AP Chemistry
1.8 Valence Electrons and Ionic Compounds
1.7 Periodic Trends
1.5 Atomic Structure and Electron Configuration
A student investigates the thermal properties of refractory ceramic materials and records the data in the table below.
Both \(\text{MgO}\) and \(\text{NaF}\) crystallize in the same cubic lattice geometry, and each ion in both compounds is isoelectronic with neon (\(10\) electrons). Which of the following statements best accounts for the significantly higher melting point of \(\text{MgO}\) compared to \(\text{NaF}\)?
| Compound | Cation | Anion | Interionic distance (\(\text{pm}\)) | Melting point (\(^\circ\text{C}\)) |
|---|---|---|---|---|
| \(\text{MgO}\) | \(\text{Mg}^{2+}\) | \(\text{O}^{2-}\) | \(212\) | \(2852\) |
| \(\text{NaF}\) | \(\text{Na}^+\) | \(\text{F}^-\) | \(231\) | \(993\) |
Both \(\text{MgO}\) and \(\text{NaF}\) crystallize in the same cubic lattice geometry, and each ion in both compounds is isoelectronic with neon (\(10\) electrons). Which of the following statements best accounts for the significantly higher melting point of \(\text{MgO}\) compared to \(\text{NaF}\)?
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