what type of intermolecular bonding would be expected between molecules of carbon monoxide and why?
so when you look up the electronegativity values, the lower value is the positive end and the higher value is the negative end?
Carbon monoxide is a dipole with the carbon end being positive and the oxygen end being negative (You can tell which end is which by looking up the electronegativity values for C and O). Therefore, one would expect these dipoles to attract one another. We call that dipole-dipole bonding although these are not as strong as regular chemical bonds.
right. That is how you determine the polarity of a molecule (and whether a molecule is polar or not). Polar covalent bonds fit into the same discussion.
To determine the type of intermolecular bonding between molecules of carbon monoxide (CO), we need to consider the molecular properties and the forces that hold molecules together.
Carbon monoxide consists of a carbon atom bonded to an oxygen atom. Carbon and oxygen both strongly electronegative atoms, meaning they have a high affinity for electrons. In the CO molecule, the oxygen atom has a partial negative charge (δ-) while the carbon atom has a partial positive charge (δ+).
Based on these properties, we can infer the type of intermolecular bonding to be expected between CO molecules. The predominant intermolecular force between CO molecules is dipole-dipole interactions. Dipole-dipole interactions occur between polar molecules that have a positive and a negative end due to differences in electronegativity.
In the case of CO, the oxygen atom with a partial negative charge attracts the neighboring carbon atom with a partial positive charge, resulting in dipole-dipole interactions. These forces help hold the CO molecules together in a liquid or solid state.
It is worth noting that while dipole-dipole interactions are the primary intermolecular force in CO, weak London dispersion forces (also known as van der Waals forces) may exist as well. London dispersion forces can occur between any two molecules due to temporary fluctuations in electron distribution, even if they are nonpolar. However, in CO, the strong dipole-dipole interactions are the dominant intermolecular force.