---
title: "The diagrams below represent equal volumes of pure water in the solid state (\\(\\text{H}_2\\text{O}(s)\\)) and in the liquid state (\\(\\text{H}_2\\text{O}(l)\\)) at \\(0^\\circ\\text{C}\\) and \\(1\\text{ atm}\\).  Which of the following best explains why liquid water has a higher density than ice at \\(0^\\circ\\text{C}\\)?"
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url: "https://nerd-notes.com/ubq/119662/"
date_modified: "2026-08-21T08:11:58+00:00"
---

# The diagrams below represent equal volumes of pure water in the solid state (\(\text{H}_2\text{O}(s)\)) and in the liquid state (\(\text{H}_2\text{O}(l)\)) at \(0^\circ\text{C}\) and \(1\text{ atm}\).

Which of the following best explains why liquid water has a higher density than ice at \(0^\circ\text{C}\)?

The diagrams below represent equal volumes of pure water in the solid state (\(\text{H}_2\text{O}(s)\)) and in the liquid state (\(\text{H}_2\text{O}(l)\)) at \(0^\circ\text{C}\) and \(1\text{ atm}\).

Which of the following best explains why liquid water has a higher density than ice at \(0^\circ\text{C}\)?

![A grayscale diagram showing two identical square boxes labeled Box 1 (\(\text{H}_2\text{O}(s)\)) on the left and Box 2 (\(\text{H}_2\text{O}(l)\)) on the right. A legend at the top maps: a large gray circle represents an oxygen atom, and two small white circles bonded to each large gray circle represent hydrogen atoms in a bent \(\text{H}_2\text{O}\) molecule; dashed lines represent hydrogen bonds. Box 1 contains exactly 6 \(\text{H}_2\text{O}\) molecules arranged in a ring forming an open hexagonal pattern with dashed lines connecting neighboring oxygen and hydrogen atoms, leaving an open space in the center. Box 2 contains exactly 8 \(\text{H}_2\text{O}\) molecules in a disordered, closely packed arrangement throughout the box with various dashed lines between adjacent molecules. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787299918-kwgWLW.jpg)

- **A.** The covalent \(\text{O}-\text{H}\) bonds within individual water molecules lengthen upon freezing, increasing the volume of each molecule in the solid state.
- **B.** The rigid, open hydrogen-bonding network in ice creates open space between molecules, whereas in liquid water molecules pack closer together.
- **C.** The molecules in the liquid state have significantly stronger London dispersion forces than in the solid state, pulling the molecules into a smaller total volume.
- **D.** The molecules in liquid water partially dissociate into \(\text{H}^+\text{(aq)}\) and \(\text{OH}^-\text{(aq)}\) ions, which occupy significantly less volume than intact \(\text{H}_2\text{O}\) molecules.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119662/*