How do you compare the magnitude of oxidation or reduction?

Look at the radius. Volatile electrons with large radius and strong reducibility. There are 10 sodium ion electrons and 11 protons, which adsorb the electrons very tightly, so it has a small radius and greater oxidation than sodium.

The radius of the same main group increases from top to bottom, the reducibility is enhanced, and the oxidation is weakened. Chloride ions have 18 electrons and 17 protons, and there are no 17 electrons and 17 protons with strong adsorption, so the chloride ion radius is large and its reducibility is strong. Perchloric acid is a strong acid, and it has the strongest oxidizing activity, but I don't know if the more oxygen there is, the stronger the oxidation.

In a redox reaction, oxidation: the oxidant is greater than the oxidizing product is greater than the reducing product is greater than the reducing agent. This is just a general rule, and some reaction principles may not conform to this law if volatile acids are made from volatile acids.

Oxidation, a method for judging the strength of reducibility.

1) Judging according to the chemical equation.

1) Oxidant (oxidizing) + reducing agent (reducing) === reducing product + oxidation product.

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) Comparison according to the order of material activity.

1) For metal reducing agents, the reducibility of metal elements is generally consistent with the order of metal activity, that is, the more metal is located behind, the less likely it is to lose electrons, and the weaker the reducibility.

Reducibility: K>Ca>Na>Mg>Al>Mn>Zn>Cr>Fe>Ni>Sn>Pb>(H)>Cu>Ag>PT>AU

2) The order of oxidation of metal cations.

k+mno2>o2

4) Judge according to the valence of oxidation products.

When the reducing agent containing valence elements acts on different oxidants under similar conditions, the oxidation strength of the oxidant can be judged according to the valence state of the oxidation products. Such as:

2Fe+3Cl2== (ignition) 2FeCl3

Fe+S== (heated) Fes

Oxidation: Cl2>s

5) Judging according to 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) Synchronous main group elements (from left to right).

The elemental reducibility is gradually enhanced, and the oxidation is gradually enhanced.

The cation oxidation gradually increased, and the anion reduction gradually decreased.

6) 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.

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.

Upstairs is a talent...

Let's simply look at it according to the periodic table.

1. Oxidation vs reduction.

2. Oxidation: the ability of a substance to obtain electrons. Reducibility: The ability of a substance to lose electrons.

3. The strength of oxidation and reduction of a substance depends on the difficulty of its electron gain and loss, and has nothing to do with the number of electrons gained and lost.

4. The method of judging the strength of oxidation and reducibility, the order of element activity, the order of metal activity, according to the order of metal activity, the reduction of the element is getting weaker and weaker, and the oxidation of the corresponding cation is getting stronger and stronger.

5. Order of non-metal activity: According to the order of non-metal activity, the oxidation of the element is getting weaker and weaker, while the reduction of the corresponding anion is gradually increasing. Pat the head according to the position of the element in the periodic table.

6. Elements of the same period: the reducibility of the element is gradually weakened, and the oxidation is gradually enhanced. The oxidation of the corresponding cation gradually increases, while the reduction of the anion gradually decreases.

7. Elements of the same main group: the oxidation of the element is gradually weakened, and the reduction of the corresponding anion is gradually enhanced.

Methods for judging the strength of reductivity:

1. Using valency to compare the oxidation and reducing strength of the substance, the strength of the oxidation and reduction of different valence substances formed by the same element is: the lowest valence state of the element only has reduction, and the intermediate valence state of the element has both oxidation and reduction.

2. Use the different activity of elements to compare the strength of oxidation and reduction of substances. For metals, the more reactive the metal (the stronger the metalicity), the stronger the reduction of its elemental matter. For non-metals, the more active the non-metals are (the stronger the non-metals), the weaker the reducing properties of the anions.

3. Use redox reaction to compare the oxidation and reducing strength of the substance, and the general redox reaction, reducibility: reducing agent reduction product. For galvanic cell reactions, there are:

Reducibility Comparison: Anode Material Cathode Material. In the case of electrolysis reactions, the more easily discharged (electron-loss) anions at the anode during electrolysis in the same electrolyte solution, the stronger their reducibility.

4. The difficulty of the reaction at the same starting point is used to compare the strength of the oxidation and reducibility of the substance, and the easier the reaction with the same oxidant, the stronger the reducing agent is (indicating that it is easier to lose electrons).