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London Dispersion Force

1930
  • Fritz London
Laboratory experiment demonstrating London dispersion force in noble gases.

The London dispersion force (LDF) is the weakest type of Van der Waals force, arising from quantum mechanical fluctuations in the electron clouds of atoms and molecules. These fluctuations create temporary, instantaneous dipoles that induce corresponding dipoles in neighboring atoms, resulting in a net attractive force. The interaction potential energy \(V\) between two atoms at distance \(r\) is approximately \(V = -\frac{C_6}{r^6}\).

The London dispersion force is a universal attractive force that exists between all atoms and molecules, even nonpolar ones where other intermolecular forces are absent. Its origin is purely quantum mechanical. According to quantum theory, the electron distribution around an atom is not static but fluctuates over time. At any given instant, the electron cloud can be momentarily distorted, creating a temporary electric dipole. This instantaneous dipole generates an electric field that polarizes the electron cloud of a neighboring atom, inducing a synchronized dipole in it. The interaction between these two correlated, temporary dipoles results in a weak, short-lived attraction.

The strength of the LDF depends on the polarizability of the molecule—how easily its electron cloud can be distorted. Larger atoms with more electrons, particularly those in outer shells far from the nucleus, are more polarizable and thus experience stronger dispersion forces. This explains why the boiling points of noble gases and nonpolar hydrocarbons increase with molecular size. Although individually weak, the cumulative effect of London forces can be substantial, playing a critical role in the structure of condensed matter, protein folding, and the adhesion of macroscopic objects.

UNESCO Nomenclature: 2202
– Atomic and molecular physics

Type

Physical Law

Disruption

Revolutionary

Usage

Widespread Use

Precursors

  • Schrödinger Equation and the development of Quantum Mechanics
  • Classical theory of electromagnetism and polarization
  • Heitler-London theory of the covalent bond, which introduced quantum exchange interactions
  • Earlier Van der Waals concepts that lacked a mechanism for nonpolar attraction

Applications

  • explaining the liquefaction of noble gases like helium and argon
  • adhesion mechanisms in gecko feet and dry adhesives
  • cohesion and physical properties of nonpolar polymers like polyethylene
  • drug-receptor binding in pharmacology, especially in hydrophobic pockets
  • stability of colloidal suspensions

Patents:

NA

Potential Innovations Ideas

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Related to: London dispersion force, induced dipole, quantum mechanics, polarizability, intermolecular force, Van der Waals, nonpolar molecules, electron correlation, adhesion, noble gases.

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Historical Context

(if date is unknown or not relevant, e.g. "fluid mechanics", a rounded estimation of its notable emergence is provided)

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