BF_3 and NF_3 both are covalent compounds but | vedclass

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(C) $BF_3$ has a trigonal planar geometry with $sp^2$ hybridization. Due to its symmetric shape,the individual bond dipoles cancel each other out,resu

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$NF_3$ is pyramidal whereas $BF_3$ is planar triangular

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(C) $BF_3$ has a trigonal planar geometry with $sp^2$ hybridization. Due to its symmetric shape,the individual bond dipoles cancel each other out,resulting in a net dipole moment of zero (non-polar).$NF_3$ has a trigonal pyramidal geometry with $sp^3$ hybridization and a lone pair on the nitrogen atom. The bond dipoles and the lone pair dipole do not cancel each other out,resulting in a net dipole moment (polar).

$BF_3$ and $NF_3$ both are covalent compounds but $NF_3$ is polar whereas $BF_3$ is non-polar. This is because

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