Question

which intermolecular force is the most important in determining the difference in boiling points of the following molecules? co (28.0 g/mol) n₂ (28.0 g/mol) london dispersion dipole - dipole (not including hydrogen bonding) hydrogen bonding which substance has the stronger total intermolecular forces/the higher boiling point? 1. first, look to see if the substance can hydrogen bond. if so, it likely has the strongest intermolecular forces (e.g., hf > hcl). 2. if you are comparing two molecules of very different molar masses, london dispersion forces are more important (e.g., hbr > hcl). 3. if you are comparing two molecules of very similar molar mass, dipole - dipole forces are more important. the molecule with the greater dipole - dipole forces (the greatest electronegativity difference between the atoms within the molecule) will have the greatest boiling point.

Explanation:

• \(CO\) is a polar molecule (due to the difference in electronegativity between \(C\) and \(O\)), while \(N_2\) is a non - polar molecule.
• London dispersion forces are present in all molecules, but for molecules of similar molar mass (both \(CO\) and \(N_2\) have a molar mass of approximately \(28.0\space g/mol\)), dipole - dipole forces (since \(CO\) is polar) play a more significant role in determining the boiling point difference.
• Hydrogen bonding is not possible for either \(CO\) or \(N_2\) as neither has \(H\) bonded to \(N\), \(O\), or \(F\).

Answer:

Dipole - dipole (not including hydrogen bonding)