Dipole interaction will not occur among molecules of PF5 (phosphorus pentafluoride) because the molecule is non-polar. However, dispersion forces will come into play because of the random motion of electrons around the 5 fluorine atoms bonded to the phosphorus. This will result in very brief attractions based upon the "bunching up" of electrons during their random motion. Dispersion forces are the weakest of the inter-molecular forces.
The two forces that are present between molecules of IF5 are dispersion and dipole-dipole interactions forces. Each I-F bond is polar.
The Londen Dispersion force
London dispersion forces
Dipole-dipole forces are dominant.
Dipole forces and London forces are present between these molecules.
Dipole forces and London forces are present as intermolecular forces in these molecules.
London forces are present in chlorine molecules.
These are polar forces, intermolecular forces of attraction between molecules.
London forces are the only forces present in neon molecules.
Dipole forces and London forces are present between these molecules.
Dipole forces and London forces are present between these molecules.
Dipole forces and London forces are present as intermolecular forces in these molecules.
London forces are present in chlorine molecules.
Dipole forces and London forces are present between these molecules.
These are polar forces, intermolecular forces of attraction between molecules.
London forces are the only forces present in neon molecules.
all such forces are intermolecular forces.
Sodium chloride does not exist as molecules.
Intermolecular forces are any forces exerted on neighboring molecules of a given compound. The forces are not the actual chemical bonds present in the substance, but rather the substances own attractiveness to its own molecules. These intermolecular forces play a crucial role in determining a compounds various physical properties such as but not limited to :solubility, melting point, boiling point, density.
Dispersion
dipole forces and induced dipole forces