All metals are reactive by definition, but two groups are
considered to be much more highly reactive than the rest. The Alkali Metals group
consists of the first row on the left side of the periodic table - lithium, sodium,
potassium, rubidium, cesium,and francium. These metals have just one electron in the
outermost orbital, called a valence electron. They lose this
electron very readily in reaction with other elements, becoming a +1 ion and releasing
energy in the process; that's where the reaction comes from. A classic lab demonstration
consists of putting a chunk of sodium into water, where it explodes violently. See the
youtube link below for a demonstration of this - it's quite
amazing!
The next column to the right, the Alkaline Earth
Metals, consists of beryllium, magnesium, calcium, strontium, barium, and radium. These
metals are not quite as reactive as the first group, but will still react- for instance,
magnesium burns very readily. They have 2 valence electrons and will produce a +2 ion
when reacting.
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