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Zinc chloride

October 15, 2023

For the battery type, see Zinc–chloride battery.

Zinc chloride is the name of inorganic chemical compounds with the formula ZnCl2. It forms 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 forms of anhydrous zinc chloride.[5] This salt is hygroscopic and even deliquescent. Zinc chloride finds wide application in textile processing, metallurgical fluxes, and chemical synthesis. No mineral with this chemical composition is known aside from the very rare mineral simonkolleite, Zn5(OH)8Cl2·H2O.

Zinc chloride
Names
IUPAC name
Zinc chloride
Other names
  • Butter of zinc
  • Neutral zinc chloride (1:2)
  • Zinc bichloride (archaic)
  • Zinc(II) chloride
Identifiers
  • 7646-85-7 Anhydrous Y
  • 29426-92-4 Tetrahydrate N
  • 21351-91-7 Mixed hydrate N
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:49976 Y
ChEMBL
  • ChEMBL1200679 Y
ChemSpider
  • 5525 Y
DrugBank
  • DB14533
ECHA InfoCard 100.028.720
EC Number
  • 231-592-0
  • 3007855
RTECS number
  • ZH1400000
UNII
  • 86Q357L16B Y
UN number 2331
  • DTXSID2035013
  • InChI=1S/2ClH.Zn/h2*1H;/q;;+2/p-2 Y
    Key: JIAARYAFYJHUJI-UHFFFAOYSA-L Y
  • InChI=1/2ClH.Zn/h2*1H;/q;;+2/p-2
    Key: JIAARYAFYJHUJI-NUQVWONBAB
  • Cl[Zn]Cl
Properties
ZnCl2
Molar mass 136.315 g/mol
Appearance White hygroscopic and very deliquescent crystalline solid
Odor odorless
Density 2.907 g/cm3
Melting point 290 °C (554 °F; 563 K)[1]
Boiling point 732 °C (1,350 °F; 1,005 K)[1]
432.0 g/(100 g) (25 °C)
Solubility soluble in ethanol, glycerol and acetone
Solubility in ethanol 430.0 g/(100 ml)
−65.0·10−6 cm3/mol
Structure
Tetrahedral, linear in the gas phase
Pharmacology
B05XA12 (WHO)
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Moderately toxic, irritant[2]
GHS labelling:
Danger
H302, H314, H410
P273, P280, P301+P330+P331, P305+P351+P338, P308+P310
NFPA 704 (fire diamond)
Health 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Lethal dose or concentration (LD, LC):
  • 350 mg/kg (rat, oral)
  • 350 mg/kg (mouse, oral)
  • 200 mg/kg (guinea pig, oral)
  • 1100 mg/kg (rat, oral)
  • 1250 mg/kg (mouse, oral)
[4]
1260 mg/m3 (rat, 30 min)
1180 mg-min/m3[4]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 1 mg/m3 (fume)[3]
REL (Recommended)
 TWA 1 mg/m3 ST 2 mg/m3 (fume)[3]
IDLH (Immediate danger)
 50 mg/m3 (fume)[3]
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)

Structure and properties Edit

Four crystalline forms (polymorphs) of ZnCl2 are known: α, β, γ, and δ. Each case features tetrahedral Zn2+ centers.[6]

Form Crystal system Pearson symbol Space group No. a (nm) 　b (nm) c (nm) Z Density (g/cm3)
α tetragonal tI12 I42d 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.[7][8][9]

The orthorhombic form (δ) rapidly changes to one of the other forms on exposure to the atmosphere. A possible explanation is that the OH− ions originating from the absorbed water facilitate the rearrangement.[6] Rapid cooling of molten ZnCl2 gives a glass.[10]

Molten ZnCl2 has a high viscosity at its melting point and a comparatively low electrical conductivity, which increases markedly with temperature.[11][12] As indicated by a Raman scattering study, the viscosity is explained by the presence of polymers,[13]. Neutron scattering study indicated the presence of tetrahedral ZnCl4 centers, which requires aggregation of ZnCl2 monomers as well..[14]

In the gas phase, ZnCl2 molecules are linear with a bond length of 205 pm.

Hydrates Edit

Five hydrates of zinc chloride are known: ZnCl2(H2O)n with n = 1, 1.5, 2.5, 3 and 4.[15] The tetrahydrate ZnCl2(H2O)4 crystallizes from aqueous solutions of zinc chloride.[15]

Preparation and purification Edit

Anhydrous ZnCl2 can be prepared from zinc and hydrogen chloride:

Zn + 2 HCl → ZnCl2 + H2

Hydrated forms and aqueous solutions may be readily prepared similarly by treating Zn metal, zinc carbonate, zinc oxide, and zinc sulfide with hydrochloric acid:

ZnS + 2 HCl + 4 H2O → ZnCl2(H2O)4 + H2S

Unlike many other elements, zinc essentially exists in only one oxidation state, 2+, which simplifies the purification of the chloride.

