## Related questions with answers

Examine the trends in lattice energy in the table below. The value of the lattice energy becomes somewhat more negative on going from NaI to NaBr to NaCl, and all are in the range from -700 to -800 kJ/mol. Propose a reason for the observation that the lattice energy of ${NaF}\left(\Delta_{\text {lattice }} U=-926 {~kJ} / {mol}\right)$ is much more negative than those of the other sodium halides.

Lattice Energies of Some Ionic Compounds

$\begin{array}{l|r} \hline \text { Compound } & \begin{array}{r} \Delta_{\text {lattice }} U \\ (\mathrm{~kJ} / \mathrm{mol}) \end{array} \\ \hline \mathrm{LiF} & -1037 \\ \hline \mathrm{LiCl} & -852 \\ \hline \mathrm{LiBr} & -815 \\ \hline \mathrm{Lil} & -761 \\ \hline \mathrm{NaF} & -926 \\ \hline \mathrm{NaCl} & -786 \\ \hline \mathrm{NaBr} & -752 \\ \hline \mathrm{Nal} & -702 \\ \hline \mathrm{KF} & -821 \\ \hline \mathrm{KCl} & -717 \\ \mathrm{KBr} & -689 \\ \mathrm{KI} & -649 \\ \hline \end{array}$

Solution

VerifiedThe problem asks to explain why the lattice energy of sodium fluoride ($\mathrm{NaF}$) is much more negative compared to $\mathrm{NaCl}$, $\mathrm{NaBr}$, and $\mathrm{NaI}$.

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