This article is about aluminium(III) oxide, Al2O3. For other uses, see Aluminium oxide (compounds).
| Aluminium oxide |
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| Identifiers |
| CAS number |
1344-28-1 Y |
| PubChem |
9989226 |
| ChemSpider |
8164808 Y |
| UNII |
LMI26O6933 Y |
| RTECS number |
BD120000 |
| ATC code |
D10AX04 |
| Jmol-3D images |
Image 1
Image 2 |
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[Al+3].[Al+3].[O-2].[O-2].[O-2]
[O-2].[O-2].[O-2].[Al+3].[Al+3]
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-
InChI=1S/2Al.3O/q2*+3;3*-2 Y
Key: PNEYBMLMFCGWSK-UHFFFAOYSA-N Y
InChI=1/2Al.3O/q2*+3;3*-2
Key: PNEYBMLMFCGWSK-UHFFFAOYAC
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| Properties |
| Molecular formula |
Al2O3 |
| Molar mass |
101.96 g mol−1 |
| Appearance |
white solid
|
| Odor |
odorless |
| Density |
3.95–4.1 g/cm3 |
| Melting point |
2,072 °C (3,762 °F; 2,345 K)[2]
|
| Boiling point |
2,977 °C (5,391 °F; 3,250 K)[3]
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| Solubility in water |
insoluble |
| Solubility |
insoluble in diethyl ether
practically insoluble in ethanol |
| Thermal conductivity |
30 W·m−1·K−1[1] |
| Refractive index (nD) |
nω=1.768–1.772
nε=1.760–1.763
Birefringence 0.008 |
| Structure |
| Crystal structure |
Trigonal, hR30, space group = R3c, No. 167 |
Coordination
geometry |
octahedral |
| Thermochemistry |
Std enthalpy of
formation ΔfHo298 |
−1675.7 kJ·mol−1[4] |
Standard molar
entropy So298 |
50.92 J·mol−1·K−1[4] |
| Hazards |
| MSDS |
External MSDS |
| EU classification |
Not listed. |
| NFPA 704 |
|
| Flash point |
non-flammable |
| Related compounds |
| Other anions |
aluminium hydroxide |
| Other cations |
boron trioxide
gallium oxide
indium oxide
thallium oxide |
| Supplementary data page |
Structure and
properties |
n, εr, etc. |
Thermodynamic
data |
Phase behaviour
Solid, liquid, gas |
| Spectral data |
UV, IR, NMR, MS |
Y (verify) (what is: Y/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
| Infobox references |
Aluminium oxide is a chemical compound of aluminium and oxygen with the chemical formula Al2O3. It is the most commonly occurring of several aluminium oxides, and specifically identified as aluminium(III) oxide. It is commonly called alumina, and may also be called aloxide, aloxite, or alundum depending on particular forms or applications. It commonly occurs in its crystalline polymorphic phase α-Al2O3, in which it comprises the mineral corundum, varieties of which form the precious gems ruby and sapphire. Al2O3 is significant in its use to produce aluminium metal, as an abrasive owing to its hardness, and as a refractory material owing to its high melting point.[5]
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Contents
- 1 Natural occurrence
- 2 Properties
- 3 Structure
- 4 Production
- 5 Applications
- 5.1 Filler
- 5.2 Catalysis
- 5.3 Purification
- 5.4 Abrasive
- 5.5 Paint
- 5.6 Composite fiber
- 5.7 Other
- 6 See also
- 7 References
- 8 External links
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Natural occurrence
Corundum is the most common naturally occurring crystalline form of aluminium oxide. Rubies and sapphires are gem-quality forms of corundum, which owe their characteristic colors to trace impurities. Rubies are given their characteristic deep red color and their laser qualities by traces of chromium. Sapphires come in different colors given by various other impurities, such as iron and titanium.
Properties
Aluminium oxide in its powdered form.