Commercial samples of zinc chloride typically contain water and products from hydrolysis as impurities. Such 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.[16] Finally, the simplest method relies on treating the zinc chloride with thionyl chloride.[17]

Reactions Edit

The Zn2+2 ion Edit

Molten anhydrous ZnCl2 at 500–700 °C dissolves zinc metal, and, on rapid cooling of the melt, a yellow diamagnetic glass is formed, which Raman studies indicate contains the Zn2+2 ion.[15]

Salts of [ZnCl4]2− and [Zn2Cl6]2− ions Edit

A number of salts containing the tetrachlorozincate anion, [ZnCl4]2−, are known.[11] "Caulton's reagent", V2Cl3(thf)6] [Zn2Cl6] is an example of a salt containing [Zn2Cl6]2−.[18][19] The compound Cs3ZnCl5 contains tetrahedral [ZnCl4]2− and Cl− anions,[6] so, the compound is not caesium pentachlorozincate, but caesium tetrachlorozincate chloride. No compounds containing the [ZnCl6]4− ion (hexachlorozincate ion) have been characterized.[6]

Aqueous solutions of zinc chloride Edit

Zinc chloride dissolves readily in water to give ZnClxH2O4−x species and some free chloride.[20][21][22] Aqueous solutions of ZnCl2 are acidic: a 6 M aqueous solution has a pH of 1.[15] The acidity of aqueous ZnCl2 solutions relative to solutions of other Zn2+ salts (say the sulfate) is due to the formation of the tetrahedral chloro aqua complexes where the reduction in coordination number from 6 to 4 further reduces the strength of the O–H bonds in the solvated water molecules.[23]

Alkaline solutions of zinc chloride Edit

In alkali solution, zinc chloride converts to various zinc hydroxychlorides. These include [Zn(OH)3Cl]2−, [Zn(OH)2Cl2]2−, [Zn(OH)Cl3]2−, and the insoluble Zn5(OH)8Cl2·H2O. The latter is the mineral simonkolleite.[24] When zinc chloride hydrates are heated, HCl gas evolves and hydroxychlorides result.[25]

Solutions of zinc chloride in ammonia Edit

When solutions of zinc chloride are treated with ammonia, various ammine complexes are produced. These include Zn(NH3)4Cl2·H2O and on concentration ZnCl2(NH3)2.[26] The former contains the [Zn(NH3)6]2+ ion,[6] and the latter is molecular with a distorted tetrahedral geometry.[27] The species in aqueous solution have been investigated and show that [Zn(NH3)4]2+ is the main species present with [Zn(NH3)3Cl]+ also present at lower NH3:Zn ratio.[28]

Zinc oxychloride cement Edit

Aqueous zinc chloride reacts with zinc oxide to form an amorphous cement that was first investigated in 1855 by Stanislas Sorel. Sorel later went on to investigate the related magnesium oxychloride cement, which bears his name.[29]

Zinc hydroxyde chloride Edit

When hydrated zinc chloride is heated, one obtains a residue of Zn(OH)Cl e.g.[30]

ZnCl2·2H2O → Zn(OH)Cl + HCl + H2O

Acidified zinc chloride Edit

The compound ZnCl2·0.5HCl·H2O may be prepared by careful precipitation from a solution of ZnCl2 acidified with HCl. It contains a polymeric anion (Zn2Cl−5)n with balancing monohydrated hydronium ions, H5O+2 ions.[6][31]

Cellulose dissolution in aqueous solutions of ZnCl2 Edit

Cellulose dissolves in aqueous solutions of ZnCl2, and zinc-cellulose complexes have been detected.[32] Cellulose also dissolves in molten ZnCl2 hydrate and carboxylation and acetylation performed on the cellulose polymer.[33]

Using zinc chloride for preparing other zinc salts Edit

Thus, although many zinc salts have different formulas and different crystal structures, these salts behave very similarly in aqueous solution. For example, solutions prepared from any of the polymorphs of ZnCl2, as well as other halides (bromide, iodide), and the sulfate can often be used interchangeably for the preparation of other zinc compounds. Illustrative is the preparation of zinc carbonate:

ZnCl2(aq) + Na2CO3(aq) → ZnCO3(s) + 2 NaCl(aq)

Role in organic chemistry Edit

Zinc chloride is used as a catalyst or reagent in diverse reactions conducted on an industrial scale. The partial hydrolysis of benzal chloride in the presence of zinc chloride is the main route to benzoyl chloride. It serves as a catalyst for the production of methylene-bis(dithiocarbamate).[5]

The combination of hydrochloric acid and ZnCl2, known as the "Lucas reagent", is effective for the preparation of alkyl chlorides from alcohols. Similar reactions are the basis of industrial routes from methanol and ethanol respectively to methyl chloride and ethyl chloride.

