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  2. Intermolecular force - Wikipedia

    en.wikipedia.org/wiki/Intermolecular_force

    The attractive force draws molecules closer together and gives a real gas a tendency to occupy a smaller volume than an ideal gas. Which interaction is more important depends on temperature and pressure (see compressibility factor). In a gas, the distances between molecules are generally large, so intermolecular forces have only a small effect.

  3. Gas - Wikipedia

    en.wikipedia.org/wiki/Gas

    The interaction of these intermolecular forces varies within a substance which determines many of the physical properties unique to each gas. [11] [12] A comparison of boiling points for compounds formed by ionic and covalent bonds leads us to this conclusion. [13] Compared to the other states of matter, gases have low density and viscosity.

  4. Category:Intermolecular forces - Wikipedia

    en.wikipedia.org/wiki/Category:Intermolecular_forces

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  5. Sigma hole interactions - Wikipedia

    en.wikipedia.org/wiki/Sigma_Hole_interactions

    In chemistry, sigma hole interactions (or σ-hole interactions) are a family of intermolecular forces that can occur between several classes of molecules and arise from an energetically stabilizing interaction between a positively-charged site, termed a sigma hole, and a negatively-charged site, typically a lone pair, on different atoms that are not covalently bonded to each other. [1]

  6. London dispersion force - Wikipedia

    en.wikipedia.org/wiki/London_dispersion_force

    Interaction energy of an argon dimer.The long-range section is due to London dispersion forces. London dispersion forces (LDF, also known as dispersion forces, London forces, instantaneous dipole–induced dipole forces, fluctuating induced dipole bonds [1] or loosely as van der Waals forces) are a type of intermolecular force acting between atoms and molecules that are normally electrically ...

  7. Molecular solid - Wikipedia

    en.wikipedia.org/wiki/Molecular_solid

    [19] [20] [21] All atoms and molecules can partake in van der Waals and London dispersion forces . It is the lack or presence of other intermolecular interactions based on the atom or molecule that affords materials unique properties. [19]

  8. Van der Waals force - Wikipedia

    en.wikipedia.org/wiki/Van_der_Waals_force

    The strength of pairwise van der Waals type interactions is on the order of 12 kJ/mol (120 meV) for low-melting Pb and on the order of 32 kJ/mol (330 meV) for high-melting Pt , which is about one order of magnitude stronger than in Xe due to the presence of a highly polarizable free electron gas. [12] Accordingly, van der Waals forces can range ...

  9. Lifshitz theory of van der Waals force - Wikipedia

    en.wikipedia.org/wiki/Lifshitz_Theory_of_Van_der...

    In condensed matter physics and physical chemistry, the Lifshitz theory of van der Waals forces, sometimes called the macroscopic theory of van der Waals forces, is a method proposed by Evgeny Mikhailovich Lifshitz in 1954 for treating van der Waals forces between bodies which does not assume pairwise additivity of the individual intermolecular forces; that is to say, the theory takes into ...