Debye Forces
This force is named after Peter J. W. Debye. It is an attractive interaction between the permanent dipoles of polar molecules and the dipoles they may induce in similar molecules. It is caused by the interaction of permanent dipoles with dipoles induced by them in electron clouds. This interaction is always attractive and does not vanish with distance. This force is one of the essential parts of force fields frequently used in molecular mechanics.
Key Features of Debye Force
Some of the key features of Debye Force are:
- Interaction: Debye forces result from the interaction between the permanent dipoles of polar molecules and the dipoles induced by them in electron clouds
- Strength: Debye forces are stronger than the London dispersion force (instantaneous dipole-induced dipole) but weaker than the Keeson orientation effect
- Attractive nature: Debye forces are always attractive and do not vanish at higher temperatures
Some example of Debye forces are a polar molecule like hydrogen bromide (HBr) and a non-polar or symmetrical molecule like argon (Ar).
Check: Argon Gas 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