Which ion in each of the following pairs would you expect to be more strongly hydrated? Why? a. \(\mathrm{Na}^{+}\) or \(\mathrm{Mg}^{2+}\) b. \(\mathrm{Mg}^{2+}\) or \(\mathrm{Be}^{2+}\) c. \(\mathrm{Fe}^{2+}\) or \(\mathrm{Fe}^{3+}\) d. \(\mathrm{F}^{-}\) or \(\mathrm{Br}^{-}\) e. \(\mathrm{Cl}^{-}\) or \(\mathrm{ClO}_{4}^{-}\) f. \(\mathrm{ClO}_{4}^{-}\) or \(\mathrm{SO}_{4}^{2-}\)

a. \(\mathrm{Mg}^{2+}\) is more strongly hydrated because it has a higher charge than \(\mathrm{Na}^{+}\). b. \(\mathrm{Be}^{2+}\) is more strongly hydrated because it has a smaller atomic radius than \(\mathrm{Mg}^{2+}\). c. \(\mathrm{Fe}^{3+}\) is more strongly hydrated because it has a higher charge than \(\mathrm{Fe}^{2+}\). d. \(\mathrm{F}^{-}\) is more strongly hydrated because it has a smaller atomic radius than \(\mathrm{Br}^{-}\). e. \(\mathrm{Cl}^{-}\) is more strongly hydrated because it has a higher effective charge density than \(\mathrm{ClO}_{4}^{-}\). f. \(\mathrm{SO}_{4}^{2-}\) is more strongly hydrated because it has a higher negative charge than \(\mathrm{ClO}_{4}^{-}\).