Why are Mn²⁺ compounds more stable than Fe²⁺ towards oxidation to their +3 state?
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Electronic configuration of Mn2+ is [Ar]18 3d5 and Electronic configuration of Fe2+ is [Ar]18 3d6.
As the half-filled and fully-filled orbitals are more stable, Mn in (+2) state has the stable d5 configuration.
Mn2+ provides resistance to the oxidation to the Mn3+.
Fe2+ has the 3d6 configuration and its configuration changes after it loses 1 electron and it turns to the 3d5 configurations which is more stable.
As a result, Fe2+ becomes oxidized easily to the Fe+3 states.
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Answer :
- Electronic configuration of Mn2+ is [Ar]18 3d5 and Electronic configuration of Fe2+ is [Ar]18 3d6.
- As the half-filled and fully-filled orbitals are more stable, Mn in (+2) state has the stable d5 configuration.
- Mn2+ provides resistance to the oxidation to the Mn3+.
- Fe2+ has the 3d6 configuration and its configuration changes after it loses 1 electron and it turns to the 3d5 configurations which is more stable.
- As a result, Fe2+ becomes oxidized easily to the Fe+3 states.
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