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Disproportionation is a specific type of redox reaction in which a species is simultaneously reduced and oxidised to form two different products. ==Overview== For example, the UV photolysis of mercury(I) chloride Hg2Cl2 → Hg + HgCl2 is a disproportionation. Mercury (I) is a diatomic dication . In this reaction, the chemical bond in the molecular ion is broken, and one mercury atom is reduced to mercury(0), and the other is oxidized to mercury(II). A similar type of reaction, but in which no element changes oxidation number, is the acid-base disproportionation reaction observed when an amphiprotic species reacts with itself. Two common examples for conjugated bases of polyprotic acids such as bicarbonate and dihydrogenophosphate are respectively: :2 → + H2CO3 :2 → + H3PO4 The oxidation numbers remain constant in these acid-base reactions: O = −2, H = +1, C = +4, P = +5. This is also called autoionization. Another variant on disproportionation is radical disproportionation, in which two radicals form an alkane and alkene. 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Disproportionation」の詳細全文を読む スポンサード リンク
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