View source for Aluminium chloride

{{short description|Chemical compound}}
{{good article}}
{{cs1 config|name-list-style=vanc|display-authors=6}}
{{Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 477245740
| Name =
| ImageFile1 = Aluminium-trichloride-hexahydrate-white-and-yellow.jpg
| ImageSize1 = 150px
| ImageCaption1 = Aluminium trichloride hexahydrate, pure (top), and contaminated with [[iron(III) chloride]] (bottom)
| ImageName1 = Aluminium(III) chloride
| ImageFileL2 = Aluminium-trichloride-dimer-3D-balls.png
| ImageSizeL2 = 125px
| ImageNameL2 = Aluminium trichloride dimer
| ImageFileR2 = Aluminium-chloride-xtal-unit-cell-3D-bs-17.png
| ImageSizeR2 = 125px
| ImageNameR2 = Aluminium trichloride unit cell
| IUPACName = Aluminium chloride
| OtherNames = Aluminium(III) chloride<br />Aluminium trichloride<br />Trichloroaluminum
|Section1={{Chembox Identifiers
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = LIF1N9568Y
| UNII1_Ref = {{fdacite|correct|FDA}}
| UNII1 = 3CYT62D3GA
| UNII1_Comment = (hexahydrate)
| InChI = 1/Al.3ClH/h;3*1H/q+3;;;/p-3
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 30114
| SMILES = Cl[Al](Cl)Cl
| SMILES_Comment = [[monomer]]
| SMILES1 = Cl[Al-]1(Cl)[Cl+][Al-]([Cl+]1)(Cl)Cl
| SMILES1_Comment = [[dimer (chemistry)|dimer]]
| SMILES2 = [OH2+][Al-3]([OH2+])([OH2+])([OH2+])([OH2+])[OH2+].[Cl-].[Cl-].[Cl-]
| SMILES2_Comment = hexahydrate
| InChIKey = VSCWAEJMTAWNJL-DFZHHIFOAR
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/Al.3ClH/h;3*1H/q+3;;;/p-3
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = VSCWAEJMTAWNJL-UHFFFAOYSA-K
| CASNo = 7446-70-0
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo_Comment = (anhydrous)
| CASNo1_Ref = {{cascite|changed|??}}
| CASNo1 = 10124-27-3
| CASNo1_Comment = (hydrate)
| CASNo2_Ref = {{cascite|correct|CAS}}
| CASNo2 = 7784-13-6
| CASNo2_Comment = (hexahydrate)
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID=22445
| PubChem = 24012
| RTECS = BD0530000
| Gmelin = 1876
| EINECS = 231-208-1
 }}
|Section2={{Chembox Properties
| Formula = {{chem2|AlCl3}}
| MolarMass = {{ubl|133.341&nbsp;g/mol (anhydrous)|241.432&nbsp;g/mol (hexahydrate)}}<ref name=crc/>
| Appearance = Colourless crystals, [[hygroscopic]]
| Density = {{ubl|2.48&nbsp;g/cm<sup>3</sup> (anhydrous)|2.398&nbsp;g/cm<sup>3</sup> (hexahydrate)}}<ref name=crc/>
| Solubility = {{ubl|439&nbsp;g/L (0&nbsp;°C)|449&nbsp;g/L (10&nbsp;°C)|458&nbsp;g/L (20&nbsp;°C)|466&nbsp;g/L (30&nbsp;°C)|473&nbsp;g/L (40&nbsp;°C)|481&nbsp;g/L (60&nbsp;°C)|486&nbsp;g/L (80&nbsp;°C)|490&nbsp;g/L (100&nbsp;°C)}}
| SolubleOther = {{ubli
 | Soluble in hydrogen chloride, ethanol, chloroform, carbon tetrachloride
 | Slightly soluble in benzene
 }}
| MeltingPt_notes = {{ubli
 | {{convert|180|C|F K}} (anhydrous, sublimes)<ref name=crc>{{RubberBible92nd|page=4.45}}</ref>
 | {{convert|100|C|F K}} (hexahydrate, decomposes)<ref name=crc/>
 }}
| pKa =
| Viscosity = {{ubl|0.35&nbsp;cP (197&nbsp;°C)|0.26&nbsp;cP (237&nbsp;°C)}}<ref name=chemister>{{cite web | url = http://chemister.ru/Database/properties-en.php?dbid=1&id=353 | title = Properties of substance: Aluminium chloride | archive-url = https://web.archive.org/web/20140505171053/http://chemister.ru/Database/properties-en.php?dbid=1&id=353 | archive-date=2014-05-05 | work = Chemister.ru | date = 2007-03-19 | access-date = 2017-03-17 }}</ref>
| VaporPressure = {{ubl|133.3&nbsp;Pa (99&nbsp;°C)|13.3&nbsp;kPa (151&nbsp;°C)}}<ref name=chemister />
 }}
|Section3={{Chembox Structure
| MolShape = Trigonal planar <br />([[monomer]]ic vapour)
| Coordination = Octahedral (solid)<br />Tetrahedral (liquid)
| CrystalStruct = [[Monoclinic]], [[Pearson symbol|mS16]]
| SpaceGroup = C12/m1, No. 12<ref name=str>{{cite journal|doi=10.1524/zkri.1935.90.1.237|title=Die Kristallstruktur der Aluminiumhalogenide II|journal=Zeitschrift für Kristallographie – Crystalline Materials|volume=90|issue=1–6|year=1935| vauthors = Ketelaar JA |pages=237–255|s2cid=100796636|author-link=Jan Ketelaar}}</ref>
| LattConst_a = 0.591&nbsp;nm
| LattConst_b = 0.591&nbsp;nm
| LattConst_c = 1.752&nbsp;nm<ref name=str/>
| UnitCellFormulas = 6
| UnitCellVolume = 0.52996&nbsp;nm<sup>3</sup>
 }}
|Section5={{Chembox Thermochemistry
| DeltaHf = −704.2&nbsp;kJ/mol<ref name=b92t>{{RubberBible92nd|page=5.5}}</ref>
| Entropy = 109.3&nbsp;J/(mol·K)<ref name=b92t/>
| DeltaGf = −628.8&nbsp;kJ/mol<ref name=b92t/>
| HeatCapacity = 91.1&nbsp;J/(mol·K)<ref name=b92t/>
}}
|Section6={{Chembox Pharmacology
| ATCCode_prefix = D10
| ATCCode_suffix = AX01
}}
|Section7={{Chembox Hazards
| GHS_ref = <ref name="sigma">{{Sigma-Aldrich|id=563919|name=Aluminium chloride|access-date=2014-05-05}}</ref>
| GHSPictograms = {{GHS05}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|H314}}
| PPhrases = {{P-phrases|P260|280|301+330+331|303+361+353|310|305+351+338+310}}

