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

Explanation

To understand why \( \text{Mn}^{2+} \) compounds are more stable than \( \text{Fe}^{2+} \) compounds towards oxidation to their +3 state, we can analyze the electronic configurations and stability of these ions.

### Step-by-Step Solution:

1. **Identify the Electronic Configurations:**
- The electronic configuration of manganese (Mn) in its elemental state is \( [Ar] 3d^5 4s^2 \).
- The electronic configuration of iron (Fe) in its elemental state is \( [Ar] 3d^6 4s^2 \).

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