Lawrie Ryan and Roger Norris Solutions for Chapter: Lattice Energy, Exercise 10: Question

For the given pair of compounds, suggest which will have the most exothermic lattice energy?

$\mathrm{KCl}$ and $\mathrm{BaO}$ (ionic radii are similar)

For the given pair of compounds, suggest which will have the most exothermic lattice energy?

${\mathrm{MgI}}_2$ and ${\mathrm{SrI}}_2$

For the given pair of compounds, suggest which will have the most exothermic lattice energy?

$\mathrm{CaO}$ and $\mathrm{NaCl}$ (ionic radii are similar)

Place the following compounds in order of increasing exothermic lattice energy. Explain your answer.

$\mathrm{LiF}, \mathrm{MgO}, \mathrm{RbCl}$

The electrostatic force between two charged particles is proportional to $\frac{{\mathrm{Q}}_1\times {\mathrm{Q}}_2}{{\mathrm{r}}^2}$ where ${\mathrm{Q}}_1$ and ${\mathrm{Q}}_2$ are the charges on the particles and $\mathrm{r}$ is the distance between the centres of the particles. Use this relationship to explain why a magnesium oxide has a greater lattice energy than lithium fluoride.

The electrostatic force between two charged particles is proportional to $\frac{{\mathrm{Q}}_1\times {\mathrm{Q}}_2}{{\mathrm{r}}^2}$ where ${\mathrm{Q}}_1$ and ${\mathrm{Q}}_2$ are the charges on the particles and $\mathrm{r}$ is the distance between the centres of the particles. Use this relationship to explain why a lithium fluoride has a greater lattice energy than potassium bromide.

Which one of these equations for the calculation of the lattice energy of sodium oxide, ${\mathrm{Na}}_2\mathrm{O}$ is correct?