To what extent do the electronic configurations decide the stability of oxidation states in the first series of the transition elements? Illustrate your answer with examples.
When d orbitals are half-filled or completely filled, the oxidation state is more stable. Thus, Mn (Z = 25) has electronic configuration [Ar]3d54s2. +2 oxidation state is most stable as it has stable electronic configuration (half filled 3d orbital). Also, Zn (Z = 30) has electronic configuration [Ar]3d104s2. +2 oxidation state is most stable as it has stable electronic configuration (completely filled 3d orbital).
