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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]
Out of the four stable halogens, only fluorine and chlorine have reduction potentials higher than that of oxygen, allowing them to form hydrofluoric acid and hydrochloric acid directly through reaction with water. [17] The reaction of fluorine with water is especially hazardous, as an addition of fluorine gas to cold water will produce ...
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]
F undergo β + decay and electron capture, lighter isotopes decay by proton emission, and those heavier than 19 F undergo β − decay (the heaviest ones with delayed neutron emission). [54] [55] Two metastable isomers of fluorine are known, 18m F, with a half-life of 162(7) nanoseconds, and 26m F, with a half-life of 2.2(1) milliseconds. [56]
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.
1,1,1,2-tetrafluorodisulfane, also known as 1,2-difluorodisulfane 1,1-difluoride or just difluorodisulfanedifluoride (FSSF 3) is an unstable molecular compound of fluorine and sulfur. The molecule has a pair of sulfur atoms, with one fluorine atom on one sulfur, and three fluorine atoms on the other.
The standard enthalpy of formation of rubidium fluoride is Δ f H 0 298 = −552.2 kJ mol−1, [7] the standard free enthalpy of formation ΔG 0 298 = −520.4 kJ mol−1, [7] and the standard molar entropy S 0 298 = 113.9 J K −1 ·mol−1. [7] The enthalpy of solution of rubidium fluoride was determined to be −24.28 kJ/mol. [8]
Fluorine gas (F 2) can act both as an electrophilic and atomic source of fluorine. [4] The weak F–F bond strength (36 kcal/mol (150 kJ/mol) [5]) allows for homolytic cleavage. The reaction of F 2 with organic compounds is, however, highly exothermic and can lead to non-selective fluorinations and C–C cleavage, as well as explosions. [6]