Three gaseous substances—carbon dioxide (CO₂), sulfur dioxide (SO₂), and carbonyl sulfide (OCS)—each have comparable molar masses (between 44 and 64 g·mol⁻¹). Assume the gases are at the same temperature.
Answer the following about the forces that operate between molecules of each substance.
(a) Rank CO₂, SO₂, and OCS from weakest to strongest net intermolecular attractions in the liquid phase. Clearly indicate any ties if you believe two substances experience comparable attractions.
(b) For each adjacent pair in your ranking, justify the ordering by explicitly identifying the dominant types of intermolecular forces present and explaining how molecular geometry, polarity, and/or polarizability determine the relative strength of those forces.
(c) Predict which of the three substances would have the highest critical temperature and provide a brief explanation that connects critical temperature to the intermolecular attractions you discussed in part (b).