7429-90-5

Usage

Uses

Used in Construction Industry:
Aluminum is used as a structural material for its lightness, strength, and corrosion resistance. It is used in building frameworks, window and door frames, and roofing.
Used in Automotive Industry:
Aluminum is used in vehicle construction for its strength-to-weight ratio, which improves fuel efficiency and reduces emissions.
Used in Electrical Industry:
Aluminum is used in electrical transmission lines due to its good electrical conductivity and light weight.
Used in Aircraft Industry:
Aluminum is used in aircraft construction for its high strength-to-weight ratio, which improves fuel efficiency and reduces overall weight.
Used in Home and Automobile Industries:
Aluminum is used to make cans for food and drinks, in pyrotechnics, for protective coatings, and to resist corrosion.
Used in Cooking Utensils:
Aluminum is used in cooking utensils for its good heat conductivity and non-reactive properties.
Used in Highway Signs, Fencing, Containers, and Packaging:
Aluminum is used in these applications for its durability, corrosion resistance, and light weight.
Used in Machinery and Corrosion-Resistant Chemical Equipment:
Aluminum is used in these applications for its strength, corrosion resistance, and light weight.
Used in Dental Alloys:
Aluminum is used in dental alloys for its non-toxicity and compatibility with other metals.
Used in Aluminothermics (Thermite Process):
Aluminum powder is used in the thermite process for producing high temperatures and reactive metals.
Used in Photography:
Aluminum powder is used in flash lights due to its bright, intense light output.
Used in Explosives and Fireworks:
Aluminum powder is used in explosives and fireworks for its high energy output and bright light.
Used in Paints:
Aluminum powder is used in paints for its bright, reflective properties.
Used in Steel Manufacturing:
Aluminum powder is used to absorb occluded gases during the manufacture of steel.
Used in Testing for Gold, Arsenic, and Mercury:
Aluminum is used in chemical tests for detecting the presence of these elements.
Used in Coagulating Colloidal Solutions:
Aluminum is used to coagulate colloidal solutions of arsenic or antimony.
Used in Precipitating Copper:
Aluminum is used as a reducing agent for precipitating copper.
Used in Determining Nitrates and Nitrites:
Aluminum is used as a reducer in chemical tests for determining the presence of nitrates and nitrites.
Used in Generating Hydrogen:
Aluminum is used as a substitute for zinc in generating hydrogen in tests for arsenic.
Used in Preparative Organic Chemistry:
Aluminum forms complex hydrides with lithium and boron, such as LiAlH4, which are used in preparative organic chemistry.
Used in Agricultural Applications:
Aluminum is an important soil constituent, but it can be toxic to plants at low pH levels. It can interfere with nutrient uptake and root growth in acidic soils.
Used in Manufacturing Synthetic Rubies and Sapphires:
Aluminum oxide is used to make synthetic rubies and sapphires for laser beams.
Used in Pharmaceutical Applications:
Aluminum has many pharmaceutical uses, including ointments, toothpaste, deodorants, and shaving creams.

Production Methods

Most aluminum is produced from its ore, bauxite, which contains between 40 to 60% alumina either as the trihydrate, gibbsite, or as the monohydrate, boehmite, and diaspore. Bauxite is refined first for the removal of silica and other impurities. It is done by the Bayer process. Ground bauxite is digested with NaOH solution under pressure, which dissolves alumina and silica, forming sodium aluminate and sodium aluminum silicate. Insoluble residues containing most impurities are filtered out. The clear liquor is then allowed to settle and starch is added to precipitate. The residue, so-called “red-mud”, is filtered out. After this “desilication,” the clear liquor is diluted and cooled. It is then seeded with alumina trihydrate (from a previous run) which promotes hydrolysis of the sodium aluminate to produce trihydrate crystals. The crystals are filtered out, washed, and calcined above 1,100°C to produce anhydrous alumina. The Bayer process, however, is not suitable for extracting bauxite that has high silica content (>10%). In the Alcoa process, which is suitable for highly silicious bauxite, the “red mud” is mixed with limestone and soda ash and calcined at 1,300°C. This produces “lime-soda sinter” which is cooled and treated with water. This leaches out water-soluble sodium alumnate, leaving behind calcium silicate and other impurites. Alumina may be obtained from other minerals, such as nepheline, sodium potassium aluminum silicate, by similar soda lime sintering process.Metal aluminum is obtained from the pure alumina at 950 to 1000°C electrolysis (Hall-Heroult process). Although the basic process has not changed since its discovery, there have been many modifications. Aluminum is also produced by electrolysis of anhydrous AlCl3. Also, the metal can be obtained by nonelectrolytic reduction processes. In carbothermic process, alumina is heated with carbon in a furnace at 2000 to 2500°C. Similarly, in “Subhalide” process, an Al alloy, Al-Fe-Si-, (obtained by carbothermic reduction of bauxite) is heated at 1250°C with AlCl vapor. This forms the subchloride (AlCl), the vapor of which decomposes when cooled to 800°C.

Production Methods

Aluminum production involves four main steps: bauxite mining,refining of bauxite to yield alumina; electrolytic reduction of alumina to yield aluminum; and aluminum casting into ingots.

Isotopes

There are 23 isotopes of aluminum, and only one of these is stable. The singlestable isotope, Al-27, accounts for 100% of the element’s abundance in the Earth’scrust. All the other isotopes are radioactive with half-lives ranging from a few nanosecondsto 7.17×10+15 years.

Origin of Name

From the Latin word alumen, or aluminis, meaning “alum,” which is a bitter tasting form of aluminum sulfate or aluminum potassium sulfate.

Characteristics

Alloys of aluminum are light and strong and can easily be formed into many shapes—thatis, it can be extruded, rolled, pounded, cast, and welded. It is a good conductor of electricityand heat. Aluminum wires are only about 65% as efficient in conducting electricity as arecopper wires, but aluminum wires are significantly lighter in weight and less expensive thancopper wires. Even so, aluminum wiring is not used in homes because of its high electricalresistance, which can build up heat and may cause fires.Aluminum reacts with acids and strong alkali solutions. Once aluminum is cut, the freshsurface begins to oxidize and form a thin outer coating of aluminum oxide that protects themetal from further corrosion. This is one reason aluminum cans should not be discarded inthe environment. Aluminum cans last for many centuries (though not forever) because atmosphericgases and soil acids and alkalis react slowly with it. This is also the reason aluminumis not found as a metal in its natural state.

