Yeah, dimers of noble gas molecules form due to dispersion aka London forces. More generally, neutral, non-polar molecules can still form very weak bound states arising entirely from the induction and interaction of instantaneous dipole moments (that is, fluctuations in the electron density around an atom arising from the motion of electrons). My understanding is that physicists would explain this interaction as a special case of the Casimir-Polder interaction. This interaction means that even noble gases are nonideal.

Correctly predicting the negative interaction energy of a noble gas dimer is a pathological test of dispersion-corrected DFT functionals, as F'x's reference¹ and the references therein indicate, and many methods fail qualitatively. I recall that Zhao and Truhlar used noble gas dimers to test the efficacy of their various metahybrid functionals^2,3. One of their papers² makes reference to a table of binding energies and equilibrium distances derived⁴ by Wang and Ogilvy, giving for instance a $\ce{Ne\cdots{}Ne}$ binding energy of 0.35 kJ mol^-1 (that's tiny) and less than half that for $\ce{He\cdots{}Ne}$. The $\ce{Ne\cdots{}Ne}$ equilibrium distance is given as 309 pm, which is extreme. As the paper⁵ you refer to indicates, however, the interaction energy for the $\ce{^4He\cdots{}^4He}$ dimer is much, much smaller than either of these and has an equilibrium distance of 5.2 nm (!!!), which is something else entirely.

(1) Ruzsinszky, A.; Perdew, J.P.; Csonka, G.I.; Binding Energy Curves from Nonempirical Density Functionals II. van der Waals Bonds in Rare-Gas and Alkaline-Earth Diatomics; J. Phys. Chem. A; 2005, 109, pp. 11015-11021

(2) Zhao, Y.; Truhlar, D.G.; Hybrid Meta Density Functional Theory Methods for Thermochemistry, Thermochemical Kinetics, and Noncovalent Interactions: The MPW1B95 and MPWB1K Models and Comparative Assessments for Hydrogen Bonding and van der Waals Interactions; J. Phys. Chem. A; 2004, 108, 6908-6918

(3) Zhao, Y.; Truhlar, D.G.; Comparative DFT Study of van der Waals Complexes: Rare-Gas Dimers, Alkaline-Earth Dimers, Zinc Dimer, and Zinc-Rare-Gas Dimers; J. Phys. Chem. A; 2006, 110, pp. 5121-5129

(4) Ogilvie, J.F.; Wang, F.Y.H.; Potential-energy functions of diatomic molecules of the noble gases: II. Unlike nuclear species; J. Mol. Struct.; 1993, 291, pp. 313-322

(5) Grisenti, R.E.; Schöllkopf, W.; Toennies, J.P.; Hegerfeldt, G.C.; Köhler, T.; Stoll, M.; Determination of the Bond Length and Binding Energy of the Helium Dimer by Diffraction from a Transmission Grating; Phys. Rev. Lett.; 2000, 85, pp. 2284-2287

Yeah, dimers of noble gas atoms are stable due to dispersion aka London forces. More generally, neutral, non-polar molecules can still form very weak bound states arising entirely from the induction and interaction of instantaneous dipole moments (that is, fluctuations in the electron density around an atom arising from the motion of electrons). My understanding is that physicists would explain this interaction as a special case of the Casimir-Polder interaction. This interaction means that even noble gases are nonideal.

Correctly predicting the negative interaction energy of a noble gas dimer is a pathological test of dispersion-corrected DFT functionals, as F'x's reference¹ and the references therein indicate, and many methods fail qualitatively. I recall that Zhao and Truhlar used noble gas dimers to test the efficacy of their various metahybrid functionals^2,3. One of their papers² makes reference to a table of binding energies and equilibrium distances derived⁴ by Wang and Ogilvy, giving for instance a $\ce{Ne\cdots{}Ne}$ binding energy of 0.35 kJ mol^-1 (that's tiny) and less than half that for $\ce{He\cdots{}Ne}$. The $\ce{Ne\cdots{}Ne}$ equilibrium distance is given as 309 pm, which is extreme. As the paper⁵ you refer to indicates, however, the interaction energy for the $\ce{^4He\cdots{}^4He}$ dimer is much, much smaller than either of these and has an equilibrium distance of 5.2 nm (!!!), which is something else entirely.