| NFPA-H = 3
| NFPA-F = 0
| NFPA-R = 2
| NFPA-S =
| LD50 = 380&nbsp;mg/kg, rat (oral, anhydrous) <br /> 3311&nbsp;mg/kg, rat (oral, hexahydrate)
| IDLH = N.D.<ref name=PGCH>{{PGCH|0024}}</ref>
| PEL = None<ref name=PGCH/>
| REL = 2&nbsp;mg/m<sup>3</sup><ref name=PGCH/>
}}
|Section8={{Chembox Related
| OtherAnions = {{ubl|[[Aluminium fluoride]]|[[Aluminium bromide]]|[[Aluminium iodide]]}}
| OtherCations = {{ubl|[[Boron trichloride]]|[[Gallium trichloride]]|[[Indium(III) chloride]]|[[Magnesium chloride]]}}
| OtherFunction_label = [[Lewis acid]]s
| OtherFunction = {{ubl|[[Iron(III) chloride]]|[[Boron trifluoride]]}}
 }}
}}
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}}

'''Aluminium chloride''', also known as '''aluminium trichloride''', is an [[inorganic compound]] with the formula {{chem2|AlCl3}}. It forms a [[hexahydrate]]  with the formula {{chem2|[Al(H2O)6]Cl3}}, containing six [[Water of hydration|water molecules of hydration]]. Both the anhydrous form and the hexahydrate are colourless crystals, but samples are often contaminated with [[iron(III) chloride]], giving them a yellow colour.

The anhydrous form is commercially important. It has a low melting and boiling point. It is mainly produced and consumed in the production of aluminium, but large amounts are also used in other areas of the chemical industry.<ref name="Ull">{{Ullmann |doi=10.1002/14356007.a01_527.pub2|title=Aluminum Compounds, Inorganic|year=2007| vauthors = Helmboldt O, Keith Hudson L, Misra C, Wefers K, Heck W, Stark H, Danner M, Rösch N |isbn=978-3527306732}}</ref> The compound is often cited as a [[Lewis acid]]. It is an example of an [[inorganic compound]] that [[Reversible reaction|reversibly changes]] from a [[polymer]] to a [[monomer]] at mild temperature.

