Why is the + 2 oxidation state of Mn (25) is quite stable, while the same is not true for iron (26)?
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Mn(25) has an outer electronic configration of 3d⁵4s² --
Mn₊² (losing 2 e⁻) the electronic configration becomes 3d⁵ (d-orbital is half-filled)
Stability of a compound is increases when outer orbital is half filled or completely filled.
Cr(26) has an outer electronic configration od 3d⁶4s²--
Cr⁺²-- the configration now becomes 3d⁶ (which is not half or completely filled.
∴ since 3d⁵ is more stable than 3d⁶
Mn⁺² is quite stable than Cr⁺²
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Mn2+ is stable because it contains half filled 3d sub-shell whereas Fe. Hence, +2 oxide state of an Mn(25) is stable while the same is not true for iron(26).
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