Answer:
Carbon cannot lose all the four
valence electrons to form \[{{C}^{4+}}\] ions because the sum of the first four
ionization enthalpies of carbon is very large. It also cannot gain four
electrons to form \[{{C}^{4-}}\]ion as this anion would be highly unstable
because it would be very difficult for a nucleus with only 6 protons to hold on
firmly 10 electrons. Therefore, carbon forms only covalent compounds by sharing
of electrons :
In
contrast, due to inert pair effect, + 2 oxidation state of Pb is more stable
than its +4 oxidation state. Further, on moving down the group, the ionization
enthalpy decreases.
As a result, the sum of the first two
ionization enthalpies of Pb is quite low and hence Pb can easily lose two
electrons to form \[P{{b}^{2+}}\] ions. Consequently, Pb forms ionic compounds.
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