Which of the following statements is not true for ionic compounds?

Which ionic compound has the largest amount of lattice energy?

The principal reason that the melting point of $NaF$ is much higher than that of $RbBr$ is that

The lattice energies of $NaCl$,$NaF$,$KCl$,and $RbCl$ follow the order:

Which pair will form the most stable ionic bond?

If the enthalpy of sublimation of $Li$ is $155 \ kJ \ mol^{-1}$,enthalpy of dissociation of $F_2$ is $150 \ kJ \ mol^{-1}$,ionization enthalpy of $Li$ is $520 \ kJ \ mol^{-1}$,electron gain enthalpy of $F$ is $-313 \ kJ \ mol^{-1}$,and standard enthalpy of formation of $LiF$ is $-594 \ kJ \ mol^{-1}$,then the magnitude of the lattice enthalpy of $LiF$ is . . . . . . $kJ \ mol^{-1}$ (nearest integer).