The reactivity of alkaline earth metals in aqueous solutions can be predicted based on their electronic configurations. Alkaline earth metals belong to Group 2 of the periodic table and have the general electron configuration of [noble gas] ns, where 'n' represents the period number. These metals include beryllium Be , magnesium Mg , calcium Ca , strontium Sr , barium Ba , and radium Ra .In general, the reactivity of alkaline earth metals increases as you move down the group. This is because the atomic size increases, and the outermost electrons are further away from the nucleus, making them easier to lose. As a result, the ionization energy decreases, and the metals become more reactive. When these metals react with water, they form alkaline basic solutions and release hydrogen gas. The general reaction can be represented as:M s + 2HO l M OH aq + H g where M represents an alkaline earth metal.Transition metals, on the other hand, are found in the d-block of the periodic table and have varying electron configurations. They generally have lower reactivity in aqueous solutions compared to alkaline earth metals. This is because transition metals have multiple oxidation states and can form complex ions with water molecules, which can stabilize the metal ions in solution. Additionally, the ionization energies of transition metals are generally higher than those of alkaline earth metals, making it more difficult for them to lose electrons and react.In summary, the reactivity of alkaline earth metals in aqueous solutions increases as you move down the group, and they form alkaline solutions when reacting with water. In comparison, transition metals have lower reactivity in aqueous solutions due to their multiple oxidation states, ability to form complex ions, and higher ionization energies.