How to compare the strength of oxidation???

1 Judging by the chemical equation.

1) Oxidant (oxidizing) + reducing agent (reducing). Reduction products + oxidation products. Oxidants --- reduction products.

Electrons are obtained, the valency decreases, they are reduced, and a reduction reaction occurs. Reducing agents --- oxidation products. Electrons are lost, valency increases, is oxidized, and oxidation reactions occur.

Oxidation: Oxidizing agent" oxidation product. Reducibility:

Reducing agent》 reducing product.

2) It can be judged according to the oxidant and reducing agent in the same reaction. Oxidizing: Oxidizing agent" reducing agent. Reducibility: Reducing agent》 Oxidant.

2 Judging by the periodic table.

1) Elements of the same main family (from top to bottom). The oxidation of non-metal atoms (or elementals) 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) Elements of the main group of the same period (from left to right). The elemental reducibility gradually weakened, and the oxidation gradually increased. The cation oxidation gradually increased, and the anion reduction gradually decreased.

3 Comparison according to the strength of the acidity and alkalinity of the elements.

Comparison of the acidity and alkalinity of hydrates according to the most ** oxides of the elements. The more acidic it is, the more oxidizing the corresponding element is. The stronger the alkalinity, the stronger the reduction of the corresponding element.

4 Judging by the electrode reaction of the galvanic battery.

Two different metals make up the poles of a galvanic cell. The negative metal is the pole where electrons flow out, and the positive metal is the pole where electrons flow in. Its reducibility: negative metal》 positive metal.

First, it can be judged according to the size of the atomic radius, the smaller the atomic radius, the stronger the oxidation, the elements of the same main group, the higher the atom oxidation, the stronger the oxidation, and the stronger the oxidation at the bottom of the metal activity order table In aqueous solution, the simplest way is to judge by the electrode potential.

There are several ways to compare the strength of oxidation.

The stronger the ability of the particle to gain electrons, the more oxidizing it is.

The stronger the non-metallic property, the stronger the oxidation activity.

The higher the number of charges, the stronger the oxidation.

The method of judging the strength of oxidation is as follows:

1) Judging according to the chemical equation.

1) Oxidant (oxidizing) + reducing agent (reducing) = = reducing product + oxidation product Oxidant --- reducing product Electrons, valency decreases, is reduced, and a reduction reaction occurs Reducing agent --- oxidation product Electron loss, valency increases, oxidation, oxidation reaction occurs Oxidation: oxidant》Oxidation product Reducibility: reducing agent》Reducing product (2) According to the oxidant and reducing agent in the same reaction, the reducing agent can be judged Oxidation:

Oxidant》 Reducing agent Reducibility: Reducing agent" oxidant.

2) Comparison according to the order of material activity.

For metal reducing agents, the oxidation of metal elements is generally opposite to the order of metal activity, that is, the more metal in the back, the less easy it is to obtain electrons, and the stronger the oxidation.

3) Judged according to the reaction conditions.

When different oxidants react with the same reducing agent, if the valence state of the oxidation products is the same, it can be judged according to the difficulty of the reaction conditions. The easier the reaction, the more oxidizing the agent will be oxidized.

4) Judge according to the valence of oxidation products.

5) Judging according to the periodic table.

1) The oxidation of non-metal atoms (or elementals) 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 the corresponding cations gradually decreases (2) The elemental reducibility of the main group elements of the same period (from left to right) gradually decreases, and the oxidation gradually increases The cationic oxidation gradually increases, and the anion reducibility gradually decreases.

6) Comparison according to the strength of the acidity and alkalinity of the elements.

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, the stronger the reduction of the corresponding element.

7) Judged according to the electrode reaction of the galvanic battery.

Two different metals make up the poles of a galvanic cell. The negative metal is the pole where electrons flow out, and the positive metal is the pole where electrons flow in. Its reducibility: negative metal》 positive metal.

8) Judged according to the concentration of the substance.

The greater the concentration of an oxidizing (or reducing) substance, the stronger its oxidizing (or reducing) and vice versa.

9) Judge according to the valence state of the element.

Generally speaking, valence elements are only oxidized when they are in the most ** state, only reducing when they are in the lowest valence state, and both oxidizing and reducing when they are in the intermediate valence state. Generally, when it is in the most advanced state, the oxidation is the strongest, and with the decrease of the valency, the oxidation weakens and the reduction is enhanced.

Oxidation refers to the ability of a substance to lose electrons in a chemical reaction, strong oxidizing agents have strong oxidizing properties, while weak oxidizing agents are relatively weak.

The following is a general order of the oxidation of some common substances:

1.Fluorine (F2): Fluorine is the strongest oxidizing agent, and it reacts directly with most elements.

2.Oxygen (O2): Oxygen has strong oxidizing properties and can react with many elements and compounds at room temperature.

3.Chlorine (Cl2): Chlorine is a common oxygen relieving agent, which can oxidize many substances.

