# Why does aluminum chloride have a higher lattice energy than aluminum fluoride?

From the table below (source: McMurry's Chemistry [1, p. 212]), it is evident that $$\ce{AlCl_3}$$ has a higher lattice energy than $$\ce{AlF3},$$ even though $$\ce{F}$$ is smaller than $$\ce{Cl}$$. Why is this so?

However, the melting point of $$\ce{AlF3}$$ $$(\pu{1291 °C})$$ is larger than that of $$\ce{AlCl3}$$ $$(\pu{192.4 °C}).$$ I think the huge melting point difference is because $$\ce{AlCl3}$$ is more covalent, while $$\ce{AlF3}$$ is more ionic. That being said, does lattice energy account for the covalent and ionic character of compounds?

### References

1. McMurry, J.; Fay, R. C.; Robinson, J. K. Chemistry, 7th ed.; Pearson: Boston, 2015. ISBN 978-0-321-94317-0.