Aluminium iodide

Short description: Chemical compound

Aluminium iodide

|  | File:Aluminium-iodide-3D-vdW.png

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Names
Preferred IUPAC name

Aluminium iodide

Other names

Aluminium(III) iodide

Aluminum iodide
Aluminium triiodide

Aluminum triiodide

Identifiers

CAS Number

* 7784-23-8 (anhydrate) Y
* 10090-53-6 (hexahydrate) Y

3D model (JSmol)

* Interactive image
* dimer: Interactive image

ChemSpider |

* 74202 (anhydrate) Y

EC Number |

* 232-054-8

PubChem CID

* 82222 (anhydrate)

UNII |

* L903Z8J9VR (anhydrate) Y
* VWS43EUO9V (hexahydrate) Y

UN number | UN 3260

InChI

* Key: CECABOMBVQNBEC-UHFFFAOYSA-K Y

* Key: CECABOMBVQNBEC-DFZHHIFOAE

SMILES

* I[Al](I)I

* dimer: I[Al-]1(I)[I+][Al-]([I+]1)(I)I

Properties

Chemical formula

| AlI3, AlI3·6H2O (hexahydrate)
Molar mass | 407.695 g/mol (anhydrous)
515.786 g/mol (hexahydrate)[1]
Appearance  | white (anhydrous) or yellow powder (hexahydrate)[1]
Density | 3.98 g/cm3 (anhydrous)[1] 2.63 g/cm3 (hexahydrate)[2]
Melting point |  188.28 °C (370.90 °F; 461.43 K) (anhydrous)
185 °C, decomposes (hexahydrate)[1][2]
Boiling point |  382 °C (720 °F; 655 K) anhydrous, sublimes[1]

Solubility in water

| very soluble, partial hydrolysis
Solubility in alcohol, ether | soluble (hexahydrate)
Structure[3]

Crystal structure

| Monoclinic, mP16

Space group

| P21/c, No. 14

Lattice constant

a = 1.1958 nm, b = 0.6128 nm, c = 1.8307 nm

α = 90°, β = 90°, γ = 90°

Formula units (Z)

| 8
Thermochemistry[1]

Heat capacity (C)

| 98.7 J/(mol·K)

Std molar
entropy (S ~~o~~ 298)

| 195.9 J/(mol·K)

Std enthalpy of
formation (ΔfH⦵298)

| −302.9 kJ/mol

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 ?)
Infobox references

Aluminium iodide is the inorganic compound with the composition AlI
3. It also exists a various hydrates formed by exposure of the anhydrous material to water.[4] For example the hexahydrate is obtained from a reaction between metallic aluminum or aluminum hydroxide with hydroiodic acid. Like the related chloride and bromide, AlI3 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.[5]

## Contents

* 1 Preparation
* 2 Structure
* 3 Aluminium(I) iodide
* 4 References
* 5 External links

## Preparation

Aluminium iodide is formed by the reaction of aluminium and iodine[6] or the action of HI on Al metal.

## Structure

Solid AlI3 is dimeric, consisting of Al2I6, similar to that of AlBr3.[3] The structure of monomeric and dimeric forms have been characterized in the gas phase.[7] The monomer, AlI3, is trigonal planar with a bond length of 2.448(6) Å, and the bridged dimer, Al2I6, at 430 K is a similar to Al2Cl6 and Al2Br6 with Al–I 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 D2h.

## Aluminium(I) iodide

Main article: Chemistry:Aluminium monoiodide

File:06. Директна синтеза на алуминиум јодид.webm 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:[8]

3 AlI → AlI
3 \+ 2 Al

An illustrative derivative of aluminium monoiodide is the cyclic adduct formed with triethylamine, Al4I4(NEt3)4.

