Defining Lattice Energy

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

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

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

$\mathrm{CaO}$ and $\mathrm{NaCl}$ (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?

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

For the pair $\mathrm{KCl}$ and $\mathrm{SrS}$, state with reasons, which one you would expect to have the higher lattice energy.

For the pair $\mathrm{NaCl}$ and $\mathrm{KBr}$, state with reasons, which one you would expect to have the higher lattice energy.

State the name of the enthalpy change represented by the equation: ${\mathrm{Cd}}^{2+}\left(\mathrm{g}\right)+2{\mathrm{Cl}}^{-}\left(\mathrm{g}\right)\stackrel{ }{\to }{\mathrm{CdCl}}_2\left(\mathrm{s}\right)$

The lattice energy of magnesium bromide, ${\mathrm{MgBr}}_2$ can be calculated using the enthalpy changes shown in the table.

State the meaning of the term lattice energy.

Calculate the lattice energy for sodium chloride, given that:

$∆{{\mathrm{H}}_{\mathrm{f}}}^{\circ }\left[\mathrm{NaCl}\right]=-411 \mathrm{kJ} {\mathrm{mol}}^{-1}$

$∆{{\mathrm{H}}_{\mathrm{at}}}^{\circ }\left[\mathrm{Na}\right]=+107 \mathrm{kJ} {\mathrm{mol}}^{-1}$

$∆{{\mathrm{H}}_{\mathrm{at}}}^{\circ }\left[\mathrm{Cl}\right]=+122 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{IE}}_1\left[\mathrm{Na}\right]=+496 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{EA}}_1\left[\mathrm{Cl}\right]=-348 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Explain why the lattice energy of sodium chloride has a value that is lower than the lattice energy of lithium chloride.

Define the term enthalpy change of atomisation.

Define the term first ionisation energy.

Define the terms crystal lattice, bond energy, enthalpy change, activation energy, standard conditions, standard enthalpy change of formation.

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.

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.

Write an equation describing the lattice energy of sodium sulfide.

Write an equation describing the lattice energy of potassium bromide.

Write equation describing the lattic energy of magnesium oxide.

Give value for the standard conditions of temperature and pressure.