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Explain why Cr2+ is reducing but Mn3+ is oxidising while both ions have d4 configuration?

Cr2+ is reducing as its configuration changes from d1 to d3 while on the other hand oxidation of Mn from Mn2+ to Mn3+ results in half filled d5 configuration which is much more stable.

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Hi sadhyaa..

Cr2+ is reducing in nature. It had a d4 configuration. While acting as a reducing agent,it gets oxidized to Cr3+ which has electronic configuration d3 . This d3 configuration Can be written as t2g to the power of 3 which is a more stable configuration

In case of Mn3+ which is a n oxidising agent gets reduced to Mn2+ . This has an exactly half filled d orbital and is highly stable

Hope it helps!!

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