The heavier elements of group $$13, 14$$ and $$15$$ besides their group oxidation state exhibit another oxidation state which is two units lower than the group oxidation state. The stability of lower oxidation state increases down the group.
The display of lower oxidation state is due to inert pair effect.
Which of the following statements is incorrect?
A
Boron shows only $$+3$$ oxidation state.
B
In $$Sn+2$$ oxidation state is more stable than $$+4$$ oxidation state.
C
In $$Tl+1$$ oxidation state is more stable than $$+3$$ oxidation state.
D
In $$Ga+3$$ oxidation state is more stable than $$+1$$ oxidation state.
Correct option is C. In $$Sn+2$$ oxidation state is more stable than $$+4$$ oxidation state.
In the group 13, 14, 15 the stability of lower oxidation state increases down in the group.
But, $$Sn^{+4}$$ is more stable than $$Sn^{+2}$$ due to its configuration.
The electronic configuration of Sn is $$5s^{2} 5p^{4}$$.
In $$Sn^{4}$$, it lose four electrons and achieve full filled electronic configuration.
Due to its stability , $$Sn^{+4}$$ is more stable than $$Sn^{2}$$.
Among the all statements mentioned, $$\textbf{(C) is incorrect}$$.
Hence, option will be $$(C)$$.