(Difference between pages)

Page 1

Page 1Revision 1

Page 2

Page 2Revision 2

Content deleted Content addedVisualWikitext

Revision as of 20:28, 16 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 477229759 of page Aluminium_chloride for the Chem/Drugbox validation project (updated: '').		Latest revision as of 19:23, 5 December 2024 edit Sphilbrick (talk | contribs)Administrators178,402 edits Reverted good faith edits by GothicWindow452 (talk)Tags: Twinkle Undo
Line 1:		Line 1:
			{{short description|Chemical compound}}
	{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}}
			{{good article}}
	{{chembox
			{{cs1 config|name-list-style=vanc|display-authors=6}}
	| verifiedrevid = 452128468
			{{Chembox
			| Verifiedfields = changed
			| Watchedfields = changed
			| verifiedrevid = 477245740
	| Name =		| Name =
	| ImageFile1 = Aluminium-trichloride-hexahydrate-white-and-yellow.jpg		| ImageFile1 = Aluminium-trichloride-hexahydrate-white-and-yellow.jpg
	<!-- | ImageSize = 150px -->		| ImageSize1 = 150px
			| ImageCaption1 = Aluminium trichloride hexahydrate, pure (top), and contaminated with ] (bottom)
	| ImageName1 = Aluminium chloride
			| ImageName1 = Aluminium(III) chloride
	| ImageFile2 =
	| ImageName2 = Aluminium(III) Chloride		| ImageFileL2 = Aluminium-trichloride-dimer-3D-balls.png
			| ImageSizeL2 = 125px
	| ImageFile3 = Aluminium-trichloride-dimer-3D-balls.png
			| ImageNameL2 = Aluminium trichloride dimer
	<!-- | ImageSize1 = 150px -->
	| ImageName3 = Aluminium trichloride dimer		| ImageFileR2 = Aluminium-chloride-xtal-unit-cell-3D-bs-17.png
			| ImageSizeR2 = 125px
	| IUPACName = aluminium chloride
			| ImageNameR2 = Aluminium trichloride unit cell
	| OtherNames = aluminium(III) chloride
			| IUPACName = Aluminium chloride
	| Section1 = {{Chembox Identifiers
			| OtherNames = Aluminium(III) chloride<br />Aluminium trichloride<br />Trichloroaluminum
			|Section1={{Chembox Identifiers
	| UNII_Ref = {{fdacite|correct|FDA}}		| UNII_Ref = {{fdacite|correct|FDA}}
	| UNII = LIF1N9568Y		| UNII = LIF1N9568Y
			| UNII1_Ref = {{fdacite|correct|FDA}}
			| UNII1 = 3CYT62D3GA
			| UNII1_Comment = (hexahydrate)
	| InChI = 1/Al.3ClH/h;3*1H/q+3;;;/p-3		| InChI = 1/Al.3ClH/h;3*1H/q+3;;;/p-3
	| ChEBI_Ref = {{ebicite|correct|EBI}}		| ChEBI_Ref = {{ebicite|correct|EBI}}
	| ChEBI = 30114		| ChEBI = 30114
	| SMILES = Cl(Cl)Cl		| SMILES = Cl(Cl)Cl
			| SMILES_Comment = ]
			| SMILES1 = Cl1(Cl)(1)(Cl)Cl
			| SMILES1_Comment = ]
			| SMILES2 = ()()()()...
