kidzsearch.com > wiki   Explore:web images videos games  

Aluminium




KidzSearch Safe Wikipedia for Kids.
Jump to: navigation, search
magnesiumaluminiumsilicon
B

Al

Ga
Appearance
silvery gray metallic
General properties
Name, symbol, number aluminium, Al, 13
Group, period, block 133, p
Standard atomic weight {{{atomic mass}}} g·mol−1
Electron configuration [Ne] 3s2 3p1
Electrons per shell 2, 8, 3 (Image)
Physical properties
Phase solid
Density (near r.t.) 2.70 g·cm−3
Liquid density at m.p. 2.375 g·cm−3
Melting point 933.47 K, 660.32 °C, 1220.58 °F
Boiling point 2743 K, 2470 °C, 4478 °F
Heat of fusion 10.71 kJ·mol−1
Heat of vaporization 284 kJ·mol−1
Specific heat capacity (25 °C) 24.20 J·mol−1·K−1
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1482 1632 1817 2054 2364 2790
Atomic properties
Oxidation states +3, +2,[1] +1,[2] −1, −2
((an amphoteric oxide))
Electronegativity 1.61 (Pauling scale)
Ionization energies
1st: {{{1st ionization energy}}} kJ·mol−1
2nd: {{{2nd ionization energy}}} kJ·mol−1
3rd: {{{3rd ionization energy}}} kJ·mol−1
Atomic radius 143 pm
Covalent radius 121±4 pm
Van der Waals radius 184 pm
Miscellanea
Crystal structure face-centered cubic
Magnetic ordering paramagnetic
Electrical resistivity (20 °C) 26.5Ω·m
Thermal conductivity (300 K) 237 W·m−1·K−1
Thermal expansion (25 °C) 23.1 µm·m−1·K−1
Speed of sound (thin rod) (r.t.) (rolled) 5000 m·s−1
Young's modulus 70 GPa
Shear modulus 26 GPa
Bulk modulus 76 GPa
Poisson ratio 0.35
Mohs hardness 2.75
Vickers hardness 160–350 MPa
Brinell hardness 160–550 MPa
CAS registry number 7429-90-5
Most stable isotopes
Main article: Isotopes of aluminium
iso NA half-life DM DE (MeV) DP
26Al trace 7.17×105 y β+ 1.17 26Mg
ε 26Mg
γ 1.8086
27Al 100% stable

Aluminium (in American and Canadian English also: aluminum) is a chemical element. The symbol for aluminium is Al, and its atomic number is 13. Aluminium is the most abundant metal. It is a mononuclidic element.

History

People have tried to produce aluminium since 1760. The first successful attempt, finished in 1824 by Danish physicist and chemist Hans Christian Ørsted. He reacted anhydrous aluminium chloride with potassium amalgam, yielding a lump of metal looking similar to tin. He presented his results and showed a sample of the new metal in 1825.[3] In 1827, German chemist Friedrich Wöhler repeated Ørsted's experiments but did not identify any aluminium.[4] (The reason for this inconsistency was only discovered in 1921.) He conducted a similar experiment in the same year by mixing anhydrous aluminium chloride with potassium and produced a powder of aluminium.[5] In 1845, he was able to produce small pieces of the metal and described some physical properties of this metal. For many years thereafter, Wöhler was credited as personewho discovered of aluminium.

Properties

Aluminium is a very good conductor of electricity and heat. It is light and strong. It can be hammered into sheets (malleable) or pulled out into wires (ductile). It is a highly reactive metal, although it is corrosion resistant.

A fresh film of aluminium is a good reflector of visible light and an excellent reflector of medium and far infrared radiation.

Aluminium prevents corrosion by forming a small, thin layer of aluminium oxide on its surface. This layer protects the metal by preventing oxygen from reaching it. Corrosion can not occur without oxygen. Because of this thin layer, the reactivity of aluminium is not seen. As a powder it burns hot. Uses include fireworks displays and rocket fuel.

