BF_3 and NF_3 are both covalent compounds. Ho | vedclass

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(D) $BF_3$ has a trigonal planar geometry with $sp^2$ hybridization. Due to its symmetry,the individual bond dipole moments cancel each other out,resu

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$BF_3$ is planar,whereas $NF_3$ has a pyramidal shape

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(D) $BF_3$ has a trigonal planar geometry with $sp^2$ hybridization. Due to its symmetry,the individual bond dipole moments cancel each other out,resulting in a net dipole moment of $0$ (non-polar).$NF_3$ has a trigonal pyramidal geometry with $sp^3$ hybridization and one lone pair on the nitrogen atom. Due to the presence of the lone pair and the difference in electronegativity,the bond dipoles do not cancel out,resulting in a net dipole moment (polar).

$BF_3$ and $NF_3$ are both covalent compounds. However,$BF_3$ is non-polar,while $NF_3$ is polar because .....

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