Nitrogen molecule London forces

The electron density changes continually, so induced dipoles never last more than about 10-11 s. Nevertheless, they last sufficiently long for an interaction to form with the induced dipole of another nitrogen molecule nearby. We call this new interaction the London dispersion force after Fritz London, who first postulated their existence in 1930. 

Intermolecular forces can be of three different tjq>es. The first t5q>e is called a London force or dispersion force. This very weak type of attraction generally occurs between nonpolar covalent molecules, such as nitrogen (Nj), hydrogen (H ), or methane (CE ). It results from the ebb and flow of the electron orbitals, giving a very wesik and very brief charge separation around the bond. 

The assumption is most valid for nonpolar gases, such as hydrogen and nitrogen, because the attractive forces involved are London forces, weak forces that have to do with the ebb and flow of the electron orbitals. However, if the gas molecules are polar, as in water and HCl, this assumption can become a problem, because the forces are stronger. (Turn to Chapter 6 for the scoop on London forces and polar things — all related to the attraction between molecules.)... 

Molecules are transported from surfaces of activated carbon by diffusion and trapped on sites by physisorption, primarily via weak London dispersion forces. Activated carbon cloth or carbon-impregnated paper, used as packing materiak for cellulose nitrate, readily adsorb nitrogen oxides - CN s primary degradation... 

---