Which ion in each of the following pairs would you expect to be more strongly hydrated?

(a) Na+ or Mg2+

Why?

thanks!!

what about when u are comparing the same charge

Be2+
Mg2+

or the same base element

Fe2+
Fe3+

It depends to a large extent on what you mean by STRONGLY hydrated. Is that the strength of the bond or the number of water molecules attracted?

In the case of Be ion vs Mg ion, the Be-H2O bonds probably are stronger because the Be ion is smaller thus the charge density is higher. However, since it is smaller (that is the Mg ion is larger), the Mg ion hydrates with 6 molecules H2O while the usual number for Be is 4.
In the case of iron(II) vs iron (III), the charge is higher on iron(III) wo it will more strongly attract water molecules.

To determine which ion in the pair would be more strongly hydrated, we need to consider the charge and size of the ions.

First, let's compare the charges of Na+ and Mg2+. Na+ has a charge of +1, whereas Mg2+ has a charge of +2. Generally, ions with higher charges tend to be more strongly hydrated because they have a greater attraction for water molecules due to their stronger electrostatic pull.

Next, let's consider the size of the ions. Na+ has a smaller ionic radius compared to Mg2+. Smaller ions have a greater charge density, meaning they have a higher charge per unit distance. This higher charge density also leads to a stronger attraction for water molecules, resulting in stronger hydration.

Combining the factors of charge and size, we can conclude that Mg2+ would be more strongly hydrated than Na+.

yolo

If you are a water molecule you are polarized with the O end slightly negative and the H end slightly positive. Which would you be more highly attracted to, a +1 charge or a +2 charge?