Aluminum (Al)
post-transition-metalSolid
Peso atómico estándar
26,981538 uConfiguración electrónica
[Ne] 3s2 3p1Punto de fusión
660,287 °CPunto de ebullición
2518,85 °CDensidad
2700 kg/m³Estados de oxidación
−2, −1, 0, +1, +2, +3Electronegatividad (Pauling)
1,61Energía de ionización (1.ª)
5,985769 eVAño de descubrimiento
1825Radio atómico
125 pmDetalles
Aluminum is a light, silvery post-transition metal and the most abundant metal in Earth’s crust. It is highly reactive thermodynamically, but a thin, adherent oxide film protects the metal from rapid corrosion in air and water. Its low density, electrical conductivity, formability, and alloying behavior make it one of the major structural and engineering metals.
Pure aluminum, a silvery-white metal, possesses many desirable characteristics. It is light, it is nonmagnetic and nonsparking, stands second among metals in the scale of malleability, and sixth in ductility.
The name derives from the Latin, alum and alumen for "stringent" because the early Romans called any substance with a stringent taste alum. The element was known in prehistoric times. In 1825, the Danish physicist, Hans Christian Oersted, isolated impure aluminium. The pure metal was first isolated by the German chemist Friedrich Wöhler in 1827.
Although aluminum is the most abundant metal in the earth's crust, it is never found free in nature. All of the earth's aluminum has combined with other elements to form compounds. Two of the most common compounds are alum, such as potassium aluminum sulfate (KAl(SO4)2·12H2O), and aluminum oxide (Al2O3). About 8.2% of the earth's crust is composed of aluminum. Scientists suspected than an unknown metal existed in alum as early as 1787, but they did not have a way to extract it until 1825. Hans Christian Oersted, a Danish chemist, was the first to produce tiny amounts of aluminum. Two years later, Friedrich Wöhler, a German chemist, developed a different way to obtain aluminum. By 1845, he was able to produce samples large enough to determine some of aluminum's basic properties. Wöhler's method was improved in 1854 by Henri Étienne Sainte-Claire Deville, a French chemist. Deville's process allowed for the commercial production of aluminum. As a result, the price of aluminum dropped from around $1200 per kilogram in 1852 to around $40 per kilogram in 1859. Unfortunately, aluminum remained too expensive to be widely used.
From the Latin word alumen, alum. The ancient Greeks and Romans used alum 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.
Friedrich 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 aluminium for the metal, undiscovered at that time, and later agreed to change it to aluminum. Shortly thereafter, the name aluminum was adopted to conform with the "ium" ending of most elements.
Aluminium was also the accepted spelling in the U.S. until 1925, at which time the American Chemical Society decided to use the name aluminum thereafter in their publications. See the Wikipedia entry on Aluminium for additional discussion on the spelling of this element.
Pure aluminum is a silvery-white metal with a bright metallic luster when freshly cut. It is soft and ductile in high purity, but most practical aluminum is used as stronger alloys. Ordinary surfaces quickly become slightly dull because of a transparent aluminum oxide film.
Aluminum is used in aircraft, vehicles, building products, packaging, electrical conductors, heat exchangers, cookware, and machinery. Alloys with magnesium, silicon, copper, zinc, or manganese provide strength, corrosion resistance, or good casting behavior. Aluminum foil and cans exploit its malleability and barrier properties. Powdered aluminum is used in some pyrotechnic mixtures and as a reducing agent in thermite processes.
Two important developments in the 1880s greatly increased the availability of aluminum. The first was the invention of a new process for obtaining aluminum from aluminum oxide. Charles Martin Hall, an American chemist, and Paul L. T. Héroult, a French chemist, each invented this process independently in 1886. The second was the invention of a new process that could cheaply obtain aluminum oxide from bauxite. Bauxite is an ore that contains a large amount of aluminum hydroxide (Al2O3·3H2O), along with other compounds. Karl Joseph Bayer, an Austrian chemist, developed this process in 1888. The Hall-Héroult and Bayer processes are still used today to produce nearly all of the world's aluminum.
With an easy way to extract aluminum from aluminum oxide and an easy way to extract large amounts of aluminum oxide from bauxite, the era of inexpensive aluminum had begun. In 1888, Hall formed the Pittsburgh Reduction Company, which is now known as the Aluminum Company of America, or Alcoa. When it opened, his company could produce about 25 kilograms of aluminum a day. By 1909, his company was producing about 41,000 kilograms of aluminum a day. As a result of this huge increase of supply, the price of aluminum fell rapidly to about $0.60 per kilogram.
