How would you account for the following: (i) Cr^2+ is reducing in nature while with the same d-orbital configuration (d^4) Mn^3+
How would you account for the following:
(i) Cr2+ is reducing in nature while with the same d-orbital configuration (d4) Mn3+ is an oxidising agent.
(ii) In a transition series of metals, the metal which exhibits the greatest number of oxidation occurs in the middle of the series.
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(i) Cr2+ is reducing as its configuration changes from d4 to d3, a more stable half filled t2g configuration while Mn3+ is oxidising as Mn3+ to Mn2+results a more stable half filled d5 configuration.
(ii) It is due to greater number of unpaired electrons in (n–1)d and ns orbitals at the middle of the series.
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