None of the inert gases (Helium, Neon, Argon, Krypton,Xenon, Radon) easily forms normal chemical bonds. All of them are monatomic gases. That is because all of them have complete outer shells of electrons. There are no "vacancies" in the outermost shell, ready to be filled by sharing electrons with another atom, which is what happens in chemical bonding.
This rule gets a bit weaker, however, with the larger members of the series, e.g. Xenon, which has some empty electron orbitals, not too much higher in energy, into which electrons can be promoted, leaving behind a gap which can be used to form bonds.
This Morse potential can however also be applied to the much weaker attraction due to London "dispersion" forces. These are not chemical bonds, but a feeble attraction due to a sort of flickering of tiny partial electric charges on neighbouring atoms due to the motion of their electrons (or to uncertainty in their position). There is a Wiki article on this here:
https://en.wikipedia.org/wiki/London_dispersion_force. in which you will see the good old Morse potential, or something very similar, pops up yet again.
These dispersion forces produce an attraction between molecules that causes molecular substances to condense into liquid and finally the solid state.