Occurrence and preparation

Pure aluminium is made from bauxite, a kind of rock that has aluminium oxide and many impurities. The bauxite is crushed and reacted with sodium hydroxide. The aluminium oxide dissolves. Then the aluminium oxide is dissolved in liquid cryolite, a rare mineral. Cryolite is normally produced artificially though. The aluminium oxide is electrolyzed to make aluminium and oxygen. The largest producer of aluminium is China. China produces about 31,873 thousand tonnes of aluminium.

Aluminium was once considered a precious metal that was even more valuable than gold. This is no longer true because, as technology improved, it became cheaper and easier to make pure metal.

In space

It is the 12th most abundant of all elements. It is the 3rd most abundant among the elements that have odd atomic numbers.[6] The only stable isotope of aluminium is aluminium-27. It is the 18th most abundant nucleus in the Universe. It is created after fusion of carbon in massive stars that will later become Type II supernovae: this fusion creates magnesium-26, which, when capturing free protons and neutrons becomes aluminium. Essentially all aluminium now in existence is aluminium-27; aluminium-26 was there in the early Solar System but is now extinct. The trace quantities of aluminium-26 that do exist are the most common gamma ray emitter in the interstellar gas.[7]

On Earth

Overall, the Earth is about 1.59% aluminium by mass.[8] In the Earth's crust, aluminium is the most abundant metallic element by mass (8.23%). It is also the third most abundant of all elements in the Earth's crust. A lot of silicates in the Earth's crust contain aluminium.[9] But, the Earth's mantle is only 2.38% aluminium by mass. Aluminium also occurs in seawater at a concentration of 2 μg/kg.[10]

Feldspars, the most common group of minerals in the Earth's crust, are aluminosilicates. Aluminium also occurs in the minerals beryl, cryolite, garnet, spinel, and turquoise.[11] Native aluminium has been reported in cold seeps in the northeastern continental slope of the South China Sea.

Compounds

Aluminium forms chemical compounds in the +3 oxidation state. They are generally unreactive. Aluminium chloride and aluminium oxide examples. Very rarely are compounds in the +1 or +2 oxidation state.

Uses

Many things are made of aluminium. Much of it is used in overhead power lines. It is also widely used in window frames and aircraft bodies. It is found at home as kitchenware, soft drink cans, and cooking foil. Aluminium is also used to coat car headlamps and compact discs. It is used in electrical transmission lines because of its light weight. It can be deposited on the surface of glass to make mirrors, where a thin layer of aluminum oxide quickly forms that acts as a protective coating. Aluminum oxide is also used to make synthetic rubies and sapphires for lasers. Aluminum can now be produced from clay, but the process is not economically feasible at today.

Pure aluminium is very soft, so a harder metal is almost always added. The harder metal is usually copper. Copper/aluminium alloys are to make ships, because the aluminium prevents corrosion, and the copper prevents barnacles.

Aluminium compounds are used in deodorants, water processing plants, food additives, and antacids. Lithium aluminium hydride is a really strong reducing agent used in organic chemistry.

Aluminium sulfate is used in water treatment. It is also used as a mordant in dyeing, in pickling seeds, deodorizing of mineral oils, in leather tanning, and in production of other aluminium compounds.

Anhydrous aluminium chloride is used as a catalyst in chemical and petrochemical industries, the dyeing industry, and in synthesis of many inorganic and organic compounds.

Aluminium hydroxychlorides are used in purifying water, in the paper industry, and as antiperspirants. Sodium aluminate is used in treating water and as an accelerator for drying of cement.

Aluminium acetate in solution is used as an astringent.

Aluminium phosphate is used to make glass, ceramic, pulp and paper products, cosmetics, paints, varnishes. Aluminium hydroxide is used as an antacid, and mordant. It is used also in water purification, the manufacture of glass and ceramics, and in the waterproofing of fabrics.

Aluminium is used in automobiles, trucks, railway cars, marine vessels, bicycles, spacecraft. Aluminium is used in making doors, siding, building wire, sheathing, roofing and other building materials.

Recycling

Since aluminium needs to be made by electrolysis, it requires a very large amount of electrical power. Recycling aluminium would be much cheaper. That's why recycling plants were opened. The cost of recycling aluminium is much less than the cost of making it from bauxite.

