What is a disproportionation reaction and how can you tell if a disproportionation reaction can occu

Difference Between Autooxidation Reaction and Disproportionation Reaction:

Self-redox reaction refers to the redox reaction in which both the oxidant and the reducing agent are the same substance, and electrons are transferred between different elements or the same element in the substance.

All of them are self-redox reactions.

Disproportionation, which refers to the redox reaction that occurs between the same element in the same valence state in the molecule of the same substance. Elements in the same valence state have "divergences in valency changes" during the redox reaction, with some increasing and some decreasing. Therefore, example 3 is a disproportionation reaction; However, example 2 is not a disproportionation reaction, because in this self-redox reaction, the transfer of electrons occurs between the same elements, but not between the same elements in the same valence state; The element in which the disproportionation reaction occurs must have the corresponding ** state and low-valence compounds, and the disproportionation reaction only occurs on the elements in the intermediate valence state.

Fluorine (F2) has no disproportionation because the fluorine element is the most electronegative, and there is no positive valency, only negative valency.

In summary, it can be seen that the autoredox reaction and the disproportionation reaction are both redox reactions between the same species, and the disproportionation reaction is a kind of self-redox reaction, but the autoredox reaction is not necessarily a disproportionation reaction.

It is an element that changes from one valence state to two or more valence states after the reaction.

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:

In the reaction, if oxidation and reduction occur on an element that is in the same oxidation state inside the same molecule, the element.

One part of the atom (or ion) of the element is oxidized and the other part is reduced. This self-oxogenic spring reduction reaction is called disproportionation. This remorse reaction is also known as the Cannizzaro reaction.

For example, Cl2+H2O=HCl+HCl

In this reaction, Cl2 is originally 0 valent.

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

The disproportionation reaction is a type of [1] chemical reaction in which the valency of an element rises and falls. As opposed to the centering reaction.

In the reaction, if oxidation and reduction occur on an element in the same oxidation state inside the same molecule, so that part of the atom (or ion) of the element is oxidized and the other part is reduced, then this own redox reaction is called disproportionation.

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

The disproportionation reaction generally requires an acidic or alkaline reaction environment to be carried out.

One of the redox reactions, such as positive 4-valent sulfur, can produce sulfur elements or sulfate, and the valence shifts to both sides.

Redox reactions that occur between the same element in the same valence state in the same substance (the disproportionated element will increase in price in part and decrease in price in part). This reaction is called disproportionation, in which the valency of the same element goes from an intermediate valence state to a decrease in part, such as sodium peroxide with water, and the valency of O changes from -1 to 0 and -2