---
title: "A student compares the lattice energies of three crystalline ionic solids: \\(\\text{NaCl}\\), \\(\\text{CaO}\\), and \\(\\text{MgO}\\). Based on Coulomb’s law and periodic trends in ionic radii, which of the following correctly ranks the compounds in order of decreasing lattice energy (from greatest to least)?"
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url: "https://nerd-notes.com/ubq/119604/"
date_modified: "2026-08-21T08:11:44+00:00"
---

# A student compares the lattice energies of three crystalline ionic solids: \(\text{NaCl}\), \(\text{CaO}\), and \(\text{MgO}\). Based on Coulomb’s law and periodic trends in ionic radii, which of the following correctly ranks the compounds in order of decreasing lattice energy (from greatest to least)?

A student compares the lattice energies of three crystalline ionic solids: \(\text{NaCl}\), \(\text{CaO}\), and \(\text{MgO}\). Based on Coulomb's law and periodic trends in ionic radii, which of the following correctly ranks the compounds in order of decreasing lattice energy (from greatest to least)?

- **A.** \(\text{MgO} > \text{CaO} > \text{NaCl}\)
- **B.** \(\text{MgO} > \text{NaCl} > \text{CaO}\)
- **C.** \(\text{CaO} > \text{MgO} > \text{NaCl}\)
- **D.** \(\text{NaCl} > \text{CaO} > \text{MgO}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119604/*