Recycling involves melting the scrap. This is a process that only needs 5% of the energy used to produce aluminium from ore. But, 15% of the input material part is lost as dross (ash-like oxide).[12] An aluminium stack melter makes a lot less dross, about 1%.[13]

White dross from primary aluminium production and from secondary recycling processes still contains useful amounts of aluminium that can be extracted industrially. The process produces aluminium billets, together with a very complex waste. This waste is difficult to manage. It reacts with water, releasing a mixture of gases (including, hydrogen, acetylene, and ammonia), which ignites on contact with air.[14] Even with these difficulties, the waste is used as a filler in asphalt and concrete.[15]

Toxicity

Aluminium is not used in the human body, although it is very common. People debate whether its use in deodorants and water treatment is healthy. Aluminium ions slow down plant growth in acidic soils. Aluminium may be a factor in Alzheimer's disease (a disease when the brain stops working and the patient is confused).[16][17] But the Alzheimer's Society says overwhelming medical and scientific opinion is that studies have not convincingly demonstrated a causal relationship between aluminium and Alzheimer's disease.[18]

In most people, aluminium is not as toxic as heavy metals. Aluminium is classified as a non-carcinogen by United States Department of Health and Human Services. There is little proof that normal exposure to aluminium is a risk to healthy adult. There is proof of no toxicity if it is taken in amounts not greater than 40 mg/day per kg of body mass.[19] Most aluminium taken will leave the body in feces. Most of the small part that enters the blood, will be excreted via urine.[20]

Aluminium rarely causes vitamin D-resistant osteomalacia, erythropoietin-resistant microcytic anemia, and central nervous system changes. People with kidney insufficiency are at a risk the most. Chronic ingestion of hydrated aluminium silicates may result in aluminium binding to the things in the intestines. It also increases the removal of other metals, like iron or zinc. Really high doses (>50 g/day) can cause anemia.

A small percentage of people have contact allergies to aluminium and experience itchy red rashes, headache, muscle pain, joint pain, poor memory, insomnia, depression, asthma, irritable bowel syndrome, or other symptoms when touching products containing aluminium.[21]

Exposure to powdered aluminium or aluminium welding fumes can cause pulmonary fibrosis. Fine aluminium powder can also explode.

Ways of exposure

Food is the main source of aluminium. Drinking water has more aluminium than solid foods.[22] Aluminium in food may be absorbed more than aluminium from water. Major sources of human exposure by mouth to aluminium include food (because of its use in food additives, food and beverage packaging, and cooking utensils), drinking water (because of its use in water treatment), and medicines that have aluminium in it.[23] Very high exposure of aluminium are mostly limited to miners, aluminium production workers, and dialysis patients.[24]

Taking of antacids, antiperspirants, vaccines, and cosmetics give possible ways of exposure.[25] Eating acidic foods or liquids with aluminium increases aluminium absorption. Maltol has been shown to increase the build up of aluminium in nerve and bone tissues.[26]

Treatment

In case of suspected sudden consumption of a large amount of aluminium, the only treatment is deferoxamine mesylate. It may be given to help remove aluminium from the body by chelation.[27][28] But, this should be applied with caution as it not only reduce aluminium in the body, but can also reduce those of other metals such as copper or iron.[27]

Environmental effects

High levels of aluminium occur near mining sites. Small amounts of aluminium are released to the environment at the coal-fired power plants or incinerators. Aluminium in the air is washed out by the rain or normally settles down. But, small particles of aluminium remain in the air for a long time.[20]

Acid rain is the main natural factor to move aluminium from natural sources. It is also the main reason for the effects of aluminium on the environment.[29] The main factor for the presence of aluminium in salt and freshwater are the industrial processes that also release aluminium into air.[30]

In water, aluminium acts as a toxiс agent on animals that with gills like fish by causing loss of plasma- and hemolymph ions leading to osmoregulatory failure.[29]

