Ask about sulfur ions Is iodide a strong or weak reducing agent and what is the criterion 55

It is difficult to judge accurately, and the order of metal activity is not absolute, for example, iron can react slowly with hydrogen gas.

However, at high temperatures, hydrogen can reduce Fe3O4 to get Fe, and the metal activity sequence table is the activity of metals, and it is impossible to judge the non-metallic ones, I think sulfur ions and iodine ions are strong reducing agents, because I 2 and S themselves are weak oxidants, and the ions corresponding to strong oxidation must be weak reducing agents.

For example, chloride ion reduction is weak because chlorine gas is highly oxidizing.

Chloride ions are only oxidized when they encounter strong oxidants such as acidic potassium permanganate, acid potassium chromate, potassium chlorate, etc., and the oxidation and reduction of substances have a lot to do with the acidic and alkaline environment.

For example, acidic potassium permanganate can oxidize chloride ions, but chlorine can oxidize basic manganate as permanganate.

The harder it is to lose electrons, the easier it is to get electrons after losing electrons, so the more reducible they are. There is no single method of comparison, and it can also be compared through chemical reaction equations. There are also other methods, and the landlord can summarize it himself, so that the harvest will be greater!!

There is no specific standard for distinguishing between strong and weak oxidants, and what is usually said is only a comparison between the oxidants that are often encountered.

Just titrate it yourself and you'll know.

The electronic formula of sulfide ion: S2-. The divalent sulfide ions are reducible, and the divalent sulfide ions are at the lowest valence, and the valence is easy to increase after the reaction, and the valency increases, showing reductivity.

When the element is the lowest negative valence, it is only reducible, because its chemical lease valence can only be increased, so that it is oxidized, and when the element is the highest positive valence, it is only oxidized. The second is the lowest negative price of sulfur, so it reflects strong reduction.

Uses of the element sulfur1. Sulfur is an important component of cystine, cysteine and methionine, and about 90% of sulfur exists in sulfur-containing amino acids in plants.

2. Sulfur is involved in the formation of chlorophyll.

3. Sulfur plays an important role in the formation and activation of certain enzymes in plants.

4. Sulfur is involved in the synthesis of vitamins H and B.

5. Formation of glycoside oil of cruciferous plants.

6. Sulfur is related to the protein structure that affects the cold and drought resistance of plants, and sulfur can increase the cold and drought resistance of some crops.

The above content refers to Encyclopedia - Sulfur Ion Ant Oak.

i2 + so2 + 2h2o = 2hi + h2so4

According to the law before and after the redox reaction.

The oxidizing properties of the oxidant are greater than the oxidation products, and the reducing agents are more reducible than the reducing products, i.e., SO2 > I-

When chlorine is introduced into the solution of I- and SO3 2-, it takes some time to see the iodine element coming out, and the sulfite is oxidized to sulfate...