4.Ozone (O3): Ozone is a strong oxidizing agent, which is more reactive than ordinary oxygen molecules.

5.Oxides: such as peroxides (e.g. H2O2) and nitrogen peroxide (e.g. N2O4), which are highly oxidizing.

6.Manganese (Mn) and Chromium (Cr): Manganese and chromium have strong oxidation in the ** state.

It should be noted that the strength of oxidation is also affected by other factors, such as reaction conditions and the nature of the reactants. Therefore, in specific chemical reactions, the relationship between the strength and weakness of oxidation may change.

Oxidation is a relative concept and is often used to describe a substance's ability to capture oxygen in a chemical reaction. There is no fixed order of oxidation, because the strength of oxidation depends on the reaction and environment of the body. However, we can roughly understand the relationship between the strength and weakness of oxidation according to the behavior of some common substances in redox reactions.

Here are some common oxidizing agents, in order of relative oxidation from highest to lowest (note that this is not a strict order, and the actual oxidation may vary depending on the reaction and environment):

1.f2 (fluorine gas).

2.Cl2 (chlorine).

3.BR2 (bromine).

4.i2 (iodine).

5.O3 (ozone).

6.HNO3 (nitric acid).

7.HCO4 (perchloric acid).

8.MNO4- (permanganate).

9.CR2O72- (dichromate).

10.H2O2 (hydrogen peroxide).

In the meantime, here are some common reducing agents, ranked from high to low in order of relative reduction:

1.Na (sodium).

2.mg (magnesium).

3.al (aluminum).

4.Zn (zinc).

5.Fe (iron).

6.SN (tin).

7.PB (lead).

8.AU (gold).

9.CU (copper).

10.ag (silver).

Please note that these sequences are for general conditions only, and actual oxidation may vary depending on the reaction and environment. In practical applications, specific chemical reactions need to be considered to determine the oxidation of one substance relative to another.

The order of oxidation from strong to weak is as follows:

1. The oxidation of metal ions in the order from strong to weak: silver ions, ferric ions, copper ions, divalent lead ions, divalent iron ions, divalent zinc ions, aluminum ions, magnesium ions, sodium ions, calcium ions, potassium ions.

2. The order of oxidation of halogen elements from strong to weak: fluorine gas, chlorine gas, bromine gas, iodine gas.

3. The oxidation of common substances as oxidants is in the order from strong to weak: permanganate, hydrogen peroxide, manganese dioxide; Hypochlorite, chlorite, perchlorate.

Reducibility from strong to weak: sulfur dioxide, thiocyanide, iodide, bromine, chloride, fluoride.

Tips for chemical reduction and oxidation:

The element is in its most ** state, only oxidizing. The element is in the lowest valence state, and only reductive. The element is in an intermediate valence state and is both oxidizing and reducing.

The oxidation of the oxidation product is less than that of the oxidant, and the reduction of the product is less than the reduction of the reducing agent.

In the order of metal activity from left to right, the reducibility gradually decreases, and the oxidation gradually increases.

The stronger the oxidation of the element, the weaker the reduction of the corresponding anion. The stronger the reduction of the element, the weaker the oxidation of the corresponding cation.

One. Non-metallic elemental oxidation: In general, the strong non-metallic nature of the element corresponds to the strong elemental oxidation.

For example: non-metallic F>Cl>Br>i>Sthen oxidizing F2>Cl2>Br2>I2>S

1.The non-metallic properties of the elements in the same period (horizontal, from left to right) increase, and the elemental oxidation increases.

Second Cycle: (Elemental Oxidation) N2S>Se>Te; (elemental non-metallic) o>s>se>te

Seventh main group: (elemental oxidizing) F2>Cl2> Br2>i2; (elemental non-metallic) f>cl>br>i

In addition, it should be noted that the non-metallic properties of oxygen are slightly stronger than those of chlorine; However, the oxidation of elemental matter is the opposite, oxidation (Cl2>O2), that is, chlorine is slightly more oxidizing than oxygen; However, ozone O3 is much more oxidizing than Cl2.

Two. Oxidation of metal cations:

The more oxidizing the metal is at the bottom of the order of activity.

Oxidizing strong) Ag > Hg2 > Cu2 >H > Pb2 > Sn2 >Fe2 >Zn2 >Al3 ...The oxidation is very weak).

The oxidation of Fe3 is between Hg2 and Cu2: Hg2 >Fe3 >Cu2

Three. The oxidation of the compound (you must look at the pH of the solution, the oxidation of the compound has a great relationship with the pH):

In general:

F2>>O3>> Kmno4(H)>Cl2>K2Cr2O7(H)>mNO2>Hno3> concentrated H2SO4>H2O2>O2>Br2>AG>Fe3 >I2>Cu2 >H

Oxidants, which are weaker than hydrogen ions, are generally considered to be non-oxidizing!