Today, aluminum and aluminum alloys are used in a wide variety of products: cans, foils and kitchen utensils, as well as parts of airplanes, rockets and other items that require a strong, light material. Although it doesn't conduct electricity as well as copper, 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.
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 alloyed with small amounts of copper, magnesium, silicon, manganese, or other elements 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 are used to coat telescope mirrors and to make decorative paper, packages, and toys.
Isotopes in Biology
26Al is a radioactive isotope (half-life of 7.1×105 years) that can be detected at the ultra-trace level (attogram range; 10−18 g levels) using accelerator mass spectrometry. 26Al is used as a tracer to study the uptake, distribution, and retention of aluminium in plants, animals, and humans under different physiological conditions [117] C. Steinhausen, G. Kislinger, C. Winklhofer, E. Beck, C. Hohl, E. Nolte, T. H. Ittel, M. J. Alvarez-Brückmann. Food Chem. Toxicol.42, 363 (2004)., [118] B. Kleja, W. Standring, D. H. Oughton, J. P. Gustafsson, K. Fifield, A. R. Fraser. Geochim. Cosmochim. Acta.69, 5263 (2005)..
Isotopes in Geochronology
26Al is produced from spallation reactions of protons, produced by cosmic rays, on argon. 26Al has been used for dating geological samples, such as marine sediments, manganese nodules, rocks, and meteorites [119] United States Geological Survey. Resources on Isotopes-Periodic Table-Aluminum, United States Geological Survey (2014), Feb. 24; http://wwwrcamnl.wr.usgs.gov/isoig/period/al_iig.html., [120] D. E. Granger. Geol. Soc. Spec. Pap.415, 1 (2006).. The abundances of 26Al to 10Be have been used to study erosion and transport of soil and sediments on a thousand- to million-year time scale, because production rates of 26Al to 10Be are greatest at the surface and decrease exponentially with depth (Fig. IUPAC.13.1) [121] K. K. Nichols, P. R. Bierman, R. L. Hooke, E. M. Clapp, M. Caffee. Geomorphology45, 105 (2002)., [122] D. Lal. Annu. Rev. Earth Planet. Sci.16, 355 (1988)..
Intense cosmic-ray bombardment in space produces 26Al in meteorites and other bodies, such as the Moon. After a meteorite falls to Earth, 26Al production ceases due to atmospheric shielding; the decay of 26Al to 26Mg has been used to determine the terrestrial age of a meteorite (i.e. the time elapsed since the meteorite fell to Earth) [119] United States Geological Survey. Resources on Isotopes-Periodic Table-Aluminum, United States Geological Survey (2014), Feb. 24; http://wwwrcamnl.wr.usgs.gov/isoig/period/al_iig.html..
Aluminum chemistry is dominated by the +3 oxidation state and by strong affinity for oxygen and fluorine. Aluminum oxide, Al₂O₃, occurs in corundum and is used as an abrasive, refractory, ceramic, and catalyst support. Aluminum hydroxide, Al(OH)₃, and alumina hydrates are important intermediates from bauxite. Aluminum chloride, AlCl₃, is a Lewis acid catalyst, while sodium aluminate, NaAlO₂, and aluminosilicates are central to industrial and mineral chemistry.
The compounds of greatest importance are aluminum oxide, the sulfate, and the soluble sulfate with potassium (alum). The oxide, alumina, occurs naturally as ruby (Al2O3), sapphire, corundum, and emery, and is used in glassmaking and refractories. Synthetic ruby and sapphire are used in lasers for producing coherent light.
See more information at the Aluminum compound page.
Massive aluminum metal is generally of low acute toxicity, but fine powder or dust can burn or explode when dispersed in air. Molten aluminum reacts dangerously with water or wet scrap because steam and hydrogen can be generated. Soluble aluminum salts and airborne industrial dusts are exposure concerns at sufficient dose. Aluminum has no known essential biological role in humans.
Aluminum is widespread in minerals, especially aluminosilicates and bauxite ores, but free metal is not found naturally because it oxidizes readily. In neutral waters it is usually poorly soluble, while acidic conditions can mobilize Al³⁺ species that are harmful to plant roots and aquatic organisms. Weathering, clay formation, and sediment burial are major parts of its natural cycling.
Primary aluminum is made mainly from bauxite by refining it to aluminum oxide, Al₂O₃, through the Bayer process and electrolytically reducing the oxide in molten cryolite-based electrolyte by the Hall-Héroult process. Production is energy-intensive, so electricity cost and power source strongly affect siting. Recycling is economically important because remelting scrap needs far less energy than primary production, and beverage cans, vehicle parts, and construction scrap form major recyclable streams.
