Zinc chloride

Zinc chloride is an inorganic chemical compound with the formula ZnCl₂·nH₂O, with n ranging from 0 to 4.5, forming hydrates. Zinc chloride, anhydrous and its hydrates, are colorless or white crystalline solids, and are highly soluble in water. Five hydrates of zinc chloride are known, as well as four polymorphs of anhydrous zinc chloride.
All forms of zinc chloride are deliquescent. They can usually be produced by the reaction of zinc or its compounds with some form of hydrogen chloride. Anhydrous zinc compound is a Lewis acid, readily forming complexes with a variety of Lewis bases. Zinc chloride finds wide application in textile processing, metallurgical fluxes, chemical synthesis of organic compounds, such as benzaldehyde, and processes to produce other compounds of zinc.

History

Zinc chloride has long been known but currently practiced industrial applications all evolved in the latter half of 20th century.
An amorphous cement formed from aqueous zinc chloride and zinc oxide was first investigated in 1855 by Stanislas Sorel. Sorel later went on to investigate the related magnesium oxychloride cement, which bears his name.
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 Following his death however, its use was largely superseded by that of carbolic acid and other proprietary products.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. Four polymorph are known: α, β, γ, and δ. Each features centers surrounded in a tetrahedral manner by four chloride ligands.

Form	Crystal system	Pearson symbol	Space group	No.	a	b	c	Z	Density
α	tetragonal	tI12	I2d	122	0.5398	0.5398	0.64223	4	3.00
β	tetragonal	tP6	P4₂/nmc	137	0.3696	0.3696	1.071	2	3.09
γ	monoclinic	mP36	P2₁/c	14	0.654	1.131	1.23328	12	2.98
δ	orthorhombic	oP12	Pna2₁	33	0.6125	0.6443	0.7693	4	2.98

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 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. Rapid cooling of molten gives a glass.
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: with n = 1, 1.33, 2.5, 3, and 4.5. The 1.33-hydrate, previously thought to be the hemitrihydrate, consists of trans-Zn₄Cl₂ centers with the chloro ligands bridging to tetrachlorozincate groups, present in 1:2 ratio. The hemipentahydrate, structurally formulated , consists of Zn₅Cl octahedra with chloro bridges to tetrachlorozincate tetrahedera. Both the trihydrate and the heminonahydrate possess distinct hexaquozinc cations and tetrachlorozincate anions with the solid structure of the latter incorporating three additional waters of crystallisation. Each of these hydrates can be produced by controlled evaporation of aqueous zinc chloride solutions under different temperature conditions.

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:
Aqueous solutions may be readily prepared similarly by treating Zn metal, zinc carbonate, zinc oxide, and zinc sulfide with hydrochloric acid:
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.
Commercial samples of zinc chloride typically contain water and products from hydrolysis as impurities. Laboratory samples may be purified by recrystallization from hot dioxane. Anhydrous samples can be purified by sublimation in a stream of hydrogen chloride gas, followed by heating the sublimate to 400 °C in a stream of dry nitrogen gas. 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. "Caulton's reagent",, named for Kenneth G. Caulton, is an example of a salt containing that is used in organic chemistry. The compound contains tetrahedral and Chloride| anions, so, the compound is not caesium pentachlorozincate, but caesium tetrachlorozincate chloride. No compounds containing the ion have been characterized. The compound crystallizes from a solution of in hydrochloric acid. It contains a polymeric anion with balancing monohydrated hydronium ions, ions.

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 . 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,. The species in aqueous solution have been investigated and show that is the main species present with also present at lower :Zn ratio.

Aqueous solutions of zinc chloride

Zinc chloride dissolves readily in water to give species and some free chloride. Aqueous solutions of are acidic: a 6 M aqueous solution has a pH of 1. The acidity of aqueous solutions relative to solutions of other Zn²⁺ salts is due to the formation of the tetrahedral chloro aqua complexes such as ⁻. 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, behave interchangeably for the preparation of other zinc compounds. These salts give
precipitates of zinc carbonate when treated with aqueous carbonate sources:
Ninhydrin reacts with amino acids and amines to form a colored compound "Ruhemann's purple". Spraying with a zinc chloride solution, which is colorless, forms a 1:1 complex RP:, which is more readily detected as it fluoresces more intensely than RP.

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. Although is unusual, mercury, a heavy congener of zinc, forms a wide variety of salts.
In the presence of oxygen, zinc chloride oxidizes to zinc oxide above 400 °C. Again, this observation indicates the nonoxidation of Zn²⁺.

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 is relevant to the utility of as a flux for soldering. It dissolves passivating oxides, exposing the clean metal surface.

Catalyst in organic syntheses

Zinc chloride is an adequate Lewis acid for electrophilic aromatic substitutions, as in the Fischer indole synthesis:
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.
A dramatic example of zinc chloride promoting carbon-carbon bond formation was first reported in 1880 by Joseph Achille Le Bel and William H. Greene. 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.