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Hydrogen bond

form of association between an electronegative atom and a hydrogen atom attached to a second, relatively electronegative atom / From Wikipedia, the free encyclopedia

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.

Model of hydrogen bonds (1) between molecules of water

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.

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