London dispersion forces (forces between the particles) are present in:

Explanation

The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction. London Dispersion Forces occurs when there is a momentary region of electron density in an atom or molecule. This momentary region is negative, giving the atom or molecule polarity. As an atom or molecule gets larger, they get more electrons, so the probability of there being a region of electron density increases. Gases have electrons, so they have London Dispersion Forces. However, their LDFs tend to be weaker as gaseous atoms and molecules tend to be smaller than liquid and solid atoms and molecules. The halogens provide an example for this concept. Fluorine and chlorine molecules exist as gases at room temperature, but iodine and bromine molecules exist as a liquid and solid respectively because they are larger molecules.