## References

1. ↑ 1.0 1.1 1.2 1.3 1.4 1.5 Haynes, William M., ed (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.45. ISBN 1439855110.
2. ↑ 2.0 2.1 Perry, Dale L. (19 April 2016). Handbook of Inorganic Compounds, Second Edition. CRC Press. p. 8. ISBN 978-1-4398-1462-8. https://books.google.com/books?id=SFD30BvPBhoC&pg=PA8.
3. ↑ 3.0 3.1 Troyanov, Sergey I.; Krahl, Thoralf; Kemnitz, Erhard (2004). "Crystal structures of GaX3(X= Cl, Br, I) and AlI3". Zeitschrift für Kristallographie 219 (2–2004): 88–92. doi:10.1524/zkri.219.2.88.26320.GaX3(X=+Cl,+Br,+I)+and+AlI3&rft.jtitle=Zeitschrift+für+Kristallographie&rft.aulast=Troyanov&rft.aufirst=Sergey+I.&rft.au=Troyanov, Sergey+I.&rft.au=Krahl, Thoralf&rft.au=Kemnitz, Erhard&rft.date=2004&rft.volume=219&rft.issue=2–2004&rft.pages=88–92&rft_id=info:doi/10.1524/zkri.219.2.88.26320&rfr_id=info:sid/en.wikibooks.org:Chemistry:Aluminium_iodide">
4. ↑ Schmidt, Horst; Hennings, Erik; Voigt, Wolfgang (2014). "Crystal structures of hydrates of simple inorganic salts. III. Water-rich aluminium halide hydrates: AlCl3·15H2O, AlBr3·15H2O, AlI3·15H2O, AlI3·17H2O and AlBr3·9H2O". Acta Crystallographica Section C Structural Chemistry 70 (9): 882–888. doi:10.1107/S2053229614014302. PMID 25186362.
5. ↑ Gugelchuk, M. (2004). "Aluminum Iodide". in L. Paquette. Encyclopedia of Reagents for Organic Synthesis. New York: J. Wiley & Sons. doi:10.1002/047084289X.ra083. ISBN 0471936235.
6. ↑ Watt, George W; Hall, James L; Taylor, William Lloyd; Kleinberg, Jacob (1953). "Aluminum Iodide". Inorganic Syntheses. 4. pp. 117–119. doi:10.1002/9780470132357.ch39. ISBN 9780470132357.
7. ↑ Hargittai, Magdolna; Réffy, Balázs; Kolonits, Mária (2006). "An Intricate Molecule: Aluminum Triiodide. Molecular Structure of AlI3and Al2I6 from Electron Diffraction and Computation". The Journal of Physical Chemistry A 110 (10): 3770–3777. doi:10.1021/jp056498e. PMID 16526661.AlI3and+Al2I6+from+Electron+Diffraction+and+Computation&rft.jtitle=The+Journal+of+Physical+Chemistry+A&rft.aulast=Hargittai&rft.aufirst=Magdolna&rft.au=Hargittai, Magdolna&rft.au=Réffy, Balázs&rft.au=Kolonits, Mária&rft.date=2006&rft.volume=110&rft.issue=10&rft.pages=3770–3777&rft_id=info:doi/10.1021/jp056498e&rft_id=info:pmid/16526661&rfr_id=info:sid/en.wikibooks.org:Chemistry:Aluminium_iodide">
8. ↑ Dohmeier, C.; Loos, D.; Schnöckel, H. (1996). "Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions". Angewandte Chemie International Edition 35 (2): 129–149. doi:10.1002/anie.199601291.

## External links

* v
* t
* e

Aluminium compounds

Al(I)|

* AlBr
* AlCl
* AlF
* AlI
* Al2O

Al(II)|

* AlB2
* AlB12
* AlO

Al(III)|

* AlAs
* Al(BH4)3
* AlBr3
* AlCl3
* AlF3
* AlH3
* AlI3
* AlN
* Al(NO3)3
* Al2(CO3)3
* Al(OH)3
* Al(OH)2OAc
* Al(OH)(OAc)2
* Al(OAc)3
* Al2SO4(OAc)4
* AlP
* AlPO4
* AlSb
* Al(C5H7O2)3
* Al(MnO4)3
* Al2(MoO4)3
* Al2O3
* Al2S3
* Al2(SO4)3
* Al2Se3
* Al2Te3
* Al2SiO5
* Al4C3
* AlOHO
* Al(OH)2CO2C17H5
* NaAlH2(OC2H4OCH3)2
* LiAlH2(OC2H4OCH3)2

| Alums|

* (NH4)Al(SO4)2
* KAl(SO4)2
* NaAl(SO4)2

|

Organoaluminium(III) compounds|

* (Al(CH3)3)2
* (Al(C2H5)3)2
* Al(CH2CH(CH3)2)3
* Al(C2H5)2Cl
* Al(C2H5)2CN
* Al(CH2CH(CH3)2)2H
* Al(C2H5)2Cl2C2H5Cl
* Ti(C5H5)2CH2ClAl(CH3)2

HI |  |  |  | He

|
|
|
|

LiI | BeI2 | BI3 | CI4 | NI3 | I2O4,
I2O5,
I4O9 | IF,
IF3,
IF5,
IF7 | Ne
NaI | MgI2 | AlI3 | SiI4 | PI3,
P2I4 | S  | ICl,
ICl3 | Ar
KI | CaI2 | Sc  | TiI4 | VI3 | CrI3 | MnI2 | FeI2 | CoI2 | NiI2 | CuI | ZnI2 | Ga2I6 | GeI2,
GeI4 | AsI3 | Se  | IBr | Kr
RbI | SrI2 | YI3 | ZrI4 | NbI5 | Mo  | Tc  | Ru  | Rh  | Pd  | AgI | CdI2 | InI3 | SnI4,
SnI2 | SbI3 | TeI4 | I  | Xe
CsI | BaI2 |  | HfI4 | TaI5 | W  | Re  | Os  | Ir  | Pt  | AuI | Hg2I2,
HgI2 | TlI | PbI2 | BiI3 | Po  | AtI | Rn
Fr  | RaI2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La  | Ce  | Pr  | Nd  | Pm  | SmI2 | Eu  | Gd  | TbI3 | Dy  | Ho  | Er  | Tm  | Yb  | Lu
Ac  | ThI4 | Pa  | UI3,
UI4 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | EsI3 | Fm  | Md  | No  | Lr

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