Difference between revisions of "Aluminium oxide"
Physchim62 (talk | contribs) |
Physchim62 (talk | contribs) |
||
| (2 intermediate revisions by the same user not shown) | |||
| Line 16: | Line 16: | ||
| ChemSpiderID=8164808 | | ChemSpiderID=8164808 | ||
| RTECS = BD120000 | | RTECS = BD120000 | ||
| + | | ATCCode_prefix = D10 | ||
| + | | ATCCode_suffix = AX04 | ||
}} | }} | ||
| Section2 = {{Chembox Properties | | Section2 = {{Chembox Properties | ||
| Line 49: | Line 51: | ||
}} | }} | ||
| Section8 = {{Chembox Related | | Section8 = {{Chembox Related | ||
| − | | OtherAnions = [[Aluminium hydroxide]] | + | | OtherAnions = [[Aluminium oxide hydroxide]]<br/>[[Aluminium hydroxide]] |
| OtherCations = [[Boron trioxide]]<br/>[[Gallium oxide]]<br/>[[Indium oxide]]<br/>[[Thallium oxide]] | | OtherCations = [[Boron trioxide]]<br/>[[Gallium oxide]]<br/>[[Indium oxide]]<br/>[[Thallium oxide]] | ||
}} | }} | ||
| Line 102: | Line 104: | ||
*{{ICSC|0351}} | *{{ICSC|0351}} | ||
*{{EHC|194|name=Aluminium}} | *{{EHC|194|name=Aluminium}} | ||
| + | *{{HSDB|name=Aluminum oxide}} | ||
[[Category:Aluminium compounds]] | [[Category:Aluminium compounds]] | ||
[[Category:Oxides]] | [[Category:Oxides]] | ||
| + | [[Category:Anti-acne preparations]] | ||
{{Imported from Wikipedia|name=Aluminium oxide|id=327906802}} | {{Imported from Wikipedia|name=Aluminium oxide|id=327906802}} | ||
Latest revision as of 07:02, 13 December 2009
Aluminium oxide is an amphoteric oxide of aluminium with the chemical formula Al2O3. It is also commonly referred to as alumina, corundum, sapphire, ruby or aloxite[3] in the mining, ceramic and materials science communities. It is produced by the Bayer process from bauxite. Its most significant use is in the production of aluminium metal, although it is also used as an abrasive due to its hardness and as a refractory material due to its high melting point.[4]
Contents
Natural occurrence
Corundum is the most common naturally-occurring crystalline form of aluminium oxide. Much less-common rubies and sapphires are gem-quality forms of corundum with their characteristic colors due to trace impurities in the corundum structure. Rubies are given their characteristic deep red color and their laser qualities by traces of the metallic element chromium. Sapphires come in different colors given by various other impurities, such as iron and titanium.
Properties
Aluminium oxide is an electrical insulator but has a relatively high thermal conductivity (40 Wm−1K−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.[4]
Aluminium oxide is responsible for resistance of metallic aluminium to weathering. Metallic aluminium is very reactive with atmospheric oxygen, and a thin passivation layer of alumina (4 nm thickness) forms in about 100 picoseconds on any exposed aluminium surface.[5] 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 alumina generated by anodising is typically amorphous, but discharge assisted oxidation processes such as plasma electrolytic oxidation result in a significant proportion of crystalline alumina in the coating, enhancing its hardness.
Aluminium oxide was taken off the United States Environmental Protection Agency's chemicals lists in 1988. Aluminium oxide is on EPA's TRI list if it is a fibrous form.[6]
Crystal structure
The most common form of crystalline alumina, α-aluminium oxide, is known as corundum. When trace elements make it appear red it is known as ruby, but all other colorations fall under the designation sapphire. Corundum has a trigonal Bravais lattice with a space group of R-3c (number 167 in the International Tables). The unit cell contains two formula units of aluminium oxide. The oxygen ions nearly form a hexagonal close-packed structure with aluminium ions filling two-thirds of the octahedral interstices. Alumina also exists in other phases, namely η-, χ-, γ-, δ- and θ-aluminas.[7] Each has a unique crystal structure and properties. The so-called β-alumina proved to be NaAl11O17.[8]
Production
Aluminium hydroxide minerals are the main component of bauxite, the principal ore of aluminium. The bauxite ore is made up of a mixture of the minerals gibbsite (Al(OH)3), boehmite (γ-AlO(OH)), and diaspore (α-AlO(OH)) along with iron oxides and hydroxides, quartz and clay minerals.[9]
Bauxite is purified by the Bayer process:
- Al2O3 + 3 H2O + 2 NaOH → 2NaAl(OH)4
The other components of bauxite do not dissolve. The SiO2 dissolves as silicate Si(OH)62-. Upon filtering, Fe2O3 is removed. When the Bayer liquor is cooled, Al(OH)3 precipitates, leaving the silicates in solution. The mixture is then calcined (heated strongly) to give aluminium oxide:[4]
- 2 Al(OH)3 → Al2O3 + 3 H2O
The formed Al2O3 is alumina. The alumina formed tends to be multi-phase; i.e., constituting several of the alumina phases rather than solely corundum.[7] 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 alumina product which, in turn, affects the cost of aluminium production and pollution control.[7]
Uses
Annual world production of alumina is approximately 45 million tonnes, over 90% of which is used in the manufacture of aluminium metal.[4]. 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.
