(i). Group 2 elements except beryllium are commonly known as alkaline earth metals because their oxides and hydroxides are alkaline in nature and these metal oxides are found in the Earth’s crust. 

(ii). Many alkaline earth metals are used in creating colours and used in fireworks.

(iii). Their general electronic configuration is ns² . 

(iv). Atomic and ionic radii of alkaline earth metals are smaller than alkali metals, on moving down the group, the radii increases. 

(v). These elements exhibit +2 oxidation state in their compounds. 

(vi). Alkaline earth metals have higher ionizatoin enthalpy values than alkali metals and they are less electropositive than alkali metals. 

(vii). Hydration enthalpies of alkaline earth metals decreases as we go down the group. 

(viii). Electronegativity values of alkaline earth metals decrease down the group. 

(ix). Alkaline earth metal salts moistened with concentrated hydrochloric acid gave a characteristic coloured flame, when heated on a platinum wire in a flame.