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The d-And-f-Block Elements
Electronic configuration of Mn is [Ar] 4s2 3d5 and Configuration of iron [Ar] 4s2 3d5.
Mn3+ + 3e– → Mn2+
(more spontaneous due to higher stability of Fe3+) Fe3+ + e– → Fe2+
(less spontaneous due to higher stability of Fe3+)
Due to stability of half filled d-orbitals, Mn2+ is more stable than Mn3+ and thus its reduction is more spontaneous. Similarly Fe3+ is more stable than Fe2+ and thus its reduction is less spontaneous.
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How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of the transition elements?
The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?
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