Search results
Results From The WOW.Com Content Network
Reactions with elemental fluorine are often sudden or explosive. Many substances that are generally regarded as unreactive, such as powdered steel, glass fragments, and asbestos fibers, are readily consumed by cold fluorine gas. Wood and even water burn with flames when subjected to a jet of fluorine, without the need for a spark. [12] [13]
Reactions of elemental fluorine with metals require varying conditions. Alkali metals cause explosions and alkaline earth metals display vigorous activity in bulk; to prevent passivation from the formation of metal fluoride layers, most other metals such as aluminium and iron must be powdered, [ 21 ] and noble metals require pure fluorine gas ...
The reaction mixture was warmed to 25°, 50 mL of water was added, and the lower organic layer was separated and dried with anhydrous magnesium sulfate and distilled to give 12.0 g (90%) of 1-fluorooctane as a colorless liquid, bp 42–43° (20 mm). 19 F NMR (CCl 3 F): -218.8 ppm (tt, 2 J = 49 Hz, 3 J = 25 Hz). [18]
Fluorine-18 (18 F, also called radiofluorine) is a fluorine radioisotope which is an important source of positrons. It has a mass of 18.0009380(6) u and its half-life is 109.771(20) minutes. It decays by positron emission 96.7% of the time and electron capture 3.3% of the time.
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.
In this approach, HF is oxidized in the presence of a hydrocarbon and the fluorine replaces C–H bonds with C–F bonds. Perfluorinated carboxylic acids and sulfonic acids are produced in this way. [15] 1,1-Difluoroethane is produced by adding HF to acetylene using mercury as a catalyst. [15] HC≡CH + 2 HF → CH 3 CHF 2
4 serves as a fluorine source to deliver an equivalent of fluoride. [2] The Balz–Schiemann reaction for the synthesis of aryl fluorides is the best known example of such a reaction. [3] Ether and halopyridine adducts of HBF 4 have been reported to be effective reagents for the hydrofluorination of alkynes. [4]
O 3 F 2 is a viscous, blood-red liquid. It remains liquid at 90 K and so can be differentiated from O 2 F 2 which has a melting point of about 109 K. [11] [3] Like the other oxygen fluorides, O 3 F 2 is endothermic and decomposes at about 115 K with the evolution of heat, which is given by the following reaction: 2 O 3 F 2 → O 2 + 2 O 2 F 2