Oxidation and reduction Disproportionation

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Disproportionation refers to a specific type of redox reaction where a single species undergoes both oxidation and reduction, resulting in the formation of two different products. The term "disproportionate" highlights the unsymmetrical nature of this process, as it involves a single reactant that is not equally divided in terms of oxidation states. This reaction typically occurs with species in a medium oxidation state, where there are available oxidation states both below and above the medium state. The unique characteristics of disproportionation reactions make them significant in understanding redox chemistry.
Cheman
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We call reactions in which one species experiences both oxidation and reduction Disproportionation - but why do we chose this particular name?

Thanks. :smile:
 
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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.
 

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