Lithium :: essays research papers

     In 1817, an aging Swedish chemist was burbling over his work on a late afternoon in Stockholm, Sweden. He was analyzing a strange ore named Petalite that had been procured from an island off the coast of Sweden c eithered Ut. The ore Petalite (which is in a flash recognized to be LiAl(Si2O5)2) had been discovered by a Brazilian scientist, Jos Bonifcio de Andrada e Silva towards the end of the 18th century on a assure to Sweden. This Swedish scientist, Johann August Arfvedson, detected traces of an unknown substance in his standard of Petalite. This was the first discovery of lithium.From the Greek word "lithos" meaning "stone", it was so named due to the fact that it was discovered from a mineral source whereas the some other two common Group 1 elements, Sodium and Potassium, were implant in plant sources. Its symbol, Li, was taken directly from its name. Soon after stumbling upon lithium, Arfvedson also found traces of the metal in t he minerals Spodumene and Lepidolite. In 1818, C.G. Gmelin discovered that Lithium salts color flames a bright red. Neither, Gmelin or Arfvedson, however, were able to isolate the element itself from the Lithium salts. They both tried to reduce the oxide by heating it with Iron or Carbon, precisely neither met with the success of W.T. Brande and Sir Humphrey Davy. They managed to per convention the first isolation of elemental Lithium by the electrolysis of Lithium oxide. Electrolysis is a chemical reaction, which is brought about by the release of current from an external energy source such as a battery. In 1855, the scientists Bunsen and Mattiessen isolated larger quantities of the metal by electrolysis of Lithium chloride.Each scientist or team of scientists had so much trouble cut back the Lithium compounds because Lithium does not exist in its elemental form in nature. It combines very easily with other elements. Lithium is a yielding silvery-white lustrous metal, which can be easily cut with a knife, and it is the lightest of all known metals. It is highly reactive with water and air, and tarnishes readily when exposed to the last mentioned due to a formation of a layer of Lithium suboxide on its surface. Because of its high rate of reaction to air, it must be stored under unstable paraffin, oil, or kerosene, which contain no air, to prevent oxidation. Lithium is detected in its compounds by the characteristic red coloration that it imparts to flames when burned, as Gmelin detected, and by spectroscopic methods.