History

The ancient Greeks and Romans used alum in medicine as an astringent, and as a mordant in dyeing. In 1761 de Morveau proposed the name alumine for the base in alum, and Lavoisier, in 1787, thought this to be the oxide of a still undiscovered metal. Wohler is generally credited with having isolated the metal in 1827, although an impure form was prepared by Oersted two years earlier. In 1807, Davy proposed the name alumium for the metal, undiscovered at that time, and later agreed to change it to aluminum. Shortly thereafter, the name aluminium was adopted to conform with the “ium” ending of most elements, and this spelling is now in use elsewhere in the world. Aluminium was also the accepted spelling in the U.S. until 1925, at which time the American Chemical Society officially decided to use the name aluminum thereafter in their publications. The method of obtaining aluminum metal by the electrolysis of alumina dissolved in cryolite was discovered in 1886 by Hall in the U.S. and at about the same time by Heroult in France. Cryolite, a natural ore found in Greenland, is no longer widely used in commercial production, but has been replaced by an artificial mixture of sodium, aluminum, and calcium fluorides. Bauxite, an impure hydrated oxide ore, is found in large deposits in Jamaica, Australia, Suriname, Guyana, Russia, Arkansas, and elsewhere. The Bayer process is most commonly used today to refine bauxite so it can be accommodated in the Hall–Heroult refining process used to make most aluminum. Aluminum can now be produced from clay, but the process is not economically feasible at present. Aluminum is the most abundant metal to be found in the Earth’s crust (8.1%), but is never found free in nature. In addition to the minerals mentioned above, it is found in feldspars, granite, and in many other common minerals. Twenty-two isotopes and isomers are known. Natural aluminum is made of one isotope, 27Al. Pure aluminum, a silvery- white metal, possesses many desirable characteristics. It is light, nontoxic, has a pleasing appearance, can easily be formed, machined, or cast, has a high thermal conductivity, and has excellent corrosion resistance. It is nonmagnetic and nonsparking, stands second among metals in the scale of malleability, and sixth in ductility. It is extensively used for kitchen utensils, outside building decoration, and in thousands of industrial applications where a strong, light, easily constructed material is needed. Although its electrical conductivity is only about 60% that of copper, it is used in electrical transmission lines because of its light weight. Pure aluminum is soft and lacks strength, but it can be alloyed with small amounts of copper, magnesium, silicon, manganese, and other elements to impart a variety of useful properties. These alloys are of vital importance in the construction of modern aircraft and rockets. Aluminum, evaporated in a vacuum, forms a highly reflective coating for both visible light and radiant heat. These coatings soon form a thin layer of the protective oxide and do not deteriorate as do silver coatings. They have found application in coatings for telescope mirrors, in making decorative paper, packages, toys, and in many other uses. The compounds of greatest importance are aluminum oxide, the sulfate, and the soluble sulfate with potassium (alum). The oxide, alumina, occurs naturally as ruby, sapphire, corundum, and emery, and is used in glassmaking and refractories. Synthetic ruby and sapphire have found application in the construction of lasers The Elements 4-3 for producing coherent light. In 1852, the price of aluminum was about $1200/kg, and just before Hall’s discovery in 1886, about $25/kg. The price rapidly dropped to 60￠ and has been as low as 33￠/kg. The price in December 2001 was about 64￠/ lb or $1.40/kg.

Air & Water Reactions

Violent reaction with water; contact may cause an explosion or may produce a flammable gas (hydrogen). Moist air produces hydrogen gas. Does not burn on exposure to air.

Reactivity Profile

ALUMINUM , MOLTEN, is a reducing agent. Coating moderates or greatly moderates its chemical reactivity compared to the uncoated material. Reacts exothermically if mixed with metal oxides and heated (thermite process). Heating a mixture with copper oxides caused a strong explosion [Mellor 5:217-19 1946-47]. Reacts with metal salts, mercury and mercury compounds, nitrates, sulfates, halogens, and halogenated hydrocarbons to form compounds that are sensitive to mechanical shock [Handling Chemicals Safely 1980. p. 135]. A number of explosions in which ammonium nitrate and powdered aluminum were mixed with carbon or hydrocarbons, with or without oxidizing agents, have occurred [Mellor 5:219 1946-47]. A mixture with powdered ammonium persulfate and water may explode [NFPA 491M 1991]. Heating a mixture with bismuth trioxide leads to an explosively violent reaction [Mellor 9:649 (1946-47)]. Mixtures with finely divided bromates(also chlorates and iodates) of barium, calcium, magnesium, potassium, sodium or zinc can explode by heat, percussion, and friction, [Mellor 2:310 (1946-47]. Burns in the vapor of carbon disulfide, sulfur dioxide, sulfur dichloride, nitrous oxide, nitric oxide, or nitrogen peroxide, [Mellor 5:209-212,1946-47]. A mixture with carbon tetrachloride exploded when heated to 153° C and also by impact, [Chem. Eng. News 32:258 (1954)]; [UL Bull. Research 34 (1945], [ASESB Pot. Incid. 39 (1968)]. Mixing with chlorine trifluoride in the presence of carbon results in a violent reaction [Mellor 2 Supp. 1: 1956]. Ignites in close contact with iodine. Three industrial explosions involving a photoflash composition containing potassium perchlorate with aluminum and magnesium powder have occurred [ACS 146:210 1945], [NFPA 491M 1991]. Is attacked by methyl chloride in the presence of small amounts of aluminum chloride to give flammable aluminum trimethyl. Give a detonable mixture with liquid oxygen [NFPA 491M 1991]. The reaction with silver chloride, once started, proceeds with explosive violence [Mellor 3:402 1946-47]. In an industrial accident, the accidental addition of water to a solid mixture of sodium hydrosulfite and powdered aluminum caused the generation of SO2, heat and more water. The aluminum powder reacted with water and other reactants to generate more heat, leading to an explosion that killed five workers [Case Study, Accident Investigation: Napp Technologies, 14th International Hazardous Material Spills Conference].

Hazard

Aluminum dust and fine powder are highly explosive and can spontaneously burst intoflames in air. When treated with acids, aluminum chips and coarse powder release hydrogen.The heat from the chemical reaction can then cause the hydrogen to burn or explode. Purealuminum foil or sheet metal can burn in air when exposed to a hot enough flame. Fumesfrom aluminum welding are toxic if inhaled.

Health Hazard

Exposures to aluminum metallic powder have been known to cause health effects with symptoms such as irritation, redness, and pain to the eyes, coughing, shortness of breath, irritation to the respiratory tract, nausea, and vomiting in extreme cases. In prolonged periods of inhalation exposures, as in occupational situations, aluminum metallic powder is known to cause pulmonary fi brosis, numbness in fi ngers, and (in limited cases) brain effects. Workers with pre-existing skin disorders, eye problems, or impaired respiratory function are known to be more susceptible to the effects of aluminum metallic powder.

Fire Hazard

Substance is transported in molten form at a temperature above 705°C (1300°F). Violent reaction with water; contact may cause an explosion or may produce a flammable gas. Will ignite combustible materials (wood, paper, oil, debris, etc.). Contact with nitrates or other oxidizers may cause an explosion. Contact with containers or other materials, including cold, wet or dirty tools, may cause an explosion. Contact with concrete will cause spalling and small pops.

