Why do the reasons of cr2+ being reducing and mn2+ being oxidising are different? I know the reasons. my question is why do they have different reasons for both of them? Why couldn't they have same reason and outcome since both of them have d4 configuration!
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Cr2+ is strongly reducing in nature. It has a d4 configuration. While acting as a reducing agent, it gets oxidized to Cr3+ (electronic configuration, d3). This d3 configuration can be written as 3t2g configuration, which is a more stable configuration.
In the case of Mn3+ (d4), it acts as an oxidizing agent and gets reduced to Mn2+ (d5). This has an exactly half-filled d-orbital and has an extra-stability.
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