== History ==
The salt was known in the 18th century as muriate of alumina, marine alum, argillaceous marine salt,<ref>{{Cite book |last1=FOURCROY |first1=Antoine François de |url=https://books.google.com/books?id=wD9XsU46qSsC&pg=RA1-PA54 |title=Elements of natural history, and of chemistry: being the second edition of the elementary lectures on those sciences ... enlarged and improved by the author ... Translated into English, with ... notes; and an historical preface by the translator W. Nicholson |date=1790 |language=en}}</ref> muriated clay.<ref>{{Cite book |last=Berthollet |first=Claude-Louis |url=https://books.google.com/books?id=TpCzhu7JkEIC&pg=PA371 |title=Elements of the Art of Dyeing ... Translated ... by William Hamilton |date=1791 |publisher=Stephen Couchman; sold by J. Johnson |language=en}}</ref> It was first chemically studied in the 1830s.<ref>{{Cite book |last=Gambold |first=Mrs |url=https://books.google.com/books?id=qqdGAQAAMAAJ&pg=PA249 |title=The American Journal of Science |date=1835 |publisher=Kline Geology Laboratory, Yale University. |language=en}}</ref>
{{Section-stub|date=November 2024}}

== Structure ==
[[File:Aluminium-trichloride-3D-structures.png|thumb|center|350x350px|Illustration of structures of aluminium chloride]]
===Anhydrous===
{{chem2|AlCl3}} adopts three structures, depending on the [[temperature]] and the [[State of matter|state]] (solid, liquid, gas). Solid {{chem2|AlCl3}} has a sheet-like layered structure with cubic close-packed chloride ions. In this framework, the Al centres exhibit [[octahedral coordination geometry]].<ref name="Wells">{{cite book | quote = In contrast, {{chem2|AlBr3}} has a more molecular structure, with the {{chem2|Al(3+)}} centers occupying adjacent tetrahedral holes of the close-packed framework of {{chem2|Br−}} ions. | vauthors = Wells AF | date = 1984 | title = Structural Inorganic Chemistry | publisher = Oxford Press | location = [[Oxford]], United Kingdom. | isbn = 0198553706}}</ref> [[Yttrium(III) chloride]] adopts the same structure, as do a range of other compounds. When aluminium trichloride is in its melted state, it exists as the [[Dimer (chemistry)|dimer]] {{chem2|Al2Cl6}}, with [[tetracoordinate]] aluminium. This change in structure is related to the lower density of the liquid phase (1.78&nbsp;g/cm<sup>3</sup>) versus solid aluminium trichloride (2.48&nbsp;g/cm<sup>3</sup>). {{chem2|Al2Cl6}} dimers are also found in the [[Vapor phase|vapour phase]]. At higher temperatures, the {{chem2|Al2Cl6}} dimers [[Dissociation (chemistry)|dissociate]] into [[Trigonal planar molecular geometry|trigonal planar]] {{chem2|AlCl3}} [[monomer]], which is structurally analogous to [[boron trifluoride|{{chem2|BF3}}]]. The melt [[Electrical conductance|conducts]] [[electricity]] poorly,<ref name="Greenwood">{{Greenwood&Earnshaw1st}}</ref> unlike more [[ionic bond|ionic]] [[halide]]s such as [[sodium chloride]].

Aluminium chloride monomer belongs to the [[point group]] D<sub>3h</sub> in its monomeric form and D<sub>2h</sub> in its dimeric form.

=== Hexahydrate ===
The hexahydrate consists of [[Octahedral molecular geometry|octahedral]] {{chem2|[Al(H2O)6](3+)}} [[cation]] centers and chloride [[anions]] ({{chem2|Cl-}}) as [[counterion]]s. [[Hydrogen bond]]s link the cation and anions.<ref>{{cite journal| vauthors = Andress KR, Carpenter C |doi=10.1524/zkri.1934.87.1.446|title=Kristallhydrate II. Die Struktur von Chromchlorid- und Aluminiumchloridhexahydrat|journal=Zeitschrift für Kristallographie – Crystalline Materials|volume=87|year=1934|s2cid=263857074 }}
</ref>
The hydrated form of aluminium chloride has an octahedral molecular geometry, with the central aluminium ion surrounded by six [[water ligand]] molecules. Being coordinatively saturated, the hydrate is of little value as a [[Catalysis|catalyst]] in [[Friedel Crafts Alkylation|Friedel-Crafts alkylation]] and related reactions.

