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Calcium chloride was apparently discovered in the 15th century but wasn't studied properly until the 18th century. [11] It was historically called "fixed sal ammoniac" (Latin: sal ammoniacum fixum [12]) because it was synthesized during the distillation of ammonium chloride with lime and was nonvolatile (while the former appeared to sublime); in more modern times (18th-19th cc.) it was called ...
Although most compounds are referred to by their IUPAC systematic names (following IUPAC nomenclature), traditional names have also been kept where they are in wide use or of significant historical interests.
A white solid, it forms by the reaction of hydrogen chloride with calcium hydroxide [3] According to X-ray crystallography, it adopts a layered structure related to brucite (magnesium hydroxide, Mg(OH) 2). [4] Calcium hydroxychloride is sometimes confused with calcium hypochlorite.
The only major inputs to the Solvay process are salt, limestone and thermal energy, and its only major byproduct is calcium chloride, which is sometimes sold as road salt. After the invention of the Haber and other new ammonia-producing processes in the 1910s and 1920s its price dropped, and there was less need in reclaiming it.
Calcium fluoride is the inorganic compound of the elements calcium and fluorine with the formula CaF 2. It is a white solid that is practically insoluble in water. It occurs as the mineral fluorite (also called fluorspar), which is often deeply coloured owing to impurities.
Hypervalent iodine compounds are useful reagents in organic chemistry (e.g. Dess–Martin periodinane) Tetra-, penta- and hexavalent phosphorus, silicon, and sulfur compounds (e.g. PCl 5, PF 5, SF 6, sulfuranes and persulfuranes) Noble gas compounds (ex. xenon tetrafluoride, XeF 4) Halogen polyfluorides (ex. chlorine pentafluoride, ClF 5)
The one-step reaction is shown below: [3] 2 Cl 2 + 2 Ca(OH) 2 → CaCl 2 + Ca(OCl) 2 + 2 H 2 O. Industrial setups allow for the reaction to be conducted in stages to give various compositions, each producing different ratios of calcium hypochlorite, unconverted lime, and calcium chloride. [3]
The main purpose of chemical nomenclature is to disambiguate the spoken or written names of chemical compounds: each name should refer to one compound. Secondarily, each compound should have only one name, although in some cases some alternative names are accepted. Preferably, the name should also represent the structure or chemistry of a compound.