Describe the differences between the solubility and basicity of Group 2 hydroxides.

Group 2 hydroxides differ in their solubility and basicity.

Group 2 hydroxides are compounds formed by the reaction of Group 2 metals with water. They are alkaline in nature and can neutralize acids. The solubility of Group 2 hydroxides increases down the group. Beryllium hydroxide is insoluble in water, while the hydroxides of magnesium, calcium, strontium, and barium are soluble. The solubility of these hydroxides increases as the atomic radius of the metal increases. This is because the larger the metal ion, the more polarizable it is, and the more easily it can attract water molecules to form hydrated ions.

The basicity of Group 2 hydroxides also increases down the group. This is because the strength of the metal-oxygen bond decreases as the atomic radius of the metal increases. This means that the hydroxides of larger Group 2 metals are more basic than those of smaller metals. For example, barium hydroxide is a stronger base than calcium hydroxide. The basicity of Group 2 hydroxides can be measured by their ability to neutralize acids. The more basic a hydroxide, the more acid it can neutralize.

In summary, the solubility and basicity of Group 2 hydroxides increase down the group. This is due to the increasing size of the metal ions, which makes them more polarizable and less strongly bonded to oxygen.