Why are `Mn^(2+)` compounds more stable than `Fe^(2+)` toward oxidation to their `+3` state?

Explanation

electronic configuration of `Mn^(2+)` is `3d^(5)` while that of `Fe^(2+)` is `3d^(6)`. This shows that `Fe^(2+)` ion has an urge to change to `Fe^(3+)` ion by losing an electron whereas `Mn^(2+)` ion has no such tendency. Thus, +2 oxidation state of Mn is more stable as compared to +2 oxidation state of Fe.