Why cr 2+ is stronger reducing but mn is strongly oxidising?
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Cr2+ is strongly reducing in nature. It has a d4configuration. While acting as a reducing agent, it gets oxidized to Cr3+ (electronic configuration, d3). This d3configuration can be written as t32g 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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