(1) Ruzsinszky, A.; Perdew, J.P.; Csonka, G.I.; Binding Energy Curves from Nonempirical Density Functionals II. van der Waals Bonds in Rare-Gas and Alkaline-Earth Diatomics; J. Phys. Chem. A; 2005, 109, pp. 11015-11021

(2) Zhao, Y.; Truhlar, D.G.; Hybrid Meta Density Functional Theory Methods for Thermochemistry, Thermochemical Kinetics, and Noncovalent Interactions: The MPW1B95 and MPWB1K Models and Comparative Assessments for Hydrogen Bonding and van der Waals Interactions; J. Phys. Chem. A; 2004, 108, 6908-6918

(3) Zhao, Y.; Truhlar, D.G.; Comparative DFT Study of van der Waals Complexes: Rare-Gas Dimers, Alkaline-Earth Dimers, Zinc Dimer, and Zinc-Rare-Gas Dimers; J. Phys. Chem. A; 2006, 110, pp. 5121-5129

(4) Ogilvie, J.F.; Wang, F.Y.H.; Potential-energy functions of diatomic molecules of the noble gases: II. Unlike nuclear species; J. Mol. Struct.; 1993, 291, pp. 313-322

(5) Grisenti, R.E.; Schöllkopf, W.; Toennies, J.P.; Hegerfeldt, G.C.; Köhler, T.; Stoll, M.; Determination of the Bond Length and Binding Energy of the Helium Dimer by Diffraction from a Transmission Grating; Phys. Rev. Lett.; 2000, 85, pp. 2284-2287

Yeah, dimers of noble gas molecules form due to dispersion aka London forces. More generally, any pair of neutral, non-polar molecules can still form very weak bound states arising entirely from the induction and interaction of instantaneous dipole moments (that is, fluctuations in the electron density around an atom arising from the motion of electrons). My understanding is that physicists would explain this interaction as a special case of the Casimir-Polder interaction. This interaction means that even noble gases are nonideal.

Correctly predicting the negative interaction energy of a noble gas dimer is a pathological test of dispersion-corrected DFT functionals, as F'x's reference¹ and the references therein indicate, and many methods fail qualitatively. I recall that Zhao and Truhlar used noble gas dimers to test the efficacy of their various metahybrid functionals^2,3. One of their papers² makes reference to a table of binding energies and equilibrium distances derived⁴ by Wang and Ogilvy, giving for instance a $\ce{Ne\cdots{}Ne}$ binding energy of 0.35 kJ mol^-1 (that's tiny) and less than half that for $\ce{He\cdots{}Ne}$. The $\ce{Ne\cdots{}Ne}$ equilibrium distance is given as 309 pm, which is extreme. As the paper⁵ you refer to indicates, however, the interaction energy for the $\ce{^4He\cdots{}^4He}$ dimer is much, much smaller than either of these and has an equilibrium distance of 5.2 nm (!!!), which is something else entirely.

(1) Ruzsinszky, A.; Perdew, J.P.; Csonka, G.I.; Binding Energy Curves from Nonempirical Density Functionals II. van der Waals Bonds in Rare-Gas and Alkaline-Earth Diatomics; J. Phys. Chem. A; 2005, 109, pp. 11015-11021

(2) Zhao, Y.; Truhlar, D.G.; Hybrid Meta Density Functional Theory Methods for Thermochemistry, Thermochemical Kinetics, and Noncovalent Interactions: The MPW1B95 and MPWB1K Models and Comparative Assessments for Hydrogen Bonding and van der Waals Interactions; J. Phys. Chem. A; 2004, 108, 6908-6918

