# Compare the alkali metals and alkaline earth metals with respect to (i) Ionisation enthalpy (ii) Basicity of oxides (iii) Solubility of hydroxides

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Hint: The elements in group one of the periodic tables (except for hydrogen-see below) are known as alkali metals since, when they react with water, they form alkaline solutions. Group two of the periodic table contains beryllium, magnesium, calcium, strontium, barium and radium elements. The elements in this group, which all appear brilliant and silvery-white, are known as alkaline earth metals.

Alkaline earth metal, any of the six chemical elements forming Group 2 ($IIa$) of the table. The components are beryllium$\left( Be \right)$, magnesium$\left( Mg \right)$, calcium$\left( Ca \right)$, strontium$\left( Sr \right)$, barium $\left( Ba \right)$and radium $\left( Ra \right)$.Alkali metal, any of the six chemical elements that compose Group 1 $\left( Ia \right)$of the periodic table—namely, lithium $\left( Li \right)$,sodium $\left( Na \right)$,potassium$\left( K \right)$, rubidium $\left( Rb \right)$, cesium $\left( Cs \right)$, and francium $\left( Fr \right)$.
(ii) Basicity of oxides: On dissolution in water, the oxides of alkali metals and alkaline-earth metal metals form basic hydroxides. The basicity of metallic element oxides is more than that of metallic element metal oxides. And as know it’s all because of the lower ionization enthalpy of alkali metals than that of corresponding alkaline earths. Because of which, the $M-OH$ bond in metal hydroxides can more easily ionize.