Final answer:
Phosphorus trifluoride (PF3) exhibits dipole-dipole attractions because it is a polar molecule and dispersion forces, which all molecules have. It does not exhibit hydrogen bonding or ionic bonding.
Step-by-step explanation:
The student has asked to identify the intermolecular forces present in phosphorus trifluoride (PF3). There are different kinds of intermolecular forces that can occur between molecules in a condensed phase, namely dispersion forces, dipole-dipole attractions, and hydrogen bonding. Since PF3 is a polar molecule without hydrogen atoms bonded to highly electronegative atoms like F, O, or N, it cannot engage in hydrogen bonding. However, it will exhibit dipole-dipole attractions because of the dipole moment due to the difference in electronegativity between phosphorus and fluorine atoms. Additionally, all molecules exhibit dispersion forces due to the temporary fluctuations in electron distribution that create temporary dipoles. Ionic bonding is not applicable here as PF3 is a covalent compound. Therefore, the correct choices for the intermolecular forces present in PF3 are dispersion forces and dipole-dipole attractions.