Hydrogen bond

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A hydrogen bond is a low kind type of dipole-dipole bond that exists between an electronegative molecule and a hydrogen molecule bonded to another electronegative molecule. This type of bond always involves a hydrogen molecule. That explains the name.

Hydrogen bonds can occur between molecules (intermolecularly), or within different parts of a single molecule (intramolecularly).[1] The typical hydrogen bond is stronger than van der Waals forces, but weaker than covalent, ionic and metallic bonds.

Intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C).

References[change | edit source]

  • George A. Jeffrey. An Introduction to Hydrogen Bonding (Topics in Physical Chemistry). Oxford University Press, USA (March 13, 1997). ISBN 0-19-509549-9
  • A New Intermolecular Interaction: Unconventional Hydrogen Bonds with Element-Hydride Bonds as Proton Acceptor Robert H. Crabtree, Per E. M. Siegbahn, Odile Eisenstein, Arnold L. Rheingold, and Thomas F. Koetzle Acc. Chem. Res. 1996, 29(7), 348 - 354.
  • Polymerization of Formic Acid under High Pressure Alexander F. Goncharov, M. Riad Manaa, Joseph M. Zaug, Richard H. Gee, Laurence E. Fried, and Wren B. Montgomery Phys. Rev. Lett. 2005, 94, 065505.
  • F. Cordier, M. Rogowski, S. Grzesiek and A. Bax. Observation of through-hydrogen-bond (2h)J(HC') in a perdeuterated protein. J Magn Reson. (1999) 140: 510-2.
  • R. Parthasarathi, V. Subramanian, N. Sathyamurthy.Hydrogen Bonding Without Borders: An Atoms-In-Molecules Perspective. J. Phys. Chem. (A) (2006) 110: 3349-3351.