Final answer:
CHF3 exhibits dipole-dipole interactions due to its polar bonds, which is the strongest intermolecular force present in this molecule as hydrogen bonding is not applicable.
Step-by-step explanation:
The strongest type of intermolecular force present in CHF3 is the dipole-dipole interaction. While all molecules exhibit London dispersion forces due to momentary fluctuations in electron distribution, molecules like CHF3 with polar bonds have permanent dipole moments due to the differing electronegativities of the atoms involved. Given that CHF3 consists of a central carbon atom bonded to one hydrogen and three fluorine atoms, the high electronegativity of fluorine relative to both carbon and hydrogen leads to a significant polarity in the molecule, making dipole-dipole interactions more significant than dispersion forces in this case. While fluorine is highly electronegative and does participate in hydrogen bonding with hydrogen when it is on another molecule, in CHF3, the hydrogen is not bonded to nitrogen, oxygen, or fluorine, hence hydrogen bonding does not occur. Therefore, option B) Dipole-dipole interactions is the correct answer.