BF_3 and NF_3 are both covalent molecules,but | vedclass

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Question

(D) $BF_3$ has a trigonal planar geometry ($sp^2$ hybridization) where the bond dipoles cancel each other out,resulting in a net dipole moment of $0$.

Vedclass · Accepted Answer

$BF_3$ is planar,whereas $NF_3$ is pyramidal.

Vedclass · Answer

(D) $BF_3$ has a trigonal planar geometry ($sp^2$ hybridization) where the bond dipoles cancel each other out,resulting in a net dipole moment of $0$. In $NF_3$,the nitrogen atom has one lone pair of electrons,leading to a trigonal pyramidal geometry ($sp^3$ hybridization). The presence of the lone pair and the pyramidal shape prevent the bond dipoles from canceling,making $NF_3$ a polar molecule.

$BF_3$ and $NF_3$ are both covalent molecules,but $BF_3$ is non-polar and $NF_3$ is polar. The reason for this is:

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