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.
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 also found in granite and in many other common minerals.
Aluminum is a moderately abundant cosmic element made chiefly by stellar nucleosynthesis in massive stars and released by supernovae and stellar winds. The radioactive isotope ²⁶Al is observed through its gamma-ray emission and is evidence of recent nucleosynthesis in the Milky Way. In rocky planets and meteorites, aluminum is concentrated in refractory minerals.
- The protective oxide film on aluminum is only nanometers thick but reforms rapidly if scratched.
- Anodizing deliberately thickens the oxide layer and can make it porous enough to take dyes.
- Aluminum was once more costly than common precious metals before electrolytic production became practical.
- Most high-strength aluminum structures are alloys, not chemically pure aluminum.
- Corundum gemstones such as ruby and sapphire are aluminum oxide colored by trace impurities.
Imágenes
Propiedades
Físicas
- Radio atómico (empírico)
- 125 pm Comparar Radio atómico (empírico) de todos los elementos →
- Radio covalente
- 121 pm Comparar Radio covalente de todos los elementos →
- Radio de van der Waals
- 184 pm Comparar Radio de van der Waals de todos los elementos →
- Radio metálico
- 125 pm Comparar Radio metálico de todos los elementos →
- Densidad
- 2700 kg/m³ Comparar Densidad de todos los elementos →
- Volumen molar
- 0,01 L/mol
- Fase en CNPT
- Sólido Comparar Fase en CNPT de todos los elementos →
- Punto de fusión
- 660,287 °C Comparar Punto de fusión de todos los elementos →
- Punto de ebullición
- 2518,85 °C Comparar Punto de ebullición de todos los elementos →
- Conductividad térmica
- 237 W/(m·K) Comparar Conductividad térmica de todos los elementos →
- Capacidad calorífica específica
- 0,897 J/(g·K) Comparar Capacidad calorífica específica de todos los elementos →
- Capacidad calorífica molar
- 24,2 J/(mol·K) Comparar Capacidad calorífica molar de todos los elementos →
- Estructura cristalina
- Cúbica centrada en las caras Comparar Estructura cristalina de todos los elementos →
Químicas
- Electronegatividad (Pauling)
- 1,61 Comparar Electronegatividad (Pauling) de todos los elementos →
- Electronegatividad (Allen)
- 1,613
- Afinidad electrónica
- 0,4328 eV
- Energía de ionización (1.ª)
- 5,985769 eV Comparar Energía de ionización (1.ª) de todos los elementos →
- Energía de ionización (2.ª)
- 18,828615 eV Comparar Energía de ionización (2.ª) de todos los elementos →
- Energía de ionización (3.ª)
- 28,44774 eV Comparar Energía de ionización (3.ª) de todos los elementos →
- Energía de ionización (4.ª)
- 119,992813 eV Comparar Energía de ionización (4.ª) de todos los elementos →
- Energía de ionización (5.ª)
- 153,825729 eV Comparar Energía de ionización (5.ª) de todos los elementos →
- Estados de oxidación
- −2, −1, 0, +1, +2, +3 Comparar Estados de oxidación de todos los elementos →
- Electrones de valencia
- 3 Comparar Electrones de valencia de todos los elementos →
- Configuración electrónica
- [Ne] 3s2 3p1
Termodinámicas
- Punto crítico (temperatura)
- 6427 °C
- Calor de fusión
- 0,11100171 eV Comparar Calor de fusión de todos los elementos →
- Calor de vaporización
- 3,047106 eV Comparar Calor de vaporización de todos los elementos →
- Calor de sublimación
- 3,382909 eV
- Calor de atomización
- 3,382909 eV
- Entalpía de atomización
- 3,429549 eV
Nucleares
- Protones
- 13 Comparar Protones de todos los elementos →
- Neutrones
- 14 Comparar Neutrones de todos los elementos →
- Isótopos conocidos
- 23 Comparar Isótopos conocidos de todos los elementos →
- Isótopos estables
- 1 Comparar Isótopos estables de todos los elementos →
- Isótopo más estable
- Al-27
- Año de descubrimiento
- 1825
Abundancia
- Abundancia (corteza terrestre)
- 8,23e+4 mg/kg Comparar Abundancia (corteza terrestre) de todos los elementos →
- Abundancia (océano)
- 0,002 mg/L Comparar Abundancia (océano) de todos los elementos →
Estructura cristalina
- Constante de red a
- 405 pm
Estructura electrónica
- Electrones por capa
- 2, 8, 3 Comparar Electrones por capa de todos los elementos →
Identificadores
- Número CAS
- 7429-90-5 Comparar Número CAS de todos los elementos →
- Símbolo del término
- 2P°1/2
- InChI
- InChI=1S/Al
- Clave InChI
- XAGFODPZIPBFFR-UHFFFAOYSA-N
Configuración electrónica Medido
Al: 3s² 3p¹[Ne] 3s² 3p¹1s² 2s² 2p⁶ 3s² 3p¹Modelo atómico
Los isótopos cambian el número de neutrones, la masa y la estabilidad, pero no la configuración electrónica de un átomo neutro.
