Related Experiment Video
Updated: Feb 28, 2026
10:37
Spatial Separation of Molecular Conformers and Clusters
Published on: January 9, 2014
11.8K
Long-Range Repulsion Between Spatially Confined van der Waals Dimers
Mainak Sadhukhan1, Alexandre Tkatchenko1
1Physics and Materials Science Research Unit, University of Luxembourg, Luxembourg L-1511, Luxembourg.
Physical Review Letters
|June 10, 2017
Summary
Contrary to established knowledge, long-range van der Waals (vdW) forces between confined quantum systems can become repulsive. This study reveals repulsion due to full Coulomb interactions, challenging the universality of vdW attraction.
Area of Science:
- Quantum mechanics
- Intermolecular forces
- Condensed matter physics
Background:
- Nonretarded van der Waals (vdW) interactions are typically attractive between isotropic dimers due to dipolar coupling.
- This attractive force is considered universal across different polarizabilities and spatial dimensions.
Purpose of the Study:
- To investigate the nature of vdW interactions in spatially confined quantum systems.
- To determine if the universality of vdW attraction holds under confinement and full Coulomb interaction.
Main Methods:
- Analytic calculations using the Coulomb potential as a perturbation.
- Modeling two quantum harmonic oscillators in reduced dimensionality.
- Analyzing dipole-correlated states.
Main Results:
- Demonstrated that long-range vdW interactions become repulsive for spatially confined dimers.
- Identified the full Coulomb interaction between charge fluctuations as the cause of repulsion.
- The phenomenon is expected to be general for confined quantum systems.
Conclusions:
- The universality of vdW attraction is not absolute and can be overcome by confinement effects.
- Repulsive vdW interactions in confined systems have implications for nanoscale environments.
- Provides a theoretical basis for observed phenomena like strong screening of vdW interactions on metal surfaces.
Related Concept Videos
01:24Van der Waals Interactions
72.6K
Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions between particles with permanent, partial, or temporary charges. The intermolecular forces between neutral atoms and molecules are ion–dipole, dipole–dipole, and dispersion forces, collectively known as van der Waals forces.
72.6K
03:13Intermolecular Forces
74.2K
Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen...
74.2K
01:26The Van der Waals Equation
19
The ideal gas law is based on two simplifying assumptions: first, that there are no intermolecular attractions between gas molecules, and second, that the volume occupied by the molecules themselves is negligible compared with the volume of the container. However, these assumptions don't hold up under all conditions - specifically, at high pressures and low temperatures, as gas tends to deviate from ideal gas behavior.The van der Waals equation is an enhanced version of the ideal gas law,...
19
02:37VSEPR Theory
15.2K
Valence shell electron-pair repulsion theory (VSEPR theory) enables us to predict the molecular structure around a central atom from an examination of the number of bonds and lone electron pairs in its Lewis structure. The VSEPR model assumes that electron pairs in the valence shell of a central atom will adopt an arrangement that minimizes repulsions between these electron pairs by maximizing the distance between them. The electrons in the valence shell of a central atom form either bonding...
15.2K
02:56Intermolecular Forces and Physical Properties
28.9K
28.9K
04:01VSEPR Theory and the Effect of Lone Pairs
53.6K
Effect of Lone Pairs of Electrons on Molecule Geometry
53.6K