A student investigates the thermodynamics of dissolution by comparing two soluble chloride salts at \(298\text{ K}\). The student records the standard entropy of dissolution, \(\Delta S^\circ_{\text{soln}}\), for each salt in the table below.

Process	\(\Delta S^\circ_{\text{soln}}\,[\text{J}/(\text{mol}\cdot\text{K})]\)
\(\text{NaCl}(s) \rightarrow \text{Na}^+(aq) + \text{Cl}^-(aq)\)	\(+43\)
\(\text{AlCl}_3(s) \rightarrow \text{Al}^{3+}(aq) + 3\text{ Cl}^-(aq)\)	\(-263\)

Which of the following best explains why \(\Delta S^\circ_{\text{soln}}\) is negative for the dissolution of \(\text{AlCl}_3(s)\)?