NaCl and KF have the same crystal structure. The only...

NaCl and KF have the same crystal structure. The only difference between the two is the distance that separates cations and anions. (a) The lattice energies of NaCl and KF are given in Table $8.1 .$ Based on the lattice energies, would you expect the Na $-$ Cl or the $\mathrm{K}-$ F distance to be longer? (b) Use the ionic radii given in Figure 7.8 to estimate the $\mathrm{Na}-\mathrm{Cl}$ and $\mathrm{K}-\mathrm{F}$ distances.

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Key Concepts

Lattice Energy

Lattice energy is the energy released when gaseous ions combine to form a solid ionic lattice. It depends on both the magnitude of the ionic charges and the distance separating the ions, as described by Coulomb’s law. A higher lattice energy typically reflects stronger attractions and shorter interionic distances of ions in the lattice.

Crystal Structure

The crystal structure is the three?dimensional arrangement of ions in an ionic solid. It determines how the ions are spatially organized, which in turn affects various properties such as lattice energy and interionic distances. In comparing compounds, understanding that they share the same crystal structure allows for a direct comparison of distance effects from other factors.

Ionic Radii

Ionic radii are measures of the size of ions in a crystal lattice. They are used to estimate distances between ions by considering the sum of the radii of cation and anion. This estimation is important when comparing ionic bond lengths in different compounds that exhibit the same crystal structure.

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