Large molecules with many electrons are most polarizable.
The higher the polarizability of a molecule, the stronger its intermolecular forces.
Which molecule has the largest London dispersion forces?
Size of Molecule. The larger the molecule, the greater the London dispersion forces. This is because larger molecules have a bigger electron cloud, thus creating a stronger temporary dipole when the electrons become asymmetrically distributed. Bromine is a much larger molecule than fluorine.
Which has the strongest dispersion forces?
London dispersion forces, under the category of van der Waal forces: These are the weakest of the intermolecular forces and exist between all types of molecules, whether ionic or covalent—polar or nonpolar. The more electrons a molecule has, the stronger the London dispersion forces are.
Which molecule has the highest Polarizability?
Large molecules with many electrons are most polarizable. The higher the polarizability of a molecule, the stronger its intermolecular forces.
What determines the strength of London dispersion forces?
Larger and heavier atoms and molecules exhibit stronger dispersion forces than smaller and lighter ones. In a larger atom or molecule, the valence electrons are, on average, farther from the nuclei than in a smaller atom or molecule. They are less tightly held and can more easily form temporary dipoles.
Photo in the article by “Wikipedia” https://en.wikipedia.org/wiki/William_P._Bidelman