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Van der Waals Interactions

Van der Waals Interactions

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.Polar molecules have a partial positive charge on one end and a partial negative charge on the other end of the molecule,...

Intermolecular Forces

Intermolecular Forces

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 bonds, and dispersion...

Intermolecular Forces

Intermolecular Forces

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 bonds, and dispersion...

Intermolecular Forces and Physical Properties

Intermolecular Forces and Physical Properties

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...

Intermolecular Forces in Solutions

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The formation of a solution is an example of a spontaneous process, a process that occurs under specified conditions without energy from some external source.
When the strengths of the intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components, the solution is formed with no accompanying energy change. Such a solution is called an ideal solution. A mixture of ideal gases (or gases such as helium and argon,...

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Related Experiment Video

Updated: Jun 13, 2026

Spatial Separation of Molecular Conformers and Clusters

Spatial Separation of Molecular Conformers and Clusters

Published on: January 9, 2014

Dispersion forces between solvated electrons.

Gennady N Chuev¹

¹Max Planck Institute for Mathematics in the Sciences, Inselstrasse 22, Leipzig 04103, Germany. genchuev@rambler.ru

The Journal of Chemical Physics

|April 22, 2010

Summary

Dispersion interactions control solvated electron behavior in metal-ammonia solutions, causing a nonmetal-metal transition. Beyond this transition, electrons exist as localized and delocalized components.

Area of Science:

Physical Chemistry
Condensed Matter Physics
Materials Science

Background:

Solvated electrons in metal-ammonia solutions are crucial for understanding electronic properties.
Dispersion interactions are hypothesized to influence electron behavior at finite metal concentrations.

Purpose of the Study:

Investigate dispersion interactions between solvated electrons.
Determine the role of these interactions in the nonmetal-metal transition.

Main Methods:

Path integral centroid approach.
Analysis of dielectric enhancement and mechanical instability.

Main Results:

Dispersion interactions govern solvated electron behavior at finite metal concentrations.

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A distinct nonmetal-metal transition is observed, marked by dielectric enhancement and mechanical instability.

Solvated electrons form a two-component mixture (localized and delocalized) beyond the critical density.

Conclusions:

Dispersion interactions are key to understanding the electronic and structural properties of metal-ammonia solutions.
The nonmetal-metal transition signifies a fundamental change in electron state and system stability.
The two-component electron model provides a more accurate description of the system beyond the critical density.