Aluminium iodide

{{short description|Chemical compound}}

{{Chembox

| Verifiedfields = changed

| Watchedfields = changed

| verifiedrevid = 449832810

| ImageFile = Aluminium-iodide-3D-balls.png

| ImageSize =

| ImageName = Ball and stick model of aluminium iodide dimer

| ImageFile2 = Jodid hlinitý.PNG

| PIN = Aluminium iodide

| OtherNames = Aluminium(III) iodide

Aluminum iodide

Aluminium triiodide

Aluminum triiodide

|Section1={{Chembox Identifiers

| InChI =

| InChIKey =CECABOMBVQNBEC-DFZHHIFOAE

| CASNo_Ref = {{cascite|correct|??}}

| CASNo = 7784-23-8

| CASNo_Comment = (anhydrate)

| CASNo1_Ref = {{cascite|correct|??}}

| CASNo1 = 10090-53-6

| CASNo1_Comment = (hexahydrate)

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = L903Z8J9VR

| UNII_Comment = (anhydrate)

| UNII1_Ref = {{fdacite|correct|FDA}}

| UNII1 = VWS43EUO9V

| UNII1_Comment = (hexahydrate)

| PubChem = 82222

| PubChem_Comment = (anhydrate)

| ChemSpiderID = 74202

| ChemSpiderID_Comment = (anhydrate)

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| EINECS = 232-054-8

| UNNumber = UN 3260

| SMILES = I[Al](I)I

| SMILES1 = I[Al-]1(I)[I+][Al-]([I+]1)(I)I

| SMILES1_Comment = dimer

| StdInChI_Ref = {{stdinchicite|changed|chemspider}}

| StdInChI =

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey = CECABOMBVQNBEC-UHFFFAOYSA-K}}

|Section2={{Chembox Properties

| Formula = {{math|size=100%|AlI₃}}, {{math|size=100%|AlI₃·6H₂O}} (hexahydrate)

| MolarMass = 407.695 g/mol (anhydrous)
515.786 g/mol (hexahydrate)

| Appearance = white (anhydrous) or yellow powder (hexahydrate)

| Density = 3.98 g/cm³ (anhydrous){{RubberBible92nd|page=4.45}} 2.63 g/cm³ (hexahydrate){{cite book|author=Perry, Dale L. |title=Handbook of Inorganic Compounds, Second Edition|url=https://books.google.com/books?id=SFD30BvPBhoC&pg=PA8|date=19 April 2016|publisher=CRC Press|isbn=978-1-4398-1462-8|page=8}}

| MeltingPtC = 188.28

| MeltingPt_notes = (anhydrous)
185 °C, decomposes (hexahydrate)

| BoilingPtC = 382

| BoilingPt_notes = anhydrous, sublimes

| Solubility = very soluble, partial hydrolysis

| Solvent = alcohol, ether

| SolubleOther = soluble (hexahydrate)

}}

|Section3={{Chembox Structure

| Structure_ref =

| CrystalStruct = Monoclinic, mP16

| SpaceGroup = P2₁/c, No. 14

| Coordination =

| LattConst_a = 1.1958 nm

| UnitCellFormulas = 8

| LattConst_b = 0.6128 nm

| LattConst_c = 1.8307 nm

| LattConst_alpha = 90

| LattConst_beta = 90

| LattConst_gamma = 90

| MolShape =

| OrbitalHybridisation =

| Dipole =

}}

| Section4 = {{Chembox Thermochemistry

| Thermochemistry_ref =

| HeatCapacity = 98.7 J/(mol·K)

| Entropy = 195.9 J/(mol·K)

| DeltaHf = −302.9 kJ/mol

| DeltaGf =

| DeltaHc =

}}

}}

Aluminium iodide is a chemical compound containing aluminium and iodine. Invariably, the name refers to a compound of the composition {{math|{{chem|Al|I|3}}}}, formed by the reaction of aluminium and iodine{{cite book|doi=10.1002/9780470132357.ch39|chapter=Aluminum Iodide|title=Inorganic Syntheses|volume=4|pages=117–119|year=1953|last1=Watt|first1=George W|last2=Hall|first2=James L|last3=Taylor|first3=William Lloyd|last4=Kleinberg|first4=Jacob|isbn=9780470132357}} or the action of Hydrogen iodide on {{chem|Al}} metal. The hexahydrate is obtained from a reaction between metallic aluminum or aluminum hydroxide with hydrogen iodide or hydroiodic acid. Like the related chloride and bromide, {{math|{{chem|Al|I|3}}}} is a strong Lewis acid and will absorb water from the atmosphere. It is employed as a reagent for the scission of certain kinds of C-O and N-O bonds. It cleaves aryl ethers and deoxygenates epoxides.{{cite book| author = Gugelchuk, M. | chapter=Aluminum Iodide|title =Encyclopedia of Reagents for Organic Synthesis |editor=L. Paquette| year = 2004| publisher =J. Wiley & Sons| place = New York| doi = 10.1002/047084289X.ra083| isbn=0471936235}}