Is Albr3 Soluble In Water

Compound

Aluminium bromide
Names


Preferred IUPAC name Aluminium bromide
Other names Aluminic bromide Aluminium(Three) bromide Aluminium tribromide
Identifiers
CAS Number	7727-15-3 ^Y 7784-eleven-4 hexahydrate^Y
3D model (JSmol)	Interactive image dimer: Interactive image
ChemSpider	22818 ^Y 9040513 hemi(acetyl bromide)^Y 9499890 ethanethiol^Y
ECHA InfoCard	100.028.891
EC Number	231-779-7
PubChem CID	24409 11062022 tertikis(tetrachloromethane) 10865226 hemi(acetyl bromide) 11324936 ethanethiol 6093832 tris(pyridine)
RTECS number	BD0350000
UNII	IY20HBK5LK ^Y
Un number	1725
CompTox Dashboard (EPA)	DTXSID2064783
InChI InChI=1S/Al.3BrH/h;three1H/q+3;;;/p-3^Y Central: PQLAYKMGZDUDLQ-UHFFFAOYSA-K^Y InChI=1/Al.3BrH/h;three1H/q+3;;;/p-3 Cardinal: PQLAYKMGZDUDLQ-DFZHHIFOAT
SMILES Br[Al](Br)Br dimer: Br[Al-]i(Br)[Br+][Al-]([Br+]1)(Br)Br
Properties
Chemic formula	AlBr₃ Al₂Br_{half dozen} AlBr_iii·6H₂O (hexahydrate)
Molar mass	266.694 thousand/mol (anhydrous) 374.785 thou/mol (hexahydrate)^[1]
Appearance	white to pale yellow pulverization^[one]
Odor	pungent
Density	3.2 g/cm^three (anhydrous) two.54 chiliad/cm³ (hexahydrate)^[1]
Melting point	97.5 °C (anhydrous) 93 °C (hexahydrate)^[1]
Boiling point	255 (anhydrous)^[1]
Solubility in water	very soluble, partially hydrolyses indicated by a fuming solution and an optional advent of white precipitate
Solubility	slightly soluble in methanol, diethyl ether, acetone
Construction^[2]
Crystal structure	Monoclinic, mP16 (anhydrous)
Space grouping	P2₁/c, No. fourteen
Lattice constant	a = 0.7512 nm, b = 0.7091 nm, c = 1.0289 nm α = 90°, β = 96.44°, γ = 90°
Formula units (Z)	4
Thermochemistry^[ane]
Heat capacity (C)	100.half dozen J/(mol·K)
Std tooth entropy (S ^⦵ ₂₉₈)	180.2 J/(mol·Chiliad)
Std enthalpy of formation (Δ_f H ^⦵ ₂₉₈)	-572.v kJ/mol
Hazards
GHS labelling:
Pictograms
Betoken discussion	Danger
Take chances statements	H302, H314
Precautionary statements	P260, P264, P270, P280, P301+P312, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P330, P363, P405, P501
NFPA 704 (fire diamond)	3 ane 1
Lethal dose or concentration (LD, LC):
LD₅₀ (median dose)	1598 mg/kg (oral, rat)
Related compounds
Other anions	aluminium trichloride aluminium triiodide
Other cations	boron tribromide
Related compounds	iron(3) bromide
Except where otherwise noted, data are given for materials in their standard country (at 25 °C [77 °F], 100 kPa). Yverify (what is^{Y N} ?) Infobox references

Chemical compound

Aluminium bromide is any chemical compound with the empirical formula AlBr_x. Aluminium tribromide is the nigh common form of aluminium bromide.^[3] Information technology is a colorless, sublimable hygroscopic solid; hence old samples tend to be hydrated, mostly as aluminium tribromide hexahydrate (AlBr_three·6H₂O).

