Spontaneity, Entropy, and Free Energy Question 1

\ce{CaCl2(s)-> Ca^{2+}(aq) + 2Cl-(aq)}

For the process of solid calcium chloride dissolving in water, represented above, the entropy change might be expected to be positive. However, $\Delta S$ for the process is actually negative. Which of the following best helps to account for the net loss of entropy?

\ce{Cl-}

ions are much larger in size than

\ce{Ca^2+}

ions.

The particles in solid calcium chloride are more ordered than are particles in amorphous solids.

Water molecules in hydration shells of

\ce{Ca^{2+}(aq)}

and

\ce{Cl-(aq)}

ions are more ordered than they are in the pure water.

The

\ce{Ca^{2+}(aq)}

and

\ce{Cl-(aq)}

ions are more free to move around in solution than they are in

\ce{CaCl2(s)}