What are the intermolecular forces of CHF3, OF2, HF, and CF4?

The relative magnitude of the inter molecular forces are: ##CF_4 < OF_2 < CHF_3 < HF.##

All molecules will have London dispersion forces which get stronger as the molecule gets heavier (more electrons causes a shift in electron cloud distribution resulting in a temporary dipole).

##CHF_3## is a polar molecule. So it will have dipole - dipole interaction along with the weaker dispersion forces.

##OF_2## is a polar molecule with a bent shape just like ##H_2O##. There are two pairs of bonded electrons and two pairs of unbonded lone pair electrons. These lone pairs repel the bonded electrons resulting in a bent shape with an angle less than ## 105^0##. The dominant inter molecular forces would be dipole-dipole.

HF is a polar molecule. Hence the primary inter molecular forces would be dipole - dipole and hydrogen bond which is a special type of dipole - dipole interaction between the hydrogen atom and electronegative F atom.

##CF_4## has a tetrahedral structure. It is non-polar molecule. The dominant inter molecular force would be London dispersion force.