Question

which member of each of the following pairs of substances would you expect to have a higher boiling point based on the intermolecular forces they exhibit?
part 1 of 2
select the single best answer.

part 2 of 2
select the single best answer.

Explanation:

• For \(N_2\) and \(I_2\):
• Both \(N_2\) and \(I_2\) are non - polar molecules. The intermolecular force acting between them is London dispersion force.
• The strength of London dispersion force is proportional to the molar mass of the molecule.
• The molar mass of \(N_2(M = 28\space g/mol)\) and \(I_2(M= 253.8\space g/mol)\). Since \(I_2\) has a higher molar mass, it has stronger London dispersion forces.
• For \(SO_2\) and \(CO_2\):
• \(CO_2\) is a non - polar molecule (\(O = C=O\), linear geometry, dipole moments cancel out). The intermolecular force acting between \(CO_2\) molecules is London dispersion force.
• \(SO_2\) is a polar molecule (\(O - S - O\), bent geometry, dipole moment does not cancel out). The intermolecular forces acting between \(SO_2\) molecules are London dispersion forces and dipole - dipole forces.
• Dipole - dipole forces are stronger than London dispersion forces (for molecules of comparable molar mass. The molar mass of \(SO_2(M = 64\space g/mol)\) and \(CO_2(M = 44\space g/mol)\)).

Answer:

• Part 1 of 2: \(I_2\)
• Part 2 of 2: \(SO_2\)