==Uses==
===Alkylation and acylation of arenes===
{{chem2|AlCl3}} is a common Lewis-acid [[catalyst]] for [[Friedel-Crafts reaction]]s, both acylations and alkylations.<ref name="Friedel"/> Important products are [[detergent]]s and [[ethylbenzene]]. These types of reactions are the major use for aluminium chloride, for example, in the preparation of [[anthraquinone]] (used in the [[dye]]stuffs industry) from [[benzene]] and [[phosgene]].<ref name="Greenwood"/> In the general Friedel-Crafts reaction, an [[acyl chloride]] or [[alkyl halide]] reacts with an [[aromatic]] system as shown:<ref name="Friedel"/>
:[[File:Benzene Friedel-Crafts alkylation-diagram.svg|330px]]

The [[alkylation]] reaction is more widely used than the [[acylation]] reaction, although its practice is more technically demanding. For both reactions, the aluminium chloride, as well as other materials and the equipment, should be dry, although a trace of moisture is necessary for the reaction to proceed.<ref>{{cite journal| vauthors = Nenitzescu CD, Cantuniari IP |date=1933|title=Durch Aluminiumchlorid Katalysierte Reaktion, VI. Mitteil.: Die Umlagerung des Cyclohexans in Metyl-cyclopentan |journal=Berichte der Deutschen Chemischen Gesellschaft (A and B Series)|language=en|volume=66|issue=8|pages=1097–1100|doi=10.1002/cber.19330660817|issn=1099-0682}}</ref> Detailed procedures are available for alkylation<ref>{{cite journal |doi=10.15227/orgsyn.089.0210|title=Synthesis of Trifluoromethyl Ketones from Carboxylic Acids: 4-(3,4-Dibromophenyl)-1,1,1-trifluoro-4-methylpentan-2-one|journal=Organic Syntheses|year=2012|volume=89|page=210| vauthors = Reeves JT, Tan Z, Fandrick DR, Song JJ, Yee NK, Senanayake CH |doi-access=free}}</ref> and acylation<ref>{{cite journal |doi=10.15227/orgsyn.080.0227|title=Preparation of 9,10-Dimethoxyphenanthrene and 3,6-Diacetyl-9,10-Dimethoxyphenanthrene|journal=Organic Syntheses|year=2003|volume=80|page=227| vauthors = Paruch K, Vyklicky L, Katz TJ }}</ref><ref>{{cite journal |doi=10.15227/orgsyn.079.0204|title=3-(4-Bromobenzoyl)propanoic Acid|journal=Organic Syntheses|year=2002|volume=79|page=204| vauthors = Seed AJ, Sonpatki V, Herbert MR }}</ref> of arenes.

A general problem with the Friedel-Crafts reaction is that the aluminium chloride catalyst sometimes is required in full [[stoichiometry|stoichiometric]] quantities, because it [[Complex (chemistry)|complex]]es strongly with the products. This complication sometimes generates a large amount of [[Corrosive substance|corrosive]] waste. For these and similar reasons, the use of aluminium chloride has often been displaced by [[zeolite]]s.<ref name="Ull" />

Aluminium chloride can also be used to introduce [[aldehyde]] groups onto [[aromatic]] rings, for example via the [[Gattermann-Koch reaction]] which uses [[carbon monoxide]], [[hydrogen chloride]] and a [[copper(I) chloride]] [[co-catalyst]].<ref>{{cite book | vauthors = Wade LG | date = 2003 | title = Organic Chemistry | edition = 5th | publisher = [[Prentice Hall]] | location = [[Upper Saddle River, New Jersey]] | isbn = 013033832X }}</ref>
:[[File:AlCl3 formylation.gif|300px]]

===Other applications in organic and organometallic synthesis===
Aluminium chloride finds a wide variety of other applications in [[organic chemistry]].<ref>{{cite book | vauthors = Galatsis P | chapter = Aluminum Chloride | date = 1999 | series = Handbook of Reagents for Organic Synthesis | title = Acidic and Basic Reagents | veditors = Reich HJ, Rigby JH | publisher = [[John Wiley & Sons|Wiley]] | location = [[New York City]] | pages = 12–15 | isbn = 978-0-471-97925-8 }}</ref> For example, it can catalyse the [[ene reaction]], such as the addition of [[3-buten-2-one]] (methyl vinyl ketone) to [[carvone]]:<ref>{{cite journal | vauthors = Snider BB | title = Lewis-acid catalyzed ene reactions | journal = [[Acc. Chem. Res.]] | volume = 13 | page = 426 | year = 1980 | doi = 10.1021/ar50155a007 | issue = 11}}</ref>
:[[File:AlCl3 ene rxn.gif|400px]]

