Hydrogen bonds can occur between molecules (intermolecularly), or within different parts of a single molecule (intramolecularly). 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). Most molecules with hydrogen bonding have high boiling points and melting points. Because hydrogen bonds are what make water stick together so well, they also help other molecules that can make hydrogen bonds dissolve in water. This is because the molecules form bonds with the hydrogen in the water, too, helping them dissolve.
References[change | change 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.