Hydrogen bond

A hydrogen bond is a type of chemical bond that weakly attaches a molecule to another molecule. It is based on the attraction between opposite electric charges. The negative charge on an electronegative atom of one molecule is attracted to a positive charge on a hydrogen atom of another molecule. The hydrogen atom carries a positive charge because it is bonded to a second electronegative atom, which shifts electrons away from the hydrogen. This type of bond always involves a hydrogen atom, and two electronegative atoms. The electronegative atoms are often oxygen or nitrogen. Hydrogen bonds are important in polar solvents such as water and alcohol,^[1] in biomolecules, and in many other materials.

Hydrogen bonds can occur between molecules (intermolecular bonds), or between different parts of a single molecule (intramolecular bonds).^[2] The typical hydrogen bond is stronger than van der Waals forces, but weaker than covalent, ionic and metallic bonds.

1. ↑ Breslyn, Wayne. "Hydrogen Bonding in Ethanol (C2H5OH)". Retrieved 31 May 2021.
2. ↑ Compendium of Chemical Terminology, hydrogen bond, accessed 15 Jan 2007.