---
title: "A student compares the properties of two crystalline ionic solids, \\(\\text{MgO}\\) and \\(\\text{NaCl}\\). Which of the following statements correctly identifies the compound with the higher melting point and provides the correct Coulombic justification?"
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url: "https://nerd-notes.com/ubq/119302/"
date_modified: "2026-08-19T12:39:43+00:00"
---

# A student compares the properties of two crystalline ionic solids, \(\text{MgO}\) and \(\text{NaCl}\). Which of the following statements correctly identifies the compound with the higher melting point and provides the correct Coulombic justification?

A student compares the properties of two crystalline ionic solids, \(\text{MgO}\) and \(\text{NaCl}\). Which of the following statements correctly identifies the compound with the higher melting point and provides the correct Coulombic justification?

- **A.** \(\text{NaCl}\) has a higher melting point than \(\text{MgO}\) because \(\text{Cl}^-\) is larger than \(\text{O}^{2-}\), creating stronger ion-ion attractive forces.
- **B.** \(\text{MgO}\) has a higher melting point than \(\text{NaCl}\) because \(\text{MgO}\) has a greater molar mass, resulting in stronger London dispersion forces.
- **C.** \(\text{MgO}\) has a higher melting point than \(\text{NaCl}\) because the magnitude of the charges on \(\text{Mg}^{2+}\) and \(\text{O}^{2-}\) is greater than on \(\text{Na}^+\) and \(\text{Cl}^-\), producing stronger Coulombic attractions.
- **D.** \(\text{NaCl}\) has a higher melting point than \(\text{MgO}\) because single charges permit closer packing in the crystal lattice, leading to greater interionic attraction.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119302/*