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Non-covalent interactions
A non-covalent interaction differs from a covalent bond in that it does not involve the sharing of electrons, but rather involves more dispersed variations of electromagnetic interactions between molecules or within a molecule. The chemical energy released in the formation of non-covalent interactions is typically on the order of 1-5 kcal/mol (1000–5000 calories per 6.02 x 10^23 molecules).〔(Noncovalent bonds ) – Molecular Cell Biology (textbook), Lodish, Berk, Zipursky, Matsudaira, Baltimore, Darnell.〕 Non-covalent interactions can be generally classified into four categories, electrostatic, π-effects, van der Waals forces, and hydrophobic effects.〔〔
Non-covalent interactions are the dominant type of interaction between supermolecules in supermolecular chemistry.,〔(Noncovalent bonding in Supramolecular Chemistry ) - Christoph A. Schalley〕 and are critical in maintaining the three-dimensional structure of large molecules, such as proteins and nucleic acids. In addition, they are also involved in many biological processes in which large molecules bind specifically but transiently to one another (see the properties section of the DNA page). These interactions also heavily influence drug design, crystallinity and design of materials, particularly for self-assembly, and, in general, the synthesis of many organic molecules.〔
Intermolecular forces are a subset of non-covalent interactions, simply because non-covalent interactions can be both inter molecular, i.e. interaction between water molecules, and intramolecular, i.e. protein folding. Intermolecular forces, on the other hand, are defined as interactions ''between'' molecules, and not within molecules.〔
== Electrostatic interactions ==
''For a more detailed introduction to electrostatics, see Coulomb's Law''
抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』
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