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

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

Tardigrade Admin · Accepted Answer

The tendency to show +2 oxidation state increases down the group. It is due to inability of ns2 electrons of valence shell to participate in bonding.

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

$C < S i < S n < P b < G e$

$C < S i < G e < S n < P b$

$G e < S n < P b < C < S i$

$P b < S n < G e < C < S i$

The tendency to show $+ 2$ oxidation state increases down the group. It is due to inability of $n s^{2}$ electrons of valence shell to participate in bonding.

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

C<Si<Sn<Pb<Ge

C<Si<Ge<Sn<Pb

Ge<Sn<Pb<C<Si

Pb<Sn<Ge<C<Si