Aluminium is one of the primary factors that reduce the growth of plants on acidic soils. In acid soils the concentration of toxic Al3+ cations increases and disturbs the growth and function of the root. It is generally harmless to plant growth in pH-neutral soils.[31][32][33][34] Wheat has developed a tolerance to aluminium. It releases organic compounds that bind to harmful aluminium cations. Sorghum is thought to have the same method of tolerating aluminium.[35]

Aluminium production has its own problems to the environment on each step of the production process. The major problem is the greenhouse gas. These gases are caused by the electrical consumption of the smelters and the byproducts of processing. The strongest of these gases are perfluorocarbons from the smelting process.[24]

A Spanish scientific report from 2001 claimed that the fungus Geotrichum candidum eats the aluminium in compact discs.[36][37] The better studied bacterium Pseudomonas aeruginosa and the fungus Cladosporium resinae are commonly found in aircraft fuel tanks that use kerosene-based fuels, and laboratory cultures can decompose aluminium.[38] However, these types of bacteria do not eat the aluminium; but rather, the metal is corroded by microbe waste products.[39]

Gallery

Pure (white) and impure (yellow) forms of aluminium chloride
A roll of aluminium
Bauxite, aluminium ore
Aluminium cans ready for recycling at Central European Waste Management's plant in Europe


