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(D) Lattice energy depends upon two main factors:$1$. Charge on the ions: Greater the charge,higher is the lattice energy.$2$. Size of the ions: Small

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$MgO, LiF, Mg_3N_2$

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(D) Lattice energy depends upon two main factors:$1$. Charge on the ions: Greater the charge,higher is the lattice energy.$2$. Size of the ions: Smaller the size of the ions,higher is the lattice energy.$(i)$ Comparing $KCl$ $(K^+, Cl^-)$ and $MgO$ $(Mg^{2+}, O^{2-})$: $MgO$ has higher ionic charges and smaller ionic radii compared to $KCl$,so $MgO$ has higher lattice energy.$(ii)$ Comparing $LiF$ $(Li^+, F^-)$ and $LiBr$ $(Li^+, Br^-)$: Both have the same cation charge,but $F^-$ is smaller than $Br^-$,so $LiF$ has higher lattice energy.$(iii)$ Comparing $Mg_3N_2$ $(Mg^{2+}, N^{3-})$ and $NaCl$ $(Na^+, Cl^-)$: $Mg_3N_2$ has significantly higher ionic charges,so it has higher lattice energy.Thus,the set with higher lattice energy is $MgO, LiF, Mg_3N_2$.

Which set of compounds in the following pair of ionic compounds has the higher lattice energy?
$(i) \, KCl$ or $MgO$ $(ii) \, LiF$ or $LiBr$ $(iii) \, Mg_3N_2$ or $NaCl$

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Which set of compounds in the following pair of ionic compounds has the higher lattice energy?$(i) \, KCl$ or $MgO$ $(ii) \, LiF$ or $LiBr$ $(iii) \, Mg_3N_2$ or $NaCl$