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Water-reactive substances [1] are those that spontaneously undergo a chemical reaction with water, often noted as generating flammable gas. [2] Some are highly reducing in nature. [ 3 ] Notable examples include alkali metals , lithium through caesium , and alkaline earth metals , magnesium through barium .
Unit cell of Hg 2 F 2, with F from adjacent molecules coordinating the Hg atoms. In common with other Hg(I) (mercurous) compounds which contain linear X-Hg-Hg-X units, Hg 2 F 2 contains linear FHg 2 F units with an Hg-Hg bond length of 251 pm (Hg-Hg in the metal is 300 pm) and an Hg-F bond length of 214 pm. [5] The overall coordination of each Hg atom is a distorted octahedron; in addition to ...
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 ...
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]
Oxygen difluoride reacts with water to form hydrofluoric acid: OF 2 + H 2 O → 2 HF + O 2. It can oxidize sulphur dioxide to sulfur trioxide and elemental fluorine: OF 2 + SO 2 → SO 3 + F 2. However, in the presence of UV radiation, the products are sulfuryl fluoride (SO 2 F 2) and pyrosulfuryl fluoride (S 2 O 5 F 2): OF 2 + 2 SO 2 → S 2 O ...
Crystallization from an aqueous solution containing NaF produces compounds containing polynuclear anions, e.g. NaSn 2 F 5 or Na 4 Sn 3 F 10 depending on the reaction conditions, rather than NaSnF 3. [20] The compound NaSnF 3, containing the pyramidal SnF 3 − anion, can be produced from a pyridine–water solution. [27]
Illustration of a redox reaction. In the reaction between hydrogen and fluorine, hydrogen is being oxidized and fluorine is being reduced: H 2 + F 2 → 2 HF. This spontaneous reaction releases 542 kJ per 2 g of hydrogen because the H-F bond is much stronger than the F-F bond. This reaction can be analyzed as two half-reactions.
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 ...