Question

what type or types of intermolecular forces exist or exists in the molecule below? london dispersion forces only dipole - dipole only h - bonding only london dispersion forces, dipole - dipole, & h - bonding dipole - dipole, & h - bonding london dispersion forces & dipole - dipole ionic bonding only london dispersion forces & ionic bonding none of these

Explanation:

1. London - Dispersion Forces: These forces exist in all molecules due to temporary fluctuations in electron - cloud distribution. All molecules, regardless of polarity, have London - dispersion forces.
2. Dipole - Dipole Forces: For dipole - dipole forces to exist, the molecule must be polar. In $SF_6$, the sulfur hexafluoride molecule has a symmetrical octahedral geometry. The individual $S - F$ bond is polar (since $F$ is more electronegative than $S$), but due to the symmetry of the molecule, the bond dipoles cancel out, and the molecule is non - polar. So, there are no dipole - dipole forces.
3. Hydrogen Bonding: Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom ($N$, $O$, or $F$) and is attracted to another electronegative atom in a neighboring molecule. In $SF_6$, there is no hydrogen atom present, so there is no hydrogen bonding.

Answer:

A. London Dispersion forces only