Notes on Hydrophobic Interactions and London Dispersion Forces

When hydrophobic molecules come close to one another, their association is stabilized by van der Waals forces.
These are weak electrical attractions caused by the constant motion of electrons, which give molecules a tiny asymmetry in charge that changes with time.
If nonpolar molecules get extremely close, the minute partial charge on one molecule induces an opposite partial charge in the nearby molecule, causing an attraction.
This specific van der Waals interaction is called the London dispersion force, named after Fritz London.
Although the interaction is very weak relative to covalent bonds or even hydrogen bonds, a large number of van der Waals interactions can significantly increase the stability of clustered hydrophobic molecules.

A type of van der Waals interaction that arises from instantaneous dipoles induced by electron motion in nonpolar molecules.
The effect occurs when nonpolar molecules come very close to each other, allowing instantaneous dipoles to induce dipoles in neighboring molecules and create attractions.

The clustering of hydrophobic molecules is stabilized by van der Waals attractions as they approach one another.
The cumulative effect of many weak London dispersion forces can greatly enhance the stability of these clusters.

The constant motion of electrons causes a tiny asymmetry in charge that changes with time, creating instantaneous dipoles.
An instantaneous dipole in one molecule induces an opposite dipole in a nearby molecule, leading to attraction (induced dipole–induced dipole interaction).

London dispersion forces are weaker than covalent bonds and hydrogen bonds on a per-interaction basis.
The aggregation and stability of hydrophobic assemblies rely on the collective strength of many such weak interactions.

Van der Waals interactions are weak electrical attractions caused by the constant motion of electrons, creating temporary charge asymmetries (instantaneous dipoles).
These forces stabilize the association of hydrophobic molecules.
The London dispersion force (LDF) is a specific type of van der Waals interaction where an instantaneous dipole in one nonpolar molecule induces an opposite dipole in a neighboring molecule, leading to attraction.
Although individually weak, the cumulative effect of many LDFs significantly increases the stability of clustered hydrophobic molecules.