Related pages

References

  1. D. C. Tyte (1964). "Red (B2Π–A2σ) Band System of Aluminium Monoxide". Nature 202 (4930): 383. doi:10.1038/202383a0 . 
  2. Dohmeier, C.; Loos, D.; Schnöckel, H. (1996). "Aluminum(I) and Gallium(I) Compounds: Syntheses, Structures, and Reactions". Angewandte Chemie International Edition 35: 129–149. doi:10.1002/anie.199601291 . 
  3. Fontani, Marco; Costa, Mariagrazia; Orna, Mary Virginia (2015) (in en). The Lost Elements: The Periodic Table's Shadow Side. Oxford University Press. ISBN 978-0-19-938334-4 . https://books.google.com/books?id=Ck9jBAAAQBAJ&pg=PA30. 
  4. Venetski, S. (1969-07). "?Silver? from clay" (in en). Metallurgist 13 (7): 451–453. doi:10.1007/BF00741130 . ISSN 0026-0894 . http://link.springer.com/10.1007/BF00741130. 
  5. "Ueber das Aluminium". Archiv der Pharmazie 130 (3): 291–292. 1854. doi:10.1002/ardp.18541300315 . ISSN 0365-6233 . http://dx.doi.org/10.1002/ardp.18541300315. 
  6. Solar System abundances and condensation temperatures of the elements. Lodders, K. 2003. ISSN 0004-637X . http://solarsystem.wustl.edu/wp-content/uploads/reprints/2003/Lodders%202003%20ApJ%20Elemental%20abundances.pdf. 
  7. Clayton, Donald (2003) (in en). Handbook of Isotopes in the Cosmos: Hydrogen to Gallium. Cambridge University Press. ISBN 978-0-521-53083-5 . https://books.google.com/books?id=fXcdHyLUVnEC. 
  8. "Wayback Machine". 2011-09-28. https://web.archive.org/web/20110928074153/http://quake.mit.edu/hilstgroup/CoreMantle/EarthCompo.pdf. 
  9. The Chemistry of Aluminium, Gallium, Indium and Thallium: Comprehensive Inorganic Chemistry. Wade, K.; Banister, A.J.. 2016. ISBN 978-1-4831-5322-3 . https://books.google.com/books?id=QwNPDAAAQBAJ&pg=PA1049. 
  10. Cosmochemical Estimates of Mantle Composition. Palme, H.; O'Neill, Hugh St. C.. 2005. https://www.geol.umd.edu/~mcdonoug/KITP%20Website%20for%20Bill/papers/Earth_Models/3.1%20Palme%20&%20O'Neill%20Primative%20mantle%20(1).pdf. 
  11. Downs, A. J. (1993-05-31) (in en). Chemistry of Aluminium, Gallium, Indium and Thallium. Springer Science & Business Media. ISBN 978-0-7514-0103-5 . https://books.google.com/books?id=v-04Kn758yIC&pg=PA17. 
  12. "Benefits of Recycling". https://web.archive.org/web/20030624162738/http://www.dnr.state.oh.us/recycling/awareness/facts/benefits.htm. 
  13. "Theoretical/Best Practice Energy Use in Metalcasting Operations". https://web.archive.org/web/20131031072356/http://www.afsinc.org/files/best%20practice%20energy-schifo-radia-may%202004.pdf. 
  14. "Why are dross & saltcake a concern?" (in en-US). http://www.experts123.com/q/why-are-dross-saltcake-a-concern.html. 
  15. Added value of using new industrial waste streams as secondary aggregates in both concrete and asphalt. Dunster, A.M.. 2005. http://webarchive.nationalarchives.gov.uk/20100402111522/http://www.wrap.org.uk/downloads/BRE_Added_value_study_report.4ca28919.1753.pdf. 
  16. Ferreira PC, Piai Kde A, Takayanagui AM, Segura-Muñoz SI (2008). "Aluminum as a risk factor for Alzheimer's disease". Rev Lat Am Enfermagem 16 (1): 151–7. doi:10.1590/S0104-11692008000100023 . PMID 18392545 . http://www.scielo.br/scielo.php?script=sci_arttext&pid=S0104-11692008000100023&lng=en&nrm=iso&tlng=en. 
  17. Rondeau, V.; Jacqmin-Gadda, H.; Commenges, D.; Helmer, C.; Dartigues, J.-F. (2008). "Aluminum and Silica in Drinking Water and the Risk of Alzheimer's Disease or Cognitive Decline: Findings From 15-Year Follow-up of the PAQUID Cohort". American Journal of Epidemiology 169 (4): 489–96. doi:10.1093/aje/kwn348 . PMC 2809081 . PMID 19064650 . 
  18. Aluminium and Alzheimer's disease, The Alzheimer's Society. Retrieved 30 January 2009.
  19. Physiology of Aluminum in Man. 1998. ISBN 0-8247-8026-4 . https://web.archive.org/web/20160519101650/https://books.google.com/books?id=wRnOytsi8boC&pg=PA90. 
  20. 20.0 20.1 "ATSDR – Public Health Statement: Aluminum". https://www.atsdr.cdc.gov/phs/phs.asp?id=1076&tid=34. 
  21. "Aluminum Allergy Symptoms and Diagnosis" (in en-US). 2016-09-20. https://allergy-symptoms.org/aluminum-allergy/. 