Laboratory syntheses Edit

Zinc chloride is a common reagent in the laboratory useful Lewis acid in organic chemistry.[34]

Molten zinc chloride catalyses the conversion of methanol to hexamethylbenzene:[35]

15 CH3OH → C6(CH3)6 + 3 CH4 + 15 H2O

Other examples include catalyzing (A) the Fischer indole synthesis,[36] and also (B) Friedel-Crafts acylation reactions involving activated aromatic rings[37][38]

  •  

Related to the latter is the classical preparation of the dye fluorescein from phthalic anhydride and resorcinol, which involves a Friedel-Crafts acylation.[39] This transformation has in fact been accomplished using even the hydrated ZnCl2 sample shown in the picture above.

  •  

Zinc chloride also activates benzylic and allylic halides towards substitution by weak nucleophiles such as alkenes:[40]

  •  

In similar fashion, ZnCl2 promotes selective Na[BH3(CN)] reduction of tertiary, allylic or benzylic halides to the corresponding hydrocarbons.

Zinc chloride is also a useful starting reagent for the synthesis of many organozinc reagents, such as those used in the palladium catalyzed Negishi coupling with aryl halides or vinyl halides.[41] In such cases the organozinc compound is usually prepared by transmetallation from an organolithium or a Grignard reagent, for example:

  •  

Zinc enolates, prepared from alkali metal enolates and ZnCl2, provide control of stereochemistry in aldol condensation reactions due to chelation on to the zinc. In the example shown below, the threo product was favored over the erythro by a factor of 5:1 when ZnCl2 in DME/ether was used.[42] The chelate is more stable when the bulky phenyl group is pseudo-equatorial rather than pseudo-axial, i.e., threo rather than erythro.

  •  

Other uses Edit

As a metallurgical flux Edit

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 reacts with metal oxides (MO) to give derivatives of the idealized formula MZnOCl2.[43][additional citation(s) needed] This reaction is relevant to the utility of ZnCl2 solution as a flux for soldering — it dissolves passivating oxides, exposing the clean metal surface.[43] Fluxes with ZnCl2 as an active ingredient are sometimes called "tinner's fluid".

Zinc chloride forms two salts with ammonium chloride: [NH4]2[ZnCl4] and [NH4]3[ZnCl4]Cl, 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 H2 gas and ammonia fumes.[44]

In textile and paper processing Edit

Concentrated aqueous solutions of zinc chloride (more than 64% weight/weight zinc chloride in water) have dissolving starch, silk, and cellulose.

Relevant to its affinity for these materials, ZnCl2 is used as a fireproofing agent and in fabric "refresheners" such as Febreze. Vulcanized fibre is made by soaking paper in concentrated zinc chloride.

Smoke grenades Edit

The zinc chloride smoke mixture ("HC") used in smoke grenades contains zinc oxide, hexachloroethane and granular aluminium powder, which, when ignited, react to form zinc chloride, carbon and aluminium oxide smoke, an effective smoke screen.[45]

Fingerprint detection Edit

Ninhydrin reacts with amino acids and amines to form a colored compound "Ruhemann's purple" (RP). Spraying with a zinc chloride solution forms a 1:1 complex RP:ZnCl(H2O)2, which is more readily detected as it fluoresces more intensely than RP.[46]

Disinfectant and wood preservative Edit

Dilute aqueous zinc chloride was used as a disinfectant under the name "Burnett's Disinfecting Fluid". [47] From 1839 Sir William Burnett promoted its use as a disinfectant as well as a wood preservative.[48] 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.

Safety Edit

Zinc chloride is a chemical irritant of the eyes, skin, and respiratory system.[5][49]

References Edit

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Further reading Edit

  • N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.
  • Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
  • The Merck Index, 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960.
  • D. Nicholls, Complexes and First-Row Transition Elements, Macmillan Press, London, 1973.
  • J. March, Advanced Organic Chemistry, 4th ed., p. 723, Wiley, New York, 1992.
  • G. J. McGarvey, in Handbook of Reagents for Organic Synthesis, Volume 1: Reagents, Auxiliaries and Catalysts for C-C Bond Formation, (R. M. Coates, S. E. Denmark, eds.), pp. 220–3, Wiley, New York, 1999.

External links Edit

  • Grades and Applications of Zinc Chloride
  • PubChem ZnCl2 summary.