			| SMILES2_Comment = hexahydrate
	| InChIKey = VSCWAEJMTAWNJL-DFZHHIFOAR		| InChIKey = VSCWAEJMTAWNJL-DFZHHIFOAR
	| SMILES1 = (Cl)(Cl)Cl
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/Al.3ClH/h;3*1H/q+3;;;/p-3		| StdInChI = 1S/Al.3ClH/h;3*1H/q+3;;;/p-3
Line 29:		Line 42:
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
	| CASNo_Comment = (anhydrous)		| CASNo_Comment = (anhydrous)
			| CASNo1_Ref = {{cascite|changed|??}}
	| CASOther = <br/>10124-27-3 (hydrate),<br/>7784-13-6 (hexahydrate)
			| 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_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID=22445		| ChemSpiderID=22445
	| PubChem = 24012		| PubChem = 24012
	| RTECS = BD0530000		| RTECS = BD0530000
	| ATCCode_prefix = D10		| Gmelin = 1876
			| EINECS = 231-208-1
	| ATCCode_suffix = AX01
			}}
			|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, ]
			| 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/>
	}}		}}
	| Section2 = {{Chembox Properties
	| Formula = AlCl<sub>3</sub>
	| MolarMass = 133.34 g/mol (anhydrous)<br />241.43 g/mol (hexahydrate)
	| Appearance = white or pale yellow solid,<br />]
	| Density = 2.48 g/cm<sup>3</sup> (anhydrous) <br> 1.3 g/cm<sup>3</sup> (hexahydrate)
	| Solubility = 43.9 g/100 ml (0 °C)<br />44.9 g/100 ml (10 °C)<br />45.8 g/100 ml (20 °C)<br />46.6 g/100 ml (30 °C)<br />47.3 g/100 ml (40 °C)<br />48.1 g/100 ml (60 °C)<br />48.6 g/100 ml (80 °C)<br />49 g/100 ml (100 °C)
	| SolubleOther = soluble in hydrogen chloride, ethanol, chloroform, carbon tetrachloride <br> slightly soluble in benzene
	| MeltingPt = 192.4 °C *(anhydrous) <br> 0 °C (hexahydrate)
	| BoilingPt = 120 °C (hexahydrate)
	| pKa =		| 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		|Section3={{Chembox Structure
	| MolShape = Trigonal planar<br />(]ic vapour)		| MolShape = Trigonal planar <br />(]ic vapour)
	| Coordination = Octahedral (solid)<br />Tetrahedral (liquid)		| Coordination = Octahedral (solid)<br />Tetrahedral (liquid)
	| CrystalStruct = ], ]		| CrystalStruct = ], ]
			| 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>
	| SpaceGroup = C12/m1, No. 12
			| 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>
	}}		}}
	| Section4 = {{Chembox Thermochemistry		|Section5={{Chembox Thermochemistry
	| DeltaHf = −704&nbsp;kJ·mol<sup>−1</sup><ref>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 061894690X}}</ref>		| DeltaHf = −704.2&nbsp;kJ/mol<ref name=b92t>{{RubberBible92nd|page=5.5}}</ref>
			| Entropy = 109.3&nbsp;J/(mol·K)<ref name=b92t/>
	| Entropy = 111&nbsp;J·mol<sup>−1</sup>·K<sup>−1</sup><ref>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 061894690X}}</ref>
			| DeltaGf = −628.8&nbsp;kJ/mol<ref name=b92t/>
	}}
			| HeatCapacity = 91.1&nbsp;J/(mol·K)<ref name=b92t/>
	| Section7 = {{Chembox Hazards
			}}
	| EUClass = Corrosive ('''C''')
			|Section6={{Chembox Pharmacology
	| RPhrases = {{R34}}
			| ATCCode_prefix = D10
	| SPhrases = {{S1/2}}, {{S7/8}}, {{S28}}, {{S45}}
			| ATCCode_suffix = AX01
	| LD50 = ''anhydrous:'' <br> 380 mg/kg, rat (oral) <hr> ''hexahydrate:'' <br> 3311 mg/kg, rat (oral)
	}}		}}
	| Section8 = {{Chembox Related		|Section7={{Chembox Hazards
			| GHS_ref = <ref name="sigma">{{Sigma-Aldrich|id=563919|name=Aluminium chloride|access-date=2014-05-05}}</ref>
	| OtherAnions = ]<br />]<br />]
			| GHSPictograms = {{GHS05}}
	| OtherCations = ]<br />]<br />]<br />]
			| GHSSignalWord = Danger
	| Function = ]s
			| HPhrases = {{H-phrases|H314}}
	| OtherFunctn = ]<br />]
			| 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|]|]|]}}
			| OtherCations = {{ubl|]|]|]|]}}
			| OtherFunction_label = ]s
			| OtherFunction = {{ubl|]|]}}
	}}		}}
	}}		}}
			{{Infobox drug
			| container_only = yes
			| image =
