---
title: "A student investigates the physical properties of two structural isomers of \\(\\text{C}_5\\text{H}_{12}\\) and compiles the data shown in the table below.  | Compound | Condensed structural formula | Molar mass (\\(\\text{g/mol}\\)) | Normal boiling point (\\(^\\circ\\text{C}\\)) | |—|—|—|—| | Pentane | \\(\\text{CH}_3\\text{CH}_2\\text{CH}_2\\text{CH}_2\\text{CH}_3\\) | \\(72.15\\) | \\(36\\) | | 2,2-dimethylpropane | \\(\\text{C(CH}_3)_4\\) | \\(72.15\\) | \\(9.5\\) |  Which of the following statements best explains why pentane has a higher boiling point than 2,2-dimethylpropane?"
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url: "https://nerd-notes.com/ubq/121375/"
date_modified: "2026-08-23T05:01:57+00:00"
---

# A student investigates the physical properties of two structural isomers of \(\text{C}_5\text{H}_{12}\) and compiles the data shown in the table below.

| Compound | Condensed structural formula | Molar mass (\(\text{g/mol}\)) | Normal boiling point (\(^\circ\text{C}\)) |
|—|—|—|—|
| Pentane | \(\text{CH}_3\text{CH}_2\text{CH}_2\text{CH}_2\text{CH}_3\) | \(72.15\) | \(36\) |
| 2,2-dimethylpropane | \(\text{C(CH}_3)_4\) | \(72.15\) | \(9.5\) |

Which of the following statements best explains why pentane has a higher boiling point than 2,2-dimethylpropane?

A student investigates the physical properties of two structural isomers of \(\text{C}_5\text{H}_{12}\) and compiles the data shown in the table below.

| Compound | Condensed structural formula | Molar mass (\(\text{g/mol}\)) | Normal boiling point (\(^\circ\text{C}\)) |
|---|---|---|---|
| Pentane | \(\text{CH}_3\text{CH}_2\text{CH}_2\text{CH}_2\text{CH}_3\) | \(72.15\) | \(36\) |
| 2,2-dimethylpropane | \(\text{C(CH}_3)_4\) | \(72.15\) | \(9.5\) |

Which of the following statements best explains why pentane has a higher boiling point than 2,2-dimethylpropane?

- **A.** Pentane has a higher boiling point because breaking the covalent \(\text{C}-\text{C}\) bonds in its linear carbon backbone requires more energy than breaking bonds in branched 2,2-dimethylpropane.
- **B.** Pentane experiences stronger intermolecular attractions because its linear carbon chain gives it a permanent dipole moment, whereas symmetrical 2,2-dimethylpropane is nonpolar.
- **C.** Pentane experiences stronger London dispersion forces because its elongated, linear shape provides a greater surface area of contact between molecules than the compact, spherical shape of 2,2-dimethylpropane.
- **D.** Pentane experiences stronger London dispersion forces because it possesses a greater number of electrons and a larger molar mass than 2,2-dimethylpropane.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121375/*