Given below are two statements:
Statement-I: Since fluorine is more electronegative than nitrogen, the net dipole moment of ${\mathrm{NF}}_3$ is greater than ${\mathrm{NH}}_3$.
Statement-II: In ${\mathrm{NH}}_3$, the orbital dipole due to lone pair and the dipole moment of $\mathrm{NH}$ bonds are in opposite direction, but in ${\mathrm{NF}}_3$ the orbital dipole due to lone pair and dipole moments of N-F bonds are in same direction.
In the light of the above statements. Choose the most appropriate from the options given below.

The lone pair of nitrogen opposes the dipole moment of ${\mathrm{NF}}_3$ while it is added to the dipole moment of ${\mathrm{NH}}_3$
In ${\mathrm{NH}}_3$

Hydrogen is less electronegative than nitrogen, so all the electrons will move towards nitrogen. Due to this, all the vectors will be in the same direction and the summation will come to maximum.

In ${\mathrm{NF}}_3$

Fluorine is more electronegative than nitrogen, so all the electrons will move towards fluorine. Due to this, all the vectors will cancel each other and the summation will come to a minimum.

In ${\mathrm{NH}}_3$, the dipole moment vector of the bond and the lone pairs are in the same direction. But in ${\mathrm{NF}}_3$, the dipole moment vector of lone pairs and bond pairs are opposite in direction. So, the net dipole moment will be the subtractive effect of the two. Hence, the dipole moment of ${\mathrm{NH}}_3$ is larger than ${\mathrm{NF}}_3$.