On the question of oxidation vs acidity, the nature of acidic oxides

The most oxidizing is HCO4 and the weakest is HCO4.

The higher the valency of Cl, the more acidic its oxygenated acid is.

Oxidation and valency have nothing to do with it, but with the stability of this valence state.

Acidic oxides are a class of oxides that react with alkalis to form only one type of salt and water. Most of the non-metallic oxides are acidic oxides, and the ** oxides of some transition elements (such as CRO3, Mn2O7, etc.) are also acidic oxides. Acidic oxides belong to anhydrides, for example, SO2 is called sulfur anhydride, SO3 is called sulfur anhydride, CO2 is called carbon anhydride, and acetic anhydride is an acid anhydride but not an acid oxide.

The hydrate corresponding to the acidic oxide is oxygenated acid, for example, the hydrate corresponding to SO3 is H2SO4, the hydrate corresponding to CO2 is H2CO3, and the hydrate corresponding to SiO2 is H2SiO3. Most of the acidic oxides can be directly combined with water to form oxygenated acids, and a few acidic oxides (SiO2) cannot react directly with water. Acid oxides are generally prepared by the oxidation of non-metallic direct sales or the thermal decomposition of oxygenated acids and oxygenates.

What are the acidic oxides? There are carbon dioxide CO2, sulfur dioxide SO2, silica SIO, sulfur trioxide SO3, phosphorus pentoxide P2O5, manganese heptaoxide Mn2O7 and chromium trioxide CRO3, etc., because there are too many, here will not list them all, if you want to know what else there are in addition to these punches, you can look up information on the Internet to understand.

The concept of acidic oxides. Acidic oxygens are a class of oxides that react with water to form acids or alkalis to form salts and water. The Concept of Basic Oxides:

Basic oxides are oxides that dissolve in water and form only one base or react with acids to produce only salts and water. Properties of acidic oxides: Most of them can react with water to form corresponding acids (except for some oxides such as silica SiO2 that cannot react with water).

Reacting with a base produces only one type of salt and water. Reacts with alkaline bright oxides. Note:

Most of the non-metallic oxides are acidic oxides. Only oxygenated acids have acidic oxides. Carbon monoxide, nitric oxide, nitrogen dioxide are not acidic oxides.

Basic oxides: basic oxides are all oxides of metal elements, their alkalinity is very different, some (such as sodium, calcium, magnesium oxides) are easy to combine with hydration and can quickly and completely neutralize with all the acidic substances.

Heavy metal oxides are only weak bases, which are insoluble in water or do not interact with water and can only neutralize with more acidic substances. There is a transition from basic oxides to acidic oxides, i.e. amphoteric oxides (e.g. alumina) are both acidic and basic.

Properties of Acid Oxides:1. Most of them can react with water to form corresponding acids (except for some oxides that cannot react with water, such as silica SiO2).

2. Reaction with alkali produces only one kind of salt and water.

3. Reaction with alkaline oxides.

Other characteristics: 1. Most of the acidic oxides can be directly combined with water to form oxygenated acids.

2. Oxygenated acids can also be decomposed by heat to form acidic oxides.

3. The most important basis for judging acidic oxides is that the valency of each element remains unchanged before and after the chemical reaction.

4. It is composed of two elements, one of which is oxygen.

Special case analysis. Silica is a special kind of acidic oxide.

Silica can react with hydrofluoric acid in liquid, but not with water (etching glass).

Most of the acidic oxides are non-metallic leakage oxides. Most of the non-metallic oxides are acidic ridge oxides.

Only oxygenated acids have acidic oxides. Carbon monoxide, nitric oxide, nitrogen dioxide are not acidic oxides.

Most of what the Spirit of Light said is correct, but it's too complicated?

Are acidity and oxidation the same thing?

To put it simply: acidic --- in the aqueous solution of any substance, there are hydrogen ions and hydroxide ions, when the concentration of hydrogen ions in the solution is greater than the concentration of hydroxide ions, the solution is acidic--- this world is not usually said acidic.

If you are in junior high school, it is enough to know that the acid solution is acidic, and the acidity refers to the ease with which the acid ionizes hydrogen ions in an aqueous solution. For example, hydrochloric acid, sulfuric acid, and nitric acid are strong acids, phosphoric acid is a moderately strong acid, and carbonic acid is a weak acid.

