the electron cloud of hf is smaller than that of f₂, however, hf has a much higher boiling point than f₂…

the electron cloud of hf is smaller than that of f₂, however, hf has a much higher boiling point than f₂ has. which of the following explains how the dispersion - force model of intermolecular attraction does not account for the unusually high boiling point of hf?\na f₂ is soluble in water, whereas hf is insoluble in water.\nb the f₂ molecule has a greater mass than the hf molecule has.\nc liquid f₂ has weak dispersion force attractions between its molecules, whereas liquid hf has strong ionic interactions between h⁺ and f⁻ ions.\nd liquid f₂ has weak dispersion force attractions between its molecules, whereas liquid hf has both weak dispersion force attractions and hydrogen bonding interactions between its molecules.

the electron cloud of hf is smaller than that of f₂, however, hf has a much higher boiling point than f₂ has. which of the following explains how the dispersion - force model of intermolecular attraction does not account for the unusually high boiling point of hf?\na f₂ is soluble in water, whereas hf is insoluble in water.\nb the f₂ molecule has a greater mass than the hf molecule has.\nc liquid f₂ has weak dispersion force attractions between its molecules, whereas liquid hf has strong ionic interactions between h⁺ and f⁻ ions.\nd liquid f₂ has weak dispersion force attractions between its molecules, whereas liquid hf has both weak dispersion force attractions and hydrogen bonding interactions between its molecules.

Answer

Brief Explanations:

  • Option A: Solubility in water is not related to boiling point differences.
  • Option B: (F_2) has a smaller mass than (HF) (molar mass of (F_2 = 38\space g/mol), molar mass of (HF=20\space g/mol)), so this is incorrect.
  • Option C: (HF) is a covalent compound, not ionic. There are no (H^+) and (F^-) ions in liquid (HF) in the sense of ionic interactions.
  • Option D: (F_2) has only weak dispersion (London) forces. (HF) has both weak dispersion forces (due to its electrons) and strong hydrogen - bonding (because of the (H - F) bond where (F) is highly electronegative). Hydrogen bonding is a much stronger intermolecular force than dispersion forces. A substance with stronger intermolecular forces (like (HF) with hydrogen bonding) will have a higher boiling point as more energy is required to break these intermolecular attractions.

Answer:

D. Liquid (F_2) has weak dispersion force attractions between its molecules, whereas liquid (HF) has both weak dispersion force attractions and hydrogen bonding interactions between its molecules.