Question

The tendency of group 14 elements to show +2 oxidation state increases in the order of:

• A. $C<Si<Sn<Pb<Ge$
• B. $C<Si<Ge<Sn<Pb$
• C. $Ge<Sn<Pb<C<Si$
• D. $Pb<Sn<Ge<C<Si$

Answer 1

The correct option is B $C<Si<Ge<Sn<Pb$

The tendency to show $+2$ oxidation state increases as we move down the group. This is due to inert pair effect which causes the inability of $n{s}^2$ electrons of valence shell to participate in bonding.

Thus, the stability of elements in $+2$ oxidation state increases as we move down the group in the order $C<Si<Ge<Sn<Pb$.

Hence, the correct answer is option $\text{B}$.