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{{short description|Chemical compound}} |
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{{Chembox |
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{{Chembox |
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| Verifiedfields = changed |
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| verifiedrevid = 436539475 |
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| Watchedfields = changed |
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| ImageFile = Aluminium-iodide-3D-balls.png |
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| verifiedrevid = 449832810 |
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| ImageSize = 200px |
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| ImageFile = Aluminium-iodide-3D-balls.png |
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| ImageName = Ball and stick model of aluminium iodide dimer |
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| ImageSize = |
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| ImageFile2 = Jodid hlinitý.PNG |
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| ImageName = Ball and stick model of aluminium iodide dimer |
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| PIN = Aluminium iodide |
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| ImageFile2 = Jodid hlinitý.PNG |
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| OtherNames = Aluminium(III) iodide<br /> |
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| PIN = Aluminium iodide |
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| OtherNames = Aluminium(III) iodide<br /> |
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Aluminum iodide<br /> |
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Aluminum iodide<br /> |
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Aluminium triiodide<br /> |
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Aluminium triiodide<br /> |
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Aluminum triiodide |
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Aluminum triiodide |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| InChI = 1/Al.3HI/h;3*1H/q+3;;;/p-3 |
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| InChI = |
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| InChIKey = CECABOMBVQNBEC-DFZHHIFOAE |
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| InChIKey =CECABOMBVQNBEC-DFZHHIFOAE |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo = 7784-23-8 |
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| CASNo = 7784-23-8 |
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| CASNo_Comment = (anhydrate) |
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| CASNo_Comment = (anhydrate) |
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| CASNo1_Ref = {{cascite|correct|??}} |
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| CASNo1 = 10090-53-6 |
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| CASNo1_Comment = (hexahydrate) |
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| CASNo1 = 10090-53-6 |
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| CASNo1_Comment = (hexahydrate) |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| PubChem = 82222 |
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| UNII = L903Z8J9VR |
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| PubChem_Comment = (anhydrate) |
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| UNII_Comment = (anhydrate) |
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| PubChem_Ref = {{Pubchemcite}} |
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| UNII1_Ref = {{fdacite|correct|FDA}} |
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| ChemSpiderID = 74202 |
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| UNII1 = VWS43EUO9V |
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| ChemSpiderID_Comment = (anhydrate) |
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| UNII1_Comment = (hexahydrate) |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| EINECS = 232-054-8 |
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| PubChem = 82222 |
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| PubChem_Comment = (anhydrate) |
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| UNNumber = UN 3260 |
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| ChemSpiderID = 74202 |
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| SMILES = I(I)I |
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| ChemSpiderID_Comment = (anhydrate) |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| StdInChI = 1S/Al.3HI/h;3*1H/q+3;;;/p-3 |
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| EINECS = 232-054-8 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| UNNumber = UN 3260 |
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| SMILES = I(I)I |
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| SMILES1 = I1(I)(1)(I)I |
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| SMILES1_Comment = ] |
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| StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChI = |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = CECABOMBVQNBEC-UHFFFAOYSA-K}} |
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| StdInChIKey = CECABOMBVQNBEC-UHFFFAOYSA-K}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = AlI<sub>3</sub> |
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| Formula = {{math|size=100%|AlI<sub>3</sub>}}, {{math|size=100%|AlI<sub>3</sub>·6H<sub>2</sub>O}} (hexahydrate) |
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| MolarMass = 407.69495 g/mol (anhydrous) <br> 515.786 g/mol (hexahydrate) |
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| MolarMass = 407.695 g/mol (anhydrous) <br> 515.786 g/mol (hexahydrate)<ref name=b92/> |
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| Appearance = colorless powder<br />but impure samples<br />are often brown |
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| Appearance = white (anhydrous) or yellow powder (hexahydrate)<ref name=b92/> |
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| Density = 3.98 g/cm<sup>3</sup> (anhydrous) <br> 2.63 g/cm<sup>3</sup> (hexahydrate) |
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| Density = 3.98 g/cm<sup>3</sup> (anhydrous)<ref name=b92>{{RubberBible92nd|page=4.45}}</ref> 2.63 g/cm<sup>3</sup> (hexahydrate)<ref name="Perry2016">{{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}}</ref> |
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| MeltingPtC = 188.28 |
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| MeltingPt = 189.4 °C (anhydrous) <br> 185 °C, decomp. (hexahydrate) |
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| MeltingPt_notes = (anhydrous) <br> 185 °C, decomposes (hexahydrate)<ref name=b92/><ref name="Perry2016"/> |
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| BoilingPt = 360 °C, sublimes |
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| BoilingPtC = 382 |
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| Solubility = reacts violently (anhydrous) <br> soluble (hexahydrate) |
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| BoilingPt_notes = anhydrous, sublimes<ref name=b92/> |
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| Solvent = ], ] |
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| SolubleOther = soluble (hexahydrate) |
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| Solubility = very soluble, partial hydrolysis |
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| Solvent = ], ] |
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| SolubleOther = soluble (hexahydrate) |
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}} |
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|Section3={{Chembox Structure |
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| Structure_ref =<ref name="TroyanovKrahl2004"/> |
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| CrystalStruct = ], ] |
