Why do some substances without oxygen also have oxidation, and what is the reductive reduction

Oxygen is very easy to get electrons due to its structural characteristics, and oxygen is very common in general substances, many substances containing oxygen have a strong electron-gaining ability, so people call this electron-gaining ability oxidation, but later found that many substances without oxygen-containing elements also have this ability. However, the name of oxidation has been conventional, and this name can well illustrate this characteristic, (mentioning oxygen can think of its strong electron ability) is retained, and the reductive reduction is the valence state, and the ** state is reduced to the low price state, which is for the oxidation of the ** state. Reducing substances provide electrons relatively.

First of all, you have to figure out the nature of oxidation and reduction.

Oxidation refers to the ability of a substance to gain electrons. Substances in the ** state are generally oxidizing.

For example, some non-metal elements: O2, Cl2 and some metal cations: Fe3+, Mno4-(Mn7+) and so on.

Substances in a low-price state are generally reducible.

Such as: some metal elements: Cu, AG and some non-metal anions: br-, i-, etc.

Oxidant --- reduction product Oxidant electrons, valency decreases, is reduced, reduction reaction occurs, reducing agent --- oxidation product Reducing agent loses electrons, valency increases, is oxidized, oxidation reaction occurs Why is it oxidized if it gets electrons, why is it called so.

It's conceptual stuff, there's no why, right? It's just a rule or convention.

As long as the valency decreases, it is a reduction reaction and has oxidizing properties.

Because the oxidation of the oxidation product cannot be greater than that of the oxidant, the reducing product cannot be greater than the reducing agent.

Valence state centering law: when redox reactions occur between different valence states of the same element, the change of valence states is "only close, not crossing".

For example: KCLO3+6HCl=3Cl2+KCL+3H2O.

The valence is high or, and the negative monovalent element cannot reduce the 3rd valence to the 1st valence and itself to the positive 5th valence. That is to say, the original high, after the reaction, the valency is still relatively high, and the low is still low. (Exceptional cases are equal).

For example: KCLO3+6HCl=3Cl2+KCL+3H2O.

Valence is the property of an element that manifests itself when one atom is atomized with other elements.

In general, the valence of valence is equal to the number of electrons gained and lost by each atom during compounding, that is, the number of electrons gained and lost when the element can achieve a stable structure, which is often determined by the electronic configuration of the element, mainly the outermost electron configuration, and of course, it may also involve the substable structure composed of sublayers that can be achieved by the subouter shell.

in redox reactions.

The substance that obtains oxygen in it is called a reductive pacemaker, which has reductive properties; The substance that is deoxygenated by the noisy rock is called an oxidant, which has oxidizing properties.

Fe2O3+3Co=High temperature 2Fe+3CO2, where Fe2O3 loses (gets, loses) oxygen, is an oxidizing agent, and has oxidizing properties.

A reduction reaction occurs; CO obtains oxygen, which is the original agent for jujube chop, which is reducible and oxidizes itself.

Broadly speaking, oxide refers to a binary compound composed of oxygen and another chemical element, such as carbon dioxide, calcium oxide, carbon monoxide, etc. However, compounds formed by the combination of oxygen and fluorine, which are more electronegative, are generally referred to as fluorides rather than oxides. There are only two elements in oxides, one of which is oxygen.

The original material, namely 2-amino-4 acetaminoanisole, is an important coupling component intermediate of disperse dyes.

To put it simply, the valency is at the most **, only oxidation; At the lowest price, only reductiveness; Those in the intermediate valence state are both oxidizing and reducing. For example, Fe3+, only oxidizing; Fe2+, oxidizing (oxidizing Zn elemental), reducing (reducing Fe3+ or Cl2); Fe elemental, only reducible.

In fact, it can also be seen from the above answer that this statement can only be used for simple ions. For complex ions, such as SO42-, where S is +6 valence, the most **, but O is -2 valence, the lowest valence, although SO42- generally exhibits oxidation, it cannot be ruled out that it exhibits reductivity;

For compounds, this is even clearer, in general, compounds must have positive and negative elements. Positive elements can certainly exhibit oxidation, while negative valence elements can certainly exhibit reductivity. For example, H2O, when electrolyzed, shows both oxidation and reduction.

Judging by the valence state of the element:

If the element in the substance has the most **, the element is only oxidized (such as metal cations: Cu2+, Ag+, Na+, Fe3+ and Mn element in KMno4, etc.); When an element in a substance has its lowest valence, the element has only reducing properties (such as metal elements: Na, Mg, Al, Zn, Fe, non-metal anions S2-, I

Cl-, Br- and their compounds NH3 in N, etc.); When an element in a substance has an intermediate valence, the element is both oxidizing and reducing. Generally, for the same element, the higher the valence state, the stronger its oxidation; The lower the valence state, the more reducible it is (the opposite of the positive valence halogen).

It can be judged from the following common important oxidants and reducing agents to find the valence. 

Oxidant active non-metallic elements: X2, O2, S

**Metal ions: Fe3+, Sn4+

Inactive metal ions: Cu2+, Ag+ Others: Ag(NH3)2+, new Cu(OH)2

Oxygenated compounds: NO2, N2O5, MNO2, Na2O2, H2O2, HCO,

HNO3, concentrated H2SO4, Naclo, Ca(clo)2, KCLO3,

kmno4, aqua regia.

Reductant active metal elements: Na, Mg, Al, Zn, Fe

Certain non-metallic elements: C, H2, S

Low-valent metal ions: Fe2+, Sn2+

Anions of non-metals and their compounds:

s2-、h2s、i

hi、nh3、cl-、hcl、br-、hbr

Low-valent oxygenates:

co、so2、h2so3、na2so3、na2s2o3、nano2、

H2C2O4, organic matter containing -CHO: aldehyde, formic acid, formate, a certain ester of formate, glucose, maltose, etc.

It can be used as both an oxidant and a reducing agent: S, SO32-, HSO3-, H2SO3, SO2, NO2-, Fe2+, etc., and organic substances containing -CHO are expected to be adopted.

Some substances can be used as both oxidants and reducing agents, such as Na2O2, H2O2, S, Fe2+, SO2, etc., but they are mainly based on one property: Na2O2, H2O2, S are mainly used as oxidants, and Fe2+ and SO2 are mainly used as reducing agents.

Most. For example, if a substance can react with sodium metal to form a monovalent sodium compound, then the sodium is oxidized, and the substance is oxidizing.

At the same time, the substance can react with F to generate monovalent fluoride, then the fluorine is reduced, and the substance has reducibility.

Obviously, a lot of substances can react like this.