Hydrogen bonding
Hydrogen Bonding
Hydrogen bonding (pronunciation: /ˈhaɪdrədʒən ˈbɒndɪŋ/) is a special type of dipole-dipole interaction that occurs between an electronegative atom and a hydrogen atom bonded to another electronegative atom. This type of bond can occur in both inorganic molecules such as water and organic molecules like DNA.
Etymology
The term "hydrogen bond" is derived from the bond's reliance on the element hydrogen. The concept of hydrogen bonding was first introduced by Wendell Mitchell Latimer and Worth H. Rodebush in 1920.
Related Terms
- Dipole-dipole interaction: A type of intermolecular force between two polar molecules.
- Electronegativity: The measure of the tendency of an atom to attract a bonding pair of electrons.
- Intermolecular forces: The forces of attraction between molecules.
- Intramolecular forces: The forces that hold atoms together within a molecule.
- Van der Waals forces: The residual attractive or repulsive forces between molecules or atomic groups.
Hydrogen Bonding in Water
In water molecules, hydrogen bonding occurs between the hydrogen atom in one water molecule and the oxygen atom in another. This is due to the high electronegativity of the oxygen atom compared to the hydrogen atom, creating a dipole-dipole interaction.
Hydrogen Bonding in DNA
In DNA, hydrogen bonding is crucial for the formation of base pairs between adenine and thymine, and between guanine and cytosine. These hydrogen bonds provide stability to the DNA molecule and are crucial for DNA replication.
External links
- Medical encyclopedia article on Hydrogen bonding
- Wikipedia's article - Hydrogen bonding
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