Aluminium bromide

This article is about the tribromide, AlBr₃, and its hexahydrate. For the unstable monobromide, AlBr, see Aluminium monobromide.

Aluminium tribromide (anhydrous)
IUPAC name	aluminium tribromide tribromoalumane tribromidoaluminium
Other names	aluminium(III) bromide
Identifiers
InChI	InChI=1/Al.3BrH/h;3*1H/q+3;;;/p-3
InChIKey	PQLAYKMGZDUDLQ-DFZHHIFOAT
Standard InChI	InChI=1S/Al.3BrH/h;3*1H/q+3;;;/p-3
Standard InChIKey	PQLAYKMGZDUDLQ-UHFFFAOYSA-K
CAS number	[7727-15-3]
EC number	231-779-7
RTECS	BD0350000
ChemSpider	22818
PubChem	24409
Properties
Chemical formula	AlBr3
Molar mass	266.72 g/mol
Appearance	white to pale yellow solid, hygroscopic
Density	2.64 g/cm3
Melting point	97.5 °C
Boiling point	265 °C
Solubility in water	reacts violently
Solubility	soluble in ethanol, acetone, carbon disulfide
Hazards
GHS pictograms
GHS signal word	DANGER
GHS hazard statements	H302, H314
GHS precautionary statements	P260, P264, P270, P280, P301+312, P301+330+331, P363, P304+340, P310, P321, P305+351+338, P405, P501
Flash point	non-flammable
Related compounds
Other anions	Aluminium fluoride Aluminium chloride Aluminium iodide
Other cations	Boron tribromide Gallium(III) bromide Indium(III) bromide Thallium(III) bromide
Other Lewis acids	Iron(III) bromide
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

Aluminium bromide is any chemical compound with the empirical formula AlBr_x. 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 + 4Al

This reaction is reversed at temperatures above 1000 °C.

Synthesis

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:

2Al + 6HBr → Al₂Br₆ + 3H₂

Alternatively, the direct bromination occurs also:

2Al + 3Br₂ → Al₂Br₆

Structure

AlBr₃ has an almost molecular structure in the solid state, with the Al³⁺ centers occupying adjacent tetrahedral holes of the close-packed framework of Br⁻ ions. "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 → 2AlBr₃

ΔH^o_diss = 59 kJ/mol

Representative reactions

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, Al₂Br₆ reacts vigorously with water 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 AlBr₃:L.

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 acidic 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.

Structures of the aluminium bromides

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 C_2v.

The monomer AlBr₃, observed only in the vapor, can be described as trigonal planar, D_3h point group. The atomic hybridization of aluminium is often described as sp². The Br-Al-Br bond angles are 120 °.

Chemical Reactions

Reacts with carbon tetrachloride at 100 °C to form carbon tetrabromide:

4AlBr₃ + 3CCl₄ → 4AlCl₃ + 3CBr₄

Reacts with phosgene to yield carbonyl bromide and aluminum chlorobromide:

AlBr₃ + COCl₂ → COBr₂ + AlCl₂Br

Uses

The anhydrous form is used as a catalyst for the Friedel–Crafts alkylation reaction. Its catalytic activity is similar to anhydrous aluminum chloride. However, commercial applications are rare.

Safety precautions

Al₂Br₆ is corrosive and can cause skin burns if not washed off immediately after contact. It should be stored in a dry area.

Further reading

• Dohmeier, C.; Loos, D.; Schnöckel, H. Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions. Angew. Chem., Int. Ed. Engl. 1996, 35, 129–49.
• Gugelchuk, M. Aluminum Bromide. In Encyclopedia of Reagents for Organic Synthesis; Paquette, Leo A., Ed.; John Wiley: New York, 2004. DOI: 10.1002/047084289.
• Armour, M. A. Hazardous Laboratory Chemicals: Disposal Guide, 2nd ed.; CRC Press: Boca Raton, FL., 1996.

External links

• NIOSH Pocket Guide to Chemical Hazards 0024
• IPCS Environmental Health Criteria 194: Aluminium