Al2O3 is an electrical insulator but has a relatively high thermal conductivity (30 Wm−1K−1[1]) for a ceramic material. In its most commonly occurring crystalline form, called corundum or α-aluminium oxide, its hardness makes it suitable for use as an abrasive and as a component in cutting tools.[5]
Aluminium oxide is responsible for the resistance of metallic aluminium to weathering. Metallic aluminium is very reactive with atmospheric oxygen, and a thin passivation layer of aluminium oxide (4 nm thickness) forms on any exposed aluminium surface.[6] This layer protects the metal from further oxidation. The thickness and properties of this oxide layer can be enhanced using a process called anodising. A number of alloys, such as aluminium bronzes, exploit this property by including a proportion of aluminium in the alloy to enhance corrosion resistance. The aluminium oxide generated by anodising is typically amorphous, but discharge assisted oxidation processes such as plasma electrolytic oxidation result in a significant proportion of crystalline aluminium oxide in the coating, enhancing its hardness.
Aluminium oxide is completely insoluble in water. However it is an amphoteric substance, meaning it can react with both acids and bases, such as hydrochloric acid and sodium hydroxide.
- Al2O3 + 6 HCl → 2 AlCl3 + 3 H2O
- Al2O3 + 6 NaOH + 3 H2O → 2 Na3Al(OH)6
Aluminium oxide was taken off the United States Environmental Protection Agency's chemicals lists in 1988. Aluminium oxide is on EPA's Toxics Release Inventory list if it is a fibrous form.[7]
Structure
Corundum from Brazil, size about 2x3 cm.
The most common form of crystalline aluminium oxide is known as corundum. The oxygen ions nearly form a hexagonal close-packed structure with aluminium ions filling two-thirds of the octahedral interstices. Each Al3+ center is octahedral. In terms of its crystallography, corundum adopts a trigonal Bravais lattice with a space group of R-3c (number 167 in the International Tables). The primitive cell contains two formula units of aluminium oxide.
Aluminium oxide also exists in other phases, namely γ-, δ-, η-, θ-, and χ-Al2O3.[8] Each has a unique crystal structure and properties. Cubic γ-Al2O3 has important technical applications. The so-called β-Al2O3 proved to be NaAl11O17.[9]
Molten aluminium oxide near the melting temperature is roughly 2/3 tetrahedral (i.e. 2/3 of the Al are surrounded by 4 oxygen neighbors), and 1/3 5-coordinated, very little (<5%) octahedral Al-O is present.[10] Around 80% of the oxygen atoms are shared among three or more Al-O polyhedra, and the majority of inter-polyhedral connections are corner-sharing, with the remaining 10-20% being edge-sharing.[10] The breakdown of octahedra upon melting is accompanied by a relatively large volume increase (~20%), the density of the liquid close to its melting point is 2.93gcm−3.[11]
Production
Aluminium hydroxide minerals are the main component of bauxite, the principal ore of aluminium. A mixture of the minerals comprise bauxite ore, including gibbsite (Al(OH)3), boehmite (γ-AlO(OH)), and diaspore (α-AlO(OH)), along with impurities of iron oxides and hydroxides, quartz and clay minerals.[12] Bauxites are found in laterites. Bauxite is purified by the Bayer process:
- Al2O3 + 3 H2O → 2 Al(OH)3
Except for SiO2, the other components of bauxite do not dissolve in base. Upon filtering the basic mixture, Fe2O3 is removed. When the Bayer liquor is cooled, Al(OH)3 precipitates, leaving the silicates in solution. The solid is then calcined (heated strongly) to give aluminium oxide:[5]
- 2 Al(OH)3 → Al2O3 + 3 H2O
The product aluminium oxide tends to be multi-phase, i.e., consisting of several phases of aluminium oxide rather than solely corundum.[8] The production process can therefore be optimized to produce a tailored product. The type of phases present affects, for example, the solubility and pore structure of the aluminium oxide product which, in turn, affects the cost of aluminium production and pollution control.[8]
Known as alundum (in fused form) or aloxite[13] in the mining, ceramic, and materials science communities, aluminium oxide finds wide use. Annual world production of aluminium oxide is approximately 45 million tonnes, over 90% of which is used in the manufacture of aluminium metal.[5] The major uses of specialty aluminium oxides are in refractories, ceramics, and polishing and abrasive applications. Large tonnages are also used in the manufacture of zeolites, coating titania pigments, and as a fire retardant/smoke suppressant.
