Question

The $SiC{l}_4$ molecule is nonpolar and chlorine is more electronegative than silicon. From this information alone it can be deduced that :
(1) $Si-Cl$ bond is nonpolar
(2) $SiC{l}_4$ molecule is planar
(3) $SiC{l}_4$ molecule is symmetrical

• A. If $1,2$ and $3$ are correct
• B. If only $1$ and $2$ are correct
• C. If only $2$ and $3$ are correct
• D. If only $1$ is correct
• E. If only $3$ is correct

Answer 1

The correct option is E If only $3$ is correct

Since chlorine is more electronegative than silicon, silicon-chlorine bond is polar.

$Si{Cl}_4$ is silicon tetrachloride, which is a non-polar molecule. Silicon tetrachloride is non-polar because the four chemical bonds between silicon and chlorine are equally distributed. The even distribution of polar bonds results in a net 0 dipole moment.

Hence, it is symmetrical.

So, only $3$ is correct.