Final answer:
Chloromethane and carbon monoxide interact through dipole-dipole interactions due to their polar natures, as well as through London dispersion forces.
Step-by-step explanation:
The intermolecular forces acting between a chloromethane (CH₃Cl) molecule and a carbon monoxide (CO) molecule include dipole-dipole interactions. Chloromethane is a polar molecule due to having a net dipole, as its bond moments, primarily from the more polar C-Cl bond, point toward the Cl end of the molecule. Carbon monoxide is also a polar molecule due to its triple bond with a lone pair of electrons creating a dipole. The electrostatic attraction between the partially positive end of one molecule and the partially negative end of another leads to dipole-dipole interactions. Additionally, London dispersion forces, which are weaker and arise due to temporary fluctuations in electron density that induce a temporary dipole in neighboring molecules, may also be present.