Safety Profile

Although aluminum is not generally regarded as an industrial poison, inhalation of finely dwided powder has been reported to cause pulmonary fibrosis. It is a reactive metal and the greatest industrial hazards are with chemical reactions. As with other metals the powder and dust are the most dangerous forms. Dust is moderately flammable and explosive by heat, flame, or chemical reaction with powerful oxidizers. To fight fire, use special mixtures of dry chemical. following dangerous interactions: explosive reaction after a delay period with KClO4 + Ba(NO3)2 + mo3 + H20, also with Ba(NO3)2 + mo3 + sulfur + vegetable adhesives + H2O. Wxtures with powdered AgCl, NH4NO3 or NH4NO3 + Ca(NO3)2 + formamide + H20 are powerful explosives. Murture with ammonium peroxodisulfate + water is explosive. Violent or explosive "thermite" reaction when heated with metal oxides, oxosalts (nitrates, sulfates), or sulfides, and with hot copper oxide worked with an iron or steel tool. Potentially explosive reaction with ccl4 during ball milling operations. Many violent or explosive reactions with the following halocarbons have occurred in industry: bromomethane, bromotrifluoromethane, ccl4, chlorodfluoromethane, chloroform, chloromethane, chloromethane + 2methylpropane, dchlorodifluoromethane, 1,2-dichloroethane, dichloromethane, 1,2dichloropropane, 1,2-difluorotetrafluoroethane, fluorotrichloroethane, hexachloroethane + alcohol, polytrifluoroethylene oils and greases, tetrachloroethylene, tetrafluoromethane, 1,1,1trichloroethane, trichloroethylene, 1,1,2trichlorotrifluoro-ethane, and trichlorotrifluoroethane-dchlorobenzene. Potentially explosive reaction with chloroform amidinium nitrate. Ignites on contact with vapors of AsCl3, SC4, Se2Cl2, and PCl5. Reacts violently on heating with Sb or As. Ignites on heating in SbCl3 vapor. Ignites on contact with barium peroxide. Potentially violent reaction with sodium acetylide. Mixture with sodum peroxide may ignite or react violently. Spontaneously igmtes in CS2 vapor. Halogens: ignites in Powdered aluminum undergoes the chlorine gas, foil reacts vigorously with liquid Br2, violent reaction with H20 + 12. Violent reaction with hydrochloric acid, hydro-fluoric acid, and hydrogen chloride gas. Violent reaction with disulfur dbromide. Violent reaction with the nonmetals phosphorus, sulfur, and selenium. Violent reaction or ignition with the interhalogens: bromine pentafluoride, chlorine fluoride, iodne chloride, iodine pentafluoride, and iodne heptafluoride. Burns when heated in CO2. Ignites on contact with O2, and mixtures with O2 + H20 ignite and react violently. Mixture with picric acid + water ignites after a delay period. Explosive reaction above 800°C with sodium sulfate. Violent reaction with sulfur when heated. Exothermic reaction with iron powder + water releases explosive hydrogen gas. Aluminum powder also forms sensitive explosive mixtures with oxidants such as: liquid Cl2 and other halogens, N2O4, tetranitromethane, bromates, iodates, NaClO3, KClO3, and other chlorates, NaNO3, aqueous nitrates, KClO4 and other perchlorate salts, nitryl fluoride, ammonium peroxodisulfate, sodium peroxide, zinc peroxide, and other peroxides, red phosphorus, and powdered polytetrafluoroethylene (PTFE). following dangerous interactions: exothermic reaction with butanol, methanol, 2-propanol, or other alcohols, sodium hydroxide to release explosive hydrogen gas. Reaction with dborane forms pyrophoric product. Ignition on contact with niobium oxide + sulfur. Explosive reaction with molten metal oxides, oxosalts (nitrates, sulfates), sulfides, and sodium carbonate. Reaction with arsenic trioxide + sodum arsenate + sodium hydroxide produces the toxic arsine gas. Violent reaction with chlorine trifluoride. Incandescent reaction with formic acid. Potentially violent alloy formation with palladium, platinum at mp of Al, 600℃. Vigorous dssolution reaction in Bulk aluminum may undergo the ALUMINUM CHLORIDE HYDROXIDE AHAOOO 45 methanol + carbon tetrachloride. Vigorous amalgamation reaction with mercury(Ⅱ) salts + moisture. Violent reaction with molten silicon steels. Violent exothermic reaction above 600℃ with sodium diuranate.

Carcinogenicity

Most animal studies have failed to demonstrate carcinogenicity attributable to aluminum administered by various routes in rats, rabbits, mice, and guinea pigs. Some of these studies even suggested some antitumor activity. However, aluminum was found to cause cancer in a few experimental studies such as sarcomas in rats when implanted subcutaneously. This observation was attributed to the dimensions of the implants rather than the chemical composition. Significantly increased incidence of gross tumors was reported in male Long Evans rats and lymphoma leukemia in female Swiss mice given aluminum potassium sulfate in drinking water respectively for 2–2.5 years. A dose–response relationship could not be determined for either species because only one dose of aluminum was used and the type of tumors and organs in which they were found were not specified.

Environmental Fate

Aluminum binds diatomic phosphates and possibly depletes phosphate, which can lead to osteomalacia. High aluminum serum values and high aluminum concentration in the bone interfere with the function of vitamin D. The incorporation of aluminum in the bone may interfere with deposition of calcium; the subsequent increase of calcium in the blood may inhibit release of parathyroid hormones by the parathyroid gland. The mechanism by which aluminum concentrates in the brain is not known; it may interfere with the blood brain barrier.

storage

Aluminum metallic powder should be kept stored in a tightly closed container, in a cool, dry, ventilated area, protected against physical damage and isolated from sources of heat, ignition, smoking areas, and moisture. Aluminum metallic powder should be kept away from acidic, alkaline, combustible, and oxidizing materials and separate from halogenated compounds.

Toxicity evaluation

Aluminum cannot be degraded in the environment in its elemental state, but can undergo various precipitation or ligand exchange reactions. The solubility of aluminum in the environment depends on the ligands present and the pH. Long-range transport The major feature cycle of aluminum include leaching of aluminum from geochemical formations and soil particulates to aqueous environments, adsorption onto soil or sediment particulates, and wet and dry deposition from the air to land and surface water. Bioaccumulation and biomagnification Aluminum does not bioaccumulate to a significant extent. Thus, certain plants can accumulate high concentrations of aluminum. Plant matter like tea leaves may contain >5000 mg kg-1 of aluminum. Lycopodium, some fern species, and members of genera Symplocos or Orites may contain high levels of aluminum. It does not appear to accumulate to any significant degree in cow’s milk or beef tissue, and it is therefore not expected to undergo biomagnification in terrestrial food chains.

