Is hydrogen bonding considered to be a type of Van der waals force?
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No. Hydrogen bonding is the electrostatic force between a hydrogen bound to an very electronegative atom (F, O, N) and a pair of nonbonding electrons on a very electronegative atom (F, O, N). It is the attraction of a permanent Lewis acid for a permanent Lewis base. Van der Waal's forces are a sort of induced electrostatic force between molecules that aren't really either acidic or basic (in a Lewis acid/base sense). The electron density of one molecule, which is always moving and changing, randomly darts toward the electron density of the other. The repulsive force between electrons pushes the electrons (electron density) in that location of the second molecule away, making that location temporarily slightly more positive than it was. That temporary partial positive charge on the second molecule attracts electron density of the first, which holds the molecules together until the distribution of electron density rearranges itself again. However, what happened at one spot will sooner or later happen at another, and the net result of all these temporary attractions is an average attraction between molecules that don't have a permanent partial negative or partial positive charge, or an electric dipole moment.
Hydrogen bonding is much stronger than Van der Waal's forces.
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Hydrogen bonding is much stronger than Van der Waal's forces.
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