London dispersion force

You never have figured out just what London dispersion forces are, but they don't sound good.

The sensors showed an atmosphere heavy with particulate matter and London dispersion forces.

The London dispersion force arises due to instantaneous dipoles in neighbouring atoms.

London dispersion forces arise from instantaneous dipoles between two nonpolar molecules close together.

Lipophilic substances interact within themselves and with other substances through the London dispersion force.

London dispersion forces are particularly useful for the function of adhesive devices, because they don't require either surface to have any permanent polarity.

(The London dispersion force, for example, depends on the correlations of the motion of the electrons.)

The induction-interaction force is far weaker than dipole-dipole interaction, but stronger than the London dispersion force.

They occur from either momentary interactions between molecules (the London dispersion force) or permanent electrostatic attractions between dipoles.

Lipophilicity, hydrophobicity, and non-polarity can describe the same tendency towards participation in the London dispersion force as the terms are often used interchangeably.

The "tail" is hydrophobic due to being non-polar and lipophobic because fluorocarbons are less susceptible to the London dispersion force than hydrocarbons.

Physically, activated carbon binds materials by van der Waals force or London dispersion force.

This effect is due to the increased strength of the molecules intermolecular forces-from London dispersion forces to dipole-dipole interactions created with the increased polarity.

These interactions include London dispersion forces, Keesom forces, Debye forces and hydrogen bonds.

London dispersion forces are also known as dispersion forces, London forces, or instantaneous dipole-induced dipole forces.

Van der Waals forces (Keesom force, Debye force, and London dispersion force)

The reduced participation in the London dispersion force makes the solid polytetrafluoroethylene (PTFE) slippery as it has a very low coefficient of friction.

The benzene dimer in the sandwich configuration is stabilized by London dispersion forces but destabilized by repulsive quadrupole/quadrupole interactions.

For atoms and nonpolar molecules, the London dispersion force is the only intermolecular force, and is responsible for their existence in liquid and solid states.

The relative binding energies of these three geometric configurations of the benzene dimer can be explained by a balance of quadrupole/quadrupole and London dispersion forces.

Otherwise known as quantum-induced instantaneous polarization or instantaneous dipole-induced dipole force, the London dispersion force is caused by correlated movements of the electrons in interacting molecules.

Thus, the London Dispersion Forces between ethane molecules are higher than that between methane molecules, resulting in stronger forces of intermolecular attraction, raising the boiling point.

These intermolecular screening forces are also known as Van der Waals forces, which is determined by the Keesom, Debye and London Dispersion forces.

His fundamental contributions to the theories of chemical bonding and of intermolecular forces (London dispersion forces) are today considered classic and are discussed in standard textbooks of physical chemistry.

They are not as susceptible to the London dispersion force, a factor contributing to lipophilicity, because the electronegativity of fluorine reduces the polarizability of the surfactants' fluorinated molecular surface.