Lattice Energy — MCQ Practice

Which of the following ionic compounds is expected to have the highest lattice energy?

Given the following thermochemical data for the formation of $MgCl_2(s)$: $\Delta H_{sub}(Mg) = +148\,\text{kJ/mol}$ $IE_1(Mg) = +738\,\text{kJ/mol}$ $IE_2(Mg) = +1451\,\text{kJ/mol}$ $D(Cl_2) = +243\,\text{kJ/mol}$ $EA_1(Cl) = -349\,\text{kJ/mol}$ $\Delta H_f^\circ(MgCl_2) = -641\,\text{kJ/mol}$ Calculate the lattice energy ($U$) of $MgCl_2(s)$.

Which of the following statements about lattice energy is INCORRECT?

Arrange the following ionic compounds in increasing order of their lattice energy: LiF, NaF, KF, RbF.

Which of the following processes represents the lattice energy of $KCl$?

Which of the following ionic compounds would be expected to have the lowest lattice energy?