To take a high level of chemistry compulsory 1 properties of all substances

All the substances, smells, and what you say are hard to find! I used to know that there was a **, but it may not have been recently! But there's a QQ group that you can add to it, and people here can talk about chemistry problems, and you can ask people in the group about the problems you have, and of course I can too!

Group 22133065 You are also welcome to ask me for advice!

Hello:1Colored solids.

White and insoluble in strong acid precipitate: AGCL, BaSO4 silvery-white: Na

Pale yellow: S, Na2O2

Yellow: FeS2, Si crystals.

Black: Cuo, FEO, Fe3O4, FeS

Red: Cu, Cu2O, Fe2O3

Reddish-brown: Fe(OH)3

Blue: copper salt, Cu(OH)2

2.Non-ferrous gases.

Cl2 (yellow-green), F2 (light yellow-green), NO2 (reddish-brown) 3Colored solutions.

Fe2+ (light green), ridge with Fe3+ (yellow), Cu2+ (blue), Mno4 (purplish-red), Fe3+ and SCN- (blood red).

4.Flame color anti-defeat preparation: NA+ (yellow), K+ (purple) is quite complete, I hope it will help you learn.

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Good luck with your studies

1. Na2O2, sodium peroxide, AGBR, AGI are light yellow solids;

2. Copper oxide and iron oxide powder are black solids;

3. Copper sulfate pentahydrate is a blue solid;

4. Basic copper carbonate is a green liquid;

5. Calcium carbonate, silver chloride, sodium chloride are white solids, etc.

Chlorine yellow-green.

Bromine vapor reddish-brown.

Iodine purple-black.

Sodium, magnesium, aluminum, iron, silvery-white.

Copper red. Ferric thiocyanide solution is blood-red.

Ferrous solution light green.

Trivalent iron solution yellow.

Divalent copper solution blue.

Iron hydroxide reddish-brown.

Let me summarize the compulsory one in the first year of high school.

1.Colored solids.

White and insoluble in strong acid precipitate: AGCL, BaSO4 silvery-white: Na

Pale yellow: S, Na2O2

Yellow: FeS2, Si crystals.

Black: Cuo, FEO, Fe3O4, FeS

Red: Cu, Cu2O, Fe2O3

Reddish-brown: Fe(OH)3

Blue: copper salt, Cu(OH)2

2.Non-ferrous gases.

Cl2 (yellow-green), F2 (light yellow-green), NO2 (reddish-brown) 3Colored solutions.

Fe2+ (light green), Fe3+ (yellow), Cu2+ (blue), Mno4 (purplish), Fe3+ and SCN- (blood red).

4.Flame reaction: Na+ (yellow), K+ (purple) is quite complete, I looked at the book to summarize for you, I also reviewed it Many other substances are colorless.

Solid white and insoluble precipitate in strong acids: AGCL, BaSO4 silvery-white: Na

Pale yellow: S, Na2O2

Yellow: FeS2, Si crystals.

Black: Cuo, FEO, Fe3O4, FeS

Red: Cu, Cu2O, Fe2O3

Reddish-brown: Fe(OH)3

Blue: copper salt, Cu(OH)2

Gas Cl2 (yellow-green), F2 (light yellow-green), NO2 (reddish-brown) 3Colored solutions.

Fe2+ (light green), Fe3+ (yellow), Cu2+ (blue), Mno4 (purplish), Fe3+ and SCN- (blood red).

4.Flame reaction: Na+ (yellow), K+ (purple).

The flame color reaction of K is purple, AGI is yellow, AGBR is pale yellow, Fe2+ is green, Fe3+ is yellow, Cu2+ is blue, and permanganate is purple

Potassium permanganate. Amaranth.

Copper solids. Red.

Bromine water is orange-yellow.

Copper sulphate. Solid.

White. Solution.

Blue. (You can use him to verify the presence of water).

NO2 reddish-brown.

1. Sulfate ions must be removed first.

2. Fractionation is required.

3. This sentence is wrong. Because silver sulfate is also a white precipitate.

Silver nitrate solution is generally used for chloride ion testing, if it contains sulfate ions, silver sulfate will be produced after adding silver nitrate solution, silver sulfate is slightly soluble, and can be used as precipitation treatment, so acidified barium nitrate solution must be added before testing chloride ions, so that carbonate, sulfate and other effects can be removed.

Fractionation, there is no need, high school chemistry generally does not involve these.

Not necessarily, it may contain other ions, such as metaaluminate and silicate. This sentence, on the other hand, adding acidified cup edge solution to the solution must contain sulfate ions, which is correct.

(1) Ag2SO4 is slightly soluble and may produce white precipitate!

2) Extract the separator, the extractant can be volatilized naturally!

3) Ag2SO4 CaSO4 PBSO4 are all white precipitates!

You're wrong.

1. Silver ions are generally used to generate precipitates to detect the presence of chloride ions, and silver sulfate is also a precipitation, so it is necessary to exclude the interference of sulfate first, and then test chloride ions.

2 Of course, because what you get after separating is a mixture of organic solvent and iodine, and what you want to get is iodine element, so you have to fractionate it.

3 No, because silver sulfate is also a precipitation, it is necessary to exclude the interference of silver ions, which is related to the first question.

(1) Chloride ions will be tested with silver nitrate precipitation, but silver sulfate is slightly soluble, there is interference, and it should be removed in theory, and it is often not considered in practice.

2) The iodine in iodine water needs to be mixed with an extractant (such as CCL4) first, this step is called extraction, and then the two layers of liquid are separated in the separating funnel, which is called separating. The obtained lower liquid is a ccl4 solution of iodine, if the amount is large, it can be separated by fractionation, and if the amount is small, it can be placed and evaporated to obtain iodine.

3) Wrong, it is not necessarily barium ions that precipitate sulfuric acid, there is also lead in junior high school demerits, and of course, there are some situations in redox, such as: Na2SO3 + Na2S + H2SO4 = S + Na2SO4 + H2O, and the amount of sulfur is small when it is also white precipitate.