Final answer:
In pure cyclohexane, the intermolecular forces are exclusively London Dispersion forces, as cyclohexane is a nonpolar molecule with no capacity for hydrogen bonding or permanent dipole-dipole interactions.
Step-by-step explanation:
The types of intermolecular forces in pure cyclohexane are primarily London Dispersion forces. Cyclohexane is a nonpolar molecule, which means that it does not have permanent dipole-dipole attractions or the capacity for hydrogen bonding with molecules of the same kind. In contrast to polar molecules that exhibit dipole-dipole interactions, the electrons in nonpolar molecules like cyclohexane can become momentarily unevenly distributed, creating instantaneous dipoles that induce dipoles in adjacent molecules. This results in attractions known as London dispersion forces. The strength of these forces increases with the size of the molecules and the number of electrons present.
Since cyclohexane does not contain highly electronegative atoms like oxygen, nitrogen, or fluorine bonded to hydrogen, it cannot form hydrogen bonds, which are a type of strong dipole-dipole attraction. Therefore, in a sample of pure cyclohexane, the only intermolecular attractions are London dispersion forces.