London Dispersion Forces
Some of the key features of London Dispersion Forces are:
London dispersion forces are present between any two molecules, even polar ones. These forces occur when the molecules are almost touching. This force is sometimes called an induced dipole-induced dipole attraction. This force is a temporary attractive force. It results when the electrons in two adjacent atoms or molecules occupy positions that make the atoms form an instantaneous dipole. They are the weakest intermolecular forces. They are responsible for any compound’s liquid, solid, and solution states.
Key Features of London Dispersion Forces
- Temporary Dipole: An atom or molecule can develop a temporary (instantaneous) dipole when its electrons are not symmetrically distributed with respect to the nucleus.
- Induced Dipole: A second atom or molecule can be distorted by the appearance of the dipole in the first atom or molecule, leading to an electrostatic attraction between them.
- Weak Intermolecular Force: London dispersion forces are weaker than dipole-dipole and hydrogen bonding forces.
- Cumulative Effect: Although the London dispersion force between individual atoms and molecules is relatively weak, the effect is cumulative over the volume of materials, making it stronger in bulk solids and liquids.
Some examples of London dispersion forces are n-pentane and neopentane.
Check: Propane Formula
Van Der Waals Force
Van der Waals forces are intermolecular forces. They include attraction and repulsion between atoms and molecules. This force is fundamental in diverse fields which include condensed matter physics, polymer science, nanotechnology, supra-molecular chemistry, biological structure, and surface science.
In this article, we look into Van der Waals forces their types, the equation of the Van der Waals force, and their applications.
Table of Content
- What are Van der Waals Forces?
- Types of Van der Waals Forces
- Keeson Interaction
- Debye Forces
- London Dispersion Forces
- Formula for Van der Waals Force
- Characteristics of Van der Waals Forces
- Factor Affecting Van der Waals Force
- Applications of Van der Waals forces