Question

Element X forms a chloride with formula ${\mathrm{XCl}}_4$ which is solid with low melting point. X would most likely to be in the same group of the periodic table is?

• A. $Na$
• B. $Mg$
• C. $Al$
• D. $Si$

Answer 1

The correct option is D

$\mathrm{Si}$

Explanation for correct option:

(D) $\mathrm{Si}$

• Silicon belongs to Group-14. It has four electrons in its outermost shell. Thus, its valency is $+4$.
• Silicon can form a chloride ${\mathrm{SiCl}}_4$ by sharing its 4 valence electrons and making covalent bonds.

Explanation for the incorrect options:

(A) Sodium has one electron in its outermost shell. Thus, the chloride so formed by it will be $\mathrm{NaCl}$.

(B) Magnesium has two electrons in its outermost shell. Thus, the chloride so formed by it will be ${\mathrm{MgCl}}_2$.

(C) Aluminum has three electrons in its outermost shell. Thus, the chloride so formed by it will be ${\mathrm{AlCl}}_3$.

Therefore, the correct option is (D). The element X is $\mathrm{Si}$.