Applications
The great majority of aluminium oxide is consumed for the production of aluminium, usually by the Hall process.
Filler
Being fairly chemically inert and white, aluminium oxide is a favored filler for plastics. Aluminium oxide is a common ingredient in sunscreen and is sometimes present in cosmetics such as blush, lipstick, and nail polish.
Catalysis
Aluminium oxide catalyses a variety of reactions that are useful industrially. In its largest scale application, aluminium oxide is the catalyst in the Claus process for converting hydrogen sulfide waste gases into elemental sulfur in refineries. It is also useful for dehydration of alcohols to alkenes.
Aluminium oxide serves as a catalyst support for many industrial catalysts, such as those used in hydrodesulfurization and some Ziegler-Natta polymerizations.
Purification
Aluminium oxide is widely used to remove water from gas streams. Other major applications are described below.[14]
Abrasive
Aluminium oxide is used for its hardness and strength. It is widely used as an abrasive, including as a much less expensive substitute for industrial diamond. Many types of sandpaper use aluminium oxide crystals. In addition, its low heat retention and low specific heat make it widely used in grinding operations, particularly cutoff tools. As the powdery abrasive mineral aloxite, it is a major component, along with silica, of the cue tip "chalk" used in billiards. Aluminium oxide powder is used in some CD/DVD polishing and scratch-repair kits. Its polishing qualities are also behind its use in toothpaste. Aluminium oxide can be grown as a coating on aluminium by anodising or by plasma electrolytic oxidation (see the "Properties" above). Both its strength and abrasive characteristics originate from the high hardness (9 on the Mohs scale of mineral hardness) of aluminium oxide.
Aluminium oxide output in 2005
Paint
Template:Main:Alumina effect pigment Aluminium oxide flakes are used in paint for reflective decorative effects, such as in the automotive or cosmetic industries.
Composite fiber
Aluminium oxide has been used in a few experimental and commercial fiber materials for high-performance applications (e.g., Fiber FP, Nextel 610, Nextel 720).[15]
Other
In lighting, transparent aluminium oxide is used in some sodium vapor lamps.[16] Aluminium oxide is also used in preparation of coating suspensions in compact fluorescent lamps.
In chemistry laboratories, aluminium oxide is a medium for chromatography, available in basic (pH 9.5), acidic (pH 4.5 when in water) and neutral formulations.
Health and medical applications include it as a material in hip replacements.[5]
As well, it is used as a dosimeter for radiation protection and therapy applications for its optically stimulated luminescence properties.
Aluminium oxide is an electrical insulator used as a substrate (Silicon on sapphire) for integrated circuits but also as a tunnel barrier for the fabrication of superconducting devices such as single electron transistors and superconducting quantum interference (SQUID) devices.
Insulation for high-temperature furnaces is often manufactured from aluminium oxide. Sometimes the insulation has varying percentages of silica depending on the temperature rating of the material. The insulation can be made in blanket, board, brick and loose fiber forms for various application requirements.
Small pieces of aluminium oxide are often used as boiling chips in chemistry.
It is also used to make spark plug insulators.
Using a plasma spray process and mixed with titania, it is coated onto the braking surface of some aluminium bicycle rims to provide abrasion and wear resistance.[citation needed]
See also
- Charged Aerosol Release Experiment (CARE)
- Corundum
- List of alumina refineries
- Micro-Pulling-Down
- Ruby
- Sapphire
- Transparent alumina
References
- ^ a b Material Properties Data: Alumina (Aluminum Oxide)
- ^ P. Patnaik (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.
- ^ Roew, Raymond (2009). "Adipic Acid". Handbook of Pharmaceutical Excipients. pp. 11–12
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. ISBN 0-618-94690-X.
- ^ a b c d e "Alumina (Aluminium Oxide) – The Different Types of Commercially Available Grades". The A to Z of Materials. Archived from the original on 10 October 2007. http://www.azom.com/details.asp?ArticleID=1389. Retrieved 2007-10-27.
