reddish-brown gas: nitrogen dioxide

18, yellowish-green gas: chlorine

19, colorless gas: oxygen, nitrogen, hydrogen, carbon dioxide. Carbon monoxide, sulfur dioxide, hydrogen chloride gas and most other gases.

Second, junior high school chemistry solutions of acidity and alkalinity

1, acidic solutions: acid solutions and some salt solutions (sodium bisulfate, potassium bisulfate, etc.)

2, alkaline solutions: alkali solutions and some salt solutions (sodium carbonate, sodium bicarbonate, etc.)

3, neutral solutions: water and most of the salt solutions

Third, junior high school chemistry open in the air changes in mass

(a) increase in mass

1, due to absorption of water: sodium hydroxide solid, calcium chloride, magnesium chloride, concentrated sulfuric acid;

2, due to the reaction with water: calcium oxide, barium oxide, potassium oxide, sodium oxide, copper sulfate;

3, due to the reaction with carbon dioxide: Sodium hydroxide, potassium hydroxide, barium hydroxide, calcium hydroxide;

(ii) Decrease in mass

1. Decrease due to volatilization: concentrated hydrochloric acid, concentrated nitric acid, alcohol, gasoline, concentrated ammonia;

2. Decrease due to weathering: sodium carbonate crystals.

Four, junior high school chemical substances test

(a), the test of gas

1, oxygen: with a spark of wood into the bottle, if the wood rekindles, it is oxygen.

2, hydrogen: in the glass tip ignited gas, cover a dry cold beaker, observe the walls of the cup whether there are water droplets, to the beaker into the clarified lime water, if not cloudy, it is hydrogen.

3, carbon dioxide: into the clarified lime water, if it becomes cloudy is carbon dioxide.

4, ammonia: moistened purple litmus paper, if the paper turns blue, it is ammonia.

5, water vapor: through anhydrous copper sulfate, if the white solid turns blue, it contains water vapor.

(ii), the test of ions.

6, hydrogen ions: drops of purple litmus test solution / add zinc grains

7, hydroxide ions: phenolphthalein test solution / copper sulfate solution

8, carbonate ions: dilute hydrochloric acid and clarified lime water

9, chloride ions: silver nitrate solution and dilute nitric acid, if a white precipitate is produced, it is a chloride ion

10, sulfate ions: Barium nitrate solution and dilute nitric acid / first drop of dilute hydrochloric acid and then drop barium chloride

11, ammonium ions: sodium hydroxide solution and heating, put the wet red litmus paper in the mouth of the test tube

12, copper ions: drop of sodium hydroxide solution, if a blue precipitate is copper ions

13, iron ions: drop of sodium hydroxide solution, if a reddish-brown precipitate is Iron ions

(C), related examples

14, how to test whether NaOH is deteriorated: drops of dilute hydrochloric acid, if bubbles are deteriorated

15, to test whether limestone is contained in quicklime: drops of dilute hydrochloric acid, if bubbles are contained in limestone

16, to test whether NaCl is contained in NaOH: drops of dilute nitric acid, then drops of AgNO3, and then drops of AgNO3.

17, test three bottles of test solution are dilute HNO3, dilute HCl, dilute H2SO4?

To the three test tubes, respectively, drop Ba (NO3) 2 solution, if a white precipitate is produced, then it is dilute H2SO4; and then drop AgNO3 solution, if a white precipitate is produced, then it is dilute H2SO4; and then drop AgNO3 solution, if a white precipitate is produced, then it is dilute HCl, and the rest of the solution is dilute H2SO4; and if a white precipitate is produced, then it is dilute H2SO4, and the rest of the test tube is dilute H2SO4; and then drop AgNO3 solution, if a white precipitate is produced, then it is dilute H2SO4. Dilute HCl, the rest is dilute HNO3

18, starch: add iodine solution, if it turns blue contains starch.

19, glucose: add freshly made copper hydroxide, if it produces a brick red cuprous oxide precipitate, it contains glucose.

V, junior high school chemistry of three

1, China's ancient three major chemical processes: papermaking, gunpowder, burning porcelain.

2, three types of oxidation reactions: explosion, combustion, slow oxidation.

3, the three kinds of particles that make up matter: molecules, atoms, ions.

4. Three types of particles that are not electrically charged: molecules, atoms, and neutrons.

5, the composition of matter and the composition of the three statements:

(1), carbon dioxide is composed of carbon and oxygen;

(2), carbon dioxide is composed of carbon dioxide molecules;

(3), a carbon dioxide molecule is composed of a carbon atom and an oxygen atom.

