Boron trichloride (BCl₃) is a nonpolar molecule. This is because the three chlorine atoms are arranged symmetrically around the boron atom, resulting in a molecule with no net dipole moment.

Therefore, the dominant intermolecular force in boron trichloride is London dispersion forces.

Here's why:

* London Dispersion Forces: These are temporary, weak attractions that arise from temporary fluctuations in electron distribution within molecules. All molecules experience London dispersion forces, even nonpolar ones.

While boron trichloride does not have dipole-dipole interactions or hydrogen bonding (which are stronger than London dispersion forces), it still experiences these weak forces due to its temporary, induced dipoles.