Final answer:
SF6 has London dispersion forces as its intermolecular force, due to its non-polar nature and lack of hydrogen atoms bonded to highly electronegative atoms; it does not feature hydrogen bonding, dipole-dipole, or ion-dipole forces.
Step-by-step explanation:
The type of intermolecular forces found in SF6 (sulfur hexafluoride) can be determined by examining the nature of its molecules. SF6 is a non-polar compound because the shape of the molecule distributes the charge evenly, so it does not have permanent dipole moments. There are no hydrogen atoms bonded to highly electronegative atoms (O, N, or F), which rules out hydrogen bonding. Moreover, since there is no polarity, there are no dipole-dipole interactions. Ion-dipole forces do not arise as SF6 is not composed of ions. Therefore, the only intermolecular forces in SF6 are London dispersion forces, which are caused by the temporary fluctuations of electron density within molecules that induce a temporary dipole moment in adjacent molecules.