Modelo atómico esquemático, no a escala.
Huella atómica
Espectro de emisión / absorción
Distribución isotópica
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración |
|---|---|---|---|
| 27 Estable | 26,98153853 ± 0,00000011 | 100,0000% | Estable |
Fase / Estado
Motivo: 635,3 °C por debajo del punto de fusión (660,287 °C)
Esquemático, no a escala
Puntos de transición de fase
Energías de transición
Energía necesaria para fundir 1 mol en el punto de fusión
Energía necesaria para vaporizar 1 mol en el punto de ebullición
Energía necesaria para sublimar 1 mol en el punto de sublimación
Densidad
En condiciones estándar
En condiciones estándar
Avanzado
Espectros atómicos
Se muestran 10 de 13. Ordenado por carga del ion (ascendente).
Líneas disponibles ?
| Ion | Carga | Total de líneas | Probabilidades de transición | Designaciones de los niveles |
|---|---|---|---|---|
| Al I | 0 | 589 | 322 | 560 |
| Al II | +1 | 1429 | 986 | 1429 |
| Al III | +2 | 344 | 259 | 344 |
| Al IV | +3 | 409 | 123 | 409 |
| Al V | +4 | 600 | 444 | 600 |
| Al VI | +5 | 515 | 491 | 515 |
| Al VII | +6 | 350 | 339 | 350 |
| Al VIII | +7 | 440 | 418 | 438 |
| Al IX | +8 | 372 | 339 | 372 |
| Al X | +9 | 189 | 169 | 189 |
Niveles disponibles ?
| Ion | Carga | Niveles |
|---|---|---|
| Al I | 0 | 192 |
| Al II | +1 | 219 |
| Al III | +2 | 84 |
| Al IV | +3 | 121 |
| Al V | +4 | 158 |
| Al VI | +5 | 87 |
| Al VII | +6 | 73 |
| Al VIII | +7 | 95 |
| Al IX | +8 | 69 |
| Al X | +9 | 61 |
Radios iónicos
| Carga | Coordinación | Espín | Radio |
|---|---|---|---|
| +3 | 4 | N/D | 39 pm |
| +3 | 5 | N/D | 48 pm |
| +3 | 6 | N/D | 53.5 pm |
Compuestos
Isótopos (1)
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración | Modo de desintegración | |
|---|---|---|---|---|---|
| 27 Estable | 26,98153853 ± 0,00000011 | 100,0000% | Estable | stable |
Líneas espectrales
Se muestran 50 de 341. De forma predeterminada, solo se muestran las líneas espectrales con intensidad medida.
| Longitud de onda (nm) | Intensidad | Estado de ionización | Tipo | Transición | Exactitud | Fuente | |
|---|---|---|---|---|---|---|---|
| 466.3046 nm | 1000 | Al II | emission | 3p2 1D → 3s.4p 1P* | Medida | NIST | |
| 559.33 nm | 800 | Al II | emission | 3s.4p 1P* → 3s.4d 1D | Medida | NIST | |
| 458.5818 nm | 500 | Al II | emission | 3s.4d 3D → 3s.7f 3F* | Medida | NIST | |
| 458.8199 nm | 400 | Al II | emission | 3s.4d 3D → 3s.7f 3F* | Medida | NIST | |
| 464.8609 nm | 400 | Al II | emission | 3s.4d 1D → 3s.10p 1P* | Medida | NIST | |
| 466.6799 nm | 400 | Al II | emission | 3s.5p 1P* → 3s.11s 1S | Medida | NIST | |
| 458.975 nm | 300 | Al II | emission | 3s.4d 3D → 3s.7f 3F* | Medida | NIST | |
| 444.7805 nm | 200 | Al II | emission | 3s.4d 1D → 3s.11p 1P* | Medida | NIST | |
| 458.968 nm | 200 | Al II | emission | 3s.4d 3D → 3s.7f 3F* | Medida | NIST | |
| 600.641 nm | 200 | Al II | emission | 3s.5p 3P* → 3s.7d 3D | Medida | NIST | |
| 390.0675 nm | 100 | Al II | emission | 3s.3p 1P* → 3p2 1D | Medida | NIST | |