Oxidizing --- substance or ion gets electrons in a chemical reaction, we say that the substance or ion has undergone an oxidation reaction and is oxidizing. The strength of oxidation is related to how easy it is to obtain electrons in a chemical reaction. The easier it is to obtain electrons, the stronger the oxidation.

The relationship between the two: Since all acids can ionize hydrogen ions, hydrogen ions themselves have weak oxidation, so acids have oxidizing properties. However, it should be noted that what we usually call "oxidizing acid" refers to the strong oxidation of the anions corresponding to the acid in the Huaxue reaction, not the weak oxidation of the hydrogen ions themselves.

For example, nitric acid and concentrated sulfuric acid have strong oxidizing properties, which means that nitrate, sulfate (concentrated sulfuric acid) +5-valent nitrogen and +6-valent sulfur have strong oxidizing properties.

I don't know if I made it clear?

Acidity mainly refers to the fact that it can react with alkali metals to form the corresponding salt and hydrogen, or react with alkali to form salt and water, and the valence does not change, and oxidation mainly refers to the properties of reactants whose valence decreases after the reaction.

Acidity is the negative logarithm of the concentration of hydrogen ions in a solution (acid in the general sense); Oxidation is the ability of a substance to combine with hydrogen.

The definition of acid in the middle school range is based on the Arrhenius definition of ionization theory, i.e., the general properties of acids are expressed by the chemical properties of H+.

If there is a chemical reaction in the acid, and the atomic clusters in the equation do not change valence, then it is possible that H+ has undergone a chemical change, and there are two types: H+ is reduced, such as a displacement reaction with a more active metal; H+ is not reduced but is involved in reactions, e.g. and OH- neutralization to produce water, etc. These are all manifestations of acidity.

It should be noted that the above actually ignores the non-redox reaction about acid roots, such as H2S2O7 + H2O = 2H2SO4. At this time, H+ is not involved in the reaction, so it is not a manifestation of acidity. Therefore, it is possible to say that "if the valency of the atomic cluster does not change through the equation, it may be that the acidity of the acid is expressed" rather than "if the valency of the atomic cluster does not change through the equation, it must be the acidity of the acid".

1. Oxidizing acids refer to acids that exhibit oxidation by obtaining electrons from non-metal atoms in the positive valence state of acid molecules or acid ions. Contains concentrated and dilute nitric acid, concentrated sulfuric acid, hypochlorous acid, chloric acid, chlorous acid, perchloric acid, nitrous acid, permanganese acid oxidizing acid is generally oxygenated acid, which refers to the central element in the acid in addition to hydrogen and oxygen elements in the chemical reaction to show strong oxidation. The more common ones are:

Concentrated and dilute nitric acid, concentrated sulfuric acid, permanganese acid, hypochlorous acid, chloric acid, chlorous acid, perchloric acid, nitrous acid, etc. Oxidizing acids refer to specific substances.

The strong oxidizing properties of oxidizing acids are manifested in:

It can react with the metal elements ranked after hydrogen in the common metal activity order table, and can oxidize the variable metal from zero to a higher valence state. For example:

Cu + 2H2SO4 (concentrated) = CuSO4 + SO2 + 2H2O (heating) 3AG+4HNO3 (dilute) = 3AGno3+NO +2H2O Second, the oxidation of acid refers to one of the general properties of acid, in which hydrogen ions (H+) can reflect oxidation and can react with most metals, and the oxidation of acid refers to the properties of substances.

Oxidation of acid: reflected in the H+ ionized by acid, for example: Zn + H2SO4 = ZnSO4 + H2 Zn + 2HCl = ZnCl2 + H2 Hydrochloric acid and sulfuric acid are oxidizing.

Oxidizing acid: refers to the non-H element that exhibits oxidation, and such acid is called oxidizing acid, such as Hno3, concentrated Hs2O4, HMNO4, etc.

Oxidation of acids: Acids are oxidizing (the valency of H+1 valence can be reduced), and acids exhibit oxidation (they can be hydrogen or other elements).

Non-oxidizing acids: refers to the oxidizing element is the H element, such acids are called non-oxidizing acids, such as HCl, dilute HS2O4, H2CO3 and so on.

The oxidizing nature of an acid is the nature of an acid, and an oxidizing acid is a type of acid.

The oxidation of an acid refers to the oxidation of the hydrogen ions in it.

Oxidizing acids are acids that have oxidizing properties.