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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.
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]
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]
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.
Iron(III) fluoride, also known as ferric fluoride, are inorganic compounds with the formula FeF 3 (H 2 O) x where x = 0 or 3. They are mainly of interest by researchers, unlike the related iron(III) chloride .
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
A third method requires heating a mix of fluorine and oxygen to 700 °C (1,292 °F), and then rapidly cooling it using liquid oxygen. [5] All of these methods involve synthesis according to the equation O 2 + F 2 → O 2 F 2. It also arises from the thermal decomposition of ozone difluoride: [6] 2 O 3 F 2 → 2 O 2 F 2 + O 2
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 ...