Oxidation and reduction Disproportionation

[Cheman]

We call reactions in which one species experiences both oxidation and reduction Disproportionation - but why do we chose this particular name?

Thanks.

 

[chem_tr]

The adjective disproportionate means "not proportioned, unsymmertrical, unsuitable to something in bulk, etc". In a redox reaction, if the two species undergoing redox are of the same kind (oxidation number), then we call this reaction as "disproportionation". There is an obvious unsymmetrical nature in this, if you study the reactions. This reaction is characteristic for species which are in a medium oxidation state; if there are oxidation states available below and above this state, disproportionation can be possible.

 

[ravenprp]

The term "disproportionation" is used in reference to reactions where a single species undergoes both oxidation and reduction simultaneously. This name is chosen because the oxidation and reduction reactions that occur within the same species are disproportionate in terms of the number of electrons involved. In other words, the species is both gaining and losing electrons at the same time, resulting in a disproportionation of its electron count. This is in contrast to typical oxidation and reduction reactions, where one species gains electrons (reduction) and another loses electrons (oxidation). Therefore, the term "disproportionation" accurately describes the unique aspect of these reactions where a single species experiences both oxidation and reduction.