Fluorine readily displaces the other halogens from their salts. It combines spontaneously with most other elements—exceptions are chlorine, nitrogen, oxygen, and the so-called inert gases (helium, neon, argon, krypton, xenon, and radon), but it even combines with most of these when heated. Fluorine reacts with most inorganic and organic compounds. With hydrogen it forms hydrogen fluoride gas, whose water solution is called hydrofluoric acid.

Because of its extreme reactivity, fluorine does not occur uncombined in nature. Fluorine gas is produced commercially by electrolysis of a solution of hydrogen fluoride containing potassium hydrogen fluoride. The mineral fluorite, or fluorspar (calcium fluoride), is the chief commercial source. Cryolite and apatite are other important natural compounds.

The importance of fluorine lies largely in its compounds. Fluorite is used as a flux in refining iron; cryolite serves as the electrolyte in the production of aluminum. Compounds of fluorine are also used in the ceramic and glass industries; hydrofluoric acid is used to etch glass and in the manufacture of light bulbs. The addition of one part per million of soluble fluorides to public water supplies has reduced the incidence of tooth decay in many communities, but water with naturally occurring levels as low as four parts per million can damage teeth and bones. In even larger amounts fluorine and fluoride compounds are poisonous. Sodium fluoride is employed as an insecticide.

Halocarbons (compounds of carbon, fluorine, chlorine, and hydrogen) are used extensively in refrigeration and air-conditioning systems. They were widely used as aerosol propellants; but, since they cause depletion of the ozone layer, government restrictions have nearly abolished such use. The linking of fluorine and carbon has created some of the most chemically inert compounds known. Fluorocarbons such as Teflon have found extensive use as lubricants and bearing materials because of their low friction. Because of their inertness and heat resistance they may be used, for example, as a coating on cooking ware. Because they are not wetted by water or oils, they are sometimes used to add antisoil properties to textiles.

The use of fluorite as a flux was described in 1529 by Georgius Agricola. Many early chemists experimented with hydrogen fluoride gas, among them Scheele, Davy, Lavoisier, and Gay-Lussac. Fluorine gas was first prepared in 1886 by Henri Moissan after nearly three quarters of a century of effort. There was no commercial production of fluorine before World War II, when the use of the gas in a process for refining uranium ores prompted its manufacture.

Nonmetallic chemical element, chemical symbol F, atomic number 9. The lightest halogen, it is the most reactive element, forming compounds with all others except helium, neon, and argon (the lighter noble gases). Its only valence is 1, in F₂ (the diatomic molecule) and fluorides. A toxic, pale yellow gas with a pungent odour, it can be produced only by electrolysis under special conditions. Its chief source is fluorite; it also occurs in cryolite, fluorapatite, seawater, bones, and teeth. Hydrogen fluoride (HF) is a raw material for many other fluorides. Its water solution, hydrofluoric acid, is used to clean metals and to polish, etch, or frost glass. Other fluorides are useful catalysts and raw materials. Sodium fluoride (NaF) is added to water and tin fluoride (SnF₂) to dental-care products to reduce dental caries (see fluoridation of water). Fluorocarbons are hydrocarbons in which some hydrogen atoms have been replaced by fluorine atoms; examples include Freons and Teflon.

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