1.1. This question focuses on the enthalpy of hydration of fluoride compounds.

i) Define the term enthalpy of hydration in relation to a fluoride ion.

ii) State whether the hydration of a fluoride ion is an exothermic or endothermic process. Explain your answer.

1.2. The enthalpy of hydration of the fluoride and chloride ions are -524 kJ mol^-1 and -364 kJ mol^-1. Explain why the value for the enthalpy of hydration for the fluoride ion is more negative than that for the chloride ion. You must refer to the attractive forces involved in your answer.

1.3. Use the enthalpy values below to suggest why there is a difference between the hydration values of calcium ions and sodium ions.

1.4. The table below gives data for the ionic compound calcium bromide, CaBr₂. 

i) Define the term enthalpy of lattice formation.

ii) Using the data from the table below, calculate the enthalpy of hydration of Ca²⁺.