The first thing that you need to do first is to figure out what type of compound you are looking at. You should realize that CH2F2 is known to be a polar molecule. The type of force that you can expect to have is dipole interaction. Aside from this type of interaction, you can expect that there are also going to be other forces that are available. If you would check something that is related to this molecule, which is CF4, you will realize that the structure is tetrahedral. This means that the force that will be the strongest for this one will be the London Dispersion Force. The attractive forces of CH2F2 will be stronger as compared to the CF4.
The correct answers to this question are London forces and dipole-dipole forces. London forces may also be known as LDF or London dispersion forces. The name of the forces comes after Fritz London, who was a physicist. London forces are forces that act between molecules and atoms. LDF's are apart of the van der Waals forces. Dipole-dipole forces are forces that are attractive. They are a positive end of a polar molecule and a negative end of a polar molecule. The strengths of dipole-dipole forces are anywhere from 5 kJ to 20 kJ per mole. These forces are weaker than ionic bonds.
There are two intermolecular forces that are available right now. These two are the following: Dipole-Dipole Forces and London Forces. The London Forces, also are known as the London Dispersion Force, is known to be a type of force that you can get between the various atoms and molecules that are available.
Dipole forces, on the other hand, is a type of force that is considered to be strong. This is between one end of the polar molecule and the negative end of another polar molecule. The forces are usually strong and are usually stronger as compared to the London Forces. It is ideal to know the various forces that are available just to be sure.