Inorganic Chemicals

Formula: AlCl3; MW 133.31; Structure and bonding: an electron-deficient compound, a Lewis acid, occurs as dimer Al2Cl6 in hexagonal crystal form. Above 300 °C, dissociation to monomer AlCl3 begins; completely dissociates to AlCl3 at 1,100°C.

Uses
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.

Physical Properties
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.

Thermochemical Data

ΔH°ƒ(s)      –168.3 kcal/mol
ΔG°ƒ(s)      –150.3 kcal/mol
S°              26.45 cal/deg mol
Hsoln.      –77.7 kcal/mol
Hfus         8.45 kcal/mol

Preparation
Aluminum chloride is made by chlorination of molten aluminum at temperatures between 650 to 750°C;

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.

Reactions
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,

Hazard
Violent exothermic reactions can occur when mixed with water or alkene. Corrosive to skin.

Formula: AlCl3•6H2O; MW 241.31

Uses
The hexahydrate is used in the preparation of deodorant and antiperspirant. Also, it is applied in textile finishing to improve the antistatic characteristics and flammability ratings of various textile materials. Commercially, it is sold as crystalline powder or as a 28% solution in water.

Physical Properties
White or yellowish deliquescent powder; faint odor of HCl; density 2.40 g/cm3; soluble in water and polar organic solvents such as alcohol; aqueous solution acidic.

Preparation
Aluminum chloride hexahydrate is prepared by dissolving Al(OH)3 in conc. HCl and passing gaseous HCl through the solution at 0°C. The precipitate is washed with diethyl ether and dried. Alternatively, it is prepared by hydrolyzing anhydrous AlCl3 in cold dilute HCl.

Reactions
Decomposes to alumina when heated at 300°C;

Reacts with caustic soda solution forming gelatinous precipitate of aluminum hydroxide (hydrous aluminum oxide); yields aluminum monobasic stearate, Al(OH)2[OOC(CH2)16CH3] when its solution is mixed with a solution of sodium stearate.

Formula AlH3; MW 30.005; Structure: polymeric, containing residual ether;

Uses
It is used as a reducing agent, and also as a catalyst for polymerization reaction.

Physical and Thermochemical Properties
Colorless cubic crystal; very unstable; decomposes in water; ΔΗ°ƒ −11.0 kcal/mol (-46.0kJ/mol)

Preparation
Aluminum hydride is prepared by the reaction of lithium hydride with aluminum chloride in diethyl ether

Chemical Reactions
Aluminum hydride decomposes in air and water. Violent reactions occur with both. It forms a complex, aluminum diethyl etherate with diethyl ether. The product decomposes in water releasing heat.

AlH3 + (C2H5)2O ——›H3Al•O(C2H5)2

Similar complexes are likely to form with other lower aliphatic ethers. It also forms a 1:1 complex with trimethyl amine, H3Al•N(CH3)3 which reacts explosively with water (Ruff 1967).
Aluminum hydride reduces CO2 to methane under heating:

Reaction with lithium hydride in ether produces lithium aluminum hydride,

Safety
Many reactions of aluminum hydride or its complexes may proceed with explosive violence, especially with water or moist air.

Formula: Al(NO3)3; MW 213.00; the anhydrous salt is covalent; also occurs as hydrated salts, Al(OH)(NO3)2, Al(OH)2NO3, and the more stable nonahydrate, Al(NO3)3 •9H2O [7784-27-2]

Uses
The nonahydrate and other hydrated aluminum nitrates have many applications. These salts are used to produce alumina for preparation of insulating papers, in cathode tube heating elements, and on transformer core laminates. The hydrated salts are also used for extraction of actinide elements.

Physical Properties
White or colorless crystalline solid (nonahydrate – rhombic crystal); deliquescent; refractive index 1.54; melts at 73.5°C; decomposes at 150°C; highly soluble in cold water (63.7% at 25°C), decomposes in hot water, soluble in polar organic solvents.

Preparation
The nonahydrate is prepared by treating aluminum, aluminum hydroxide, aluminum oxide, or aluminous mineral with nitric acid. The nitrate is crystallized from the solution.

Reactions
Since Al(NO3)3 or its salt hydrates dissociates to Al3+ and NO3– ions in the aqueous solution, its reactions in solutions are those of Al3+ . It is partially hydrolyzed, producing H3O+ and thus accounting for the acidity of its solution in water. The products constitute a complex mixture of mono- and polynuclear hydroxo species.
Aluminum nitrate is soluble in bases, forming aluminates, [Al(OH)4(H2O)2]–. It decomposes to Al2O3 when heated at elevated temperatures.

Chemical Analysis
Elemental composition: Al 12.67%, N 19.73%, O 67.60%. Al may be analyzed by various instrumental techniques, including atomic absorption or emission spectroscopy, or colorimetry (see under Aluminum). The nitrate anion in aqueous phase may be measured by the NO3– ion selective electrode, ion chromatography, or reduction with cadmium or hydrazine, followed by colorimetric tests.

Formula: AlN; MW 40.99

Uses
Aluminum nitride is used in manufacturing of steel and in semiconductors.

Physical Properties
White crystalline solid, hexagonal; odor of ammonia in moist air; sublimes at 2000°C; melts in N2 atmosphere over 2200°C; density 3.26 g/cm3 ; decomposes in water, alkalies and acids

Thermochemical Properties

ΔH°ƒ(s)          –76.0 kcal/mol
ΔG°ƒ(s)          –68.6 kcal/mol
S°                  4.82 cal/degree mol
Cρ                 7.20 cal/degree mol

Preparation
Aluminum nitride may be prepared in the laboratory by heating powdered aluminum metal with nitrogen.

Commercially, it is made by heating an aluminous mineral, such as, bauxite with coal in a stream of nitrogen.

Chemical Reactions
The nitride reacts with water forming aluminum hydroxide and ammonia.

AlN + 3H2O ——›Al(OH)3 + NH3

The compound decomposes in alkalies and acids forming products of complex stoichiometry.

Analysis
Elemental composition: Al 65.82%, N 34.18%, the metal is determined by wet analysis or AA spectroscopy. NH3 liberated on hydrolysis may be determined by titration or colorimetry (see under Ammonia).