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Perchloryl fluoride is produced primarily by the fluorination of perchlorates. The initial syntheses in the early 1950s used fluorine gas or fluorides and anodic oxidation as the fluorinating agents, but these give explosive gaseous mixtures. [8] A common fluorinator in modern syntheses is antimony pentafluoride: [3]: 372–373 ClO − 4 + 3 HF ...
Organofluorine compounds are prepared by numerous routes, depending on the degree and regiochemistry of fluorination sought and the nature of the precursors. The direct fluorination of hydrocarbons with F 2, often diluted with N 2, is useful for highly fluorinated compounds: R 3 CH + F 2 → R 3 CF + HF
The well-characterized heavier halogens (chlorine, bromine, and iodine) all form mono-, tri-, and pentafluorides: XF, XF 3, and XF 5. Of the neutral +7 species, only iodine heptafluoride is known. [93] While chlorine and bromine heptafluorides are not known, the corresponding cations ClF + 6 and BrF + 6, extremely strong oxidizers, are. [94]
Such reagents include cobalt trifluoride, chlorine trifluoride, and iodine pentafluoride. [4] The method electrochemical fluorination is used commercially for the production of perfluorinated compounds. It generates small amounts of elemental fluorine in situ from hydrogen fluoride. The method avoids the hazards of handling fluorine gas.
ClO 2 F was first reported by Schmitz and Schumacher in 1942, who prepared it by the fluorination of ClO 2. [2] The compound is more conveniently prepared by reaction of sodium chlorate and chlorine trifluoride [3] and purified by vacuum fractionation, i.e. selectively condensing this species separately from other products. This species is a ...
Chlorine pentafluoride (ClF 5) is made on a large scale by direct fluorination of chlorine with excess fluorine gas at 350 °C and 250 atm, and on a small scale by reacting metal chlorides with fluorine gas at 100–300 °C. It melts at −103 °C and boils at −13.1 °C.
[142] [143] Chlorine, bromine, and iodine can each form mono-, tri-, and pentafluorides, but only iodine heptafluoride has been characterized among possible interhalogen heptafluorides. [144] Many of them are powerful sources of fluorine atoms, and industrial applications using chlorine trifluoride require precautions similar to those using ...
By far most chlorine is manufactured from table salt (NaCl) by electrolysis in the chlor-alkali process. The resulting gas at atmospheric pressures is liquified at high pressure. The liquefied gas is transported and used as such. [citation needed] As a strong oxidizing agent, chlorine kills via the oxidation of organic molecules. [16]