Precautions

The dry powder is stable but the damp or moist bulk dust may heat spontaneously and form flammable hydrogen gas. Moist aluminum powder may ignite in air, with the formation of flammable hydrogen gas and a combustible dust. Powdered material may form explosive dust-air mixtures. Contact with water, strong acids, strong bases, or alcohols releases flammable hydrogen gas. The dry powder can react violently or explosively with many inorganic and organic chemicals

InChI:InChI=1/Al

Synthetic route

aluminium trichloride (7446-70-0) → aluminium (7429-90-5)

Conditions	Yield
With hydrogen In neat (no solvent) byproducts: HCl; other Radiation; AlCl3 powder placed in quartz tube; tube evacuated and flushed with Ar and then heated under Ar/H2 flow to 90°C; rf discharge ignited for20 min and tube then cooled; XRD;	100%
With potassium In neat (no solvent) heating AlCl3 in a rectangular glass tube and passing the vapor over pieces of K in the horizontal part of the tube;;
With lithium hydride; 1-ethyl-3-methyl-1H-imidazol-3-ium chloride In neat (no solvent) mixed by stirring; deposited at 25-45°C for 15 min - 2 h;

bis(η6-diphenyl)chromium(0) (12099-15-9) + aluminium bromide (7727-15-3) → {(C6H5C6H5)2Cr}(1+)*AlBr4(1-)*0.25C6H6={(C6H5C6H5)2Cr}AlBr4*0.25C6H6 + aluminium (7429-90-5)

Conditions	Yield
In benzene at room temp.;	A 92% B n/a
In benzene at room temp.;	A 92% B n/a

trimethylamine alane (16842-00-5, 855944-65-9) → aluminium (7429-90-5)

Conditions	Yield
With hydrogen In 1,2,5-trimethyl-benzene High Pressure; a soln. of Al complex degassed, pressurized with 3 bar of H2, heated to 150°C for 1 h; allowed to settle, the supernatant removed, washed (n-pentane), dried (vac.); obtained as nanoparticles;	86%
With hydrogen In further solvent(s) byproducts: N(CH3)3; High Pressure; pressurized with 3 bar of H2 in mesitylene-d12, heated to 150°C for 1 h;
byproducts: N(CH3)3, H2; film deposition using CVD method (P<1E-6 Torr, gold covered quartz crystal, Teflon, silicon or gallium arsenide as substrates, laser at 5 or 500mW, cooling with liq. N2); SEM;

aluminium trichloride (7446-70-0) + bis(η6-toluene)titanium(0) (55527-82-7) → Ti(ηtoluene){(μ-Cl)2(AlCl2)}2 + aluminium (7429-90-5)

Conditions	Yield
In toluene under purified Ar atm.; AlCl3 added to soln. of Ti(η6-MeC6H5)2 in toluene; mixt. stirred for 18 h at room temp.; solid sepd. by filtration; washed (toluene); dried (vac.); identified asAl; soln. evapd. to dryness; solid washed (heptane); dried (vac.); iden tified as Ti-Al complex;	A 80% B 85%

decamethylsamarocene(II) bis(tetrahydrofurane) (79372-14-8) + trimethylaluminum (75-24-1) → tetrahydrofuran (109-99-9) + (C5Me5)2Sm{(μ-Me)AlMe2(μ-Me)}2Sm(C5Me5)2 (115756-72-4) + aluminium (7429-90-5)

Conditions	Yield
In toluene byproducts: methane; all manipulations conducted under nitrogen excluding air and water; after 24 h standing of the reaction mixt. the formed metallic-like ppt. was removed by filtration and washed with hot toluene, filtrates combined, solvent removed by rotary evapn.;; recrystn. (hot toluene), elem. anal.;;	A n/a B 80% C n/a

strontium(II) hydride + strontium tetrahydroaluminate → strontium pentahydroaluminate + hydrogen (1333-74-0) + aluminium (7429-90-5)

Conditions	Yield
In solid SrH2 mechanically treated for 3-4 h, mixed with AlH3 at molar ratio 1:1 in vibrating mechanical load, heated for 3-4 h; DTA-DGV, XRD, IR;	A 80% B n/a C n/a
In solid mechanolysis at 165-220°C; DTA-DGV, IR, XRD;

aluminum oxide (1333-84-2, 1344-28-1) + beryllium + aluminium (7429-90-5)

Conditions	Yield
In neat (no solvent) heating a 1:1 mixture up to 1280°C for 3h; formation of a mixture of the metals and oxides;;	A 64% B n/a

aluminium trichloride (7446-70-0) + (pentamethylcyclopentadienyl)Al (137013-38-8) → {(η5-C5Me5)2Al}{(η1-C5Me5)AlCl3} + aluminium (7429-90-5)

Conditions	Yield
In toluene under N2, after 3 days heated at 100°C for 15 h; slowly cooled;	A 50% B n/a

[1,3-(tBu)2(C5H3)]2Sm + aluminium hydride (7784-21-6) + aluminium hydride*TMEDA → (C5H3(C(CH3)3)2)5Sm4(AlH4)4H3((CH3)2NC2H4N(CH3)2)2 + aluminium (7429-90-5)

Conditions	Yield
In diethyl ether byproducts: H2; dropwise addn. of AlH3 in ether to soln. of Sm-compd. in diethyl ether, addn. of AlH3*TMEDA, stirred for 24 h; pptn. filtered off, filtrate concd., sepn. after 48 h, washed with pentane, dried in vac.; elem. anal.;	A 35% B n/a

aluminum(I) chloride + diethyl ether (60-29-7) + toluene (108-88-3) + lithium hexamethyldisilazane (4039-32-1) → 54Al*15Al(1+)*18N(SiC3H9)2(1-)*2Li(OC4H10)3(1+)*Li(OC4H10)4(1+)*1.5C6H5CH3=[Al69N18Si36C108H324](C40H100Li3O10)*1.5C7H8 + diethyl ether ; compound with aluminium trichloride (17634-40-1) + aluminium (7429-90-5)

Conditions	Yield
In diethyl ether; toluene byproducts: LiCl*3Et2O; soln. of AlCl in toluene/Et2O (3/1) was added to LiN(SiMe3)2 at -78°C; soln. was warmed to room temp. within 1 d; heated at 60°C for 1 h; filtered; soln. was left at 60°C for 2 mo; pptd.;	A 7% B n/a C n/a

aluminium hydride*(dibutyl ether)0.3 → AlH2OC3H6CH3 + aluminium (7429-90-5)

Conditions	Yield
In neat (no solvent) Kinetics; byproducts: O(C4H9)2, H2; thermal decompn. at 50-100°C; identification of products by IR;	A 5% B n/a

aluminum(I) chloride + diethyl ether (60-29-7) + toluene (108-88-3) + lithium hexamethyldisilazane (4039-32-1) → 54Al*15Al(1+)*18N(Si(CH3)3)2(1-)*3Li(O(C2H5)2)4(1+)*6C6H5CH3=[Al69(N(Si(CH3)3)2)18](Li(O(C2H5)2)4)3*6C6H5CH3 + diethyl ether ; compound with aluminium trichloride (17634-40-1) + aluminium (7429-90-5)

Conditions	Yield
In diethyl ether; toluene byproducts: LiCl*3Et2O; gaseous AlCl were condensed with toluene and diethyl ether at -196°C; soln. of AlCl*Et2O was added to LiN(SiMe3)2 at 25°C; mixt. was left for 1 h; filtered; soln. was heated at 60°C for 1.5 h; pptd.;	A 5% B n/a C n/a

