Chemistry - CHEMICAL BONDING Question with Solution | TestHub

The dipole moments of the given species are as follows

$\mathrm{N}{\mathrm{H}}_3>\mathrm{N}{\mathrm{F}}_3>\mathrm{B}{\mathrm{F}}_3$

$\mathrm{B}{\mathrm{F}}_3$is a planar molecule, so it has zero dipole moment.$\mathrm{N}{\mathrm{H}}_3$has more dipole moment than$\mathrm{N}{\mathrm{F}}_3$. The resultant dipole moment of three$\mathrm{N}-\mathrm{H}$bonds and dipole moment due to lone pair of electrons are acting in the same direction, but in case of$\mathrm{N}{\mathrm{F}}_3$the resultant dipole moment of the three$\mathrm{N}-\mathrm{F}$bonds is acting opposite to the direction of dipole moment due to lone pair of electrons.