In carbon monoxide (CO), the predominant intermolecular force present is the dipole-dipole interaction. This is because CO is a polar molecule, with a significant difference in electronegativity between the carbon and oxygen atoms. Oxygen is more electronegative, causing the molecule to have a partial negative charge (δ-) on the oxygen side and a partial positive charge (δ+) on the carbon side.
Additionally, London dispersion forces, which are weak intermolecular forces due to temporary fluctuations in electron distribution, are also present in CO. However, these forces are generally weaker compared to the dipole-dipole interactions in this case. Therefore, while both types of forces exist, the dipole-dipole interactions play a more significant role in the behavior of CO at the molecular level.