)With same d-orbital configuration Mn(3+) is an oxidizing agent whereas Cr(2+) is a reducing agent. why
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If something is behaving as reducing agent, that means, it itself is undergoing oxidation , that is , there is loss of electron. While for reduction there is gain of electron.
So we can explain this observation:
Cr2+ has the configuration 3d4. It can lose electron to form Cr3+ which has stable 3d3configuration ( as it has half -filled t2g level). Hence , it is reducing.
On the other hand, Mn3+ also has 3d4configuration but it can gain electron to form Mn2+ which has stable 3d5 configuration (as it is exactly half - filled). Hence oxidising.
So we can explain this observation:
Cr2+ has the configuration 3d4. It can lose electron to form Cr3+ which has stable 3d3configuration ( as it has half -filled t2g level). Hence , it is reducing.
On the other hand, Mn3+ also has 3d4configuration but it can gain electron to form Mn2+ which has stable 3d5 configuration (as it is exactly half - filled). Hence oxidising.
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