---
title: "The normal boiling point of  \\(\\text{HF}\\) is \\(293 \\text{ K}\\), whereas the normal boiling point of \\(\\text{HCl}\\) is \\(188 \\text{ K}\\). Which of the following best explains why \\(\\text{HF}\\) has a significantly higher boiling point than \\(\\text{HCl}\\)?"
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url: "https://nerd-notes.com/ubq/119274/"
date_modified: "2026-08-19T12:39:36+00:00"
---

# The normal boiling point of 
\(\text{HF}\) is \(293 \text{ K}\), whereas the normal boiling point of \(\text{HCl}\) is \(188 \text{ K}\). Which of the following best explains why \(\text{HF}\) has a significantly higher boiling point than \(\text{HCl}\)?

The normal boiling point of 
\(\text{HF}\) is \(293 \text{ K}\), whereas the normal boiling point of \(\text{HCl}\) is \(188 \text{ K}\). Which of the following best explains why \(\text{HF}\) has a significantly higher boiling point than \(\text{HCl}\)?

- **A.** \(\text{HF}\) has a higher boiling point because \(\text{HF}\) molecules form intermolecular hydrogen bonds, which are stronger than the dipole-dipole forces between \(\text{HCl}\) molecules.
- **B.** \(\text{HF}\) has a higher boiling point because the covalent \(\text{H-F}\) bond is stronger than the covalent \(\text{H-Cl}\) bond, requiring more energy to break during boiling.
- **C.** \(\text{HCl}\) has a higher boiling point because \(\text{HCl}\) has a larger electron cloud, resulting in greater polarizability and stronger London dispersion forces than in \(\text{HF}\).
- **D.** \(\text{HF}\) has a higher boiling point because \(\text{HCl}\) molecules form hydrogen bonds that are weaker due to the lower electronegativity of chlorine.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119274/*