7446-70-0 Usage
Description
White or light-yellow crystalline solid (or amorphous solid depending on the method of production); odor of HCl; hygroscopic; melts at 190°C at 2.5 atm; sublimes at 181.2°C; density 2.44 g/cm3 at 25°C; decomposes in water evolving heat; soluble in HCl; soluble in many organic solvents, including absolute ethanol, chloroform, carbon tetrachloride and ether; slightly soluble in benzene.
Aluminum chloride is important industrial chemical. Anhydrous Aluminum chloride is used as the catalyst in variety of Friedel-Crafts type of reactions. Large amounts of ethylbenzene are prepared in this way and are used to make styrene.
C6H6 + CH3CH2Cl + AlCl3→C6H5CH2CH3 + H+ + [AlCl4]-
Aluminum chloride is also used in the manufacture of anthraquinone (used in dyestuffs industry) and dodecylbenzene (used to make detergents) and in the isomerisation of hydrocarbons (petroleum industry).
Aluminum chloride reacts vigorously with water and fumes in air. It is used as a catalyst in cracking petroleum and in organic synthesis.
Uses
Different sources of media describe the Uses of 7446-70-0 differently. You can refer to the following data:
1. Aluminum chloride has extensive commercial applications. It is used primarily in the electrolytic production of aluminum. Another major use involves its catalytic applications in many organic reactions, including Friedel-Crafts alkylation, polymerization, isomerization, hydrocracking, oxidation, decarboxylation, and dehydrogenation. It is also used in the production of rare earth chlorides, electroplating of aluminum and in many metal finishing and metallurgical operations.
2. A yellowish-white crystalline or granular powder made
by passing chlorine gas over alumina in a heated state and
collecting the product by sublimation. Aluminum chloride
was occasionally used in gold and platinum toning baths.
3. Aluminum chloride is used as a catalyst in many organic reactions.
Preparation
Aluminum chloride is made by chlorination of molten aluminum at temperatures between 650 to 750°C;
2 Al + 3Cl2→ 2AlCl3
or by chlorination of alumina (bauxite or clay) at 800°C in the presence of a reducing agent, such as carbon or CO. It can be prepared by similar high temperature chlorination of bauxite in the presence of a chlorinated organic reductant such as CCl4.
A pelletized mixture of clay, lignite and a small amount of NaCl is chlorinated at 900°C, producing gaseous AlCl3 (Toth process). Alternatively, alumina is mixed with about 20% by weight carbon and a small amount of sodium salt. The mixture is chlorinated at 600°C (Bayer process).
In the laboratory, anhydrous AlCl3 can be prepared by heating the metal with dry HCl gas at 150°C. The product sublimes and deposits in the cool air condenser. Unreacted HCl is vented out.
Reaction
Reacts with calcium and magnesium hydrides in tetrahydrofuran forming tetrahydro aluminates, Ca(AlH4)2; reacts with hydrides of alkali metals in ether forming aluminum hydride;
Hydrolyzes in chilled, dilute HCl forming aluminum chloride hexahydrate, AlCl3?6H2O; reacts violently with water, evolving HCl,
AlCl3 + H2O ——? Al(OH)3 + HCl ↑
Chemical Properties
Aluminum chloride is a noncombustible but highly reactive whitish-gray, yellow, or green powder or liquid. Strong, acidic, irritating odor like hydrochloric acid.The vapor consists of double molecules Al2Cl6 . Soluble in water.
Definition
aluminium chloride: A whitishsolid, AlCl3, which fumes in moist airand reacts violently with water (togive hydrogen chloride). It is knownas the anhydrous salt (hexagonal; r.d.2.44 (fused solid); m.p. 190°C (2.5atm.); sublimes at 178°C) or the hexahydrateAlCl3.6H2O (rhombic; r.d.2.398; loses water at 100°C), both ofwhich are deliquescent. Aluminiumchloride may be prepared by passinghydrogen chloride or chlorine overhot aluminium or (industrially) bypassing chlorine over heated aluminiumoxide and carbon. The chlorideion is polarized by the smallpositive aluminium ion and thebonding in the solid is intermediatebetween covalent and ionic. In theliquid and vapour phases dimer moleculesexist, Al2Cl6, in which thereare chlorine bridges making coordinatebonds to aluminium atoms (seeformula). The AlCl3 molecule can alsoform compounds with other moleculesthat donate pairs of electrons(e.g. amines or hydrogen sulphide);i.e. it acts as a Lewis acid. At hightemperatures the Al2Cl6 molecules inthe vapour dissociate to (planar)AlCl3 molecules. Aluminium chlorideis used commercially as a catalyst inthe cracking of oils. It is also a catalystin certain other organic reactions,especially the Friedel–Craftsreaction.
