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Why Hydrogen bonding is not a van der Waal force?

Hydrogen bonding is a type of electrostatic interaction occurring in molecules in which the H atom is sandwiched between highly electronegative atoms like F, O, and N, one to which it is covalently bonded. For example, HF, H2O, NH3, etc.

Hydrogen bonding dipole-dipole interaction

 

The strong covalent bond polarization between the small H atom and a highly electronegative atom (like F, O, and N) creates dipoles.

Dipoles in Hydrogen bonding

 

When such molecules associate, they do so with their dipole to have dipole-dipole interactions. But only a small class of molecules have such high electronegative atoms. Therefore, though such molecules are polar and show dipole-dipole interactions, the Hydrogen Bonding interactions are relatively stronger and treated separately than the other intermolecular Vander Waal interactions- Debye, Keesom, and London Dispersion Forces.

For example, only HF shows Hydrogen Bonding dipole-dipole interaction. HCl, HBr, and HI will not show Hydrogen bonding, but they will interact using Vander Waal Keesom Forces (dipole-dipole interactions).

Only HF shows Hydrogen Bonding and HCl, HBr, HI don't

 

Related Reading-

 Hydrogen Bonding 

Introduction to Vander Waal Forces

Keesom Forces 

What is electronegativity?

 

Intermolecular Forces
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