Which of the following is the correct order of dipole moment?

$\mathrm{BF}_3$ 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