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

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Solution

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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C r^{2 +}

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How would you account for the following:

(i) Of the d⁴species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.

(ii) Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.

(iii) The d¹ configuration is very unstable in ions.

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