User:GoBlue18/sandbox
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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[1]. The 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).[2] Non-covalent interactions can be generally classified into 4 categories: electrostatic, π-effects, van der Waals forces, and hydrophobic effects[1] [2]. In fact, van der Waals forces are responsible for why geckos can walk up and down walls![3]
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Non-covalent interactions are the dominant type of interaction between supermolecules in supermolecular chemistry.[4], 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[1] [5][6][7].
Intermolecular forces are a subset of non-covalent interactions, simply because non-covalent interactions can be both intermolecular (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[1].