Group 2 elements - the alkaline earth metals

The chemistry of these elements (except Be) is dominated by their tendency to lose two electrons and their compounds are generally ionic. The general equation for this reaction is 

The metals tend to be less reactive than their corresponding alkali metals because removal of two electrons requires more energy. The alkaline earth metals also have higher densities and melting points than the alkali metals. Reactivity of the Group 2 metals increases as the group is descended (Table 12.3). 

Some chemical properties of Group 2 metals (with the exception of Be, which forms mostly covalent compounds) are  

They burn in air to form normal oxides (barium forms some peroxide). The general equation is 

The alkaline earth metals, when heated, also react with nitrogen to form ionic nitrides  

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