Mn exhibits maximum oxidation states from +2 to +7 and it lies in the first half of the transition series. With an increase in atomic number of the elements, the stability of +2 oxidation state increases. As more and more electrons are filled in the d-orbital, this occurs repeatedly with increase in atomic number. The +2 oxidation state is not shown by Scandium. It has an electronic configuration of 4s2 3d1. Scandium undergoes a loss of all its three electrons to form Sc3+ and this +3 oxidation state of Sc is very stable. This is so because by losing all three electrons, it attains nearest noble gas electronic configuration, which is of [Ar]. Ti (+ 4) and V(+5) are very stable for the same reason. For Mn, +2 oxidation state is very stable as after losing two electrons, it achieves half-filled stable electronic configuration, [Ar] 3d5.
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.
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.