The group 2 elements are known as the Alkali earth metals . They react easily with other elements to form compounds such as sulfates and carbonates. Calcium is found extensively as calcium carbonate (CaCO₃) in the form of limestone and marble. It also id the major constituent of sea-shells. All group 2 metals are harder and less reactifve than group 1.All the oxides formed, with the exception of BeO, are basic. During reactions these elements, like the group 1 elements, act as reductants forming ions with a charge of 2+.

Magnesium is used as a structural material as it strong and less dense than aluminium. It is used mainly in aircraft and must be protected oxygen.

 2Mg_(s) + O_2(g) => 2Mg₂O_(s)

Reactions with water

Mg_(s) + H₂O_(l) => 2Mg(OH)_2(aq) + H_2(g)

The electronic configuration of these elements is as follows.
Be 1s², 2s²

Mg 1s², 2s², 2p⁶, 3s²

Ca 1s², 2s², 2p⁶, 3s², 3p⁶, 4s²

Sr 1s², 2s², 2p⁶, 3s², 3p⁶, 3d¹⁰, 4s², 4p⁶, 5s²

Ba 1s², 2s², 2p⁶, 3s², 3p⁶, 3d¹⁰, 4s², 4p⁶, 4d¹⁰, 5s², 5p⁶, 6s²

Notice how there is always two outer shell electron. All elements in group 2 have similar properties due to the similarity in their electronic configuration.