(3) Zhao, Y.; Truhlar, D.G.; Comparative DFT Study of van der Waals Complexes: Rare-Gas Dimers, Alkaline-Earth Dimers, Zinc Dimer, and Zinc-Rare-Gas Dimers; J. Phys. Chem. A; 2006, 110, pp. 5121-5129

(4) Ogilvie, J.F.; Wang, F.Y.H.; Potential-energy functions of diatomic molecules of the noble gases: II. Unlike nuclear species; J. Mol. Struct.; 1993, 291, pp. 313-322

(5) Grisenti, R.E.; Schöllkopf, W.; Toennies, J.P.; Hegerfeldt, G.C.; Köhler, T.; Stoll, M.; Determination of the Bond Length and Binding Energy of the Helium Dimer by Diffraction from a Transmission Grating; Phys. Rev. Lett.; 2000, 85, pp. 2284-2287

Yeah, dimers of noble gas molecules form due to dispersion aka London forces. More generally, neutral, non-polar molecules can still form very weak bound states arising entirely from the induction and interaction of instantaneous dipole moments (that is, fluctuations in the electron density around an atom arising from the motion of electrons). My understanding is that physicists would explain this interaction as a special case of the Casimir-Polder interaction. This interaction means that even noble gases are nonideal.

Correctly predicting the negative interaction energy of a noble gas dimer is a pathological test of dispersion-corrected DFT functionals, as F'x's reference¹ and the references therein indicate, and many methods fail qualitatively. I recall that Zhao and Truhlar used noble gas dimers to test the efficacy of their various metahybrid functionals^2,3. One of their papers² makes reference to a table of binding energies and equilibrium distances derived⁴ by Wang and Ogilvy, giving for instance a $\ce{Ne\cdots{}Ne}$ binding energy of 0.35 kJ mol^-1 (that's tiny) and less than half that for $\ce{He\cdots{}Ne}$. The $\ce{Ne\cdots{}Ne}$ equilibrium distance is given as 309 pm, which is extreme. As the paper⁵ you refer to indicates, however, the interaction energy for the $\ce{^4He\cdots{}^4He}$ dimer is much, much smaller than either of these and has an equilibrium distance of 5.2 nm (!!!), which is something else entirely.

(1) Ruzsinszky, A.; Perdew, J.P.; Csonka, G.I.; Binding Energy Curves from Nonempirical Density Functionals II. van der Waals Bonds in Rare-Gas and Alkaline-Earth Diatomics; J. Phys. Chem. A; 2005, 109, pp. 11015-11021

(2) Zhao, Y.; Truhlar, D.G.; Hybrid Meta Density Functional Theory Methods for Thermochemistry, Thermochemical Kinetics, and Noncovalent Interactions: The MPW1B95 and MPWB1K Models and Comparative Assessments for Hydrogen Bonding and van der Waals Interactions; J. Phys. Chem. A; 2004, 108, 6908-6918

(3) Zhao, Y.; Truhlar, D.G.; Comparative DFT Study of van der Waals Complexes: Rare-Gas Dimers, Alkaline-Earth Dimers, Zinc Dimer, and Zinc-Rare-Gas Dimers; J. Phys. Chem. A; 2006, 110, pp. 5121-5129

(4) Ogilvie, J.F.; Wang, F.Y.H.; Potential-energy functions of diatomic molecules of the noble gases: II. Unlike nuclear species; J. Mol. Struct.; 1993, 291, pp. 313-322

(5) Grisenti, R.E.; Schöllkopf, W.; Toennies, J.P.; Hegerfeldt, G.C.; Köhler, T.; Stoll, M.; Determination of the Bond Length and Binding Energy of the Helium Dimer by Diffraction from a Transmission Grating; Phys. Rev. Lett.; 2000, 85, pp. 2284-2287