More enthalpy changes

1. More enthalpy changes L.O.: Define and apply the terms enthalpy of hydration and enthalpy of solution. Calculate enthalpies of solution for ionic compounds from lattice enthalpies and enthalpies of hydration. Compare lattice enthalpies from Born–Haber cycles with those from calculations based on a perfect ionic model.

2. ZnSe has an experimental lattice formation enthalpy of -3611 kJmol-1. The theoretical value is -3305 Kjmol-1 Why is the experimental value greater?

3. Enthalpy of hydration is the standard enthalpy of change when water molecules surround one mole of gaseous ions. Enthalpy of solution, is the standard enthalpy change when one mole of solute dissolves completely in sufficient solvent to form a solution in which the molecules or ions are far enough apart no to interact with each other.

5. The solubility of ionic compounds can be calculated using the lattice energy of the compound and the hydration energy of the ions according to the following Hess' Law cycle: ∆H(solution) = Σ(∆H(hydration)) - ∆H(lattice formation) Or ∆H(solution) = Σ(∆H(hydration))+ ∆H(lattice dissociation)

6. 5.1 Exercise 3

7. More enthalpy changes L.O.: Define and apply the terms enthalpy of hydration and enthalpy of solution. Calculate enthalpies of solution for ionic compounds from lattice enthalpies and enthalpies of hydration. Compare lattice enthalpies from Born–Haber cycles with those from calculations based on a perfect ionic model.