October 15, 2023
zinc, chloride, battery, type, zinc, chloride, battery, name, inorganic, chemical, compounds, with, formula, zncl2, forms, hydrates, anhydrous, hydrates, colorless, white, crystalline, solids, highly, soluble, water, five, hydrates, zinc, chloride, known, well. For the battery type see Zinc chloride battery Zinc chloride is the name of inorganic chemical compounds with the formula ZnCl2 It forms 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 forms of anhydrous zinc chloride 5 This salt is hygroscopic and even deliquescent Zinc chloride finds wide application in textile processing metallurgical fluxes and chemical synthesis No mineral with this chemical composition is known aside from the very rare mineral simonkolleite Zn5 OH 8Cl2 H2O Zinc chloride NamesIUPAC name Zinc chlorideOther names Butter of zincNeutral zinc chloride 1 2 Zinc bichloride archaic Zinc II chlorideIdentifiersCAS Number 7646 85 7 Anhydrous Y29426 92 4 Tetrahydrate N21351 91 7 Mixed hydrate N3D model JSmol Interactive imageChEBI CHEBI 49976 YChEMBL ChEMBL1200679 YChemSpider 5525 YDrugBank DB14533ECHA InfoCard 100 028 720EC Number 231 592 0PubChem CID 3007855RTECS number ZH1400000UNII 86Q357L16B YUN number 2331CompTox Dashboard EPA DTXSID2035013InChI InChI 1S 2ClH Zn h2 1H q 2 p 2 YKey JIAARYAFYJHUJI UHFFFAOYSA L YInChI 1 2ClH Zn h2 1H q 2 p 2Key JIAARYAFYJHUJI NUQVWONBABSMILES Cl Zn ClPropertiesChemical formula ZnCl2Molar mass 136 315 g molAppearance White hygroscopic and very deliquescent crystalline solidOdor odorlessDensity 2 907 g cm3Melting point 290 C 554 F 563 K 1 Boiling point 732 C 1 350 F 1 005 K 1 Solubility in water 432 0 g 100 g 25 C Solubility soluble in ethanol glycerol and acetoneSolubility in ethanol 430 0 g 100 ml Magnetic susceptibility x 65 0 10 6 cm3 molStructureCoordination geometry Tetrahedral linear in the gas phasePharmacologyATC code B05XA12 WHO HazardsOccupational safety and health OHS OSH Main hazards Moderately toxic irritant 2 GHS labelling PictogramsSignal word DangerHazard statements H302 H314 H410Precautionary statements P273 P280 P301 P330 P331 P305 P351 P338 P308 P310NFPA 704 fire diamond 300Lethal dose or concentration LD LC LD50 median dose 350 mg kg rat oral 350 mg kg mouse oral 200 mg kg guinea pig oral 1100 mg kg rat oral 1250 mg kg mouse oral 4 LC50 median concentration 1260 mg m3 rat 30 min 1180 mg min m3 4 NIOSH US health exposure limits PEL Permissible TWA 1 mg m3 fume 3 REL Recommended TWA 1 mg m3 ST 2 mg m3 fume 3 IDLH Immediate danger 50 mg m3 fume 3 Safety data sheet SDS External MSDSRelated compoundsOther anions Zinc fluorideZinc bromideZinc iodideOther cations Cadmium chlorideMercury II chlorideExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa N verify what is Y N Infobox references Contents 1 Structure and properties 1 1 Hydrates 2 Preparation and purification 3 Reactions 3 1 The Zn2 2 ion 3 2 Salts of ZnCl4 2 and Zn2Cl6 2 ions 3 3 Aqueous solutions of zinc chloride 3 4 Alkaline solutions of zinc chloride 3 5 Solutions of zinc chloride in ammonia 3 6 Zinc oxychloride cement 3 7 Zinc hydroxyde chloride 3 8 Acidified zinc chloride 3 9 Cellulose dissolution in aqueous solutions of ZnCl2 3 10 Using zinc chloride for preparing other zinc salts 4 Role in organic chemistry 4 1 Laboratory syntheses 5 Other uses 5 1 As a metallurgical flux 5 2 In textile and paper processing 5 3 Smoke grenades 5 4 Fingerprint detection 5 5 Disinfectant and wood preservative 6 Safety 7 References 8 Further reading 9 External linksStructure and properties EditFour crystalline forms polymorphs of ZnCl2 are known a b g and d Each case features tetrahedral Zn2 centers 6 Form Crystal system Pearson symbol Space group No a nm b nm c nm Z Density g cm3 a tetragonal tI12 I4 2d 122 0 5398 0 5398 0 64223 4 3 00b tetragonal tP6 P42 nmc 137 0 3696 0 3696 1 071 2 3 09g monoclinic mP36 P21 c 14 0 654 1 131 1 23328 12 2 98d orthorhombic oP12 Pna21 33 0 6125 0 6443 0 7693 4 2 98Here a b and c are lattice constants Z is the number of structure units per unit cell and r is the density calculated from the structure parameters 7 8 9 The orthorhombic form d rapidly changes to one of the other forms on exposure to the atmosphere A possible explanation is that the OH ions originating from the absorbed water facilitate the rearrangement 6 Rapid cooling of molten