The alkaline earth metals, situated in group 2 of the periodic table, are, like the alkali metals, silvery-white and relatively soft, but they have higher melting and boiling points than their near neighbours. Beryllium, for example, which has the highest melting point of the alkaline earth metals, melts at 1289 degrees Celsius, whereas lithium, which has the highest melting point of the alkali metals, melts at 180.6 degrees Celsius.
The alkaline earth metals are denser than the alkali metals, but not as reactive. They are reactive enough, however, never to be found in nature uncombined. Like the alkali metals, they react with water to form alkaline solutions. Both beryllium and magnesium, when exposed to air, develop a layer of oxide which protects them from further corrosion, but the other group members tarnish readily.
Because they readily give up the two electrons present in each of their outer shells, they are good reducing agents. Like the alkali metals, they are good conductors of electricity, and burn in air with characteristic flame colours. Magnesium gives a brilliant white light, calcium an orange-red, strontium a bright red, barium a yellowish-green, and radium a vivid crimson. This makes them of use in fireworks.
