The reactivity of the alkali family increases from Li to Cs, except for nitrogen molecules. In solution, the Li + ion stabilizes by high solvation energy. The major chemistry of metal is described by the Li + ion. The large difference between the first and second ionization energy of lithium suggests that the preferred oxidation state of the metal is +1 oxidation. About 1000 tonnes of lithium metal and several thousands of salts are prepared annually for various purposes of use. The major commercial form of the metal Li 2CO 3, is produced from ores or brines by different processes and uses largely in the chemical industry. Therefore, fused chloride and hydroxide are used for the preparation of lithium and sodium. Due to electropositivity, alkali metals readily react with water and cannot be produced by electrolysis. The alkali metals beings most electropositive and have never been found in nature in elementary states. In this century, Australia, Chile, and Portugal are the largest commercial suppliers of the metal or its compound. In the 19th century, the United States was the largest producer of chemical elements and compounds like Li 2CO 3. Searles Lake in California is an important source of nearly dry and alkaline ( pH scale = 9.5) lithium metal. It also occurs in many springs and some radioactive decay minerals like carnallite, ashes of planets, in taboo, milk, and blood of living animals. It may facilitate nuclear reaction to heavier elements like beryllium or boron. The very low terrestrial or cosmic abundance of lithium compared to other alkali metals describe by its small nuclear charge and low potential barrier. It is found mainly in the United States, Canada, Brazil, Argentina, the Soviet Union, Spain, and Congo.
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