Answer:
(i) The elements
of group 13, exhibit two oxidation states of +3 and +1 in their compounds. Due
to small size and high ionisation enthalpies of boron, it forms only covalent
compounds showing +3oxidation state. Aluminium shows +3 oxidation state by
forming both electrovalent and covalent compounds. However, down the group from
\[Ga\]to\[Tl\]due to poor shielding effect of intervening electrons of d- and orbitals,
the ns electrons are held firmly and thereby restrict the \[n{{s}^{2}}\]
electrons to participate in bonding. As a result of this, only p-orbital
electron may be involved in bonding. In fact,\[Ga\], In and\[~Tl\] show both +1
and +3 oxidation states but the relative stability of +1 oxidation state
increases and stability of +3 oxidation state decreases due to the inert pair
effect.
(ii) Carbon and silicon exhibit +4
oxidation due to presence of four electrons in the valence shell and due to not
having inert pair effect as d-electrons are not present in penultimate energy
shell. In contrast all other elements from \[Ge\]to \[Pb\]exhibit+2 and 44
oxidation states due to the presence of d-and f-electrons. However, the stability
of +2oxidation state increases while stability of +4oxidation state decreases
due to inert pair effect from \[Ge\]to\[~Pb\], i.e., +2 state of\[~Pb\] is more
stable than +4 state of\[~Pb\].
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