Zinc chloride

Zinc chloride has long been known but currently practiced industrial applications all evolved in the latter half of 20th century. Dilute aqueous zinc chloride was used as a disinfectant under the name "Burnett's Disinfecting Fluid". From 1839 Sir William Burnett promoted its use as a disinfectant as well as a wood preservative. The Royal Navy conducted trials into its use as a disinfectant in the late 1840s, including during the cholera epidemic of 1849; and at the same time experiments were conducted into its preservative properties as applicable to the shipbuilding and railway industries. Burnett had some commercial success with his eponymous fluid. Following his death however, its use was largely superseded by that of carbolic acid and other proprietary products. ==Structure and properties==

Unlike other metal dichlorides, zinc dichloride adopts several crystalline forms (polymorphs). Four polymorph are known: α, β, γ, and δ. Each features centers surrounded in a tetrahedral manner by four chloride ligands. Here a, b, and c are lattice constants, Z is the number of structure units per unit cell, and ρ is the density calculated from the structure parameters. The orthorhombic form (δ) rapidly changes to another polymorph upon exposure to the atmosphere. A possible explanation is that the ions originating from the absorbed water facilitate the rearrangement. Molten has a high viscosity at its melting point and a comparatively low electrical conductivity, which increases markedly with temperature. As indicated by a Raman scattering study, the viscosity is explained by the presence of polymers. Neutron scattering study indicated the presence of tetrahedral centers, which requires aggregation of monomers as well. Hydrates A variety of hydrated zinc chloride are known: {{chem2|ZnCl2(H2O)_{n}|}} with n = 1, 1.33, 2.5, 3, and 4.5. The 1.33-hydrate, previously thought to be the hemitrihydrate, consists of trans-Zn(H2O)4Cl2 centers with the chloro ligands bridging to tetrachlorozincate ([ZnCl4]2-) groups, present in 1:2 ratio. ==Preparation and purification==

Historically, zinc chlorides are prepared from the reaction of hydrochloric acid with zinc metal or zinc oxide. Aqueous acids cannot be used to produce anhydrous zinc chloride. According to an early procedure, a suspension of powdered zinc in diethyl ether is treated with hydrogen chloride, followed by drying The overall method remains useful in industry, but without the solvent: : Hydrates can be produced by evaporation of an aqueous solution of zinc chloride. The temperature of the evaporation determines the hydrates. For example, evaporation at room temperature produces the 1.33-hydrate. Lower evaporation temperatures produce higher hydrates. A simple method relies on treating the zinc chloride with thionyl chloride. ==Reactions==

