---
title: "The table below provides the ionic radii for selected alkali metal cations and halide anions.  | Ion | Ionic radius (pm) | | :— | :— | | \\(\\text{Li}^+\\) | \\(76\\) | | \\(\\text{Na}^+\\) | \\(102\\) | | \\(\\text{F}^-\\) | \\(133\\) | | \\(\\text{Cl}^-\\) | \\(181\\) |  Based on Coulomb’s law and the data in the table, which of the following correctly ranks the four ionic compounds in order of decreasing magnitude of lattice energy, and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/121382/"
date_modified: "2026-08-23T05:02:00+00:00"
---

# The table below provides the ionic radii for selected alkali metal cations and halide anions.

| Ion | Ionic radius (pm) |
| :— | :— |
| \(\text{Li}^+\) | \(76\) |
| \(\text{Na}^+\) | \(102\) |
| \(\text{F}^-\) | \(133\) |
| \(\text{Cl}^-\) | \(181\) |

Based on Coulomb’s law and the data in the table, which of the following correctly ranks the four ionic compounds in order of decreasing magnitude of lattice energy, and provides the correct justification?

The table below provides the ionic radii for selected alkali metal cations and halide anions.

| Ion | Ionic radius (pm) |
| :--- | :--- |
| \(\text{Li}^+\) | \(76\) |
| \(\text{Na}^+\) | \(102\) |
| \(\text{F}^-\) | \(133\) |
| \(\text{Cl}^-\) | \(181\) |

Based on Coulomb's law and the data in the table, which of the following correctly ranks the four ionic compounds in order of decreasing magnitude of lattice energy, and provides the correct justification?

- **A.** \(\text{LiF} > \text{LiCl} > \text{NaF} > \text{NaCl}\), because the smaller \(\text{Li}^+\) cation creates a higher charge density than \(\text{Na}^+\), ensuring all lithium salts have larger lattice energies than sodium salts.
- **B.** \(\text{LiF} > \text{NaF} > \text{LiCl} > \text{NaCl}\), because the magnitude of lattice energy is inversely proportional to the internuclear distance (\(r_+ + r_-\)), which increases in the order \(\text{LiF} < \text{NaF} < \text{LiCl} < \text{NaCl}\).
- **C.** \(\text{NaCl} > \text{LiCl} > \text{NaF} > \text{LiF}\), because \(\text{NaCl}\) possesses the greatest total number of electrons, resulting in the highest polarizability and strongest attractions in the crystal lattice.
- **D.** \(\text{NaCl} > \text{LiCl} > \text{NaF} > \text{LiF}\), because larger internuclear separations allow for greater polarization of the electron clouds, which increases the electrostatic potential energy.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121382/*