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Fluorine is a chemical element; it has symbol F and atomic number 9. It is the lightest halogen [ note 1 ] and exists at standard conditions as pale yellow diatomic gas. Fluorine is extremely reactive as it reacts with all other elements except for the light inert gases .
The fluorine–fluorine bond of the difluorine molecule is relatively weak when compared to the bonds of heavier dihalogen molecules. The bond energy is significantly weaker than those of Cl 2 or Br 2 molecules and similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines. [8]
Fluoride (/ ˈ f l ʊər aɪ d, ˈ f l ɔːr-/) [3] is an inorganic, monatomic anion of fluorine, with the chemical formula F − (also written [F] −), whose salts are typically white or colorless. Fluoride salts typically have distinctive bitter tastes, and are odorless.
O 2 F 2 precipitates as a brown solid upon the UV irradiation of a mixture of liquid O 2 and F 2 at −196 °C. [8] It also only appears to be stable below −160 °C. [9] The general method of preparation of many oxygen fluorides is a gas-phase electric discharge in cold containers including O 2 F 2. [10] O 2 + F 2 → O 2 F 2 (electric ...
Calcium fluoride is the inorganic compound of the elements calcium and fluorine with the formula CaF 2. It is a white solid that is practically insoluble in water. It occurs as the mineral fluorite (also called fluorspar), which is often deeply coloured owing to impurities.
Fluorene / ˈ f l ʊər iː n /, or 9H-fluorene is an organic compound with the formula (C 6 H 4) 2 CH 2. It forms white crystals that exhibit a characteristic, aromatic odor similar to that of naphthalene. Despite its name, it does not contain the element fluorine, but rather it comes from the violet fluorescence it exhibits.
Carbon is stable in a fluorine atmosphere up to about 400 °C, but between 420-600 °C a reaction takes place to give substoichiometric carbon monofluoride, CF 0.68 appearing dark grey. With increasing temperature and fluorine pressure stoichiometries up to CF 1.12 are formed. With increasing fluorine content the colour changes from dark grey ...
Introducing the carbon–fluorine bond to organic compounds is the major challenge for medicinal chemists using organofluorine chemistry, as the carbon–fluorine bond increases the probability of having a successful drug by about a factor of ten. [30]