Predict which substance in each of the following pairs would have the greater intermolecular forces. a. \(\mathrm{CO}_{2}\) or OCS b. \(\mathrm{SeO}_{2}\) or \(\mathrm{SO}_{2}\) c. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) or \(\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) d. \(\mathrm{CH}_{3} \mathrm{CH}_{3}\) or \(\mathrm{H}_{2} \mathrm{CO}\) e. \(\mathrm{CH}_{3} \mathrm{OH}\) or \(\mathrm{H}_{2} \mathrm{CO}\)

In each pair of molecules, identify which type of intermolecular force(s) is present (London dispersion forces, dipole-dipole forces, or hydrogen bonding). a. CO₂: London dispersion forces, dipole-dipole forces OCS: London dispersion forces, dipole-dipole forces b. SeO₂: London dispersion forces, dipole-dipole forces SO₂: London dispersion forces, dipole-dipole forces c. CH₃CH₂CH₂NH₂: London dispersion forces, dipole-dipole forces, hydrogen bonding H₂NCH₂CH₂NH₂: London dispersion forces, dipole-dipole forces, hydrogen bonding d. CH₃CH₃: London dispersion forces H₂CO: London dispersion forces, dipole-dipole forces e. CH₃OH: London dispersion forces, dipole-dipole forces, hydrogen bonding H₂CO: London dispersion forces, dipole-dipole forces

For each pair of molecules, compare the strength of their intermolecular forces, keeping in mind that London dispersion forces are the weakest, followed by dipole-dipole forces, and hydrogen bonding being the strongest. a. CO₂ and OCS both have London dispersion forces and dipole-dipole forces; however, OCS has a larger molar mass, contributing to stronger London dispersion forces, so OCS has the greater intermolecular forces. b. Both SeO₂ and SO₂ have London dispersion forces and dipole-dipole forces. However, SeO₂ has a larger molar mass, leading to stronger London dispersion forces, so SeO₂ has the greater intermolecular forces. c. Both CH₃CH₂CH₂NH₂ and H₂NCH₂CH₂NH₂ have London dispersion forces, dipole-dipole forces, and hydrogen bonding. However, CH₃CH₂CH₂NH₂ has a larger molar mass, which contributes to stronger London dispersion forces, so CH₃CH₂CH₂NH₂ has greater intermolecular forces. d. CH₃CH₃ has only London dispersion forces, while H₂CO has both London dispersion forces and dipole-dipole forces. Therefore, H₂CO has greater intermolecular forces. e. CH₃OH has London dispersion forces, dipole-dipole forces, and hydrogen bonding, while H₂CO has only London dispersion forces and dipole-dipole forces. The presence of hydrogen bonding in CH₃OH leads to stronger intermolecular forces, so CH₃OH has greater intermolecular forces.