Hydrogen Bonding
A hydrogen bond is the attraction between the lone pair of an electronegative atom and a hydrogen atom that is bonded to either nitrogen, oxygen, or fluorine. The hydrogen bond is often described as a strong electrostatic dipole–dipole interaction. However, it also has some features of covalent bonding: it is directional, stronger than a van der Waals interaction, produces interatomic distances shorter than sum of van der Waals radii, and usually involves a limited number of interaction partners, which can be interpreted as a kind of valence.
Intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C) compared to the other group 16 hydrides that have no hydrogen bonds. Intramolecular hydrogen bonding is partly responsible for the secondary, tertiary, and quaternary structures of proteins and nucleic acids. It also plays an important role in the structure of polymers, both synthetic and natural.
Read more about this topic: Intermolecular Force
Famous quotes containing the words hydrogen and/or bonding:
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—Edward D. Wood, Jr. (1922–1978)
“The bottom line on bonding with multiples seems to be that if you see bonding as a static event—a moment in time at which you must have eye contact and skin contact simultaneously with two or more infants—you may indeed be in trouble.”
—Pamela Patrick Novotny (20th century)