Ion oxidation or reduction, how to judge the oxidation and reduction of ions

The properties of ions are inversely proportional to elemental substances. In fact, the ability to gain electrons is inversely proportional to the ability to lose electrons.

Fluorine gas is the most reactive gas in the element, the most oxidizing, and its ions should be relatively weak. So your words are wrong.

Oxidation: fluorine gas, chlorine gas, bromine element, iodine element.

Reducibility: fluoride ions, chloride ions, bromine ions, iodide ions.

Addendum: Steady state is relative. There are no absolutely stable particles.

For example, when copper elements encounter concentrated sulfuric acid, electrons are lost and become copper ions (in water) At this time, copper ions should be relatively stable, but when encountering iron elements, iron atoms have a stronger ability to bind electrons. Iron robs the outer electrons of the copper particle and turns it back into a copper element.

Therefore, the statement that "ions are stable structures" is incorrect.

In the high and high points, there is a special way to judge whether the inside of the molecule has reached a stable structure. Therefore, there is no reason why molecules or ions are absolutely stable.

I think you're mistaken, fluoride ion f- is not oxidizing. Oxidizing is the fluorine element F2

Halone ions such as f-, cl- have no oxidation because they have reached the lowest price and cannot be lowered again.

The ions of halogen elements are only reducible, i.e., volatile electrons. The elemental elements of halogens have strong oxidizing properties. Chlorochlorobromoiodine (oxidizing from strong to weak, the reducing strength of ions is in reverse order).

You are indeed mistaken, fluoride ions are not oxidizing.

1. According to the law of the periodic table

During the same period, from left to right, the reducibility of non-metallic anions decreases and the oxidation of metal cations increases.

In the same family, from top to bottom, the oxidation of metal cations is weakened, and the reducibility of non-metal anions is enhanced.

2. Judging according to the valence:

For the same cation, the higher the valence state, the stronger the oxidation.

For the same anion, the lower the valence state, the stronger the reduction.

3. Judging according to the reaction equation:

Oxidation: The oxidant is greater than the oxidation product.

Reducibility: The reducing agent is greater than the reducing product.

4. Judging according to the reaction conditions: the stronger the oxidation of the ions when reacting with the same reducing agent, the simpler the conditions.

5. Judging according to the intensity of the reaction: the stronger the ion reduction with the same oxidant, the more intense the reaction.

6. Judging according to the state of the product: the stronger the reduction of the ion when reacting with the same oxidant, the higher the valence state of the product.

1. Oxidation of ions: refers to the ability of substances to obtain electrons, substances in the ** state and active non-metallic elementals, generally have oxidation, and substances in the low-valence state generally have reducibility;

2. The greater the concentration of oxidizing pants dust and substances, the stronger its oxidation, and vice versa;

3. When the variable valence element is in the most advanced state, it is only oxidized, when it is in the lowest valence state, it is only reductive, and when it is in the middle valence state, it has both oxidation and reduction;

4. Generally, when it is in the most advanced state, the oxidation is the strongest, and with the decrease of the valency, the oxidation is weakened and the reduction is enhanced.

The order of reductive properties of ions in aqueous solution at 25, pH = 0:

s²⁻ so₃(²i⁻＞fe²⁺＞br⁻＞cl⁻＞f⁻。

Order of ionic oxidation (25, pH = 1 in aqueous solution):

li note that sn, pb, not sn, pb hg correspond to hg instead of hg.

The oxidation of metal ions (to complement the brother above).

Oxidation: AG (1 valent) > Fe (3 valent) > Cu (2 valent) > Fe (2 valent) > Zn (2 valent) > Al (3 valent) > mg (2 valent).

In the same period, the reducibility of the metal from left to right decreases, and its cationic oxidation increases. The oxidation of non-metallic elements is enhanced, and the anion reduction is weakened.

From top to bottom with the main family. When the reducibility of the metal is enhanced, the cationic oxidation is weakened. The oxidation of non-metallic elements is weakened, and their anionic reduction is enhanced.

Cations are oxidizing and anions are reducing. Because cations are positive after losing electrons, correspondingly, to turn back into atoms, it needs to get electrons to become atoms, reduce the valency, and act as an oxidant, which is reducible. The anion gets electrons with negative valence, correspondingly, it needs to lose electrons to form atoms, and the valency should be increased, and it is a reducing agent, which is reducible.

For example, if the oxidation of the halogen element fluorochlorobromoiodine decreases sequentially, its anionic reducing property increases sequentially.

In the third week, the oxidation of the elements silicon, phosphorus, sulfur and chlorine increased in turn, and its anionic reducing property weakened in turn.

Strengthen, weaken, weaken, strengthen.

Cations, such as Mg2+, Cu2+, etc., are oxidizing. Anions, such as I-, S2-, etc., are reducible.

liter oxygen loss also (as a reducing agent).

Strong strong strong reduction oxidation is relative.

1. Common oxidizing ions:

Iron ions, copper ions, silver ions, permanganate ions, nitrate ions (in acidic environments), hypochlorite ions, chlorate ions, bromate ions.

2. Common reducing ions:

Sulfite ions, hydrosulfate ions, bromine ions, iodine ions, nitrite ions, oxalate ions.

Common strong oxidizing and strongly reducing ions.

【】Common oxidizing ions:

permanganate ions, manganate ions, dichromate ions, perchlorate ions, chlorate ions, hypochlorite ions, periodate ions, iodate ions, bromate ions;

Common reducing ions:

Sulfite ions, hydrosulfate ions, bromine ions, iodine ions, nitrite ions, oxalate ions.