To what extent do the eletronic configuration decide the stability of oxidation states in the first series of the transition elements ? Illustrate your answer with examples.

Explanation

If orbital is half-filled or completely filled, it imparts stability to an atom or ion .
e.g. `{:("(i) " ""_(25)Mn = [Ar]3d^(5)4s^(2)),(" "Mn^(2+) = [Ar]3d^(5)" (most stable)"),(" "Mn^(3+) = [Ar] 3d^(4)),(" "Mn^(4+) = [Ar] 3d^(3)),("(ii) " ""_(29)Cu = [Ar]3d^(10) 4s^(1)),(" "Cu^(+) = [ Ar] 3d^(10) " (most stable)"),(" "Cu^(2+) = [Ar] 3d^(9)):}`
In manganese, `Mn^(2+)` ion is most stable due to symmetry and half-filled d-orbitals . In the same way in copper , `Cu^(+)` ion is most stable due to symmetry and completely filled d-orbitals .