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(B) The elements of group $14$ have $4$ valence electrons in their outermost shell $(ns^2 np^2)$.Therefore,they typically exhibit $+4$ and $+2$ oxidat

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exhibit oxidation state of $+2$ and $+4$

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(B) The elements of group $14$ have $4$ valence electrons in their outermost shell $(ns^2 np^2)$.Therefore,they typically exhibit $+4$ and $+2$ oxidation states.Due to the inert pair effect,the stability of the $+2$ oxidation state increases down the group,while the stability of the $+4$ oxidation state decreases.						Group $14$ element			Oxidation state							$C$			$+4$							$Si$			$+4$							$Ge, Sn, Pb$			$+2, +4$

Elements of group $14$:

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