The following is a quote from Lehninger's Principles of Biochemistry, 4th edition, pg.52:
(...) dissolving hydrophobic compounds in water produces a measurable decrease in entropy. Water molecules in the immediate vicinity of a nonpolar solute are constrained in their possible orientations as they form a highly ordered cagelike shell around each solute molecule.
Why is this so? My intuition tells me that dissolving polar molecules (hydrophilic) would cause a higher ordering of water molecules in the vicinity of the solute than the ordering caused by dissolving nonpolar compounds. This is because I think that the polar solutes should align with the dipoles of the water molecules, thus constraining the alignment of water molecules in the vicinity of the hydrophilic solute.
Is there a simple explanation for the opposite behavior?
Edit: I want to understand, at least intuitively, the physical mechanism behind the entropy decrease of the water molecules around an hydrophobic molecule.