The principle of disproportionation reaction, explained in terms of electrons gained and lost, thank

The so-called disproportionation reaction refers to the reaction in which the same element is both oxidized and reduced. In fact, the principle is very simple, that is, the element involved in the reaction provides one part of itself with electrons to another part of itself, the part that provides electrons is oxidized, and the part that obtains electrons is reduced. Let's take the simplest example of a disproportionation reaction.

Decomposition of hydrogen peroxide:

2 h2o2== 2 h2o + o2↑

The valency of hydrogen in this reaction.

It is not changed (+1 valence before and after), so it is the oxygen element that disproportionates.

Two molecules of hydrogen peroxide are assumed.

Decomposition, then there is 1 molecule of hydrogen peroxide in two oxygen to give 2 electrons, the valency rises from its own -1 valence to 0 valence, forming 1 molecule of oxygen, oxidation reaction occurs.

After the two electrons given out earlier allow the two oxygen in the hydrogen peroxide of the other 1 molecule involved in the reaction to be obtained, the valency is reduced from -1 valence to -2 valence, and the product water is formed, and a reduction reaction occurs.

In conclusion, the transfer of electrons in the disproportionation reaction takes place on the same element, catch that!

A disproportionation reaction is a reaction in which the valency of atoms of the same element rises and falls before and after the reaction formula.

In the reaction, if oxidation and reduction occur on an element in the same oxidation state inside the same molecule, the atoms of the element (or a part of the element are oxidized, and the other part is reduced. This own redox reaction is called disproportionation.

Some of them gain electrons and some of them lose electrons.

Disproportionation reaction, that is, in the reaction, if oxidation and reduction occur on an element in the same oxidation state inside the same molecule, so that one part of the atoms (or ions) of the element is oxidized and the other part is reduced. This own redox reaction is called disproportionation.

For example: 2Na2O2+2CO2====2Na2CO3+O2In this reaction, the O in Na2O2 is -1 valence, and he reacts with CO2 to produce Na2CO3 with O at -2 valence and O2 with O at 0valence

cl2+h2o=hclo+hcl

In this reaction, Cl2 is originally 0 valent.

After the reaction, one rises to +1 and the other decreases to -1.

Disproportionation is a type of chemical reaction in which the valency of an element rises and falls.

Determine whether disambiguation can occur.

The stability of an element with different oxidation numbers depends mainly on the standard electrode potential values of adjacent pairs. If the value of the adjacent pairs is consistent with the value of e right > e left, then the individual in the middle must be in an unstable state and can undergo a disproportionation reaction, and its product is two adjacent substances.

This is evident that if two adjacent pairs are used to form a battery, the reductive half-reaction of the pair from the middle species to the right species is the positive reaction of the battery, and the reaction to the left species is the negative reaction. The electromotive force of the battery is e = e right e left, if e right > e left , e > 0, it means that the battery reaction can be carried out spontaneously, that is, the intermediate species can undergo disproportionation reaction.

If on the contrary, e left > e right, then the individuals on both sides are unstable, and a reverse disproportionation reaction can occur, with the individuals at both ends being the reactants and the product being the one in the middle.

Find the electrode potential of an unknown pair.

Using the admixture of the Gibbs function variation, the electrode potential of any unknown pair can be calculated from the known electrode potential of several adjacent pairs.

A typical example is shown in the figure below:

The centering reaction refers to the redox reaction of different compounds of the same species of Acacia species, and the valency of that element is closer to the middle.

The disproportionation reaction is just the opposite of the centering reaction, the valency of an element spreads out to both sides, and the redox reaction of the same element in different valence states occurs, and the result is that the two valence states can only be close to each other or reach the same valence state at most, and there will never be a crossover phenomenon of ** state becoming low and low price state becoming high. -- The law of centering reaction.

Valence state centering means that the valency of the ** state decreases, and the valency of the low-price state increases, but it is impossible for the low state to rise more than the original ** state valence.