Final answer:
The substance with the highest boiling point among CH₄, KCl, CS₂, and HF is HF (D) due to its ability to form strong hydrogen bonds, which are stronger than the other intermolecular forces present in the listed compounds option d is correct.
Step-by-step explanation:
option d is correct. To determine which substance has the highest boiling point among CH₄, KCl, CS₂, and HF, we must consider the types of intermolecular forces present in each compound. Methane (CH₄) is a nonpolar molecule with weak London dispersion forces. Potassium chloride (KCl) is an ionic compound with strong ionic bonds. Carbon disulfide (CS₂) is a nonpolar molecule with moderately strong London dispersion forces. Hydrogen fluoride (HF), on the other hand, has the ability to form hydrogen bonds, which are exceptionally strong intermolecular forces.
Since hydrogen bonding is significantly stronger than dispersion forces or even most ionic interactions in the liquid state, HF will have the highest boiling point. The boiling points of substances generally increase with the strength of intermolecular forces. Therefore, the correct answer is D. HF.
The substance with the highest boiling point among CH₄, KCl, CS₂, and HF is D. HF (Hydrogen Fluoride).
Boiling point is determined by the strength of intermolecular forces. Hydrogen bonding is the strongest intermolecular force, and HF is capable of forming hydrogen bonding within its compounds. This results in a higher boiling point for HF compared to the other substances.