Na/K alloy + triethylaluminum (97-93-8) → potassium tetraethylaluminate + sodium tetraethylaluminate (2397-68-4) + aluminium (7429-90-5)

Conditions	Yield
Stage #1: Na/K alloy; triethylaluminum at 85 - 90℃; for 1.25h; Stage #2: triethylaluminum In toluene at 60 - 80℃; for 4h; Product distribution / selectivity;
Stage #1: Na/K alloy; triethylaluminum at 87 - 95℃; for 3.5h; Stage #2: triethylaluminum In toluene at 20 - 88℃; for 1h; Product distribution / selectivity;
In toluene at 20 - 35℃; for 9.25h; Product distribution / selectivity;

lithium aluminium tetrahydride (16853-85-3) → hydrogen (1333-74-0) + lithium hydride + aluminium (7429-90-5)

Conditions	Yield
titanium(III) chloride at 90℃; for 5h; Product distribution / selectivity; Neat (no solvent); Balled milled;
In solid Kinetics; thermal decomposition of ball milled for various times or as-received LiAlH4; powder XRD;
chromium(VI) oxide In diethyl ether; toluene Kinetics; Catalytic decompn. of LiAlH4 in solution;

lithium aluminium tetrahydride (16853-85-3) → lithium hexahydroaluminate + hydrogen (1333-74-0) + aluminium (7429-90-5)

Conditions	Yield
titanium(III) chloride at 50 - 150℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
at 100 - 200℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
In neat (no solvent) 170°C - 220°C;
With magnesium hydride; titanium(II) hydride In neat (no solvent) at 54 - 171℃; Kinetics; Inert atmosphere;

magnesium hydride → hydrogen (1333-74-0) + magnesium (7439-95-4) + aluminium (7429-90-5)

Conditions	Yield
titanium(III) chloride at 250 - 350℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;

sodium aluminum tetrahydride → sodium alanate + hydrogen (1333-74-0) + aluminium (7429-90-5)

Conditions	Yield
titanium(III) chloride at 50 - 200℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
In neat (no solvent) in stainless steel reactor, at 480-490 K for 3 h, according to: E. C. Ashby, P. Kobertz, Inorg. Chem., 1966, 5, 1615.; XRD;
In neat (no solvent) on heating;
at 210℃;

sodium alanate → hydrogen (1333-74-0) + sodium hydride (7646-69-7) + aluminium (7429-90-5)

Conditions	Yield
titanium(III) chloride at 200 - 250℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
In neat (no solvent, solid phase) decompd. at heating;

lithium hexahydroaluminate → hydrogen (1333-74-0) + lithium hydride + aluminium (7429-90-5)

Conditions	Yield
titanium(III) chloride at 150 - 250℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
at 200 - 250℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
In solid 220°C - 275°C;

→ magnesium hydride + hydrogen (1333-74-0) + aluminium (7429-90-5)

Conditions	Yield
titanium(III) chloride at 50 - 250℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
at 100℃; under 760.051 Torr; Product distribution / selectivity; Neat (no solvent); Balled milled;
at 145 - 305℃;

Al12Mg17 + hydrogen (1333-74-0) + magnesium (7439-95-4) → magnesium hydride + aluminium (7429-90-5)

Conditions	Yield
hydrogenation at 30 bar H2 at 350°C for 0 to 24 h; detd. by XRD;

aluminum sulfide → aluminium (7429-90-5)

Conditions	Yield
With iron In neat (no solvent) Al2S3 is decomposed on Fe;; not isolated;;
With iron In neat (no solvent) Al2S3 is molten with iron shavings;;
With H2 or hydrocarbons reduction of Al2S3 by hydrogen or hydrocarbons;;

aluminum oxide (1333-84-2, 1344-28-1) + aluminum sulfide → aluminium (7429-90-5)

Conditions	Yield
byproducts: SO2;
With pyrographite In neat (no solvent) fractionated reduction; first portion: Al alloy with contaminating metalls (Si, Fe, Ti), second portion (using charcoal as reducing reagent):pure Al;;
With pyrographite In neat (no solvent) fractionated reduction; first portion: Al alloy with contaminating metalls (Si, Fe, Ti), second portion (using charcoal as reducing reagent):pure Al;;

aluminum oxide (1333-84-2, 1344-28-1) → aluminium nitride + aluminium carbide (1299-86-1) + aluminium (7429-90-5)

Conditions	Yield
With pyrographite In neat (no solvent) byproducts: graphite; Electric Arc; on heating in an electric arc; formation of Al4C3 containing Al2O3, AlN, Al and graphite;; yield of Al (at best: 30%) increases with decreasing cooling velocity;;
With pyrographite In neat (no solvent) on heating in an electric furnace; formation of Al4C3 containing Al2O3, AlN and Al;; yield of Al (at best: 30%) increases with decreaseing cooling velocity;;

aluminum oxide (1333-84-2, 1344-28-1) → aluminium carbide (1299-86-1) + aluminium (7429-90-5)

Conditions	Yield
With caebon In neat (no solvent) byproducts: CO; heating Al2O3 with carbon; formation of solid Al, Al2O3, and Al4C3 as product mixture with residual carbon; reaction mechanism discussed;;
With pyrographite In neat (no solvent) byproducts: CO; Electric Arc; reaction temp. above b.p. of Al at 1 atm; favouring by pressure or by elimination of CO by flushing with H or city gas;; best yield about 49g Al per 106g Al4C3;;
With pyrographite; calcium oxide In neat (no solvent) byproducts: CO; Electric Arc; heating with BaO or Sr-compunds; requirement of energy: 5kWh;;

aluminum oxide (1333-84-2, 1344-28-1) → aluminium (7429-90-5)

Conditions	Yield
With pyrographite In melt byproducts: CO, CO2; Electrolysis; in molten cryolite; coal-electrodes; decompn. voltage 1.2 V;;
Electrolysis; if Al2O3 contaminated with 0.45% (Fe2O3+SiO2), purity of product 99%, if with 0.15-0.25%, then 99.5%; other impurities: water (<1%), alkali (0.5-2%);
Electrolysis; impurities of Al2O3: water 0.18%, Fe2O3 0.04%, SiO2 0.05%, Na2O 0.18 %;

cadmium sulfate + aluminium (7429-90-5) → aluminum(III) sulfate + cadmium (7440-43-9)

Conditions	Yield
In water Al powder activated with HCl; pptn. of Cd;	A n/a B 100%
In water Al powder activated with HCl; pptn. of Cd;	A n/a B 100%
In water Al wire; incomplete pptn. of Cd; pptn. within some minutes in presence of sodium potassium tartrate;
In water Al wire; incomplete pptn. of Cd; pptn. within some minutes in presence of sodium potassium tartrate;

lithium (7439-93-2) + aluminium (7429-90-5) + silicon (7440-21-3) → lithium aluminium silicide