Structure [edit]

The dimeric course of aluminium tribromide (Al₂Br₆) predominates in the solid state, in solutions in noncoordinating solvents (e.m. CS₂), in the melt, and in the gas phase. Simply at high temperatures do these dimers intermission up into monomers:

Al₂Br_vi → two AlBr₃ ΔH°_diss = 59 kJ/mol

The species aluminium monobromide forms from the reaction of HBr with Al metallic at loftier temperature. It disproportionates near room temperature:

6/n "[AlBr]_n" → Al_twoBr₆ + four Al

This reaction is reversed at temperatures higher than k °C. Aluminium monobromide has been crystallographically characterized in the form the tetrameric adduct Al_fourBr_iv(Cyberspace₃)₄ (Et = C₂H_v). This species is electronically related to cyclobutane. Theory suggest that the diatomic aluminium monobromide condenses to a dimer and so a tetrahedral cluster Al₄Br₄, akin to the analogous boron chemical compound.^[four]

Al₂Br₆ consists of ii AlBr₄ tetrahedra that share a common edge. The molecular symmetry is D_2h.

The monomer AlBr₃, observed only in the vapor, can be described as trigonal planar, D_3h indicate group. The diminutive hybridization of aluminium is often described as sp^two . The Br-Al-Br bond angles are 120 °.

Synthesis [edit]

Experiment showing synthesis of aluminum bromide from the elements.

By far the almost common course of aluminium bromide is Al₂Br₆. This species exists as hygroscopic colorless solid at standard conditions. Typical impure samples are xanthous or even ruby-brown due to the presence of iron-containing impurities. It is prepared by the reaction of HBr with Al:

2 Al + 6 HBr → Al₂Br₆ + iii H₂

Alternatively, the direct bromination occurs also:

2 Al + 3 Br_ii → Al₂Br₆

Reactions [edit]

A demonstration of the reaction of the exothermic reaction of the potent Lewis acrid (Al_twoBr_vi) and strong Lewis base (H₂O).

Al₂Br₆ dissociates readily to give the strong Lewis acid, AlBr₃. Regarding the trend of Al₂Br_vi to dimerize, it is common for heavier main group halides to be equally aggregates larger than implied by their empirical formulae. Lighter main grouping halides such as boron tribromide do not evidence this tendency, in role due to the smaller size of the central atom.

Consistent with its Lewis acidic character, Al₂Br_{half dozen} is hydrolyzed by water with evolution of HBr and germination of Al-OH-Br species. Similarly, it besides reacts quickly with alcohols and carboxylic acids, although less vigorously than with water. With simple Lewis bases (L), Al_iiBr₆ forms adducts, such as AlBr₃L.

Aluminium tribromide reacts with carbon tetrachloride at 100 °C to course carbon tetrabromide:

iv AlBr_three + three CCl₄ → iv AlCl₃ + 3 CBr₄

and with phosgene yields carbonyl bromide and aluminium chlorobromide:^{[ citation needed ]}

AlBr_three + COCl₂ → COBr₂ + AlCl₂Br

Al_iiBr_half-dozen is used as a catalyst for the Friedel-Crafts alkylation reaction.^[3] Related Lewis acid-promoted reactions include equally epoxide ring openings and decomplexation of dienes from iron carbonyls. It is a stronger Lewis acid than the more common Al_twoCl_vi.

Safe [edit]

Aluminium tribromide is a highly reactive fabric.^[5]

References [edit]

^ ^a ^b ^c ^d ^east ^f Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Printing. p. four.45. ISBN1-4398-5511-0.
^ Troyanov, Sergey I.; Krahl, Thoralf; Kemnitz, Erhard (2004). "Crystal structures of $GaX 3 (Ten= Cl, Br, I)$ and $AlI iii$ ". Zeitschrift für Kristallographie. 219 (2–2004): 88–92. doi:10.1524/zkri.219.2.88.26320. S2CID 101603507.
^ ^a ^b Paquette, Leo A. (2001). Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X. hdl:10261/236866. ISBN0471936235.
^ Dohmeier, Carsten; Loos, Dagmar; Schnöckel, Hansgeorg (1996). "Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions". Angewandte Chemie International Edition in English. 35 (ii): 129. doi:10.1002/anie.199601291.
^ Renfew, Malcom M. (1991). "Hazardous laboratory chemicals: Disposal guide (Armour, M.A.)". Journal of Chemical Education. 68 (9): A232. Bibcode:1991JChEd..68Q.232R. doi:10.1021/ed068pA232.2.