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| SpaceGroup = P2<sub>1</sub>/c, No. 14 |
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| Coordination = |
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| LattConst_a = 1.1958 nm |
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| UnitCellFormulas = 8 |
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| LattConst_b = 0.6128 nm |
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| LattConst_c = 1.8307 nm |
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| LattConst_alpha = 90 |
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| LattConst_beta = 90 |
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| LattConst_gamma = 90 |
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| MolShape = |
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| OrbitalHybridisation = |
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| Dipole = |
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}} |
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| Section4 = {{Chembox Thermochemistry |
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| Thermochemistry_ref =<ref name=b92/> |
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| HeatCapacity = 98.7 J/(mol·K) |
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| Entropy = 195.9 J/(mol·K) |
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| DeltaHf = -302.9 kJ/mol |
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| DeltaGf = |
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| DeltaHc = |
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}} |
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}} |
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}} |
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}} |
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'''Aluminium iodide''' is any ] containing only ] and ]. Invariably, the name refers to a compound of the composition AlI<sub>3</sub>, formed by the reaction of aluminium and iodine<ref>{{cite book| author = G. W. Watt, J. L. Hall| title = Inorganic Syntheses| year = 1953| volume =IV| pages = 117–119}}</ref> or the action of ] on Al metal. The hexahydrate is obtained from a reaction between metallic aluminum or ] with ] or ]. As for the related chloride and bromide, AlI<sub>3</sub> is a strong ] and should be protected from the atmosphere. |
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'''Aluminium iodide''' is a ] containing ] and ]. Invariably, the name refers to a compound of the composition {{chem|Al|I|3}}, formed by the reaction of aluminium and iodine<ref>{{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}}</ref> or the action of ] on {{chem|Al}} metal. The hexahydrate is obtained from a reaction between metallic aluminum or ] with ] or ]. Like the related chloride and bromide, {{chem|Al|I|3}} is a strong ] and will absorb water from the atmosphere. It is employed as a ] for the scission of certain kinds of C-O and N-O bonds. It cleaves aryl ]s and deoxygenates ]s.<ref>{{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}}</ref> |
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==Structure== |
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==Applications in organic synthesis== |
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Solid {{chem|Al|I|3}} is dimeric, consisting of {{chem|Al|2|I|6}}, similar to that of ].<ref name="TroyanovKrahl2004">{{cite journal|last1=Troyanov|first1=Sergey I.|last2=Krahl|first2=Thoralf|last3=Kemnitz|first3=Erhard|title=Crystal structures of {{math|size=100%|1=GaX<sub>3</sub>(X= Cl, Br, I)}} and {{math|size=100%|AlI<sub>3</sub>}}|journal=Zeitschrift für Kristallographie|volume=219|issue=2–2004|year=2004|pages=88–92|doi=10.1524/zkri.219.2.88.26320|s2cid=101603507}}</ref> The structure of monomeric and dimeric forms have been characterized in the gas phase.<ref name="HargittaiRéffy2006">{{cite journal|last1=Hargittai|first1=Magdolna|last2=Réffy|first2=Balázs|last3=Kolonits|first3=Mária|title=An Intricate Molecule: Aluminum Triiodide. Molecular Structure of {{math|size=100%|AlI<sub>3</sub>}}and {{math|size=100%|Al<sub>2</sub>I<sub>6</sub>}} from Electron Diffraction and Computation|journal=The Journal of Physical Chemistry A|volume=110|issue=10|year=2006|pages=3770–3777|doi=10.1021/jp056498e|pmid=16526661}}</ref> The monomer, {{chem|Al|I|3}}, is trigonal planar with a bond length of 2.448(6) Å, and the bridged dimer, {{chem|Al|2|I|6}}, at 430 K is a similar to ] and ] with {{chem2|Al\sI}} bond lengths of 2.456(6) Å (terminal) and 2.670(8) Å (bridging). The dimer is described as floppy with an equilibrium geometry of D<sub>2h</sub>. |
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Aluminium iodide is employed as a ] to break certain kinds of C-O and N-O bonds. It cleaves aryl ]s and deoxygenates ]s.<ref>{{cite book| author = M. Gugelchuk | title =Aluminum Iodide, in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette)| year = 2004| publisher =J. Wiley & Sons| location = New York| doi = 10.1002/047084289}}</ref> |
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==Aluminium(I) iodide== |
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==Aluminium(I) iodide== |
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{{main|Aluminium monoiodide}} |
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The name "aluminium iodide" is widely assumed to describe the triiodide or its dimer. In fact, a monoiodide also enjoys a role in the Al-I system, although composition AlI is unstable at room temperature with respect to the triiodide<ref>{{cite journal| title = Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions| author = Dohmeier, C.; Loos, D.; Schnöckel, H.| journal = Angewandte Chemie International Edition | year =1996| volume =35| pages =129–149| doi =10.1002/anie.199601291}}</ref> |
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] |
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:3 AlI → AlI<sub>3</sub> + 2 Al |
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The name "aluminium iodide" is widely assumed to describe the triiodide or its dimer. In fact, a monoiodide also enjoys a role in the Al–I system, although the compound AlI is unstable at room temperature relative to the triiodide:<ref>{{cite journal| title = Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions|author1=Dohmeier, C. |author2=Loos, D. |author3=Schnöckel, H. | journal = Angewandte Chemie International Edition | year =1996| volume =35|issue=2 | pages =129–149| doi =10.1002/anie.199601291}}</ref> |
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An illustrative derivative of aluminium monoiodide is the cyclic ] formed with ], AI<sub>4</sub>I<sub>4</sub>(NEt<sub>3</sub>)<sub>4</sub>. |
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:<chem>3AlI -> AlI3 + 2Al</chem> |
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An illustrative derivative of aluminium monoiodide is the cyclic ] formed with ], {{chem|Al|4|I|4|(NEt|3|)|4}}. |
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==Safety== |
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Hydrolysis of aluminium triiodide will release some HI, which is corrosive. Lewis acids are skin irritants. |
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==References== |
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==References== |
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{{reflist}} |
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{{reflist}} |
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==External links== |
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*{{Commonscatinline}} |
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{{Aluminium compounds}} |
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{{Aluminium compounds}} |
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{{Iodides}} |
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{{Use dmy dates|date=March 2018}} |
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{{inorganic-compound-stub}} |
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