Conditions	Yield
In melt in a tantalum tube weld-seald under Ar and protected from air by a silica jacket sealed under vac.; mixt. Li, Al, Si (15:3:6 mol) heated at 1223K, 10 h in vertical furnace and shaken several times;; cooled at rate of 6 K h**-1; elem. anal.;	100%

(C4H9)4N(1+)*F(1-)*14HF*7H2O = (C4H9)4NF*14HF*7H2O + aluminium (7429-90-5) → (C4H9)4N(1+)*AlF4(1-) = (C4H9)4NAlF4 (115631-72-6)

Conditions	Yield
In acetonitrile Electrolysis; galvanostatic conditions (300 mA, 10-70 V, 1.7 Ah), aluminum anode, platinum cathode; filtn., evapn. (reduced pressure), recrystn. (Et2O/CHCl3 1:4); elem. anal.;	100%

lanthanum(III) bromide (13536-79-3) + aluminium (7429-90-5) → La4Br2Al5

Conditions	Yield
In neat (no solvent, solid phase) all manipulations under Ar atm.; stoich. mixt. of compds. sealed in Ta tubes then tubes sealed inside silica ampoules under vac. (ca. 1E-2 mbar), heated at 900°C for 10 d;	100%

[Ni(ammonia)6](2+) + aluminium (7429-90-5) → Al(3+)*4OH(1-)=Al(OH)4(1-) + nickel

Conditions	Yield
With Sulfate In further solvent(s) Kinetics; byproducts: NH3, H2; ammine Ni complex reacted with metallic Al in aq. soln. at pH 11.0-12.0; unreacted Al is removed by dissoln. in alkaline soln.;	A n/a B 99.9%
With Nitrate In further solvent(s) Kinetics; byproducts: NH3, H2; ammine Ni complex reacted with metallic Al in aq. soln. at pH 11.0-12.0;	A n/a B 0%

diphenylmercury(II) (587-85-9) + aluminium (7429-90-5) + zinc (7440-66-6) → diphenylzinc (1078-58-6) + triphenylaluminium (841-76-9)

Conditions	Yield
In neat (no solvent)	A 1% B 99%

hydrogenchloride (7647-01-0) + aluminium (7429-90-5) → aluminum(I) chloride

Conditions	Yield
In neat (no solvent) liquid Al reacted with HCl gas in graphite furnace in high vac. at 750°C (by Schnoeckel, H. Z. Naturforsch. 1976, 31b, 1291);	99%
In neat (no solvent) passing HCl gas over liq. Al at 1000°C and 1E-5 mbar;
In neat (no solvent) passing HCl over Al in graphite cell heated to 900°C;

isopropyl alcohol (67-63-0) + aluminium (7429-90-5) → AlCl3*4(CH3)2CHOH

Conditions	Yield
With hydrogen chloride org. compd. cooling to -80°C, satn. with hydrogen chloride for 3 h, metal turnings addn., mixt. heating under reflux condenser for 5-6 h,crystn. at room temp.; crystals sepn. from mother liquor, washing (isopropyl alcohol), recrystn. from alcohol; elem. anal.; X-ray diffraction;	99%

strontium + aluminium (7429-90-5) → SrAl2

Conditions	Yield
In melt under Ar atm. mixt. Sr and Al was pressed into pellets and arc-melted;	99%
In melt Electric Arc; remelted several times; XRD;
In melt Electric Arc; arc melting of elements with 3 wt. % excess of Sr, remelting four times;

germanium (7440-56-4) + rubidium pentasulfide + sulfur (7704-34-9) + aluminium (7429-90-5) → Rb3(AlS2)3(GeS2)7

Conditions	Yield
In neat (no solvent) stoich. amt. of Rb2S5, Al, Ge and S sealed in fused silica tube; heated at 850°C for 3 d; cooled to 400°C over 4 d; detd. by energy-dispersive X-ray analysis;	99%

rhodium (378784-00-0, 7440-16-6) + aluminium (7429-90-5) → Al0733Rh0267

Conditions	Yield
Stage #1: rhodium; aluminium In melt Electric arc; Inert atmosphere; Stage #2: at 999.84℃; for 72h; Sealed tube; Inert atmosphere; Stage #3: at 999.84℃; under 675068 Torr; for 0.333333h; Inert atmosphere;	99%

rhodium (378784-00-0, 7440-16-6) + iridium + aluminium (7429-90-5) → Al0.733(Rh0.75Ir0.25)0.267

Conditions	Yield
Stage #1: rhodium; iridium; aluminium In melt Electric arc; Inert atmosphere; Stage #2: at 999.84℃; for 72h; Sealed tube; Inert atmosphere; Stage #3: at 999.84℃; under 675068 Torr; for 0.333333h; Inert atmosphere;	99%

rhodium (378784-00-0, 7440-16-6) + iridium + aluminium (7429-90-5) → Al0.733(Rh0.5Ir0.5)0.267

Conditions	Yield
Stage #1: rhodium; iridium; aluminium In melt Electric arc; Inert atmosphere; Stage #2: at 999.84℃; for 72h; Sealed tube; Inert atmosphere; Stage #3: at 999.84℃; under 675068 Torr; for 0.333333h; Inert atmosphere;	99%

rhodium (378784-00-0, 7440-16-6) + iridium + aluminium (7429-90-5) → Al0.733(Rh0.25Ir0.75)0.267

Conditions	Yield
Stage #1: rhodium; iridium; aluminium In melt Electric arc; Inert atmosphere; Stage #2: at 999.84℃; for 72h; Sealed tube; Inert atmosphere; Stage #3: at 999.84℃; under 675068 Torr; for 0.333333h; Inert atmosphere;	99%

iridium + aluminium (7429-90-5) → Al0733Ir0267

Conditions	Yield
Stage #1: iridium; aluminium In melt Electric arc; Inert atmosphere; Stage #2: at 999.84℃; for 72h; Sealed tube; Inert atmosphere; Stage #3: at 999.84℃; under 675068 Torr; for 0.333333h; Inert atmosphere;	99%

ethene (74-85-1) + aluminium (7429-90-5) → triethylaluminum (97-93-8)

Conditions	Yield
With Na; Al2(C2H5)3Cl3 In not given byproducts: NaCl; NMR spect. anal.;	98.7%
With titanium; hydrogen at 120 - 130℃; under 2250.23 - 75007.5 Torr; for 13h;

aluminium (7429-90-5) + barium(II) oxide → barium (7440-39-3)

Conditions	Yield
5h in vac. at 1300-1340 °C; Metal distilles off. Repeated distn. gives 99.5% purity;	98.5%
4h in vac. at 1010-1030 °C; opening of apparatus under CO2, crushing of product under desiccated toluene to avoid self inflammation; Metal sublimes off. Repeated distn. gives 99.48% purity;
sublimation in vac.; 99.9% Ba;
sublimation in vac.; 99.9% Ba;

ethyl bromide (74-96-4) + aluminium (7429-90-5) → triethylaluminum (97-93-8)

