Aluminium iodide
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Aluminium iodide
| Aluminium iodide | |
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Aluminium iodide |
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Other names
Aluminium(III) iodide Aluminum iodide |
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| Identifiers | |
| CAS number | 7784-23-8 (anhydrate), 10090-53-6 (hexahydrate) |
| PubChem | 82222 (anhydrate)  |
| ChemSpider | 74202 (anhydrate) |
| EC number | 232-054-8 |
| UN number | UN 3260 |
| Jmol-3D images | Image 1 |
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| Properties | |
| Molecular formula | AlI3 |
| Molar mass | 407.69495 g/mol (anhydrous) 515.786 g/mol (hexahydrate) |
| Appearance | colorless powder but impure samples are often brown |
| Density | 3.98 g/cm3 (anhydrous) 2.63 g/cm3 (hexahydrate) |
| Melting point |
189.4 °C (anhydrous) |
| Boiling point |
360 °C, sublimes |
| Solubility in water | reacts violently (anhydrous) soluble (hexahydrate) |
| Solubility in alcohol, ether | soluble (hexahydrate) |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
Aluminium iodide is any chemical compound containing only aluminium and iodine. Invariably, the name refers to a compound of the composition AlI3, formed by the reaction of aluminium and iodine[1] or the action of HI on 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, AlI3 is a strong Lewis acid and should be protected from the atmosphere.
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Contents
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Applications in organic synthesis
Aluminium iodide is employed as a catalyst to break certain kinds of C-O and N-O bonds. It cleaves aryl ethers and deoxygenates epoxides.[2]
Aluminium(I) iodide
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[3]
- 3 AlI → AlI3 + 2 Al
An illustrative derivative of aluminium monoiodide is the cyclic adduct formed with triethylamine, AI4I4(NEt3)4.
Safety
Hydrolysis of aluminium triiodide will release some HI, which is corrosive. Lewis acids are skin irritants.
References
- ^ G. W. Watt, J. L. Hall (1953). Inorganic Syntheses. IV. pp. 117–119.
- ^ M. Gugelchuk (2004). Aluminum Iodide, in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette). New York: J. Wiley & Sons. doi:10.1002/047084289X.ra083.
- ^ Dohmeier, C.; Loos, D.; Schnöckel, H. (1996). "Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions". Angewandte Chemie International Edition 35: 129–149. doi:10.1002/anie.199601291.
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