General Description
Aluminum chloride may be manufactured by chlorination of liquid aluminum in ceramic lined reaction vessels at 600-700oC.
Reactivity Profile
ALUMINUM CHLORIDE behaves as an acidic salt. Self-reactive. After long storage in closed containers, explosions often occur upon opening [Chem. Abst. 41:6723d 1947]. Can cause ethylene(also other alkenes) to polymerize violently [J. Inst. Pet. 33:254 1947]. Causes ethylene oxide to rearrange and polymerize, liberating heat [J. Soc. Chem. Ind. 68:179 1949]. Can catalyze violent polymerization of allyl chloride [Ventrone 1971]. Addition to nitrobenzene containing about 5% phenol caused a violent explosion [Chem. Eng. News 31:4915 1953]. Mixtures with nitromethane may explode when organic matter is present [Chem. Eng. News 26:2257 1948].
Hazard
Powerful irritant to tissue; moderately toxic by ingestion. Reacts violently with water, evolving hydrogen chloride gas.
Health Hazard
Contact with the skin or eyes in the presence of moisture causes thermal and acid burns.
Fire Hazard
Behavior in Fire: Reacts violently with water used in extinguishing adjacent fires
Flammability and Explosibility
Aluminum chloride is not flammable but reacts violently with water, so fires
involving this substance should be extinguished with carbon dioxide or dry
chemicals. Toxic fumes (HCl and reaction products) can be released during fires.
Industrial uses
Different sources of media describe the Industrial uses of 7446-70-0 differently. You can refer to the following data:
1. Aluminum chloride (AlCl3) is a volatile solid which sublimes at 458 K. The vapour formed on sublimation consists of an equilibrium mixture of monomers (AlCl3) and dimers (Al2Cl6). It is used to prepare the powerful and versatile reducing agent lithium tetrahydridoaluminate (LiAlH4). Aluminium trichloride (AlCl3) act as Lewis acids to a wide range of electron-pair donors, and this has led to their widespread use as catalysts. In the important Friedel-Crafts acylation, AlCl3 is used as a strong Lewis acid catalyst in order to achieve the acylation of an aromatic ring.
2. Aluminum chloride (AlCl3) act as Lewis acids to a wide range of
electron-pair donors, and this has led to their widespread use as catalysts. In the important Friedel–Crafts
acylation, AlCl3 is used as a strong Lewis acid catalyst in order to achieve the acylation of an aromatic ring.
Safety Profile
Moderately toxic by ingestion. Experimental teratogenic and reproductive effects. Mutation data reported. The dust is an irritant by ingestion, inhalation, and skin contact. Highly exothermic polymerization reactions with alkenes. Incompatible with nitrobenaenes or nitrobenzene + phenol. Highly exothermic reaction with water or steam produces toxic fumes of HCl. See also ALUMINUM COMPOUNDS, CHLORIDES, and HYDROCHLORIC ACID.
Potential Exposure
It is used as ethylbenzene catalyst, dyestuff intermediate, and detergent alkylate; in making other chemicals and dyes, astringents, deodorants, in the petroleum refining, and the rubber industries
storage
work with this substance should be conducted in a
fume hood, and impermeable gloves should be worn at all times when handling AlCl3.
Aluminum chloride should be stored in sealed containers under an inert atmosphere in a cool,
dry place. Care should be taken in opening containers of this compound because of the
possibility of the buildup of HCl vapor from hydrolysis with traces of moisture.
Shipping
UN1726 Aluminum chloride, anhydrous, Hazard class: 8; Labels: 8-Corrosive material. UN2581 Aluminum chloride solution, Hazard class: 8; Labels: 8-Corrosive material
Purification Methods
Sublime it several times in an all-glass system under nitrogen at 30-50mm pressure. It has also been sublimed in a stream of dry HCl and has been subjected to a preliminary sublimation through a section of granular aluminium metal [for manipulative details see Jensen J Am Chem Soc 79 1226 1957]. It fumes in moist air.
Incompatibilities
A strong reducing agent. Contact with air or water forms hydrochloric acid and hydrogen chloride gas. Reaction with water may be violent. Water, alcohol, and alkenes can cause polymerization. Incompatible with nitrobenzene, organic material, and bases. Attacks metal in presence of moisture, forming flammable hydrogen gas.
Waste Disposal
May be sprayed with aqueous ammonia in the presence of ice and, when reaction is complete, flushed down drain with running water.
Check Digit Verification of cas no
The CAS Registry Mumber 7446-70-0 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,4,4 and 6 respectively; the second part has 2 digits, 7 and 0 respectively.
