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(C) $CH_4$ and $PF_5$ are non-polar molecules with a net dipole moment $\mu_{net} = 0$. In $NH_3$ and $NF_3$,both have a trigonal pyramidal geometry w

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$NH_3$

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(C) $CH_4$ and $PF_5$ are non-polar molecules with a net dipole moment $\mu_{net} = 0$. In $NH_3$ and $NF_3$,both have a trigonal pyramidal geometry with one lone pair on the central atom. In $NH_3$,the direction of the bond dipoles $(N-H)$ is towards the nitrogen atom,which is in the same direction as the lone pair moment. Thus,they add up. In $NF_3$,the fluorine atoms are more electronegative than nitrogen,so the bond dipoles $(N-F)$ point away from the nitrogen atom,opposing the direction of the lone pair moment. Therefore,the dipole moment of $NH_3$ $(1.46 \ D)$ is greater than that of $NF_3$ $(0.24 \ D)$.

Which one of the following molecules has the maximum dipole moment?

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