6. Three kinds of particles make up an atom: protons, neutrons, and electrons.

7, the three causes of water pollution: (1) industrial "three wastes" arbitrary discharge, (2) arbitrary discharge of domestic sewage (3) pesticides and fertilizers arbitrarily applied

8, the collection of methods of the three methods: water drainage (not allowed to be in the water of the gas), upward exhaust air method (density than the air of the gas), downward exhaust air method (density than the air of the gas). Downward air displacement method (gases less dense than air).

9, the law of conservation of mass of the three does not change: the atomic species remains unchanged, the number of atoms remains unchanged, the mass of atoms remains unchanged.

10, unsaturated solution into saturated solution of three ways:

increase solute, reduce the solvent, change the temperature (higher or lower).

11, compound decomposition reaction can occur in three conditions: the production of water, gas or precipitate

12, the three major chemical fertilizers: N, P, K

13, three gaseous pollutants emitted into the air: carbon monoxide, oxides of nitrogen, and oxides of sulfur.

14, burning white light substances: magnesium strips, charcoal, candles (carbon dioxide and water).

15, combustible, reducing substances: hydrogen, carbon monoxide, carbon monoxide.

16, three gases that are flammable are: hydrogen (ideal), carbon monoxide (toxic), and methane (common).

17, three chemical properties of CO: flammability, reducibility, toxicity.

18, three major fossil fuels: coal, oil, natural gas. (all mixtures)

19, three ferrous metals: iron, manganese, chromium.

20, three oxides of iron: ferrous oxide, ferric oxide, ferric tetraoxide.

21, three oxides of iron making: iron ore, coke, limestone.

22, three common strong acids: hydrochloric acid, sulfuric acid, nitric acid.

23, concentrated sulfuric acid three properties: water absorption, dehydration, strong oxidation.

24, three common names for sodium hydroxide: caustic soda, caustic soda, caustic soda.

25. Three oxides produced by the thermal decomposition of basic copper carbonate: copper oxide, water (hydrogen oxide), and carbon dioxide.

26, laboratory production of CO2 can not be used three substances: nitric acid, concentrated sulfuric acid, sodium carbonate.

27, the three flames of the alcohol lamp: inner flame, outer flame, flame center.

28, the use of alcohol lamps have three prohibitions: it is forbidden to add alcohol to the burning lamp, it is forbidden to use the alcohol lamp to ignite another alcohol lamp, it is forbidden to use the mouth to blow out the alcohol lamp.

29, the glass rod in the purification of crude salt in the three roles: stirring, drainage, transfer

30, liquid filtration operation of the three leaning: (1) pouring the filtrate beaker mouth close to the glass rod, (2) the glass rod lightly leaning on the end of the three layers of filter paper, (3) funnel lower end of the mouth of the tube close to the inside wall of the beaker.

31. The three steps in preparing a solution of a solid: calculating, weighing, and dissolving.

32. Three steps in matching a concentration to a dilution: calculate, measure, and dissolve.

33, concentrated with dilute three instruments: beaker, measuring cylinder, glass rod.

34, three exothermic substances in contact with water: concentrated sulfuric acid, sodium hydroxide, quicklime.

35, filtration twice filtrate is still turbid cause: the filter paper is torn, the instrument is not clean, the liquid level is higher than the edge of the filter paper.

36, the three no principles of drug access: can not touch the drug with your hands, do not put your nostrils to the mouth of the container to smell the odor of the drug, shall not taste any drug.

37, the three meanings of the order of metal activity: (1) the position of the metal in front, it is in aqueous solution, the more likely to lose electrons into ions, the stronger its activity; (2) ranked in front of the hydrogen in the metal can replace the hydrogen in the acid, ranked behind the hydrogen in the metal can not be replaced by hydrogen in the acid; (3) in front of the metal in front of the metal in the back of the metal from the saline solution they are replaced out.

38, the effect of temperature on the solubility of solids: (1) the solubility of most solids increases with increasing temperature, (2) the solubility of a few solids by the temperature does not change much (3) the solubility of very few solids decreases with increasing temperature.

39, factors affecting the rate of dissolution: (1) temperature, (2) whether or not to stir (3) the size of the solid particles

40, three substances that make iron rust: iron, water, oxygen.

41, three states of solutes: solid, liquid, gas.

42, three factors affecting solubility: nature of the solute, nature of the solvent, temperature.

