Why is Cr 2+ reducing and Mn 3+ oxidizing when both have d 4 configuration?

Question

Why is Cr 2+ reducing and Mn 3+ oxidizing when both have d 4 configuration?, Cr 2+ is reducing as its configuration changes from d 4 to d 3 (half-filled t 2g level) but the change from Mn 3+ to Mn 2+ results in the half-filled (d 5 ) configuration which has extra stability., Mn 3+ has a higher effective nuclear charge than Cr 2+ ., Cr 2+ has a higher ionization energy than Mn 3+ ., Mn 3+ has a greater number of unpaired electrons in its d-orbitals.

MARKS App · Accepted Answer

Correct Option is : (A) Cr 2+ is reducing as its configuration changes from d 4 to d 3 (half-filled t 2g level) but the change from Mn 3+ to Mn 2+ results in the half-filled (d 5 ) configuration which has extra stability.

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