Question

Which of the following is expected to have a dipole moment of zero?

• A. $SOC{l}_2$
• B. $O{F}_2$
• C. $Se{F}_6$
• D. $Cl{F}_5$

Answer 1

The correct option is C $Se{F}_6$

In $Se{F}_6$, $Se$ has six $\sigma$ bonds, steric number = 6. So, it is $s{p}^3{d}^2$ hybridized and posseses octahedral geometry. In an octahedron, all dipole moment vectors cancel out each other. Hence, it has a net dipole moment = 0 and thus is non-polar in nature.$SOC{l}_2$ - has 3 sigma bonds, 1 lone pair and 1 pi bond. So, it is $s{p}^3$ hybridised with tetrahedral geometry. It has a net resultant dipole moment vector. Hence, $\mu \ne 0$.

$O{F}_2$ - has bent shape. It has a net resultant dipole moment vector. Hence, $\mu \ne 0$.

$Cl{F}_5$ - has square pyramidal shape. It has a net resultant dipole moment vector. Hence, $\mu \ne 0$.