Why do smaller ions tend to be more strongly hydrated? For instance, why is Mg
2+ expected to be more strongly hydrated than Be
2+?
I looked in my textbook, but their explanation isn't helpful making sense to me:
The smaller ions presumably are able to bind the hydrating water molecules more firmly and thus show a more negative value for ∆S˚solution
But if this is true, then wouldn't smaller ions have weaker hydration, since they don't negative ∆S leads to positive ∆G
Thanks!