			| width =
			| alt =
			| caption =
			<!-- Clinical data -->
			| pronounce =
			| tradename =
			| Drugs.com = {{drugs.com|monograph|aluminum-chloride-topical}}
			| MedlinePlus =
			| DailyMedID = aluminum chloride
			| pregnancy_AU = <!-- A / B1 / B2 / B3 / C / D / X -->
			| pregnancy_AU_comment =
			| pregnancy_category =
			| routes_of_administration = ]
			| class =
			| ATCvet =
			| ATC_prefix = None
			| ATC_suffix =
			| ATC_supplemental =
			| biosimilars =
			<!-- Legal status -->
			| legal_AU = <!-- S2, S3, S4, S5, S6, S7, S8, S9 or Unscheduled -->
			| legal_AU_comment =
			| legal_BR = <!-- OTC, A1, A2, A3, B1, B2, C1, C2, C3, C4, C5, D1, D2, E, F -->
			| legal_BR_comment =
			| legal_CA = <!-- OTC, Rx-only, Schedule I, II, III, IV, V, VI, VII, VIII -->
			| legal_CA_comment =
			| legal_DE = <!-- Anlage I, II, III or Unscheduled -->
			| legal_DE_comment =
			| legal_NZ = <!-- Class A, B, C -->
			| legal_NZ_comment =
			| legal_UK = <!-- GSL, P, POM, CD, CD Lic, CD POM, CD No Reg POM, CD (Benz) POM, CD (Anab) POM or CD Inv POM / Class A, B, C -->
			| legal_UK_comment =
			| legal_US = <!-- OTC / Rx-only / Schedule I, II, III, IV, V -->
			| legal_US_comment =
			| legal_EU =
			| legal_EU_comment =
			| legal_UN = <!-- N I, II, III, IV / P I, II, III, IV -->
			| legal_UN_comment =
			| legal_status = <!-- For countries not listed above -->
			<!-- Pharmacokinetic data -->
			| bioavailability =
			| protein_bound =
			| metabolism =
			| metabolites =
			| onset =
			| elimination_half-life =
			| duration_of_action =
			| excretion =
			<!-- Identifiers -->
			| CAS_number =
			| CAS_supplemental =
			| PubChem =
			| IUPHAR_ligand =
			| DrugBank =
			| ChemSpiderID =
			| UNII =
			| KEGG =
			| ChEBI =
			| ChEMBL =
			| NIAID_ChemDB =
			| PDB_ligand =
			| synonyms =
			<!-- Chemical and physical data -->
			| IUPAC_name =
			| chemical_formula_ref =
			| chemical_formula =
			| C= | H= | Ag= | Al= | As= | Au= | B= | Bi= | Br= | Ca= | Cl= | Co= | F= | Fe= | Gd= | I=
			| K= | Li= | Mg= | Mn= | N= | Na= | O= | P= | Pt= | S= | Sb= | Se= | Sr= | Tc= | Zn= | charge=
			| molecular_weight =
			| molecular_weight_comment =
			| SMILES =
			| StdInChI =
			| StdInChI_comment =
			| StdInChIKey =
			| density =
			| density_notes =
			| melting_point =
			| melting_high =
			| melting_notes =
			| boiling_point =
			| boiling_notes =
			| solubility =
			| sol_units =
			| specific_rotation =
			}}
			'''Aluminium chloride''', also known as '''aluminium trichloride''', is an ] with the formula {{chem2|AlCl3}}. It forms a ] with the formula {{chem2|Cl3}}, containing six ]. Both the anhydrous form and the hexahydrate are colourless crystals, but samples are often contaminated with ], 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 ]. It is an example of an ] that ] from a ] to a ] 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 ==
			]
			===Anhydrous===
			{{chem2|AlCl3}} adopts three structures, depending on the ] and the ] (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 ].<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 = ], United Kingdom. | isbn = 0198553706}}</ref> ] adopts the same structure, as do a range of other compounds. When aluminium trichloride is in its melted state, it exists as the ] {{chem2|Al2Cl6}}, with ] 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 ]. At higher temperatures, the {{chem2|Al2Cl6}} dimers ] into ] {{chem2|AlCl3}} ], which is structurally analogous to ]. The melt ] ] poorly,<ref name="Greenwood">{{Greenwood&Earnshaw1st}}</ref> unlike more ] ]s such as ].
			Aluminium chloride monomer belongs to the ] D<sub>3h</sub> in its monomeric form and D<sub>2h</sub> in its dimeric form.