ZnCl2 gives a glass 10 Molten ZnCl2 has a high viscosity at its melting point and a comparatively low electrical conductivity which increases markedly with temperature 11 12 As indicated by a Raman scattering study the viscosity is explained by the presence of polymers 13 Neutron scattering study indicated the presence of tetrahedral ZnCl4 centers which requires aggregation of ZnCl2 monomers as well 14 In the gas phase ZnCl2 molecules are linear with a bond length of 205 pm Hydrates Edit Five hydrates of zinc chloride are known ZnCl2 H2O n with n 1 1 5 2 5 3 and 4 15 The tetrahydrate ZnCl2 H2O 4 crystallizes from aqueous solutions of zinc chloride 15 Preparation and purification EditAnhydrous ZnCl2 can be prepared from zinc and hydrogen chloride Zn 2 HCl ZnCl2 H2Hydrated forms and aqueous solutions may be readily prepared similarly by treating Zn metal zinc carbonate zinc oxide and zinc sulfide with hydrochloric acid ZnS 2 HCl 4 H2O ZnCl2 H2O 4 H2SUnlike many other elements zinc essentially exists in only one oxidation state 2 which simplifies the purification of the chloride Commercial samples of zinc chloride typically contain water and products from hydrolysis as impurities Such 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 16 Finally the simplest method relies on treating the zinc chloride with thionyl chloride 17 Reactions EditThe Zn2 2 ion Edit Molten anhydrous ZnCl2 at 500 700 C dissolves zinc metal and on rapid cooling of the melt a yellow diamagnetic glass is formed which Raman studies indicate contains the Zn2 2 ion 15 Salts of ZnCl4 2 and Zn2Cl6 2 ions Edit A number of salts containing the tetrachlorozincate anion ZnCl4 2 are known 11 Caulton s reagent V2Cl3 thf 6 Zn2Cl6 is an example of a salt containing Zn2Cl6 2 18 19 The compound Cs3ZnCl5 contains tetrahedral ZnCl4 2 and Cl anions 6 so the compound is not caesium pentachlorozincate but caesium tetrachlorozincate chloride No compounds containing the ZnCl6 4 ion hexachlorozincate ion have been characterized 6 Aqueous solutions of zinc chloride Edit Zinc chloride dissolves readily in water to give ZnClxH2O4 x species and some free chloride 20 21 22 Aqueous solutions of ZnCl2 are acidic a 6 M aqueous solution has a pH of 1 15 The acidity of aqueous ZnCl2 solutions relative to solutions of other Zn2 salts say the sulfate is due to the formation of the tetrahedral chloro aqua complexes where the reduction in coordination number from 6 to 4 further reduces the strength of the O H bonds in the solvated water molecules 23 Alkaline solutions of zinc chloride Edit In alkali solution zinc chloride converts to various zinc hydroxychlorides These include Zn OH 3Cl 2 Zn OH 2Cl2 2 Zn OH Cl3 2 and the insoluble Zn5 OH 8Cl2 H2O The latter is the mineral simonkolleite 24 When zinc chloride hydrates are heated HCl gas evolves and hydroxychlorides result 25 Solutions of zinc chloride in ammonia Edit When solutions of zinc chloride are treated with ammonia various ammine complexes are produced These include Zn NH3 4Cl2 H2O and on concentration ZnCl2 NH3 2 26 The former contains the Zn NH3 6 2 ion 6 and the latter is molecular with a distorted tetrahedral geometry 27 The species in aqueous solution have been investigated and show that Zn NH3 4 2 is the main species present with Zn NH3 3Cl also present at lower NH3 Zn ratio 28 Zinc oxychloride cement Edit Aqueous zinc chloride reacts with zinc oxide to form an amorphous cement that was first investigated in 1855 by Stanislas Sorel Sorel later went on to investigate the related magnesium oxychloride cement which bears his name 29 Zinc hydroxyde chloride Edit When hydrated zinc chloride is heated one obtains a residue of Zn OH Cl e g 30 ZnCl2 2H2O Zn OH Cl HCl H2OAcidified zinc chloride Edit The compound ZnCl2 0 5HCl H2O may be prepared by careful precipitation from a solution of ZnCl2 acidified with HCl It contains a polymeric anion Zn2Cl 5 n with balancing monohydrated hydronium ions H5O 2 ions 6 31 Cellulose dissolution in aqueous solutions of ZnCl2 Edit Cellulose dissolves in aqueous solutions of ZnCl2 and zinc cellulose complexes have been detected 32 Cellulose also dissolves in molten ZnCl2 hydrate and carboxylation and acetylation performed on the cellulose polymer 33 Using zinc chloride for preparing other zinc salts Edit Thus although many zinc salts have different