Answer:
CH₃F and CF₄ share two types of intermolecular forces: London dispersion forces and dipole-dipole forces
London dispersion forces are present in all molecules and arise from the temporary fluctuation of electron density in the molecule. These forces increase with the size of the molecule and the number of electrons it contains. In CH₃F and CF₄, both molecules have London dispersion forces because of the presence of electrons that can create temporary dipoles
Dipole-dipole forces arise due to the permanent dipoles present in polar molecules. In CH₃F and CF₄, CH₃F is polar due to the difference in electronegativity between the carbon and fluorine atoms, while CF₄ is nonpolar due to the symmetry of the molecule. Therefore, CH₃F exhibits dipole-dipole forces, while CF₄ does not.
