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.
The
elements in the first-half of the
transition series exhibit many oxidation states with Mn exhibiting
maximum number of oxidation states (+2 to +7). The stability of +2
oxidation state increases with the increase in atomic number. This
happens as more electrons are getting filled in the d-orbital.
However, Sc does not show +2 oxidation state. Its electronic
configuration is 4s2
3d1.
It loses all the three electrons to form Sc3+.
+3 oxidation state of Sc is very stable as by losing all three
electrons, it attains stable noble gas configuration, [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, its d-orbital
is exactly half-filled, [Ar] 3d5.
The elements in the first-half of the transition series exhibit many oxidation states with Mn exhibiting maximum number of oxidation states (+2 to +7). The stability of +2 oxidation state increases with the increase in atomic number. This happens as more electrons are getting filled in the d-orbital. However, Sc does not show +2 oxidation state. Its electronic configuration is 4s2 3d1. It loses all the three electrons to form Sc3+. +3 oxidation state of Sc is very stable as by losing all three electrons, it attains stable noble gas configuration, [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, its d-orbital is exactly half-filled, [Ar] 3d5.
