Hydrogen bonds
Hydrogen Bonds
Hydrogen bonds (pronunciation: /ˈhaɪdrədʒən bɒndz/) are a type of attractive intermolecular force that occurs when a hydrogen atom bonded to a highly electronegative atom exists in the vicinity of another electronegative atom with a lone pair of electrons.
Etymology
The term "hydrogen bond" is derived from the fact that the bond involves a hydrogen atom. The word "hydrogen" comes from the Greek words "hydro" (water) and "genes" (forming), while "bond" is derived from the Old English "bendan", meaning "to bind or fasten together".
Definition
Hydrogen bonds are usually stronger than a van der Waals interaction, but weaker than covalent or ionic bonds. This type of bond can occur between molecules (intermolecular) or within different parts of a single molecule (intramolecular).
Properties
Hydrogen bonds have a typical length of 1.97 Ångström (Å) and a strength of 5 to 30 kJ/mol. They are responsible for the unique properties of water and important in many biological systems, including DNA and proteins.
Related Terms
See Also
External links
- Medical encyclopedia article on Hydrogen bonds
- Wikipedia's article - Hydrogen bonds
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