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.

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Solution

When d orbitals are half-filled or completely filled, the oxidation state is more stable.

Thus, Mn (Z = 25) has electronic configuration $[A r] 3 d^{5} 4 s^{2}$ . $+ 2$ oxidation state is most stable as it has stable electronic configuration (half filled 3d orbital).

Also, Zn (Z = 30) has electronic configuration $[A r] 3 d^{10} 4 s^{2} .$ $+ 2$ oxidation state is most stable as it has stable electronic configuration (completely filled 3d orbital).

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