Question

Mn(iii) undergoes disproportionate reaction easily. Explain.

Answer 1

Explanation:

Disproportionation reaction is defined as a type of reaction in which same substance gets oxidized as well as reduced. This is a type of redox reaction.

$2A\rightarrow A'+A''$

Oxidation reaction means a substance looses its electrons. The oxidation state is increased in this process.

Reduction reaction is a type of reaction in which a substance gains electrons. The oxidation state gets reduced in this process.

$Mn^{2+}$ undergoes disproportionation reaction and the equation for the same follows:

$2Mn^{3+}\rightarrow Mn^{2+}+MnO_2$

Here, $Mn^{3+}$ is getting reduced to $Mn^{2+}$ and $Mn^{3+}$ is getting oxidized to $MnO_2$

Answer 2

Answer:

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).