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(D) . The dipole moment $(\mu)$ depends on the electronegativity difference between the central atom $(N)$ and the surrounding atoms,as well as the di

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$NH_3$

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(D) . The dipole moment $(\mu)$ depends on the electronegativity difference between the central atom $(N)$ and the surrounding atoms,as well as the direction of the bond dipoles and the lone pair dipole.
In $NH_3$,the bond dipoles of $N-H$ bonds and the lone pair dipole are in the same direction,which results in a large net dipole moment $(\mu = 1.46 \ D)$.
In $NF_3$,the electronegativity of $F$ is higher than $N$,so the bond dipoles point away from the nitrogen atom,opposing the direction of the lone pair dipole,resulting in a smaller net dipole moment $(\mu = 0.24 \ D)$.
$NCl_3$ and $NBr_3$ also have lower dipole moments compared to $NH_3$ due to the smaller electronegativity difference and the geometry of the molecules.
Therefore,$NH_3$ has the maximum dipole moment.

Which of the following will have the maximum dipole moment?

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