BF3, or boron trifluoride, does not have a dipole moment. This is mainly due to its molecular geometry and the arrangement of its bonds.
BF3 has a trigonal planar structure, with boron at the center and three fluorine atoms positioned at the corners of an equilateral triangle. The bond between boron and fluorine is polar, as fluorine is much more electronegative than boron. However, because of the symmetrical arrangement of these polar bonds, the individual dipole moments cancel each other out.
As a result, while the bonds themselves are polar, the overall molecule is nonpolar. In summary, BF3 does not have a net dipole moment, and thus, it cannot interact strongly with electric fields like polar molecules can.