Question

Mn(iii) undergoes disproportionate reaction easily. Explain.

Answer 1

Dear User,
Disproportionation reaction are those in which the same substance undergoes oxidation as well as reduction.
$2{\mathrm{Mn}}^{3+}\to {\mathrm{Mn}}^{2+}+{\mathrm{MnO}}_2$
Here, Mn(III) undergoes disproportionation to form Mn(II) and Mn(IV).
Electronic configuration of Mn(III)= 3d⁴
Electronic configuration of Mn(II)= ​ 3d⁵
Since, +2 oxidation state is more stable as compared to +3 oxidation state due to stable half filled electronic configuration, therefore Mn(III) disproportionates to Mn(II).