It is used to induce a variety of hydrocarbon couplings and rearrangements.<ref>{{cite journal |doi=10.15227/orgsyn.059.0085|title=Highly Reactive Magnesium for the Preparation of Grignard Reagents: 1-Norbornanecarboxylic Acid|journal=Organic Syntheses|year=1979|volume=59|page=85| vauthors = Rieke RD, Bales SE, Hudnall PM, Burns TP, Poindexter GS }}</ref><ref>{{cite journal |doi=10.15227/orgsyn.061.0062|title=Hexamethyl Dewar Benzene|journal=Organic Syntheses|year=1983|volume=61|page=62| vauthors = Shama SA, Wamser CC }}</ref>

Aluminium chloride combined with aluminium in the presence of an arene can be used to synthesize bis(arene) metal complexes, e.g. [[bis(benzene)chromium]], from certain metal halides via the [[Fischer–Hafner synthesis]]. [[Dichlorophenylphosphine]] is prepared by reaction of [[benzene]] and [[phosphorus trichloride]] catalyzed by aluminium chloride.<ref>{{cite journal | vauthors = Buchner B, Lockhart Jr LB | title = Phenyldichlorophosphine |journal=Organic Syntheses | doi = 10.15227/orgsyn.031.0088 | volume = 31 | page = 88 | year = 1951}}</ref>

=== Medical ===

Topical aluminum chloride hexahydrate is used for the treatment of [[hyperhidrosis]] (excessive sweating).<ref name="pmid30215934">{{cite journal | vauthors = McConaghy JR, Fosselman D | title = Hyperhidrosis: Management Options | journal = American Family Physician | volume = 97 | issue = 11 | pages = 729–734 | date = June 2018 | pmid = 30215934 | doi =  }}</ref><ref name="pmid30710603">{{cite journal | vauthors = Nawrocki S, Cha J | title = The etiology, diagnosis, and management of hyperhidrosis: A comprehensive review: Therapeutic options | journal = Journal of the American Academy of Dermatology | volume = 81 | issue = 3 | pages = 669–680 | date = September 2019 | pmid = 30710603 | doi = 10.1016/j.jaad.2018.11.066 }}</ref><ref>{{cite web | title = Aluminum Chloride (Topical) (Monograph) | url = https://www.drugs.com/monograph/aluminum-chloride-topical.html | work = American Society of Health System Pharmacists (ASHP) | publisher =  drugs.com }}</ref>

==Reactions==
Anhydrous aluminium chloride is a powerful [[Lewis acid]], capable of forming Lewis acid-base [[adduct]]s with even weak [[Lewis base]]s such as [[benzophenone]] and [[mesitylene]].<ref name="Friedel">{{cite book | veditors = Olah GA |year=1963 |title=Friedel-Crafts and Related Reactions |volume=1 |publisher=Interscience |place=New York City}}</ref> It forms [[tetrachloroaluminate]] ({{chem2|[AlCl4]−}}) in the presence of [[chloride]] ions.

Aluminium chloride reacts with [[calcium hydride|calcium]] and [[magnesium hydride]]s in [[tetrahydrofuran]] forming tetrahydroaluminates.{{cn|date=September 2023}}

===Reactions with water===
Anhydrous aluminium chloride is [[Hygroscopy|hygroscopic]], having a very pronounced affinity for water. It fumes in moist air and hisses when mixed with liquid water as the Cl<sup>−</sup> ligands are displaced with H<sub>2</sub>O molecules to form the hexahydrate {{chem2|[Al(H2O)6]Cl3}}. The anhydrous phase cannot be regained on heating the hexahydrate. Instead HCl is lost leaving aluminium hydroxide or alumina (aluminium oxide):
:{{chem2|[Al(H2O)6]Cl3 → Al(OH)3 + 3 HCl + 3 H2O}}

Like [[metal aquo complex]]es, [[aqueous solution|aqueous]] {{chem2|AlCl3}} is acidic owing to the ionization of the [[aquo ligand]]s:
:{{chem2|[Al(H2O)6](3+) ⇌ [Al(OH)(H2O)5](2+) + H+}}

