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The '''London dispersion force''' is a type of [[intermolecular force]] named for the physicist Fritz London. It occurs between molecules that do not have permanent dipoles (ie. do not have a permanently positive and a permanently negative end), and is also known as induced dipole-dipole forces.

The '''London dispersion force''' is a type of [[intermolecular force]] named for the physicist Fritz London. It occurs between molecules that do not have permanent dipoles (ie. do not have a permanently positive and a permanently negative end), and is also known as induced dipole-dipole forces.

The [[electrons]] about a [[molecule]] of [[Bromine]], Br-Br, are, in theory, evenly distributed. However, in practice, they are randomly scattered, meaning that there is a high probability that they are found more towards one end than the other. This creates a slight charge on both ends, which then causes other nearby molecules to form temporary dipoles as well. This charge creates a weak attraction between the molecules, which means, when the temperature is low enough, they will form liquids. The dipoles are temporary, unlike polar substances, which have a permanent dipole. The London dispersion force explain why non-polar solvents do not exist only as [[gas]]; due to the London dispersion force, they have a [[liquid]] and a  [[solid]] form.

The [[electrons]] about a [[molecule]] of [[Bromine]], Br-Br, are, in theory, evenly distributed around the two Bromine atoms. However, in practice, they are randomly scattered, meaning that there is a high probability that they are found more towards one end than the other. This creates a slight charge on both ends, which then causes other nearby molecules to form temporary dipoles as well. This charge creates a weak attraction between the molecules, which means, when the temperature is low enough, they will form liquids. The dipoles are temporary, unlike polar substances, which have a permanent dipole. The London dispersion force explain why non-polar solvents do not exist only as [[gas]]; due to the London dispersion force, they have a [[liquid]] and a  [[solid]] form.