Alumina is a medium for chemical chromatography, available in basic (pH 9.5), acidic (pH 4.5 when in water) and neutral formulations.
In lighting, GE developed "Lucalox" in 1961,[10] a transparent alumina used in sodium vapor lamps. Aluminium oxide is also used in preparation of coating suspensions in compact fluorescent lamps.
Health and medical applications include it as a material in hip replacements.[4] It is used in water filters (derived water treatment chemicals such as aluminium sulfate, aluminium chlorohydrate and sodium aluminate, are one of the few methods available to filter water-soluble fluorides out of water). It is also used in toothpaste formulations.
Aluminium oxide is used for its hardness and strength. Most pre-finished wood flooring now uses aluminium oxide as a hard protective coating. In 2004, 3M developed a technique for making a ceramic composed of aluminium oxide and rare earth elements to produce a strong glass called transparent alumina. Alumina can be grown as a coating on aluminium by anodising or by plasma electrolytic oxidation (see the "Properties" section, above). Both its strength and abrasive characteristics are due to aluminium oxide's great hardness (position 9 on the Mohs scale of mineral hardness).
It is widely used as a coarse or fine 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 is widely used in the fabrication of superconducting devices, particularly single electron transistors and superconducting quantum interference devices (SQUID), where it is used to form highly resistive quantum tunneling barriers.
References
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-74. ISBN 0-8493-0462-8.
- ↑ GHS classification – ID 738, <http://www.safe.nite.go.jp/english/ghs_index.html#results> (accessed 26 November 2009), Japanese GHS Inter-ministerial Committee, 2006.
- ↑ Aloxite; ChemIndustry.com, <http://www.chemindustry.com/chemicals/14835.html>. (accessed 24 February 2007).
- ↑ 4.0 4.1 4.2 4.3 4.4 Alumina (Aluminium Oxide) – The Different Types of Commercially Available Grades, <http://www.azom.com/details.asp?ArticleID=1389> (accessed 27 October 2007), The A to Z of Materials; azom.com.
- ↑ Campbell, Timothy; Kalia, Rajiv K.; Nakano, Aiichiro; Vashishta, Priya; Ogata, Shuji; Rodgers, Stephen Dynamics of Oxidation of Aluminum Nanoclusters using Variable Charge Molecular-Dynamics Simulations on Parallel Computers. Phys. Rev. Lett. 1999, 82 (24), 4866–69. DOI: 10.1103/PhysRevLett.82.4866.
- ↑ EPCRA Section 313 Chemical List For Reporting Year 2006; U.S. Environmental Protection Agency, <http://www.epa.gov/tri/chemical/chemical%20lists/RY2006ChemicalList.pdf>. (accessed 30 September 2008).
- ↑ 7.0 7.1 7.2 Paglia, G. Determination of the Structure of γ-Alumina using Empirical and First Principles Calculations Combined with Supporting Experiments; Curtin University of Technology, Perth, 2004, <http://espace.library.curtin.edu.au/R?func=search-simple-go&ADJACENT=Y&REQUEST=adt-WCU20040621.123301>. (accessed 5 May 2009).
- ↑ Holleman, A. F.; Wiberg, E. Inorganic Chemistry; Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ↑ Bauxite and Alumina Statistics and Information; United States Geological Survey, <http://minerals.usgs.gov/minerals/pubs/commodity/bauxite/>. (accessed 5 May 2009).
- ↑ GE Innovation Timeline 1957–1970; General Electric, <http://www.ge.com/innovation/timeline/eras/science_and_research.html>. (accessed 12 January 2009).
External links
- International Chemical Safety Card 0351
- IPCS Environmental Health Criteria 194: Aluminium
- NLM Hazardous Substances Data Bank entry for Aluminum oxide
| Error creating thumbnail: Unable to save thumbnail to destination |  |
This page was originally imported from Wikipedia, specifically this version of the article "Aluminium oxide". Please see the history page on Wikipedia for the original authors. This WikiChem article may have been modified since it was imported. It is licensed under the Creative Commons Attribution–Share Alike 3.0 Unported license. |
