The d-And-f-Block Elements
Why is the + 2 oxidation state of manganese quite stable while the same is not true for iron? |Mn = 25, Fe = 26]
Electronic configuration of Mn2+ is 4s0 3d5 and electronic configuration for Fe2+ is 3d6. Mn2+ is more stable due to half filled d-orbitals but Fe2+ is not stable because it does not have half filled d-orbitals.
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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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