Which one of the following arrangements of mo | vedclass

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(D) The dipole moment of a molecule depends on its geometry and the polarity of its bonds.$BF_3$ has a trigonal planar geometry,and the bond dipoles c

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$NH_3 > NF_3 > BF_3$

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(D) The dipole moment of a molecule depends on its geometry and the polarity of its bonds.$BF_3$ has a trigonal planar geometry,and the bond dipoles cancel each other out,resulting in a net dipole moment of $0 \ D$.$NH_3$ has a pyramidal geometry with a lone pair on the $N$ atom. The bond dipoles of $N-H$ bonds and the lone pair dipole point in the same direction,resulting in a high dipole moment of approximately $1.47 \ D$.$NF_3$ also has a pyramidal geometry,but the $N-F$ bond dipoles point in the opposite direction to the lone pair dipole,which partially cancels the net dipole moment,resulting in a value of approximately $0.24 \ D$.Therefore,the correct order of dipole moments is $NH_3 > NF_3 > BF_3$.

Which one of the following arrangements of molecules is correct on the basis of their dipole moments?

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