Question

What intermolecular forces are present in $ C{H_3}F $ ?

Answer 1

Hint: In order to this question, to know the types of intermolecular forces that are present in $ C{H_3}F $ , we should go through the structure of $ C{H_3}F $ and check whether which type of forces properties are present with their bonds.

Complete step by step answer:
Dipole-Dipole and London (Dispersion) Forces are present in $ C{H_3}F $ .
If we look at the molecule, there are no metal atoms to form ionic bonds. Furthermore, the molecule lacks hydrogen atoms bonded to nitrogen, oxygen, or fluorine; ruling out hydrogen bonding. Finally, there is a dipole formed by the difference in electronegativity between the carbon and fluorine atoms. This means the fluoromethane molecule will have a strong dipole-dipole force. As all molecules have the London (dispersion) force as caused by the electrons and positive nuclei, it too is present.
 Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole forces have strengths that range from 5 kJ to 20 kJ per mole. They are much weaker than ionic or covalent bonds and have a significant effect only when the molecules involved are close together (touching or almost touching).
Dispersion forces are the weakest intermolecular attractive forces. The presence of scattering powers represents the way that low-sub-atomic weight, non-polar substances, like hydrogen $ {H_2} $ , Neon $ (Ne) $ , and methane $ \left( {C{H_4}} \right) $ can be liquified. To imagine the cause of scattering drives, it is important to think regarding the momentary dispersion of electron thickness as opposed to average appropriation.

Note:
Dispersion forces are usually dominant over the three van der Waals forces (orientation, induction, dispersion) between atoms and molecules, with the exception of molecules that are small and highly polar, such as water.