The molecule which has zero dipole moment is :

Solution :
TIPS/Formulae : Dipole moment of compound having regular geometry and same type of atoms is zero. It is vector quantity.
The zero dipole moment of $$B{F_3}$$  is due to its symmetrical (triangular planar) structure. The three fluorine atoms lie at the corners of an equilateral triangle with boron at the centre.
NOTE: The vectorial addition of the dipole moments of the three bonds gives a net sum of zero because the resultant of any two dipole moments is equal and opposite to the third. The dipole moment of $$N{H_3}$$  is $$1.46$$ $$D$$  indicating its unsymmetrical structure. The dipole moment of$$C{H_2}C{l_2}$$   ( the molecule uses $$s{p^3}$$  hybridisation but is not symmetric ) is $$1.57\,{\text{D}}.$$