VI. Important components of common mixtures in junior high school chemistry

1, air: nitrogen (N2) and oxygen (O2)

2, water gas: carbon monoxide (CO) and hydrogen (H2)

3, coal gas: carbon monoxide (CO)

4, natural gas: methane (CH4)

5, limestone/ Marble: (CaCO3)

6. Pig iron/steel: (Fe)

7. Charcoal/coke/carbon black/activated carbon: (C)

8. Rust: (Fe2O3)

6. Important Components of Common Mixtures in Middle School Chemistry

1. Air: Nitrogen (N2) and oxygen (O2)

2, Water gas: carbon monoxide (CO) and hydrogen (H2)

3, gas: carbon monoxide (CO)

4, natural gas: methane (CH4)

5, limestone/marble: (CaCO3)

6, pig iron/steel: (Fe)

7, charcoal/coke/carbon black/activated carbon: (C)

8, rust: (Fe2O3)

Seven, junior high school chemistry common substances commonly known as

1, sodium chloride (NaCl) : table salt

2, sodium carbonate (Na2CO3) : soda, soda, mouth alkali

3, sodium hydroxide (NaOH) : soda ash, caustic soda, caustic soda

4, calcium oxide (CaO) : quicklime

5, calcium hydroxide (Ca(OH)2): slaked lime, slaked lime

6, carbon dioxide solids (CO2): dry ice

7, hydrochloric acid (HCl): hydrochloric acid

8, alkaline carbonate of copper (Cu2(OH)2CO3): cupric green

9, copper sulfate crystals (CuSO4 . 5H2O): blue alum, bile alum

10, methane (CH4): methane gas

11, ethanol (C2H5OH): alcohol

12, acetic acid (CH3COOH): acetic acid

13, hydrogen peroxide (H2O2): hydrogen peroxide

14, mercury (Hg): mercury

15, Sodium bicarbonate (NaHCO3): baking soda

VIII. DEMULGENATION OF SUBSTANCES

1. CO2 (CO): pass the gas through scorched copper oxide,

2. CO (CO2): pass through a sufficient amount of sodium hydroxide solution

3. H2 (water vapor): pass through concentrated sulphuric acid/pass through sodium hydroxide solid

4. CuO (C): burn the mixture in air (in a stream of oxygen)

5, Cu (Fe) :add sufficient amount of dilute sulfuric acid

6, Cu (CuO): add sufficient amount of dilute sulfuric acid

7, FeSO4 (CuSO4): add sufficient amount of powdered iron

8, NaCl (Na2CO3): add sufficient amount of hydrochloric acid

9, NaCl (Na2SO4): add a sufficient amount of barium chloride solution

10, NaCl (NaOH): add a sufficient amount of hydrochloric acid

11, NaOH (Na2CO3): add a sufficient amount of calcium hydroxide solution

12, NaCl (CuSO4): add a sufficient amount of barium hydroxide solution

13, NaNO3 (NaCl): add sufficient amount of silver nitrate solution

14, NaCl (KNO3): evaporation of the solvent

15, KNO3 (NaCl): cooling hot saturated solution.

16, CO2 (water vapor): through concentrated sulfuric acid.

9, the best of chemistry

1, the most ideal fuel for the future is H2 .

2. The simplest organic substance is CH4 .

3. The least dense gas is H2 .

4. The substance with the smallest relative molecular mass is H2 .

5. The oxide with the smallest relative molecular mass is H2O .

6. The smallest particle in a chemical change is an atom.

7. When PH=0, acidity is the strongest and alkalinity is the weakest.

When PH=14, alkalinity is the strongest and acidity is the weakest.

8, the soil is most deficient in N, K, P three elements, the most efficient nitrogen fertilizer is urea.

9. The hardest naturally occurring substance is diamond.

10. The first country to utilize natural gas was China.

11. The most abundant element in the earth's crust is oxygen.

12. The most abundant metal element in the Earth's crust is aluminum.

13. The most abundant gas in the air is nitrogen.

14. The most abundant element in the air is nitrogen.

15. The three most important fossil fuels in the world today are coal, oil and natural gas.

16, the formation of the largest variety of compounds: carbon

X, about different

1, diamond and graphite have different physical properties: because of the different arrangement of carbon atoms.

2, pig iron and steel properties are different: because of the different carbon content.

3. The chemical properties of carbon monoxide and carbon dioxide are different because of different molecular compositions.

(Oxygen and ozone have different chemical properties because of different molecular compositions; water and hydrogen peroxide have different chemical properties because of different molecular compositions.)

4. The types of elements are different: because of the different numbers of protons.

5. Different elemental valences: because of different numbers of outermost electrons.

6. The chemical properties of sodium atoms and sodium ions are different: because of the different numbers of outermost electrons

XI: Poisonous Substances

1. Toxic solids: Sodium Nitrite (NaNO2), Lead Acetate, etc.;

2. Poisonous liquids: Mercury, Copper Sulphate solution, Methanol, Ba2+-containing solutions (except BaSO4);

< p>3. Toxic gases: CO, oxides of nitrogen, oxides of sulfur.

XII: Laboratory Preparation

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1. Laboratory oxygen: 2KMnO4=====2K2MnO4+MnO2+O2↑

MnO2

2KClO3=======2KCl+3O2↑