Chemistry - CHEMICAL BONDING Question with Solution | TestHub

${\mathrm{BF}}_3$ has zero dipole moment as it is symmetrical in nature. ${\mathrm{H}}_2\mathrm{O}$ has maximum dipole moment as it possess two lone pair of electrons. Between ${\mathrm{NH}}_3$ and ${\mathrm{NF}}_3,{\mathrm{NH}}_3$ has greater dipole moment though in ${\mathrm{NH}}_3$ and ${\mathrm{NF}}_3$, both $\mathrm{N}$ possesses one lone pair of electrons. This is beacuse in case of ${\mathrm{NH}}_3$, the net $\mathrm{N}-\mathrm{H}$ bond dipole is in the same direction as the direction of dipole of lone pair. But in case of ${\mathrm{NF}}_3$, the direction of net dipole moment of three $-\mathrm{N}-\mathrm{F}$ bonds is opposite to that of the dipole moment of the lone pair. Thus, the correct of dipole moment is