Question

Is the London dispersion force greater between molecules of hydrogen sulfide (${H_2}S$) or molecules of water?

Answer 1

Hint: The intermolecular force of attraction describes the forces of attraction that hold molecules together. Intermolecular forces are stronger than intramolecular forces. These forces are responsible for any compound's liquids, solids, and solutions states. London dispersion, dipole-dipole, hydrogen bonding, and ion-ion force are some examples of intermolecular forces.

Complete answer:
The atomic or molecular weight of the substance determines the London dispersion forces. More electrons and stronger London forces are found in heavier atoms or molecules. This makes them more difficult to melt or boil.
The number of electrons that form temporary dipoles determines the strength of London dispersion forces. An atom of sulphur has more electrons than an atom of oxygen.
Therefore, the London dispersion force is greater between molecules of hydrogen sulfide (${H_2}S$) than molecules of water.
London dispersion forces exist between all types of molecules, whether ionic or covalent, polar or nonpolar, and are the weakest of the intermolecular interactions. The stronger the London dispersion forces are, the more electrons a molecule has.
Long-chain molecules have strong London dispersion forces because they can allow more displacement.

Note:
The order of strength of these intermolecular forces is given below.
London’s dispersion force $ < $ dipole-dipole $ < $ H-bonding $ < $ Ion-ion. Because of transient dipoles, London's dispersion forces are weaker than dipole-dipole forces.