Conditions	Yield
With Mg; Na In not given byproducts: MgBr2, NaBr; NMR spect. anal.;	98.2%

gallium (7440-55-3) + aluminium (7429-90-5) → aluminum gallium

Conditions	Yield
In neat (no solvent) Al and Ga metals were heated in sealed quartz tube to 700° and then cooled to room temp.;	98%
In neat (no solvent)
In neat (no solvent)
In neat (no solvent) melting Ga and Al in a porcelain tube in vac.;;

iodine (7553-56-2) + aluminium (7429-90-5) → aluminium(III) iodide (7784-23-8)

Conditions	Yield
In hexane thin foil of Al was suspended in degassed n-hexane under argon, 1.5 equiv. I2 was added, mixt. was boiled under reflux for 1-3 h; filtered into a heated receiver; elem. anal.;	96%
In further solvent(s) sheet aluminium in I2/ethyl iodide soln.;; impurities of I2;;
In neat (no solvent) addn. of Al to molten I2, ignition and melting of the metal;;

tetrahydrofuran (109-99-9) + aluminium (7429-90-5) → C12H24O3Al2

Conditions	Yield
With catalyst: HgCl2-ZnCl2-MeI In tetrahydrofuran refluxing (60°C, 5 h); addn. of benzene, filtration, evapn.; elem. anal.;	96%

tantalum(V) oxide + hafnium(IV) oxide + aluminium (7429-90-5) → Hf(b),Ta(185-19) (W%)

Conditions	Yield
With Al; KClO3; CaO In melt Electric Arc; thermit smelting; ball-milled powdered mixt. HfO2, Ta2O5, CaO, CaF2, KClO3 (10:1.2:4:3:6.5 wt.), 15% excess Al was poured inside MgO-lined steelreactor; ignition with burning Mg of trigger mixt. (KClO3:Al=2:1); also in Ar in copper double wall reactor; remelting by electron beam (2.7 kW, 1 h, vac. 3.9E-4 Pa) or arc melting (under Ar, tungsten electrode) to evap. Al excess; elem. anal.;	95.5%
With Al; KClO3; CaO In melt Electric Arc; thermit smelting; ball-milled powdered mixt. HfO2, Ta2O5, CaO, CaF2, KClO3 (10:1.2:4:3:6.5 wt.), 10% excess Al was poured inside MgO-lined steelreactor; ignition with burning Mg of trigger mixt. (KClO3:Al=2:1); also in Ar in copper double wall reactor; remelting by electron beam (2.7 kW, 1 h, vac. 3.9E-4 Pa) or arc melting (under Ar, tungsten electrode) to evap. Al excess; elem. anal.;	95%
With Al; KClO3; CaO In melt Electric Arc; thermit smelting; ball-milled powdered mixt. HfO2, Ta2O5, CaO, CaF2, KClO3 (10:1.2:4:3:6.5 wt.), 5% excess Al was poured inside MgO-lined steel reactor; ignition with burning Mg of trigger mixt. (KClO3:Al=2:1); also in Ar in copper double wall reactor; remelting by electron beam (2.7 kW, 1 h, vac. 3.9E-4 Pa) or arc melting (under Ar, tungsten electrode) to evap. Al excess; elem. anal.;	85%

aluminium (7429-90-5) + phenol (108-95-2) → aluminium(III) phenoxide (15086-27-8)

Conditions	Yield
With mercury dichloride In tetrahydrofuran for 24h; Reflux; Inert atmosphere;	95%

titanium (7440-32-6) + graphite + aluminium (7429-90-5) → titanium-aluminium carbide

Conditions	Yield
With Sn In neat (no solvent) other Radiation; mixt. milled for 2 h; coldly pressed into rods; combustion reaction carried out in CO2 laser; XRD;	95%
In solid self-propagating high-temperature synthesis;

triethylaluminum (97-93-8) + aluminium (7429-90-5) → trimethylaluminum (75-24-1) + diethylaluminum iodide (2040-00-8)

Conditions	Yield
With iodine; methyl iodide In ethanol Sonication; N2; CH3I, I2 and Al introduced in a condenser with C2H5OH at -20°C, ultrasonic acceleration at room temp. for 2 h, Et3Al (ratio MeI/Et3Al = 1.50) dropped into soln. within 10 min, sonication for 30 min; distilled (vac.);	A 86% B 95%

chromium (7440-47-3) + nickel (7440-02-0) + aluminium (7429-90-5) + tungsten (7440-33-7) → Ni(77.1),Cr(2.0),Al(17.9),W(3.0) (A%) + Ni(79.8),Cr(5.8),Al(12.2),W(2.2) (A%)

Conditions	Yield
In melt Electric Arc; ingots by arc melting of Ni(75)-Cr(2.5)-Al(20)-W(2.5) (at%), several remelts, sealed in silica tube under vac. with partial pressure of Ar, 1573K (2 weeks), furnace cooled to 1523K, 4 weeks, 1273K (6 weeks), quenched in iced water; electron microscopy, electron probe microanalysis, x-ray diffraction;	A 95% B 5%

dicyclopropylmercury (13955-96-9) + aluminium (7429-90-5) → {((CH2)2CH)3Al}2

Conditions	Yield
In neat (no solvent) The reactants in sealed tube were heated in an oil bath to 75°C for 1 week;; sublimed at 50°C and 10E-6 torr;;	95%

(-)-menthol (2216-51-5) + aluminium (7429-90-5) → aluminium tri(-)-menthylate

Conditions	Yield
In toluene byproducts: H2; (inert atmosphere); reflux (12-15 h); decantation, extn., centrifugation, distn., recrystn. (benzene); elem. anal.;	95%
In benzene byproducts: H2; (inert atmosphere); reflux (25-30 h); decantation, extn., centrifugation, distn., recrystn. (benzene); elem. anal.;	87%

isopropyl alcohol (67-63-0) + aluminium (7429-90-5) → aluminum tris(iso-propoxide)

Conditions	Yield
With mercury dichloride for 9h; Reflux; Inert atmosphere;	95%

Upstream product

• 97-93-8 triethylaluminum 
• 7440-23-5 sodium 
• 7440-09-7 potassium 
• 16853-85-3 lithium aluminium tetrahydride 
• 1333-74-0 hydrogen 
• 7439-95-4 magnesium 
• 1333-84-2 aluminum oxide 
• 75-15-0 carbon disulfide 
• 1299-86-1 aluminium carbide 
• 7784-18-1 aluminum(III) fluoride 
• 7439-98-7 molybdenum 
• 7440-18-8 ruthenium 

