Answer:
Among the elements of group 14,
carbon does not have d- or f-electrons. Therefore, it does not show inert pair
effect. Consequently, it shows an oxidation state of +4 due to the presence of
two electrons is the s- and two electrons in the p-orbital of the valence
shell. In contrast, all other elements from Ge to Pb contain either d or both
d- and f-electrons and hence show oxidation states of + 2 and + 4 due to inert
pair effect. Further, as the number of d-and f-electrons increases, the inert
pair effect becomes more and more prominent. In other words, as we move down
the group from Ge to Pb, the stability of +2 oxidation state increases while that
of +4 oxidation state decreases. Therefore, the tendency of Ge, Sn and Pb to
exhibit + 2 oxidation state increases with increasing atomic number in group
14.
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