Calculate Digit Verification of CAS Registry Number 7446-70:
(6*7)+(5*4)+(4*4)+(3*6)+(2*7)+(1*0)=110
110 % 10 = 0
So 7446-70-0 is a valid CAS Registry Number.
InChI:InChI=1/Al.3ClH.3H/h;3*1H;;;/p-3/rAlH3.3ClH/h1H3;3*1H/p-3
7446-70-0Relevant articles and documents
Metal-Urea Complex - A Precursor to Metal Nitrides
Qiu, Yu,Gao, Lian
, p. 352 - 357 (2004)
A novel and general route to synthesize various metal nitrides (AlN, CrN, and ζ-Fe2N) from metal-urea complexes is presented. These complexes, especially metal-urea chloride, have proved to be useful precursors to metal nitrides, because urea molecules construct a coordination sphere around the metal atom and form a stable structure, compared with the air-sensitive halide. Different anions in the second coordination sphere determine the reaction mechanism. The transformation from metal-urea chloride to nitride is thought to follow a nucleation-growth mechanism, while that from metal-urea nitrate is thought to follow a nitridation mechanism. We anticipate that this metal-urea complex will find applications in the fabrication of other, more complex, nitrides.
ETHYL-SUBSTITUTED (η5-CYCLOPENTADIENYL)-BIS(DIHALOALANEDI-μ-HALO)TITANIUM(III) AND (η6-BENZENE)BIS(DIHALOALANEDI-μ-HALO)TITANIUM(II) CHLORO AND BROMO COMPLEXES
Mach, Karel,Antropiusova, Helena,Polacek, Jindrich
, p. 285 - 296 (1980)
Ethyl-substituted trinuclear complexes CpTiAl2Cl8-xEtx (x=1-4) were prepared by the reaction of CpTiCl3 with two equivalents of ethylaluminium compounds.The complexes were characterized by the half-width of their EPR single-line spectra, which decreased f
Paddock, N. L.
, p. 1070 - 1071 (1951)
Bertoti I.,Toth, A.,Szekely, T.,Pap, I. S.
, p. 325 - 332 (1981)
Use of 1,4-bis(2,2,6,6-tetramethyl-1-oxyl-4-piperidyl)butane as a probe for studying acid sites
Fionov,Sadykov
, p. 174 - 177 (2007)
ESR spectroscopy was applied to study paramagnetic complexes of the nitroxyl biradical of 1,4-bis(2,2,6,6-tetramethyl-1-oxyl-4-piperidyl)butane formed with AlCl3 in a toluene solution and resulted from the interaction with the acid sites on the SiO2 and γ-Al 2O3 surface. This biradical in solution forms a complex with two AlCl3 molecules, and a complex with two hydroxyl groups is formed on the SiO2 surface. When the biradical is adsorbed on the γ-Al2O3 surface, complex formation is complicated because of steric hindrance preventing bidentate coordination. Springer Science+Business Media, Inc. 2007.
Speciation in the AlCl3/SO2Cl2 catholyte system
Boyle, Timothy J.,Andrews, Nicholas L.,Alam, Todd M.,Tallant, David R.,Rodriguez, Mark A.,Ingersoll, David
, p. 5934 - 5940 (2005)
The fundamental chemical behavior of the AlCl3/SO 2Cl2 catholyte system was investigated using 27Al NMR spectroscopy, Raman spectroscopy, and single-crystal X-ray diffraction. Three major Al-containing species were found to be present in this catholyte system, where the ratio of each was dependent upon aging time, concentration, and/or storage temperature. The first species was identified as [Cl2Al(μ-Cl)]2 in equilibrium with AlCl3. The second species results from the decomposition of SO2Cl 2 which forms Cl2(g) and SO2(g). The SO 2(g) is readily consumed in the presence of AlCl3 to form the crystallographically characterized species [Cl2Al(μ-O 2SCl)]2 (1). For 1, each Al is tetrahedrally (T d) bound by two terminal Cl and two μ-O ligands whereas, the S is three-coordinated by two μ-O ligands and one terminal Cl. The third molecular species also has Td-coordinated Al metal centers but with increased oxygen coordination. Over time it was noted that a precipitate formed from the catholyte solutions. Raman spectroscopic studies show that this gel or precipitate has a component that was consistent with thionyl chloride. We have proposed a polymerization scheme that accounts for the precipitate formation. Further NMR studies indicate that the precipitate is in equilibrium with the solution.
