|CAS number||, hexahydrate|
|PubChem||, tertikis(tetrachloromethane), hemi(acetyl bromide), ethanethiol, tris(pyridine)|
|ChemSpider||, hemi(acetyl bromide) , ethanethiol|
|Jmol-3D images||Image 1|
|Molar mass||266.69 g/mol|
|Appearance||white to pale yellow
|Melting point||97.8 °C (208.0 °F; 370.9 K)|
|Boiling point||265 °C (509 °F; 538 K)|
|Solubility in water||reacts|
|Solubility||slightly soluble in methanol, diethyl ether, acetone|
|EU classification||not listed|
|LD50||1598 mg/kg (oral, rat)|
|Other anions||aluminium trichloride
|Other cations||boron tribromide|
|Related compounds||iron(III) bromide|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Aluminium bromide is any chemical compound with the empirical formula AlBrx. The species called "aluminium tribromide," is the most common aluminium bromide. The species aluminium monobromide forms from the reaction of HBr with Al metal at high temperature. It disproportionates near room temperature:
- 6/n "[AlBr]n" → Al2Br6 + 4 Al
This reaction is reversed at temperatures higher than 1000 °C.
"Aluminium tribromide" is really dialuminium hexabromide with the molecular formula of Al2Br6 in the solid state, solutions in noncoordinating solvents (e.g. CS2), and in the melt. Even upon evaporation, Al2Br6 exists in the gas phase. At high temperatures, the gaseous molecules break up into monomers:
- Al2Br6 → 2 AlBr3 ΔH°diss = 59 kJ/mol
Aluminium monobromide has been crystallographically characterized in the form the tetrameric adduct Al4Br4(NEt3)4 (Et = C2H5). This species is electronically related to cyclobutane. Theory suggest that the diatomic aluminium monobromide condenses to a dimer and then a tetrahedral cluster Al4Br4, akin to the analogous boron compound.
Al2Br6 consists of two AlBr4 tetrahedra that share a common edge. The molecular symmetry is D2h.
The monomer AlBr3, observed only in the vapor, can be described as trigonal planar, D3h point group. The atomic hybridization of aluminium is often described as sp2. The Br-Al-Br bond angles are 120 °.
By far the most common form of aluminium bromide is Al2Br6. This species exists as hygroscopic colorless solid at standard conditions. Typical impure samples are yellowish or even red-brown due to the presence of iron-containing impurities. It is prepared by the reaction of HBr with Al:
- 2 Al + 6 HBr → Al2Br6 + 3 H2
Alternatively, the direct bromination occurs also:
- 2 Al + 3 Br2 → Al2Br6
Al2Br6 dissociates readily to give the strong Lewis acid, AlBr3. Regarding the tendency of Al2Br6 to dimerize, it is common for heavier main group halides to exist as aggregates larger than implied by their empirical formulae. Lighter main group halides such as boron tribromide do not show this tendency, in part due to the smaller size of the central atom.
Consistent with its Lewis acidic character, water hydrolizes Al2Br6 with evolution of HBr and formation of Al-OH-Br species. Similarly, it also reacts quickly with alcohols and carboxylic acids, although less vigorously than with water. With simple Lewis bases (L), Al2Br6 forms adducts, such as AlBr3L.
- 4 AlBr3 + 3 CCl4 → 4 AlCl3 + 3 CBr4
- AlBr3 + COCl2 → COBr2 + AlCl2Br
Al2Br6 is an excellent reagent for Friedel-Crafts and related Lewis acid-promoted reactions such as epoxide ring openings and decomplexation of dienes from iron carbonyls. It is a stronger Lewis acid than the more common Al2Cl6. Because it is hygroscopic, older samples tend to be hydrated and less useful. Impure samples can be purified by vacuum sublimation.
||This article includes a list of references, related reading or external links, but its sources remain unclear because it lacks inline citations. (November 2012)|
- Dohmeier, Carsten; Loos, Dagmar; Schnöckel, Hansgeorg (1996). "Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions". Angewandte Chemie International Edition in English 35 (2): 129. doi:10.1002/anie.199601291.
- Encyclopedia of Reagents for Organic Synthesis. 2001. doi:10.1002/047084289X. ISBN 0471936235.
- Renfew, Malcom M. (1991). "Hazardous laboratory chemicals: Disposal guide (Armour, M.A.)". Journal of Chemical Education 68 (9): A232. doi:10.1021/ed068pA232.2.