Chemical elements
  Lithium
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
      Lithium hydride
      Lithium chloride
      Lithium bromide
      Lithium iodide
      Lithium iodide tetrachloride
      Lithium hypochlorite
      Lithium chlorate
      Lithium perchlorate
      Lithium bromate
      Lithium iodate
      Lithium periodates
      Lithium monoxide
      Lithium peroxide
      Lithium hydroxide
      Lithium monosulphide
      Lithium polysulphides
      Lithium sulphite
      Lithium sulphate
      Lithium persulphate
      Lithium thiosulphate
      Lithium dithionate
      Lithium selenide
      Lithium selenite
      Lithium selenate
      Lithium chromate
      Lithium permanganate
      Lithium molybdates
      Lithium nitride
      Lithium hydrazoate
      Lithamide
      Lithium nitrite
      Lithium nitrate
      Lithium phosphide
      Lithium orthophosphate
      Lithium pyrophosphate
      Lithium metaphosphate
      Lithium arsenide
      Lithium meta-arsenite
      Lithium arsenate
      Lithium antimonide
      Lithium antimonate
      Lithium carbide
      Lithium carbonate
      Lithium percarbonate
      Lithium cyanide
      Lithium thiocyanate
      Lithium silicide
      Lithium silicates
      Lithium borates

Chemical Properties of Lithium






Although less reactive than potassium and sodium, lithium is analogous in chemical character to those metals. At ordinary temperature it is unaffected by dry oxygen or air, but the presence of moisture causes oxidation. At 200° C. it ignites in air or oxygen, burning with a bright white light, and forming the monoxide and a small proportion of the peroxide. In nitrogen it is converted without application of heat into the nitride, so that this substance is probably a product of its combustion in air. Its affinity for nitrogen has been applied in the isolation of argon from the atmosphere. This reaction exemplifies the similarity between lithium and calcium, a resemblance also manifested in the direct combination of lithium with chlorine, bromine, iodine, and sulphur-vapour. When heated in hydrogen, lithium yields a hydride. In its compounds the metal invariably exhibits univalency.

Experiments on photographic plates with lithium and its salts produced no effect, indicating a lack of radioactivity.


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