			=== Hexahydrate ===
			The hexahydrate consists of ] {{chem2|(3+)}} ] centers and chloride ] ({{chem2|Cl-}}) as ]s. ]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 ] molecules. Being coordinatively saturated, the hydrate is of little value as a ] in ] and related reactions.
			==Uses==
			===Alkylation and acylation of arenes===
			{{chem2|AlCl3}} is a common Lewis-acid ] for ]s, both acylations and alkylations.<ref name="Friedel"/> Important products are ]s and ]. These types of reactions are the major use for aluminium chloride, for example, in the preparation of ] (used in the ]stuffs industry) from ] and ].<ref name="Greenwood"/> In the general Friedel-Crafts reaction, an ] or ] reacts with an ] system as shown:<ref name="Friedel"/>
			:]
			The ] reaction is more widely used than the ] 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 ] quantities, because it ]es strongly with the products. This complication sometimes generates a large amount of ] waste. For these and similar reasons, the use of aluminium chloride has often been displaced by ]s.<ref name="Ull" />
			Aluminium chloride can also be used to introduce ] groups onto ] rings, for example via the ] which uses ], ] and a ] ].<ref>{{cite book | vauthors = Wade LG | date = 2003 | title = Organic Chemistry | edition = 5th | publisher = ] | location = ] | isbn = 013033832X }}</ref>
			:]
			===Other applications in organic and organometallic synthesis===
			Aluminium chloride finds a wide variety of other applications in ].<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 = ] | location = ] | pages = 12–15 | isbn = 978-0-471-97925-8 }}</ref> For example, it can catalyse the ], such as the addition of ] (methyl vinyl ketone) to ]:<ref>{{cite journal | vauthors = Snider BB | title = Lewis-acid catalyzed ene reactions | journal = ] | volume = 13 | page = 426 | year = 1980 | doi = 10.1021/ar50155a007 | issue = 11}}</ref>
			:]
			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. ], from certain metal halides via the ]. ] is prepared by reaction of ] and ] 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 ] (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 ], capable of forming Lewis acid-base ]s with even weak ]s such as ] and ].<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 ] ({{chem2|−}}) in the presence of ] ions.
			Aluminium chloride reacts with ] and ]s in ] forming tetrahydroaluminates.{{cn|date=September 2023}}
			===Reactions with water===
			Anhydrous aluminium chloride is ], 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|Cl3}}. The anhydrous phase cannot be regained on heating the hexahydrate. Instead HCl is lost leaving aluminium hydroxide or alumina (aluminium oxide):
			:{{chem2|Cl3 → Al(OH)3 + 3 HCl + 3 H2O}}
			Like ]es, ] {{chem2|AlCl3}} is acidic owing to the ionization of the ]s:
			:{{chem2|(3+) ⇌ (2+) + H+}}
			Aqueous solutions behave similarly to other ] ] containing hydrated {{chem2|Al(3+)}} ]s, giving a gelatinous ] of ] upon reaction with dilute ]:
			:{{chem2|AlCl3 + 3 NaOH → Al(OH)3 + 3 ]}}
			==Synthesis==
			Aluminium chloride is manufactured on a large scale by the ] reaction of ] metal with chlorine or ] 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 ] between ] 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 ]. 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 ] when heated:
			:{{chem2|Cl3 → Al(OH)3 + 3 HCl + 3 H2O}}
			Aluminium also forms a lower ], ] (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=]}}</ref> A more complex, basic and hydrated aluminium chloride mineral is ].<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 ]s, so suitable precautions are required.
			It can cause irritation to the eyes, skin, and the respiratory system if inhaled or on contact.<ref>. solvaychemicals.us</ref>
			== See also ==
			* ]
			{{clear}}
			== References ==
			{{reflist}}
			== External links ==
			{{Commons category|Aluminium chloride}}
			*
			*
			*
			* {{Webarchive|url=https://web.archive.org/web/20110722155335/http://www.solvaychemicals.us/static/wma/pdf/5/1/1/8/ALCL.pdf |date=2011-07-22}}
			*
			{{Aluminium compounds}}
			{{Chlorides}}
			{{Authority control}}
			]
			]
			]
			]
			]
			]
			]