Aqueous solutions behave similarly to other [[aluminium]] [[salt (chemistry)|salts]] containing hydrated {{chem2|Al(3+)}} [[ion]]s, giving a gelatinous [[precipitate]] of [[aluminium hydroxide]] upon reaction with dilute [[sodium hydroxide]]:
:{{chem2|AlCl3 + 3 NaOH → Al(OH)3 + 3 [[sodium chloride|NaCl]]}}

==Synthesis==
Aluminium chloride is manufactured on a large scale by the [[exothermic]] reaction of [[aluminium]] metal with chlorine or [[hydrogen chloride]] at temperatures between {{convert|650|and|750|C}}.<ref name="Greenwood"/>
:{{chem2|2 Al + 3 Cl2 → 2 AlCl3}}
:{{chem2|2 Al + 6 HCl → 2 AlCl3 + 3 H2}}

Aluminium chloride may be formed via a [[single displacement reaction]] between [[copper(II) chloride]] and aluminium.
:{{chem2|2 Al + 3 CuCl2 → 2 AlCl3 + 3 Cu}}
In the US in 1993, approximately 21,000 tons were produced, not counting the amounts consumed in the production of aluminium.<ref name="Ull" />

Hydrated aluminium trichloride is prepared by dissolving aluminium oxides in [[hydrochloric acid]]. Metallic aluminium also readily dissolves in hydrochloric acid ─ releasing hydrogen gas and generating considerable heat. Heating this solid does not produce anhydrous aluminium trichloride, the hexahydrate decomposes to [[aluminium hydroxide]] when heated:
:{{chem2|[Al(H2O)6]Cl3 → Al(OH)3 + 3 HCl + 3 H2O}}

Aluminium also forms a lower [[chloride]], [[aluminium(I) chloride]] (AlCl), but this is very unstable and only known in the vapour phase.<ref name="Greenwood"/>

==Natural occurrence==
Anhydrous aluminium chloride is not found as a mineral. The hexahydrate, however, is known as the rare mineral chloraluminite.<ref name="ima-mineralogy.org">{{cite web |url=https://www.ima-mineralogy.org/Minlist.htm |title=List of Minerals|date=March 21, 2011 |website=www.ima-mineralogy.org |publisher=[[International Mineralogical Association]]}}</ref> A more complex, basic and hydrated aluminium chloride mineral is [[cadwaladerite]].<ref>{{cite web |url=https://www.mindat.org/min-845.html|title=Cadwaladerite|website=www.mindat.org}}</ref><ref name="ima-mineralogy.org" />

==Safety==
Anhydrous {{chem2|AlCl3}} reacts vigorously with [[base (chemistry)|base]]s, so suitable precautions are required.
It can cause irritation to the eyes, skin, and the respiratory system if inhaled or on contact.<ref>[https://web.archive.org/web/20110722155335/http://www.solvaychemicals.us/enwiki/static/wma/pdf/5/1/1/8/ALCL.pdf Aluminium Chloride]. solvaychemicals.us</ref>

== See also ==
* [[Aluminium monochloride]]

{{clear}}

== References ==
{{reflist}}

== External links ==
{{Commons category|Aluminium chloride}}
* [http://www.inchem.org/documents/icsc/icsc/eics1125.htm International Chemical Safety Card 1125]
* [http://www.orgsyn.org/orgsyn/chemname.asp?nameID=33169 Index of Organic Synthesis procedures that utilize AlCl<sub>3</sub>]
* [http://www.chemguide.co.uk/inorganic/period3/chlorides.html The period 3 chlorides]
* [http://www.solvaychemicals.us/enwiki/static/wma/pdf/5/1/1/8/ALCL.pdf MSDS] {{Webarchive|url=https://web.archive.org/web/20110722155335/http://www.solvaychemicals.us/enwiki/static/wma/pdf/5/1/1/8/ALCL.pdf |date=2011-07-22}}
* [http://www.chemicalsubstanceschimiques.gc.ca/fact-fait/alum-salts-sels-eng.php Government of Canada Fact Sheets and Frequently Asked Questions: Aluminum Salts]

{{Aluminium compounds}}
{{Chlorides}}
{{Authority control}}

[[Category:Chlorides]]
[[Category:Metal halides]]
[[Category:Aluminium compounds]]
[[Category:Inorganic compounds]]
[[Category:Reagents for organic chemistry]]
[[Category:Deliquescent materials]]
[[Category:Acid catalysts]]