Question

An unknown element 'E' forms two compounds: \(EO_{2}\) and \(EX_{4}\). To which group does element 'E' belong?

• A. 13th group (B, Al)
• B. 14th group (C, Si)
• C. 15th group (N, P)
• D. 16th group (O, S)

Hint:

Remember these common compounds: \[ \boxed{ \begin{aligned} CO_2,\;CCl_4\\ SiO_2,\;SiCl_4 \end{aligned} } \] Both carbon and silicon belong to \[ \boxed{\text{Group 14}.} \] If an element forms compounds of the type \(EO_2\) and \(EX_4\), it generally belongs to Group 14.

Answer 1

The Correct Option is B

In $EO_2$, with oxygen at $-2$, the oxidation state of E works out to $+4$; $EX_4$ (X = halogen at $-1$) also confirms a $+4$ state for E. Elements that characteristically show a $+4$ oxidation state and form such compounds belong to Group 14 (e.g., Si, Ge, Sn, Pb).