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Atomic Number: 3
Atomic Symbol: Li
Atomic Weight: 6.941
Electron Configuration: [He]2s1
History
(Gr. lithos, stone) Discovered by Arfvedson in 1817. Lithium is the
lightest of all metals, with a density only about half that of water.
Sources
It does not occur free in nature; combined it is found in small units
in nearly all igneous rocks and in the waters of many mineral springs.
Lepidolite, spodumeme, petalite, and amblygonite are the more important minerals
containing it.
Lithium is presently being recovered from brines of Searles
Lake, in California, and from those in Nevada. Large deposits of quadramene are
found in North Carolina. The metal is produced electrolytically from the fused
chloride. Lithium is silvery in appearance, much like Na and K, other members of
the alkali metal series. It reacts with water, but not as vigorously as sodium.
Lithium imparts a beautiful crimson color to a flame, but when the metal burns
strongly, the flame is a dazzling white.
Uses
Since World War II, the production of lithium metal and its compounds
has increased greatly. Because the metal has the highest specific heat of any
solid element, it has found use in heat transfer applications; however, it is
corrosive and requires special handling. The metal has been used as an alloying
agent, is of interest in synthesis of organic compounds, and has nuclear
applications. It ranks as a leading contender as a battery anode material as it
has a high electrochemical potential. Lithium is used in special glasses and
ceramics. The glass for the 200-inch telescope at Mt. Palomar contains lithium
as a minor ingredient. Lithium chloride is one of the most lyproscopic materials
known, and it, as well as lithium bromide, is used in air conditioning and
industrial drying systems. Lithium stearate is used as an all-purpose and
high-temperature lubricant. Other lithium compounds are used in dry cells and
storage batteries.
Sources: CRC Handbook of Chemistry and
Physics and the American Chemical Society.
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