formulas and different crystal structures these salts behave very similarly in aqueous solution For example solutions prepared from any of the polymorphs of ZnCl2 as well as other halides bromide iodide and the sulfate can often be used interchangeably for the preparation of other zinc compounds Illustrative is the preparation of zinc carbonate ZnCl2 aq Na2CO3 aq ZnCO3 s 2 NaCl aq Role in organic chemistry EditZinc chloride is used as a catalyst or reagent in diverse reactions conducted on an industrial scale The partial hydrolysis of benzal chloride in the presence of zinc chloride is the main route to benzoyl chloride It serves as a catalyst for the production of methylene bis dithiocarbamate 5 The combination of hydrochloric acid and ZnCl2 known as the Lucas reagent is effective for the preparation of alkyl chlorides from alcohols Similar reactions are the basis of industrial routes from methanol and ethanol respectively to methyl chloride and ethyl chloride Laboratory syntheses Edit Zinc chloride is a common reagent in the laboratory useful Lewis acid in organic chemistry 34 Molten zinc chloride catalyses the conversion of methanol to hexamethylbenzene 35 15 CH3OH C6 CH3 6 3 CH4 15 H2OOther examples include catalyzing A the Fischer indole synthesis 36 and also B Friedel Crafts acylation reactions involving activated aromatic rings 37 38 nbsp Related to the latter is the classical preparation of the dye fluorescein from phthalic anhydride and resorcinol which involves a Friedel Crafts acylation 39 This transformation has in fact been accomplished using even the hydrated ZnCl2 sample shown in the picture above nbsp Zinc chloride also activates benzylic and allylic halides towards substitution by weak nucleophiles such as alkenes 40 nbsp In similar fashion ZnCl2 promotes selective Na BH3 CN reduction of tertiary allylic or benzylic halides to the corresponding hydrocarbons Zinc chloride is also a useful starting reagent for the synthesis of many organozinc reagents such as those used in the palladium catalyzed Negishi coupling with aryl halides or vinyl halides 41 In such cases the organozinc compound is usually prepared by transmetallation from an organolithium or a Grignard reagent for example nbsp Zinc enolates prepared from alkali metal enolates and ZnCl2 provide control of stereochemistry in aldol condensation reactions due to chelation on to the zinc In the example shown below the threo product was favored over the erythro by a factor of 5 1 when ZnCl2 in DME ether was used 42 The chelate is more stable when the bulky phenyl group is pseudo equatorial rather than pseudo axial i e threo rather than erythro nbsp Other uses EditAs a metallurgical flux Edit 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 reacts with metal oxides MO to give derivatives of the idealized formula MZnOCl2 43 additional citation s needed This reaction is relevant to the utility of ZnCl2 solution as a flux for soldering it dissolves passivating oxides exposing the clean metal surface 43 Fluxes with ZnCl2 as an active ingredient are sometimes called tinner s fluid Zinc chloride forms two salts with ammonium chloride NH4 2 ZnCl4 and NH4 3 ZnCl4 Cl 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 H2 gas and ammonia fumes 44 In textile and paper processing Edit Concentrated aqueous solutions of zinc chloride more than 64 weight weight zinc chloride in water have dissolving starch silk and cellulose Relevant to its affinity for these materials ZnCl2 is used as a fireproofing agent and in fabric refresheners such as Febreze Vulcanized fibre is made by soaking paper in concentrated zinc chloride Smoke grenades Edit The zinc chloride smoke mixture HC used in smoke grenades contains zinc oxide hexachloroethane and granular aluminium powder which when ignited react to form zinc chloride carbon and aluminium oxide smoke an effective smoke screen 45 Fingerprint detection Edit Ninhydrin reacts with amino acids and amines to form a colored compound Ruhemann s purple RP Spraying with a zinc chloride solution forms a 1 1 complex RP ZnCl H2O 2 which is more readily detected as it fluoresces more intensely than RP 46 Disinfectant and wood preservative Edit Dilute aqueous zinc chloride was used as a disinfectant under the name Burnett s Disinfecting Fluid 47 From 1839 Sir William Burnett