Downstream Products

• 1333-84-2 aluminum oxide 
• 163705-72-4 1-(3-cyclopentyloxy-4-methoxyphenyl)-1-phenylmethanol 
• 26171-27-7 1-methyl-5-(4-nitrobenzoyl)pyrrole-2-acetonitrile 
• 3592-25-4 1,5-dichloropentan-3-one 
• 829-85-6 diphenylphosphane 
• 177582-89-7 trans-4-Aminocyclohexylmethyl N-2-phenylethyl-3-cyclohexyl-D-alanyl-L-proline amide 
• 939-37-7 1-(sec-butyl)-3,5-dimethylbenzene 
• 215164-94-6 9-(trichlorosilyl)methyl-3-phenylfluorene 
• 24544-08-9 2,6-diethyl-4-methylaniline 
• 2095-02-5 2,4-diethyl-6-methyl-1,3-phenylenediamine 
• 2095-01-4 2-methyl-4,6-diethylphenylene-1,3-diamine 
• 75251-24-0 1-(4-ethylphenyl)propan-2-one 
• 836-30-6 4-ntrophenyl(phenyl)amine 
• 1100-10-3 4,4'-dinitrotriphenylamine 

Relevant academic research and scientific papers

Optimization of pulsed electrodeposition of aluminum from AlCl 3-1-ethyl-3-methylimidazolium chloride ionic liquid

In this study, Al was electrodeposited on a platinum substrate at room temperature from an ionic liquid bath of EMIC containing AlCl3 using potentiostatic polarization (PP), galvanostatic polarization (GP), monopolar current pulse polarization

Electrodeposition of nanocrystalline metals and alloys from ionic liquids

Better than water: A method for the electrodeposition of nanocrystalline metals and alloys from ionic liquids has been developed (see schematic representation). This method enables the synthesis of aluminum nanocrystals with average grain sizes of about 10 nm, Al-Mn alloys, as well as Fe and Pd nanocrystals.

Modeling of aluminium deposition from chloroaluminate ionic liquids

A finite-element model of the electrodeposition of aluminium from chloroaluminate ionic liquids is introduced. The purpose of this model is to give an explanation for the reasonable current densities that can be achieved in chloroaluminate ionic liquids despite the fact that the electrochemically active Al 2 Cl 7 - complexes are transformed into inactive AlCl 4 - complexes during the electrodeposition of aluminium. The obtainable current density in the electrodeposition from chloroaluminate ionic liquids strongly depends on the chemical rate constants for establishing the equilibrium Al 2 Cl 7 - + Cl - 2 AlCl 4 -. A high current (up to 3000 A m-2) was found for both high and low rate constants whereas a minimum current (200 A m-2) was found for intermediate rate constants due to kinetics and thermodynamics. The model is compared to experiments conducted in the ionic liquid AlCl3 - [C2mim]Cl (60/40 mol) where [C2mim]Cl is 1-ethyl-3-methylimidazolium chloride.

Electrodeposition of bright Al-Zr alloy coatings from dimethylsulfone-based baths

Electrodeposition of Al coatings from dimethylsulfone (DMSO 2)-AlCl3 baths with the addition of ZrCl4 was studied. Although pure Al coatings electrodeposited from the bath without ZrCl4 are lusterless, bright and smooth coatings were obtained when the ZrCl4 content in the baths was 0.005-0.015 mol per 10 mol DMSO2. The Zr content in the coatings varied up to 3.5 at% in proportion to the ZrCl4 content in the baths. The bright Al-Zr alloy coating showed high reflectance of 50-80% in the wavelength range of 450-1000 nm, whereas that of the matte pure Al coating was 10-20%. Morphological observations confirmed a reduction in the grain size of Al and surface leveling caused by the addition of ZrCl4 to the baths. Moreover, a strong 100 preferential orientation of Al crystals was observed for the bright coatings. The bright coating containing ～3.5 at% Zr had a higher corrosion potential by 0.1 V than the pure Al coating.

Electroless plating of aluminum using diisobutyl aluminum hydride as liquid reducing agent in room-temperature ionic liquid

We investigated an electroless aluminum plating based on using AlCl3-1-ethyl-3-methylimidazolium chloride (AlCl3-EMIC) ionic liquid with diisobutyl aluminum hydride (DIBAH) as a liquid reducing agent. The plating film was analyzed by

Interaction of electrochemically deposited aluminium nanoparticles with reactive gases

Metastable induced electron spectroscopy (MIES), ultraviolet photoelectron spectroscopy (UPS) and X-ray photoelectron spectroscopy (XPS) were used to study the interaction of nanocrystalline aluminium with oxygen and carbon monoxide, respectively. High resolution scanning electron microscopy (HRSEM) was used to investigate the morphology of the nanocrystalline aluminium films. These films were prepared by electrodeposition from the ionic liquid 1-butyl-1-methylpyrrolidinium bis(trifluoromethylsulfonyl)imide containing 1.6 Mol per litre AlCl3 in an argon filled glove box. Only a slight oxidation under exposure to oxygen and carbon monoxide was observed. After carbon monoxide dosage, no significant amount of carbon contamination was detected on the sample. These results indicate that the nanocrystalline aluminium is rather inert.

Aluminum-electrocrystallization from metal-organic electrolytes

Aluminum electrodeposition from aprotic solutions of the organic complex KF·2Al(C2H5)3 on polycrystalline aluminum and vitreous carbon is described for potentiostatic and voltage pulse conditions. Near the equilibrium of the aluminum electrode, below currents of about -3 mA cm-2, electron transfer controls the deposition rate. Stationary polarizations over -0.1 V generate a material transport limitation which was controlled and eliminated by the rotating disk electrode technique. Extending the overvoltage to -0.1 to -0.3 V a slow chemical process characterized by a reaction current of ca -5 mA cm-2 precedes charge transfer. Above -0.3 and -0.7 V two further deposition mechanisms possibly involving slow chemical and crystallization steps were observed.

Co-deposition of Al-Zn on AZ91D magnesium alloy in AlCl3-1-ethyl-3-methylimidazolium chloride ionic liquid

The co-deposition of Al and Zn on AZ91D magnesium alloy from a Lewis acidic aluminum chloride-1-ethyl-3-methylimidazolium chloride (AlCl3-EMIC, with a molar ratio of 60:40) ionic liquid containing 1 wt% ZnCl2 at room temperature was studied. The effect of potential on the deposition rate, the microstructure and the chemical composition of the deposit was explored. The experimental results show that the simultaneous deposition of Al and Zn on Mg alloy can be achieved under properly controlled potential conditions. The deposition rate increased while the amount of Zn existing in the coating decreased with increasing negative deposition potential. In the ionic liquid studied, a uniform chemical composition of the coating was obtained when the deposition was performed at -0.2 V (vs. Al).

Co-reduction behaviors of lanthanum and aluminium ions in LiCl-KCl eutectic

In this work, the co-reduction of La(III) and Al(III) ions on the Mo electrode was investigated in LiCl-KCl eutectic at 723-806 K. Cyclic voltammetry (CV), square wave voltammetry (SWV), and open-circuit chronopotentiometry (OCP) techniques were employed

Production of nanodisperse particles of doped yttrium-aluminum garnet by a sol-gel process

Method for synthesis of nanodisperse yttrium-aluminum garnet powders activated with cerium and silicon ions was developed. The method is based on a combination of sol-gel synthesis and coprecipitation of hydroxides of the corresponding metals. The process modes were optimized and the structural, physicochemical, and spectral-luminescent characteristics of the samples obtained were studied.