Question

Why cr2+ is reducing while mn3+ is oxidising while both have d4 configuration?

Answer 1

Explanation:

Cr2+ is strongly reducing in nature. It has a d4configuration. While acting as a reducing agent, it gets oxidized to Cr3+ (electronic configuration, d3). In the case of Mn3+ (d4), it acts as an oxidizing agent and gets reduced to Mn2+ (d5).

Answer 2

$\large\underline\bold{ANSWER \red{\huge{\checkmark}}}$

Cr2+ is strongly reducing in nature. It has a d4configuration. While acting as a reducing agent, it gets oxidized to Cr3+ (electronic configuration, d3). In the case of Mn3+ (d4), it acts as an oxidizing agent and gets reduced to Mn2+ (d5).

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