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 :
$$C < Si < Ge < Sn < Pb$$
Solution :
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.
Releted MCQ Question on Inorganic Chemistry >> P - Block Elements
Releted Question 1
The reddish brown coloured gas formed when nitric oxide is oxidised by air is