Why is the ability of a substance to gain electrons called oxidation?

Originally, oxidation reaction was a narrow concept, which refers to the reaction of oxygen in combination with other substances. Later, it was recognized that oxygen gets electrons when it undergoes oxidation reactions, so the type of electron-gaining reactions is called oxidation reactions (generalized), and the ability of substances to obtain electrons is also called oxidation.

The valency increases, electrons are lost, and they are oxidized, and they are reducing agents.

The valency decreases, electrons are obtained, they are reduced, and they are oxidants.

After gaining and losing electrons, the outer electrons of the atom exist in a stable state.

To put it simply: because to gain an electron is to oxidize other substances, and to lose an electron is to be reduced by other substances.

This is related to the redox reaction learned in junior high school, from the perspective of oxygen gain and oxygen loss, Cuo + H2 = Cu + H2O, Cu in Cuo is an oxidant, oxidizing, H2 is reducing. From the perspective of electron gain and loss, the valency of Cu in Cuo is reduced, electrons are obtained, and they are reduced to be used as oxidants, which are oxidizing. In this way, the two are consistent.

This is consistent with oxygen gain and loss, valency rise and fall, and electron gain and loss. The reverse must be confusing.

Electrons. The valency is reduced.

is restored. Hence oxidizing.

The electrons are reduced and oxidized.

Lost electrons are oxidized and are reducible.

This is artificially prescribed, and for no reason.

Oxidation is the acquisition of electrons.

The oxidant has oxidizing properties, so in the process of the reaction, it is electrons, in this case, the valency will be reduced, because of the oxidizing properties, the reduction reaction occurs, it is reduced, and then the reduction product is generated. From another point of view, oxidizing means that it can oxidize other substances, that is, it causes other substances to lose electrons and gain electrons by itself.

Oxidation Strength Order:

1) It can be reacted according to redox. Oxidation: oxidant oxidation product;

2) Metal activity order: K>Ca>Na>Mg>Al>Mn>Zn>Cr>Fe>Ni>Sn>Pb(H)>Cu>Hg>Ag>Pt>Au reduction, corresponding to cationic oxidation enhancement;

3) Comparison of the order of non-metal activity: the oxidation of F, O, CI, BR, I, and S atoms decreased from left to right, while the anion reducibility increased.

4) The same element has strong oxidation in the general valence state, Fe3+>Fe2+Sn4+>Sn2+S(+6)>S(+4)>S(0)>S(-2).

Oxidation is the ability to gain electrons.

Conversely, the property of a substance that gives (loses) electrons is called reductiveness.

A reducing agent is a donor of electrons. The property of a substance that accepts (gets) electrons is called oxidation, and the oxidizing agent is the acceptor of electrons.

Due to the giving or accepting of electrons causes valency.

Therefore, it can be judged from the valency of the elements in the substance. The law is: the element is at its most **, it is impossible to give (lose) electrons, and it is only oxidizing; The element is at its lowest valence, it is impossible to accept (get) electrons, and it is only reductive.

The element is in an intermediate valence state, which may both give (lose) electrons and may accept (gain) electrons, so it is both oxidizing and reducing, but it mainly presents one property when reacting. If a substance contains a variety of elements, its properties are a comprehensive manifestation of the properties of these elements.

Oxidizing substances:

An oxidizing substance may not be burned by itself, but it can release oxygen, a chemical property that may cause or cause other substances to combust.

Comparatively reactive substance. Often refers to inorganic compounds.

contains ** state atomic structure.

and substances containing a dioxygen structure. It generally does not burn on its own.

However, if it encounters acid or is exposed to moisture, strong heat, or contact with other reducing substances and flammable substances, it can carry out oxidative decomposition reaction, release heat and oxygen, cause the combustion of combustible substances, and sometimes form a first-class mixture. The International Maritime Dangerous Goods Code classifies oxidizing substances as Class I dangerous goods. Oxidation reactions.

There are oxidants and reducing agents in the reduction reaction.

Electrolytes are compounds that are able to conduct electricity (ionize themselves into cations and anions) when dissolved in aqueous solution or in the molten state.

Metal oxides such as: Na2O, MGO, CaO, Al2O3, etc. are ionic compounds that are capable of conducting electricity in the molten state and are therefore electrolytes.

Electrolyte refers to a compound that can conduct electricity in water or in a molten state, and metal oxides are soluble in water, and chemical reactions generally occur, even if the solution can conduct electricity, it cannot be said that metal oxides are electrolytes, so it is generally judged by whether they can conduct electricity in a molten state.

Na2O Fe2O3 and other high temperature non-decomposition is an electrolyte (which is an ionic compound) If some metal oxides are covalent, they are not electrolytes. SO2 SO3 CO2 is not an electrolyte (belongs to the covalent compound).

Nao, Na2O, etc., are made up of a metal element and an oxygen element.

2kmNO4 + 16HCl = 2KCl + 2mnCl + 8H2O + 5Cl2KMno4 is the oxidant to gain electrons, the valency is reduced, the generation of MNO2HCL is the reducing agent, the loss of electrons, the valency increases, the generation of Cl2,1, KMno4 is the oxidant, the electrons are obtained, where the +7 valence MN is converted to +6 valence, becomes K2Mno4,2, and the MNO4- electrons become MN2+ Mn with 7 units of positive charge to get 5 electrons with negative valence becomes 2 units of positive charge, 0, oxidant is a substance that gets electrons before the dust knows how to understand.

2kmNO4+4HCl=2KCl+2mnCl+8H2O+5Cl2 It stands to reason that KMno4 is an oxidant, but is it KMNO4-

Oxidation refers to the ability of a substance to gain electrons. Substances in the ** state are generally oxidizing, such as: some non-metallic elemental O2

Cl2 part ** metals: Fe, Mno4

Wait a minute. Substances in the low-valent state are generally reducible (e.g., some metal elements (in middle school, metal elemental elements are only reducing, in fact, negative valence metals are very common), and some non-metal anions:

BR, I and so on. Substances in the intermediate valence state are generally both reducing and oxidizing (e.g., tetravalent sulfur).

1.The oxidation of non-metal atoms (or elemental elements) of the same main group elements (from top to bottom) gradually decreases, and the corresponding anion reduction gradually increases. The reducibility of metal atoms gradually increases, and the oxidation of corresponding cations gradually decreases.

2.In the same period, the elemental reducibility of the main group elements (from left to right) gradually decreased, the oxidation gradually increased, the cationic oxidation gradually increased, and the negative finger Shenzi gradually weakened.

3.According to the comparison of the acidity and alkalinity of the hydrate of the most ** oxide of the element, the stronger the acidity, the stronger the oxidation of the corresponding element, the stronger the alkalinity, and the stronger the reduction of the corresponding element.

Reducibility refers to the ability of atoms, molecules, or ions to lose electrons in a chemical reaction. The more electron-losing the particle belongs, the more reducible it belongs; Conversely, the weaker it is, the more non-reducible it is. For metal reducing agents, the reducibility of metal elements is generally consistent with the order of metal activity, that is, the more metal in the back, the less likely it is to lose electrons, and the weaker the reducibility.