- #1
chikou24i
- 45
- 0
Hello! In Van der Waals interaction, how to prove that : H= - (2*e^2*x1*x2) / R^3 ?
chikou24i said:Hello! In Van der Waals interaction, how to prove that : H= - (2*e^2*x1*x2) / R^3 ?
chikou24i said:I'm talking about the Coulomb interaction energy between two harmonic oscillator ( two atoms modelised by two harmonic oscillator)
Now you understand me, and this is what I'm looking for if you can help me.Quantum Defect said:What you will do is approximate the 1/(R_1,2) terms in a Taylor approximation when R_1,2 >> r, where r is the length of the dipole. You will find that the terms that survive are the ones that look like 1/R^3. The sign (attractive, repulsive) and leading coefficient depend upon the orientation of the two dipoles.
A Van der Waals interaction is a type of intermolecular force that occurs between neutral molecules. It is caused by the temporary dipoles that are formed due to the random movement of electrons in a molecule.
Van der Waals forces can affect the physical properties of molecules, such as their boiling and melting points, as well as their ability to dissolve in certain solvents. These forces also contribute to the stability of certain molecular structures.
Van der Waals forces are generally weaker than other types of intermolecular forces, such as hydrogen bonding or covalent bonding. However, they can still play a significant role in determining the overall behavior of molecules.
While Van der Waals forces cannot be directly manipulated, they can be affected by changing the conditions in which molecules are present. For example, temperature and pressure can influence the strength of Van der Waals interactions between molecules.
The strength of Van der Waals interactions is directly related to the size and shape of molecules. Larger molecules with more surface area tend to have stronger Van der Waals forces, as there is more opportunity for temporary dipoles to form.