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Wikipedia article:  Fluorine

Fluorine

Fluorine (100)

·         At standard pressure and temperature, fluorine is a pale yellow gas composed of diatomic molecules, F2.

·         It was not until 1886 that elemental fluorine was obtained by French chemist Henri Moissan, whose method of electrolysis remains the only industrial production method of fluorine gas.

·         Fluorine forms stable compounds, fluorides, with all elements except helium and neon, for which the reaction has been attempted.

·         Heavier metal elements such as uranium can form volatile coordination compounds (separate molecules with several fluorine atoms surrounding a metal atom).

·         Fluorine occurs naturally on Earth exclusively in the form of its only stable isotope, fluorine-19, which makes the element both monoisotopic and mononuclidic.

·         All isotopes heavier than the stable fluorine-19 decay via beta minus decay (electron emission), for some isotopes possibly together with neutron emission.

·         Fluorine is so reactive that water, halogens, and most other substances, even generally nonreactive ones such as radon, burn with a bright flame in a jet of fluorine gas.

·         Three minerals exist on earth that contain enough fluorine to be mined and used as industrial resources.

·         Fluorine exists in the −1 oxidation state in all compounds except for elemental fluorine, where the atoms are bonded to each other and thus at oxidation state 0.

·         Organofluorine compounds are synthesized via both direct reaction with fluorine gas, which can be dangerously reactive, or reaction with fluorinating reagents such as sulfur tetrafluoride.

·         The enzyme adenosyl-fluoride synthase is capable of biologically synthesizing the carbon–fluorine bond.

metals (100)

·         Most frequently, the metals must be in powder forms, because many metals form layers of fluoride on their surfaces that resist further oxidation.

fluoride (78)

·         Most frequently, the metals must be in powder forms, because many metals form layers of fluoride on their surfaces that resist further oxidation.

·         The most important is fluorite, which is used in smelting, construction, and the manufacture of hydrogen fluoride.

·         Due to the basicity of the fluoride ion, soluble fluorides give basic water solutions.

·         The enzyme adenosyl-fluoride synthase is capable of biologically synthesizing the carbon–fluorine bond.

elemental fluorine (64)

·         It was not until 1886 that elemental fluorine was obtained by French chemist Henri Moissan, whose method of electrolysis remains the only industrial production method of fluorine gas.

·         Fluorine exists in the −1 oxidation state in all compounds except for elemental fluorine, where the atoms are bonded to each other and thus at oxidation state 0.

gas (64)

·         At standard pressure and temperature, fluorine is a pale yellow gas composed of diatomic molecules, F2.

·         It was not until 1886 that elemental fluorine was obtained by French chemist Henri Moissan, whose method of electrolysis remains the only industrial production method of fluorine gas.

·         Fluorine is so reactive that water, halogens, and most other substances, even generally nonreactive ones such as radon, burn with a bright flame in a jet of fluorine gas.

·         Tetrafluorides are the borderline: for example, zirconium tetrafluoride is an ionic solid, but germanium tetrafluoride is a molecular gas.

·         Organofluorine compounds are synthesized via both direct reaction with fluorine gas, which can be dangerously reactive, or reaction with fluorinating reagents such as sulfur tetrafluoride.

fluorine-19 (61)

·         Fluorine occurs naturally on Earth exclusively in the form of its only stable isotope, fluorine-19, which makes the element both monoisotopic and mononuclidic.

·         All isotopes heavier than the stable fluorine-19 decay via beta minus decay (electron emission), for some isotopes possibly together with neutron emission.

chemicals (61)

·         Inorganic fluorides and organofluorine compounds find use in a variety of materials and chemicals, including important pharmaceuticals, agrochemicals, lubricants, and textiles.

molecules (54)

·         At standard pressure and temperature, fluorine is a pale yellow gas composed of diatomic molecules, F2.

·         Heavier metal elements such as uranium can form volatile coordination compounds (separate molecules with several fluorine atoms surrounding a metal atom).

·         The bond energy is similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines and significantly weaker than those of dichlorine or dibromine molecules.

acid (43)

·         Hydrofluoric acid, in contrast to other haloacids such as hydrochloric acid, is only a weak acid in water, but it is nonetheless extremely corrosive.

·         Andreas Sigismund Marggraf made the first recorded preparation of "fluoric acid" (hydrofluoric acid in modern nomenclature) in 1764, when he heated fluorite with sulfuric acid in glass, which was greatly corroded by the product.

minerals (41)

·         Three minerals exist on earth that contain enough fluorine to be mined and used as industrial resources.

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