In CH2F2, also known as difluoromethane, the intermolecular forces present include dipole-dipole interactions and London dispersion forces.
Firstly, CH2F2 is a polar molecule due to the significant difference in electronegativity between carbon and fluorine atoms. This polarity leads to dipole-dipole interactions, where the positive end of one molecule attracts the negative end of another. The strong electronegativity of fluorine creates a partial negative charge around the fluorine atoms, while the carbon and hydrogen atoms create a partial positive charge, resulting in these attractive forces.
In addition to dipole-dipole interactions, London dispersion forces also play a role in CH2F2. These are weaker forces that arise from the temporary fluctuations in electron density within molecules. Despite being a nonpolar force, it is always present in all molecules, contributing to the overall intermolecular attractions.
In summary, CH2F2 experiences dipole-dipole interactions due to its polarity, as well as London dispersion forces due to the presence of electrons in all molecules.