promoted its use as a disinfectant as well as a wood preservative 48 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 Safety EditZinc chloride is a chemical irritant of the eyes skin and respiratory system 5 49 References Edit a b O Neil M J et al 2001 The Merck index an encyclopedia of chemicals drugs and biologicals N J Whitehouse Station ISBN 978 0911910131 Zinc chloride toxicity a b c NIOSH Pocket Guide to Chemical Hazards 0674 National Institute for Occupational Safety and Health NIOSH a b Zinc chloride fume Immediately Dangerous to Life or Health Concentrations IDLH National Institute for Occupational Safety and Health NIOSH a b c Dieter M M Rohe Hans Uwe Wolf 2007 Zinc Compounds Ullmann s Encyclopedia of Industrial Chemistry Weinheim Wiley VCH pp 1 6 doi 10 1002 14356007 a28 537 a b c d e f Wells A F 1984 Structural Inorganic Chemistry Oxford Clarendon Press ISBN 978 0 19 855370 0 Oswald H R Jaggi H 1960 Zur Struktur der wasserfreien Zinkhalogenide I Die wasserfreien Zinkchloride Helvetica Chimica Acta 43 1 72 77 doi 10 1002 hlca 19600430109 Brynestad J Yakel H L 1978 Preparation and Structure of Anhydrous Zinc Chloride Inorganic Chemistry 17 5 1376 1377 doi 10 1021 ic50183a059 Brehler B 1961 Kristallstrukturuntersuchungen an ZnCl2 Zeitschrift fur Kristallographie 115 5 6 373 402 Bibcode 1961ZK 115 373B doi 10 1524 zkri 1961 115 5 6 373 Mackenzie J D Murphy W K 1960 Structure of Glass Forming Halides II Liquid Zinc Chloride The Journal of Chemical Physics 33 2 366 369 Bibcode 1960JChPh 33 366M doi 10 1063 1 1731151 a b Prince R H 1994 King R B ed Encyclopedia of Inorganic Chemistry John Wiley amp Sons ISBN 978 0 471 93620 6 Ray H S 2006 Introduction to Melts Molten Salts Slags and Glasses Allied Publishers ISBN 978 81 7764 875 1 Danek V 2006 Physico Chemical Analysis of Molten Electrolytes Elsevier ISBN 978 0 444 52116 3 Price D L Saboungi M L Susman S Volin K J Wright A C 1991 Neutron Scattering Function of Vitreous and Molten Zinc Chloride Journal of Physics Condensed Matter 3 49 9835 9842 Bibcode 1991JPCM 3 9835P doi 10 1088 0953 8984 3 49 001 S2CID 250902741 a b c d Holleman A F Wiberg E 2001 Inorganic Chemistry San Diego Academic Press ISBN 978 0 12 352651 9 Glenn J McGarvey Jean Francois Poisson Sylvain Taillemaud 2016 Zinc chloride Encyclopedia of Reagents for Organic Synthesis 1 20 doi 10 1002 047084289X rz007 pub3 ISBN 9780470842898 Pray A P 1990 Anhydrous Metal Chlorides Inorganic Syntheses Vol 28 pp 321 322 Mulzer J Waldmann H eds 1998 Organic Synthesis Highlights Vol 3 Wiley VCH ISBN 978 3 527 29500 5 Bouma R J Teuben J H Beukema W R Bansemer R L Huffman J C Caulton K G 1984 Identification of the Zinc Reduction Product of VCl3 3THF as V2Cl3 THF 6 2 Zn2Cl6 Inorganic Chemistry 23 17 2715 2718 doi 10 1021 ic00185a033 Irish D E McCarroll B Young T F 1963 Raman Study of Zinc Chloride Solutions The Journal of Chemical Physics 39 12 3436 3444 Bibcode 1963JChPh 39 3436I doi 10 1063 1 1734212 Yamaguchi T Hayashi S Ohtaki H 1989 X Ray Diffraction and Raman Studies of Zinc II Chloride Hydrate Melts ZnCl2 R H2O R 1 8 2 5 3 0 4 0 and 6 2 The Journal of Physical Chemistry 93 6 2620 2625 doi 10 1021 j100343a074 Pye C C Corbeil C R Rudolph W W 2006 An ab initio Investigation of Zinc Chloro Complexes Physical Chemistry Chemical Physics 8 46 5428 5436 Bibcode 2006PCCP 8 5428P doi 10 1039 b610084h ISSN 1463 9076 PMID 17119651 S2CID 37521287 Brown I D 2006 The Chemical Bond in Inorganic Chemistry The Bond Valence Model Oxford University Press ISBN 978 0 19 929881 5 Zhang X G 1996 Corrosion and Electrochemistry of Zinc Springer ISBN 978 0 306 45334 2 Staff writer s Simonkolleite Mineral Data webmineral com Retrieved October 16 2014 Feigl F Caldas A 1956 Some Applications of Fusion Reactions with Zinc Chloride in Inorganic Spot Test Analysis Microchimica Acta 44 7 8 1310 1316 doi 10 1007 BF01257465 S2CID 96823985 Vulte H T 2007 Laboratory Manual of Inorganic Preparations Read Books ISBN 978 1 4086 0840 1 Yamaguchi T Lindqvist O 1981 The Crystal Structure of Diamminedichlorozinc II ZnCl2 NH3 2 A New Refinement PDF Acta Chemica Scandinavica A 35 9 727 728 doi 10 3891 acta chem scand 35a 0727 Yamaguchi T Ohtaki H 1978 X Ray Diffraction Studies on the Structures of Tetraammine and Triamminemonochlorozinc II Ions in Aqueous Solution Bulletin of the Chemical Society