8.2     Why are $Mn^{2+}$ compounds more stable than $Fe^{2+}$ towards oxidation to their $+3$ state?

$Mn^{2+}= 1s^2,2s^2p^6,3s^2p^6d^5\:\:\:(Half\:filled \:d-orbital)$

$Fe^{2+}= 1s^2,2s^2p^6,3s^2p^6d^6$

In +2 oxidation state of manganese has more stability than +2 oxidation state of iron, it is because half filled and fully filled d-orbitals are more stable and $Mn^{2+}$has half filled electron stability Manganese ($Mn^{2+}$) has $d^{5}$ configuration so it wants to remain in this configuration. On the other hand, $Fe^{2+}$has $d^{6}$ configuration and after losing one electron it becomes$d^{5}$ configuration and attains its stability. That's why $Mn^{2+}$ compounds more stable than $Fe^{2+}$ towards oxidation to their $+3$ state.

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