The d-And-f-Block Elements

Short Answer Type

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Why are Mn2+ compounds more stable than Fe2+ towards oxidation to their +3 state?

Exactly half-filled and completely filled subshells are relatively more stable. Species try to attain the state of exactly half-filled and completely filled subshells configuration.
Mn2+ has extra stability as it has exactly half filled configuration of 4s° 3d5 in its outermost shell while Fe2+ has 45° 3d6 configuration. Therefore, Fe2+ has a tendency to loose one electron (or tends to oxidise to Fe3+) to acquire extra stability by having 4s0 3d5configuration.
Fe2+  → Fe3+ + e–(4s03d6) (4s03d5)
Since Mn2+ has half filled orbital thus it is more stable to Fe2+.

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