True. The bigger or smaller the molecule the stronger the London dispersion force will most likely be.
The strength of London dispersion forces (also known as van der Waals forces or induced dipole-induced dipole forces) is influenced by the size of the molecules involved.
Larger molecules generally have more electrons, leading to greater polarization and stronger London dispersion forces. Smaller molecules, with fewer electrons, tend to exhibit weaker London dispersion forces.
This is because larger electron clouds are more easily distorted, creating temporary dipoles and inducing a polarization effect that results in attractive forces between molecules.