Question

$M{n}^{2+}$ compounds are more stable than $F{e}^{2+}$ compounds towards oxidation to their $+3$ state, because

• A. $M{n}^{2+}$ is more stable with high 3rd Ionisation energy.
• B. $M{n}^{2+}$ is bigger in size.
• C. $M{n}^{2+}$ has completely filled d-orbitals.
• D. $M{n}^{2+}$ does not exist.

Answer 1

Answer: (A)

$M{n}^{2+}$ compounds are more stable than $F{e}^{2+}$ compounds towards oxidation to $+3$ state due to its completely half-filled stable configuration.



$F{e}^{2+}$ can easily acquire $+3$ oxidation state by losing one electron as it attains the stable configuration but 3rd ionisation energy for $M{n}^{2+}$ is very high as it is very difficult to loose one electron from stable configuration $\left(d^5\right)$ therefore, $M{n}^{2+}$ is more stable than $F{e}^{2+}$