of Japan 51 11 3227 3231 doi 10 1246 bcsj 51 3227 Wilson A D Nicholson J W 1993 Acid Base Cements Their Biomedical and Industrial Applications Cambridge University Press ISBN 978 0 521 37222 0 House J E 2008 Inorganic Chemistry Academic Press ISBN 978 0 12 356786 4 Mellow J W 1946 A Comprehensive Treatise on Inorganic and Theoretical Chemistry Longmans Green Xu Q Chen L F 1999 Ultraviolet Spectra and Structure of Zinc Cellulose Complexes in Zinc Chloride Solution Journal of Applied Polymer Science 71 9 1441 1446 doi 10 1002 SICI 1097 4628 19990228 71 9 lt 1441 AID APP8 gt 3 0 CO 2 G Fischer S Leipner H Thummler K Brendler E Peters J 2003 Inorganic Molten Salts as Solvents for Cellulose Cellulose 10 3 227 236 doi 10 1023 A 1025128028462 S2CID 92194004 Olah George A Doggweiler Hans Felberg Jeff D Frohlich Stephan Grdina Mary Jo Karpeles Richard Keumi Takashi Inaba Shin ichi Ip Wai M Lammertsma Koop Salem George Tabor Derrick 1984 Onium Ylide chemistry 1 Bifunctional acid base catalyzed conversion of heterosubstituted methanes into ethylene and derived hydrocarbons The onium ylide mechanism of the C1 C2 conversion J Am Chem Soc 106 7 2143 2149 doi 10 1021 ja00319a039 Chang Clarence D 1983 Hydrocarbons from Methanol Catal Rev Sci Eng 25 1 1 118 doi 10 1080 01614948308078874 Shriner R L Ashley W C Welch E 1942 2 Phenylindole Organic Syntheses 22 98 doi 10 15227 orgsyn 022 00981955 Collective Volume vol 3 p 725 Cooper S R 1941 Resacetophenone Organic Syntheses 21 103 doi 10 15227 orgsyn 021 0103 Collective Volume vol 3 p 761 Dike S Y Merchant J R Sapre N Y 1991 A New and Efficient General Method for the Synthesis of 2 Spirobenzopyrans First Synthesis of Cyclic Analogues of Precocene I and Related Compounds Tetrahedron 47 26 4775 4786 doi 10 1016 S0040 4020 01 86481 4 Furnell B S 1989 Vogel s Textbook of Practical Organic Chemistry 5th ed New York Longman Wiley Bauml E Tschemschlok K Pock R Mayr H 1988 Synthesis of g Lactones from Alkenes Employing p Methoxybenzyl Chloride as CH2 CO2 Equivalent PDF Tetrahedron Letters 29 52 6925 6926 doi 10 1016 S0040 4039 00 88476 2 Kim S Kim Y J Ahn K H 1983 Selective Reduction of Tertiary Allyl and Benzyl Halides by Zinc Modified Cyanoborohydride in Diethyl Ether Tetrahedron Letters 24 32 3369 3372 doi 10 1016 S0040 4039 00 86272 3 House H O Crumrine D S Teranishi A Y Olmstead H D 1973 Chemistry of Carbanions XXIII Use of Metal Complexes to Control the Aldol Condensation Journal of the American Chemical Society 95 10 3310 3324 doi 10 1021 ja00791a039 a b Wiberg Nils 2007 Lehrbuch der Anorganischen Chemie Holleman amp Wiberg Textbook of Inorganic chemistry in German de Gruyter Berlin p 1491 ISBN 978 3 11 017770 1 American Society for Metals 1990 ASM handbook ASM International ISBN 978 0 87170 021 6 Sample B E 1997 Methods for Field Studies of Effects of Military Smokes Obscurants and Riot control Agents on Threatened and Endangered Species DIANE Publishing ISBN 978 1 4289 1233 5 Menzel E R 1999 Fingerprint Detection with Lasers CRC Press ISBN 978 0 8247 1974 6 Watts H 1869 A Dictionary of Chemistry and the Allied Branches of Other Sciences Longmans Green McLean David April 2010 Protecting wood and killing germs Burnett s Liquid and the origins of the preservative and disinfectant industries in early Victorian Britain Business History 52 2 285 305 doi 10 1080 00076791003610691 S2CID 154790730 NIOSH Pocket Guide to Chemical Hazards CDC gov Retrieved 30 October 2020 Further reading EditN N Greenwood A Earnshaw Chemistry of the Elements 2nd ed Butterworth Heinemann Oxford UK 1997 Lide D R ed 2005 CRC Handbook of Chemistry and Physics 86th ed Boca Raton FL CRC Press ISBN 0 8493 0486 5 The Merck Index 7th edition Merck amp Co Rahway New Jersey USA 1960 D Nicholls Complexes and First Row Transition Elements Macmillan Press London 1973 J March Advanced Organic Chemistry 4th ed p 723 Wiley New York 1992 G J McGarvey in Handbook of Reagents for Organic Synthesis Volume 1 Reagents Auxiliaries and Catalysts for C C Bond Formation R M Coates S E Denmark eds pp 220 3 Wiley New York 1999 External links EditGrades and Applications of Zinc Chloride PubChem ZnCl2 summary Retrieved from https en wikipedia org w index php title Zinc chloride amp oldid 1176946932, wikipedia, wiki, book, books, library,

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