---
title: "A student compares the normal boiling points of two structural isomers with the molecular formula \\(\\text{C}_2\\text{H}_6\\text{O}\\): ethanol (\\(\\text{CH}_3\\text{CH}_2\\text{OH}\\), boiling point \\(78^\\circ\\text{C}\\)) and dimethyl ether (\\(\\text{CH}_3\\text{OCH}_3\\), boiling point \\(-24^\\circ\\text{C}\\)). Which of the following best identifies the isomer with the stronger intermolecular forces and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/119158/"
date_modified: "2026-08-19T12:32:24+00:00"
---

# A student compares the normal boiling points of two structural isomers with the molecular formula \(\text{C}_2\text{H}_6\text{O}\): ethanol (\(\text{CH}_3\text{CH}_2\text{OH}\), boiling point \(78^\circ\text{C}\)) and dimethyl ether (\(\text{CH}_3\text{OCH}_3\), boiling point \(-24^\circ\text{C}\)). Which of the following best identifies the isomer with the stronger intermolecular forces and provides the correct justification?

A student compares the normal boiling points of two structural isomers with the molecular formula \(\text{C}_2\text{H}_6\text{O}\): ethanol (\(\text{CH}_3\text{CH}_2\text{OH}\), boiling point \(78^\circ\text{C}\)) and dimethyl ether (\(\text{CH}_3\text{OCH}_3\), boiling point \(-24^\circ\text{C}\)). Which of the following best identifies the isomer with the stronger intermolecular forces and provides the correct justification?

- **A.** Dimethyl ether has stronger intermolecular forces because its oxygen atom forms a more symmetric dipole moment that enhances London dispersion forces.
- **B.** Ethanol has stronger intermolecular forces because its molecules form hydrogen bonds with one another, whereas dimethyl ether molecules interact primarily through weaker dipole-dipole forces and London dispersion forces.
- **C.** Ethanol has stronger intermolecular forces because the \(\text{O-H}\) covalent bond in ethanol is stronger and requires more thermal energy to break than the \(\text{C-O}\) covalent bonds in dimethyl ether.
- **D.** Ethanol has stronger intermolecular forces because ethanol has a larger molar mass and more total electrons than dimethyl ether, resulting in a more polarizable electron cloud.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119158/*