Phase diagrams of some non-quasi-binary joins of the AlCl 3-BiCl3-NaCl system
Kaloev,Turieva
, p. 312 - 314 (2009)
Phase diagrams of NaAlCl4-(70.0 mol % AlCl3 + 30.0 mol % BziCl3), NaAlCl4-(34.2 mol % AlCl3 + 65.8 mol % BiCl3), and (61.0 mol % AlCl3 + 39.0 mol % NaCl)-AlCl3 ? BiCl
AlN substrates: Fabrication via vapor phase growth and characterization
Melnik,Soukhoveev,Ivantsov,Sizov,Pechnikov,Tsvetkov,Kovalenkov,Dmitriev,Nikolaev,Kuznetsov,Silveira,Freitas Jr.
, p. 22 - 25 (2003)
A new vapor phase crystal growth technique was applied to fabricate single crystal AlN wafers up to 1.75-inch diameter. The wafers were sliced from AlN crystals and polished. Fabricated AlN wafers were investigated by X-ray diffraction, TEM, and cathodoluminescence. X-ray diffraction and TEM studies confirmed single crystal structure of grown material. High electrical resistivity of these AlN wafers was verified. AlN homoepitaxial layers exhibiting sharp near-band-edge emission were grown on fabricated AlN substrates. These results open the door for the commercialization of AlN substrates for advanced high-power mm-wave devices and optoelectronic devices based on Group III-nitride semiconductors.
Synthesis in ionic liquids: [Bi2Te2Br](AlCl 4), a direct gap semiconductor with a cationic framework
Biswas, Kanishka,Zhang, Qichun,Chung, In,Song, Jung-Hwan,Androulakis, John,Freeman, Arthur J.,Kanatzidis, Mercouri G.
, p. 14760 - 14762 (2010)
The Lewis acidic ionic liquid EMIMBr-AlCl3 (EMIM = 1-ethyl-3-methylimidazolium) allows a novel synthetic route to the semiconducting layered metal chalcogenides halide [Bi2Te 2Br]-(AlCl4) and its Sb analogue. [Bi2Te 2Br](AlCl4) is a direct band gap, strongly anisotropic semiconductor and consists of cationic infinite layers of [Bi2Te 2Br]+ and [AlCl4] anions inserted between the layers.
New luminescent terbium complex for the determination of DNA
Yegorova, Alla,Karasyov, Alexander,Duerkop, Axel,Ukrainets, Igor,Antonovich, Valery
, p. 109 - 116 (2005)
New terbium complexes of derivatives of 2-oxo-4-hydroxy-quinoline-3- carboxylic acid are reported, which are highly luminescent, water soluble and do not require luminescence enhancers. The triplet-state energy levels of the ligands, the relative quantum yields (QYs) and the excitation maxima of the respective terbium chelates were determined. The large luminescence enhancement of one of these complexes by nucleic acids was investigated and a mechanism of its interaction with DNA is proposed. The optimal conditions for determination of DNA are equal concentrations of Tb3+ and ligand R1 (C = 1 × 10-6 M), pH 9.0. Under optimal conditions the luminescence intensity (RI) is proportional to the concentration of fish sperm DNA (fsDNA) or calf thymus DNA (ctDNA), respectively, within the range of 0.05-1.5 μg ml-1. The detection limits were 10ng ml-1 for fsDNA and 12 ng mr-1 for ctDNA.
Dawson, G. A.
, p. 133 (1928)
Regioselective Synthesis of 1,5-Disubstituted 1,2,3-Triazoles by Reusable AlCl3 Immobilized on γ-Al2O3
Nanjundaswamy, Hemmaragala M.,Abrahamse, Heidi
supporting information, p. 967 - 974 (2015/03/30)
(Chemical Equation Presented) There is rapidly growing interest in the synthesis and use of substituted 1,2,3-triazoles. We report an easy and interesting procedure that demonstrates the effectiveness of surface-modified γ-Al2O3, which is reusable, efficient, catalytic, safe, and environmentally acceptable for the regioselective synthesis of 1,5-disubstituted-1,2,3-triazoles via [3 + 2] cycloaddition of phenyl and benzyl azides with a series of aryl nitroolefins in good yields. No adverse effect on substituents such as nitro, cyano, hydroxy, ether linkage, and halogens was observed. The catalyst could easily be recycled and was reused for nine runs without losing its activity.
High quality Al-doped ZnO thin films deposited using targets prepared by chemical coprecipitation
Cai,Jiang,Zhu,Wang
, p. 1461 - 1464 (2010/02/15)
In order to grow high-quality aluminum-doped zinc oxide films (AZO), the chemical coprecipitation method was adopted to synthesize ultra-fine AZO powder, in which Al2O3O was more easily and more uniformly doped in ZnO compared to the