Table of Contents
Introduction to the London Dispersion Force
London Dispersion Forces – Examples: The London dispersion force (LDF) is a weak intermolecular force that arises from the interaction of the electron clouds of neighboring atoms. The LDF is responsible for the attractive forces between molecules that leads to the formation of liquids and also solids. The LDF is also responsible for the boiling point of a liquid and the melting point of a solid.
London Forces Definition
London dispersion forces are intermolecular forces that occur between non-polar molecules. These forces are responsible for the attraction between molecules and also for the cohesion of non-polar substances. London dispersion forces weak compared to other intermolecular forces, but they important because they the only intermolecular force that present in all substances. London dispersion forces are caused by the uneven distribution of electrons in the electron clouds of atoms. This uneven distribution creates temporary dipoles, which are responsible for the attractive force between molecules. However london dispersion forces increase with the size of the molecule and with the number of electrons in the molecule.
London Dispersion Forces Examples
The London dispersion forces are weak forces that exist between the electron clouds of adjacent atoms. Therefore these forces are caused by the interactions of the electrons’ electron clouds. The London dispersion forces are the weakest of the intermolecular forces.
London Dispersion Forces Formula
The London dispersion forces are weak forces that arise from the interaction of the electron clouds of adjacent atoms. These forces responsible for the attraction of nonpolar molecules to one another. The London dispersion forces also known as van der Waals forces.
London dispersion forces the weakest of the intermolecular forces. They present between all molecules and due to the uneven distribution of electrons around the nucleus of an atom. The formula for London dispersion forces is:
F = C₁/r₁³ + C₂/r₂³
Where:
F is the force between the molecules (in dynes)
C₁ and C₂ are the London dispersion coefficients for the two molecules (in atomic units)
r₁ and r₂ are the distances between the centers of the two molecules (in Angstroms)
