---
title: "A student compares the physical properties of ethanol, \\(\\text{CH}_3\\text{CH}_2\\text{OH}\\), and dimethyl ether, \\(\\text{CH}_3\\text{OCH}_3\\), which are structural isomers with the same molar mass. Which of the following correctly identifies the substance with the higher boiling point and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/119183/"
date_modified: "2026-08-19T12:39:10+00:00"
---

# A student compares the physical properties of ethanol, \(\text{CH}_3\text{CH}_2\text{OH}\), and dimethyl ether, \(\text{CH}_3\text{OCH}_3\), which are structural isomers with the same molar mass. Which of the following correctly identifies the substance with the higher boiling point and provides the correct justification?

A student compares the physical properties of ethanol, \(\text{CH}_3\text{CH}_2\text{OH}\), and dimethyl ether, \(\text{CH}_3\text{OCH}_3\), which are structural isomers with the same molar mass. Which of the following correctly identifies the substance with the higher boiling point and provides the correct justification?

- **A.** Dimethyl ether has a higher boiling point because its symmetrical structure allows for stronger London dispersion forces than ethanol.
- **B.** Ethanol has a higher boiling point because the covalent bonds within the \(\text{CH}_3\text{CH}_2\text{OH}\) molecule are stronger than the covalent bonds within \(\text{CH}_3\text{OCH}_3\).
- **C.** Ethanol has a higher boiling point because ethanol molecules form intermolecular hydrogen bonds, which require more energy to overcome than the dipole-dipole interactions between dimethyl ether molecules.
- **D.** Dimethyl ether has a higher boiling point because the central oxygen atom creates a larger permanent dipole moment, resulting in stronger dipole-dipole forces than in ethanol.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119183/*