  22. Yokel, Robert A.; Hicks, Clair L.; Florence, Rebecca L. (2008-6). "Aluminum bioavailability from basic sodium aluminum phosphate, an approved food additive emulsifying agent, incorporated in cheese". Food and chemical toxicology : an international journal published for the British Industrial Biological Research Association 46 (6): 2261–2266. doi:10.1016/j.fct.2008.03.004 . ISSN 0278-6915 . PMC 2449821 . PMID 18436363 . https://www.ncbi.nlm.nih.gov/pmc/articles/PMC2449821/. 
  23. United States. Agency for Toxic Substances and Disease Registry, issuing body.. Toxicological profile for aluminum.. OCLC 832737188 . http://worldcat.org/oclc/832737188. 
  24. 24.0 24.1 "Aluminum" (in en-US). https://enviroliteracy.org/special-features/its-element-ary/aluminum/. 
  25. Chen, Jennifer K., editor. Thyssen, Jacob P., editor.. Metal allergy : from dermatitis to implant and device failure. ISBN 978-3-319-58503-1 . OCLC 1031466049 . http://worldcat.org/oclc/1031466049. 
  26. van Ginkel, M. F.; van der Voet, G. B.; D'Haese, P. C.; De Broe, M. E.; de Wolff, F. A. (1993-03). "Effect of citric acid and maltol on the accumulation of aluminum in rat brain and bone". The Journal of Laboratory and Clinical Medicine 121 (3): 453–460. ISSN 0022-2143 . PMID 8445293 . https://www.ncbi.nlm.nih.gov/pubmed/8445293. 
  27. 27.0 27.1 "ARL: Aluminum Toxicity". http://www.arltma.com/Articles/AlumToxDoc.htm. 
  28. "Aluminum Toxicity". http://www.med.nyu.edu/content?ChunkIID=164929. 
  29. 29.0 29.1 Rosseland, B. O.; Eldhuset, T. D.; Staurnes, M. (1990-03). "Environmental effects of aluminium". Environmental Geochemistry and Health 12 (1-2): 17–27. doi:10.1007/BF01734045 . ISSN 0269-4042 . PMID 24202562 . https://www.ncbi.nlm.nih.gov/pubmed/24202562. 
  30. Dolara, Piero (2014-12). "Occurrence, exposure, effects, recommended intake and possible dietary use of selected trace compounds (aluminium, bismuth, cobalt, gold, lithium, nickel, silver)". International Journal of Food Sciences and Nutrition 65 (8): 911–924. doi:10.3109/09637486.2014.937801 . ISSN 1465-3478 . PMID 25045935 . https://www.ncbi.nlm.nih.gov/pubmed/25045935. 
  31. Pereira, Luciane Belmonte; Tabaldi, Luciane Almeri; Gonçalves, Jamile Fabbrin; Jucoski, Gládis Oliveira; Pauletto, Mareni Maria; Weis, Simone Nardin; Nicoloso, Fernando Teixeira; Borher, Denise et al. (2006-08). "Effect of aluminum on δ-aminolevulinic acid dehydratase (ALA-D) and the development of cucumber (Cucumis sativus)" (in en). Environmental and Experimental Botany 57 (1-2): 106–115. doi:10.1016/j.envexpbot.2005.05.004 . https://linkinghub.elsevier.com/retrieve/pii/S0098847205000717. 
  32. Toxicity and tolerance of aluminium in vascular plants. Andersson, Maud. 1988. https://link.springer.com/article/10.1007/BF00279487. 
  33. Horst, Walter J. (1995). "The role of the apoplast in aluminium toxicity and resistance of higher plants: A review" (in de). Zeitschrift für Pflanzenernährung und Bodenkunde 158 (5): 419–428. doi:10.1002/jpln.19951580503 . http://doi.wiley.com/10.1002/jpln.19951580503. 
  34. Ma, Jian Feng; Ryan, Peter R; Delhaize, Emmanuel (2001-06). "Aluminium tolerance in plants and the complexing role of organic acids" (in en). Trends in Plant Science 6 (6): 273–278. doi:10.1016/S1360-1385(01)01961-6 . https://linkinghub.elsevier.com/retrieve/pii/S1360138501019616. 
  35. Magalhaes, Jurandir V.; Garvin, David F.; Wang, Yihong; Sorrells, Mark E.; Klein, Patricia E.; Schaffert, Robert E.; Li, Li; Kochian, Leon V. (2004-08). "Comparative Mapping of a Major Aluminum Tolerance Gene in Sorghum and Other Species in the Poaceae". Genetics 167 (4): 1905–1914. doi:10.1534/genetics.103.023580 . ISSN 0016-6731 . http://dx.doi.org/10.1534/genetics.103.023580. 
  36. Bosch, Xavier (2001-06-27). "Fungus eats CD" (in en). Nature. doi:10.1038/news010628-11 . ISSN 1476-4687 . https://www.nature.com/articles/news010628-11. 
  37. (in en-GB) Fungus 'eats' CDs. 2001-06-22. http://news.bbc.co.uk/2/hi/science/nature/1402533.stm. Retrieved 2020-08-28. 
  38. "Studies on the ‘Kerosene Fungus’ Cladosporium Resinae (Lindau) De Vries — Part I. The Problem of Microbial Contamination of Aviation Fuels | NZETC". http://nzetc.victoria.ac.nz/tm/scholarly/tei-Bio19Tuat01-t1-body-d4.html. 
  39. "Aircraft Fuel System Contamination & Starvation | Intelligence". 2015-02-25. https://web.archive.org/web/20150225051128/http://www.duncanaviation.aero/intelligence/201102/fuel_starvation_system_contamination.php. 

Other websites