11. Bonding & Molecular Structure

The lattice energy for ionic crystals decreases as the charge of the ions _____ and the size of the ions _____.

Which of the following compounds would you expect to have the highest boiling point?

The solubilities of CaCrO₄ and PbCrO₄ in water at 25°C are approximately 0.111 g/L and 0.0905 g/L in H₂O respectively. Based on this information, which compound do you think has the smaller lattice energy?

Illustrated are four ions — A, B, X, and Y— showing their relative ionic radii. The ions shown in red carry positive charges: a 2+ charge for A and a 1+ charge for B. Ions shown in blue carry negative charges: a 1- charge for X and a 2- charge for Y. (b) Among the combinations in part (a), which leads to the ionic compound having the largest lattice energy?

A portion of a two-dimensional 'slab' of NaCl(s) is shown here (see Figure 8.2) in which the ions are numbered. (d) Consider ion 5. How many repulsive interactions are shown for it?

(c) Would you expect salts like NaCl, which have singly charged ions, to have larger or smaller lattice energies compared to salts like CaO which are composed of doubly-charged ions?

(b) Write the chemical equation that represents the process of lattice energy for the case of NaCl.