Zinc chloride is an occasional laboratory reagent, often as a Lewis acid. Chloride complexes A number of salts containing the tetrachlorozincate anion, , are known. is an example of a salt containing that is used in organic chemistry. The compound contains tetrahedral and Chloride| anions,--> Adducts The adduct with thf illustrates the tendency of zinc chloride to form 1:2 adducts with weak Lewis bases. Being soluble in ethers and lacking acidic protons, this complex is used in the synthesis of organozinc compounds. A related 1:2 complex is (zinc dichloride di(hydroxylamine)). Known as Crismer's salt, this complexes releases hydroxylamine upon heating. The distinctive ability of aqueous solutions of to dissolve cellulose is attributed to the formation of zinc-cellulose complexes, illustrating the stability of its adducts. Cellulose also dissolves in molten hydrate. Overall, this behavior is consistent with Zn2+ as a hard Lewis acid. When solutions of zinc chloride are treated with ammonia, diverse ammine complexes are produced. In addition to the tetrahedral 1:2 complex . the complex also has been isolated. The latter contains the ion,. Aqueous solutions of zinc chloride Zinc chloride dissolves readily in water to give {{chem2|ZnCl_{x}(H2O)_{4−x}|}} species and some free chloride. Aqueous solutions of are acidic: a 6 M aqueous solution has a pH of 1. Most metal dichlorides form octahedral complexes, with stronger O-H bonds. The combination of hydrochloric acid and gives a reagent known as "Lucas reagent". Such reagents were once used as a test for primary alcohols. Similar reactions are the basis of industrial routes from methanol and ethanol respectively to methyl chloride and ethyl chloride. In alkali solution, zinc chloride converts to various zinc hydroxychlorides. These include , , , and the insoluble . The latter is the mineral simonkolleite. When zinc chloride hydrates are heated, hydrogen chloride evolves and hydroxychlorides result. In aqueous solution , as well as other halides (bromide, iodide), behave interchangeably for the preparation of other zinc compounds. These salts give precipitates of zinc carbonate when treated with aqueous carbonate sources: Redox Anhydrous zinc chloride melts and even boils without any decomposition up to 900 °C. When zinc metal is dissolved in molten at 500–700 °C, a yellow diamagnetic solution is formed consisting of the , which has zinc in the oxidation state +1. The nature of this dizinc dication has been confirmed by Raman spectroscopy. Zinc hydroxychloride Concentrated aqueous zinc chloride dissolves zinc oxide to form zinc hydroxychloride, which is obtained as colorless crystals: : The same material forms when hydrated zinc chloride is heated. The ability of zinc chloride to dissolve metal oxides (MO) is relevant to the utility of as a flux for soldering. It dissolves passivating oxides, exposing the clean metal surface. : Related Lewis-acid behavior is illustrated by a traditional preparation of the dye fluorescein from phthalic anhydride and resorcinol. The key reaction is a Friedel-Crafts acylation: : This transformation has in fact been accomplished using even the hydrated sample shown in the picture above. Many examples describe the use of zinc chloride in Friedel-Crafts acylation reactions. Zinc chloride also activates benzylic and allylic halides towards substitution by weak nucleophiles such as alkenes: : In similar fashion, promotes selective sodium cyanoborohydride| reduction of tertiary, allylic or benzylic halides to the corresponding hydrocarbons. They reported the formation of a mixture aromatic and non-aromatic hydrocarbons when methanol is added to molten zinc chloride. An idealised equation for the formation of hexamethylbenzene by this process is : This kind of reactivity has been investigated for the valorization of C1 precursors. Zinc enolates, prepared from alkali metal enolates and , provide control of stereochemistry in aldol condensation reactions. This control is attributed to chelation at the zinc centre. In the example shown below, the threo product was favored over the erythro by a factor of 5:1 in the presence of . : Organozinc precursor Being inexpensive and anhydrous, ZnCl2 is a widely used for the synthesis of many organozinc reagents, such as those used in the palladium catalyzed Negishi coupling with aryl halides or vinyl halides. The prominence of this reaction was highlighted by the award of the 2010 Nobel Prize in Chemistry to Ei-ichi Negishi. : Rieke zinc, a highly reactive form of zinc metal, is generated by reduction of zinc dichloride with lithium. Rieke Zn is useful for the preparation of polythiophenes and for the Reformatsky reaction. ==Industrial applications==

Industrial organic chemistry Zinc chloride is used as a catalyst or reagent in diverse reactions conducted on an industrial scale. Benzaldehyde, 20,000 tons of which is produced annually in Western countries, is produced from inexpensive toluene by exploiting the catalytic properties of zinc dichloride. This process begins with the chlorination of toluene to give benzal chloride. In the presence of a small amount of anhydrous zinc chloride, a mixture of benzal chloride are treated continuously with water according to the following stoichiometry: : Similarly zinc chloride is employed in hydrolysis of benzotrichloride, the main route to benzoyl chloride. It serves as a catalyst for the production of methylene-bis(dithiocarbamate). As a metallurgical flux The use of zinc chloride as a flux, sometimes in a mixture with ammonium chloride (see also Zinc ammonium chloride), involves the production of HCl and its subsequent reaction with surface oxides. Zinc chloride forms two salts with ammonium chloride: and , which decompose on heating liberating HCl, just as zinc chloride hydrate does. The action of zinc chloride/ammonium chloride fluxes, for example, in the hot-dip galvanizing process produces gas and ammonia fumes. Other uses Relevant to its affinity for these paper and textiles, is used as a fireproofing agent and in the process of making Vulcanized fibre, which is made by soaking paper in concentrated zinc chloride. Zinc chloride is also used as a deodorizing agent and to make zinc soaps. ==Safety and health==

Zinc and chloride are essential for life. Zn2+ is a component of several enzymes, e.g., carboxypeptidase and carbonic anhydrase. Thus, aqueous solutions of zinc chlorides are rarely problematic as an acute poison. Another source of zinc chloride is zinc chloride smoke mixture ("HC") used in smoke grenades. Containing zinc oxide, hexachloroethane and aluminium powder release zinc chloride, carbon and aluminium oxide smoke, an effective smoke screen. Such smoke screens can lead to fatalities. ==References==