- ^ Campbell, Timothy; Kalia, Rajiv; Nakano, Aiichiro; Vashishta, Priya; Ogata, Shuji; Rodgers, Stephen (1999). "Dynamics of Oxidation of Aluminium Nanoclusters using Variable Charge Molecular-Dynamics Simulations on Parallel Computers". Physical Review Letters 82 (24): 4866. Bibcode 1999PhRvL..82.4866C. doi:10.1103/PhysRevLett.82.4866. http://cacs.usc.edu/papers/Campbell-nAloxid-PRL99.pdf.
- ^ "EPCRA Section 313 Chemical List For Reporting Year 2006" (PDF). US EPA. Archived from the original on 2008-07-16. http://web.archive.org/web/20080716070117/http://www.epa.gov/tri/chemical/chemical+lists/RY2006ChemicalList.pdf. Retrieved 2008-09-30.
- ^ a b c G. Paglia (2004). "Determination of the Structure of γ-Alumina using Empirical and First Principles Calculations Combined with Supporting Experiments" (free download). Curtin University of Technology, Perth. http://espace.library.curtin.edu.au/R?func=search-simple-go&ADJACENT=Y&REQUEST=adt-WCU20040621.123301. Retrieved 2009-05-05.
- ^ E. Wiberg and A. F. Holleman (2001). Inorganic Chemistry. Elsevier. ISBN 0-12-352651-5.
- ^ a b Skinner, L.B., et al. (2013). "Joint diffraction and modeling approach to the structure of liquid alumina". Phys. Rev. B 87: 024201. doi:10.1103/PhysRevB.87.024201. http://prb.aps.org/abstract/PRB/v87/i2/e024201.
- ^ Paradis, P.-F., et al.. (2004). "Non-Contact Thermophysical Property Measurements of Liquid and Undercooled Alumina". Jap. J. Appl. Phys. 43 (4): 1496–1500. doi:10.1143/JJAP.43.1496. http://jjap.jsap.jp/link?JJAP/43/1496/.
- ^ "Bauxite and Alumina Statistics and Information". USGS. Archived from the original on 6 May 2009. http://minerals.usgs.gov/minerals/pubs/commodity/bauxite/. Retrieved 2009-05-05.
- ^ "Aloxite". ChemIndustry.com database. http://www.chemindustry.com/chemicals/14835.html. Retrieved 24 February 2007.
- ^ L. Keith Hudson, Chanakya Misra, Anthony J. Perrotta, Karl Wefers, F. S. Williams “Aluminum Oxide” in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a01_557.
- ^ Mallick, P.K. (2008). Fiber-reinforced composites materials, manufacturing, and design (3rd ed., [expanded and rev. ed.] ed.). Boca Raton, FL: CRC Press. pp. Ch.2.1.7. ISBN 0-8493-4205-8.
- ^ "GE Innovation Timeline 1957–1970". Archived from the original on 16 February 2009. http://www.ge.com/innovation/timeline/eras/science_and_research.html. Retrieved 2009-01-12.
External links
Media related to Aluminium oxide at Wikimedia Commons
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Aluminium compounds
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| Al(I) |
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| Al(II) |
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| Al(III) |
- AlAs
- Al(BH4)3
- AlBr3
- AlCl3
- AlF3
- AlH3
- AlI3
- AlN
- Al(NO3)3
- Al(OH)3
- AlP
- AlPO4
- AlSb
- Al2(MoO4)3
- Al2O3
- Al2S3
- Al2(SO4)3
- Al2Se3
- Al2SiO5
- Al4C3
- AlOHO
- Al(OH)2CO2C17H5
- NaAlH2(OC2H4OCH3)2
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Organoaluminium(III) compounds
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- (Al(CH3)3)2
- (Al(C2H5)3)2
- Al(CH2CH(CH3)2)3
- Al(C2H5)2Cl
- Al(C2H5)2CN
- Al(CH2CH(CH3)2)2H
- Al(C2H5)2Cl2C2H5Cl
- Ti(C5H5)2CH2ClAl(CH3)2
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