London dispersion forces, named after the German-American physicist Fritz London, are weak intermolecular forces that arise from the interactive forces between instantaneous multipoles in molecules without permanent multipole moments.
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The strength of London dispersion forces is proportional to the polarizability of the molecule, which in turn depends on the total number of electrons and the area over which they are spread.
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Later computational work from the Sherill group revealed that the substituent effects for the sandwich configuration are additive, which points to a strong influence of dispersion forces and direct interactions between substituents.
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London dispersion forces are particularly useful for the function of adhesive devices, because they don't require either surface to have any permanent Dispersive forces are a consequence of statistical quantum mechanics.
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A classic molecular solid consists of small, non-polar covalent molecules, and is held together by London dispersion forces ( van der Waals forces ); a classic example is paraffin wax.
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:Basically, in a substance, the atoms that make it up are pulled toward eachtother by intermolecular forces ( Hydrogen, Ionic, and Covalent bonds, London dispersion forces, etc . ).
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:: Forces " stronger " than London dispersion forces that are also van der Waals include Debye forces, Keesom forces, hydrogen bonds, ionic bonds and induced ion forces; see intermolecular force.
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Disjoining pressure is interpreted as a sum of several interactions : dispersion forces, electrostatic forces between charged surfaces, interactions due to layers of neutral molecules adsorbed on the two surfaces, and the structural effects of the solvent.
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Again a large amount of energy is required to melt / boil as covalent bonds must be broken; by contrast, nitrogen and oxygen are covalent molecular substances with individual diatomic molecules held together by only very weak dispersion forces.
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When hydrocarbon molecules ( oil ) are forced into water layer, hydrogen bond of water molecules and some dispersion forces between hydrocarbon molecules must have been destroyed, and new water-hydrocarbon interaction must have been formed in this state.
