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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 at ...
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 ...
1,2-Difluoroethane is a saturated hydrofluorocarbon containing an atom of fluorine attached to each of two carbons atoms. The formula can be written CH 2 FCH 2 F. It is an isomer of 1,1-difluoroethane.
Hydrogen fluoride is typically produced by the reaction between sulfuric acid and pure grades of the mineral fluorite: [14] CaF 2 + H 2 SO 4 → 2 HF + CaSO 4. About 20% of manufactured HF is a byproduct of fertilizer production, which generates hexafluorosilicic acid. This acid can be degraded to release HF thermally and by hydrolysis: H 2 SiF ...
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]
It can be prepared by direct reaction of fluorine with sulfur dioxide: SO 2 + F 2 → SO 2 F 2. On a laboratory scale, sulfuryl fluoride has been conveniently prepared from 1,1'-sulfonyldiimidazole, in the presence of potassium fluoride and acid. [6] [7] Sulfuryl fluoride is unreactive toward molten sodium metal. [3]
Cyanogen fluoride undergoes violent reaction when in the presence of boron trifluoride or hydrogen fluoride. [3] Pure gaseous FCN at atmospheric pressure and room temperature does not ignite by a spark or hot wire. [2] FCN air mixtures however are more susceptible to ignition and explosion than pure FCN.
Above 200 °C, OF 2 decomposes to oxygen and fluorine by a radical mechanism. 2 OF 2 → O 2 + 2 F 2. OF 2 reacts with many metals to yield oxides and fluorides. Nonmetals also react: phosphorus reacts with OF 2 to form PF 5 and POF 3; sulfur gives SO 2 and SF 4; and unusually for a noble gas, xenon reacts (at elevated temperatures) yielding ...