| 528.3733 nm | 100 | Al II | emission | 3s.5p 3P* → 3s.8d 3D | Medida | NIST | |
| 561.329 nm | 100 | Al II | emission | 3s.4d 1D → 3s.7f 1F* | Medida | NIST | |
| 585.376 nm | 100 | Al II | emission | 3s.4d 3D → 3s.6f 3F* | Medida | NIST | |
| 624.337 nm | 100 | Al II | emission | 3s.4p 3P* → 3s.4d 3D | Medida | NIST | |
| 704.208 nm | 100 | Al II | emission | 3s.4s 3S → 3s.4p 3P* | Medida | NIST | |
| 747.141 nm | 90 | Al II | emission | 3s.3d 1D → 3s.4f 1F* | Medida | NIST | |
| 586.177 nm | 80 | Al II | emission | 3s.4d 3D → 3s.6f 3F* | Medida | NIST | |
| 597.197 nm | 80 | Al II | emission | 3s.5p 1P* → 3s.7d 1D | Medida | NIST | |
| 683.713 nm | 80 | Al II | emission | 3s.4p 3P* → 3s.5s 3S | Medida | NIST | |
| 623.175 nm | 75 | Al II | emission | 3s.4p 3P* → 3s.4d 3D | Medida | NIST | |
| 600.187 nm | 60 | Al II | emission | 3s.5p 3P* → 3s.7d 3D | Medida | NIST | |
| 422.6816 nm | 50 | Al II | emission | 3s.4d 3D → 3s.8f 3F* | Medida | NIST | |
| 422.7495 nm | 50 | Al II | emission | 3s.4d 3D → 3s.8f 3F* | Medida | NIST | |
| 422.7987 nm | 50 | Al II | emission | 3s.4d 3D → 3s.8f 3F* | Medida | NIST | |
| 586.79 nm | 50 | Al II | emission | 3s.4d 3D → 3s.6f 3F* | Medida | NIST | |
| 607.32 nm | 50 | Al II | emission | 3s.5p 3P* → 3s.8s 3S | Medida | NIST | |
| 622.619 nm | 50 | Al II | emission | 3s.4p 3P* → 3s.4d 3D | Medida | NIST | |
| 682.339 nm | 50 | Al II | emission | 3s.4p 3P* → 3s.5s 3S | Medida | NIST | |
| 705.671 nm | 50 | Al II | emission | 3s.4s 3S → 3s.4p 3P* | Medida | NIST | |
| 744.944 nm | 50 | Al II | emission | 3s.5p 1P* → 3s.6d 1D | Medida | NIST | |
| 399.5837 nm | 40 | Al II | emission | 3s.4d 3D → 3s.9f 3F* | Medida | NIST | |
| 450.371 nm | 40 | Al IV | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4p 2[5/2] | Medida | NIST | |
| 600.192 nm | 40 | Al II | emission | 3s.5p 3P* → 3s.7d 3D | Medida | NIST | |
| 399.6141 nm | 30 | Al II | emission | 3s.4d 3D → 3s.9f 3F* | Medida | NIST | |
| 450.237 nm | 30 | Al IV | emission | 2s2.2p5.(2P*<1/2>).4s 2[1/2]* → 2s2.2p5.(2P*<1/2>).4p 2[3/2] | Medida | NIST | |
| 463.576 nm | 30 | Al II | emission | 3s.5p 3P* → 3s.10d 3D | Medida | NIST | |
| 528.5838 nm | 30 | Al II | emission | 3s.5p 1P* → 3s.8d 1D | Medida | NIST | |
| 606.112 nm | 30 | Al II | emission | 3s.5p 1P* → 3s.8s 1S | Medida | NIST | |
| 633.571 nm | 30 | Al II | emission | 3s.3d 1D → 3s.5p 1P* | Medida | NIST | |
| 399.6368 nm | 20 | Al II | emission | 3s.4d 3D → 3s.9f 3F* | Medida | NIST | |
| 402.6318 nm | 20 | Al II | emission | 3s.3d 1D → 3s.6p 1P* | Medida | NIST | |
| 446.894 nm | 20 | Al IV | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4p 2[3/2] | Medida | NIST | |
| 569.66 nm | 17 | Al III | emission | 2p6.4s 2S → 2p6.4p 2P* | Medida | NIST | |
| 572.273 nm | 16 | Al III | emission | 2p6.4s 2S → 2p6.4p 2P* | Medida | NIST | |
| 462.038 nm | 15 | Al IV | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4p 2[5/2] | Medida | NIST | |
| 531.6073 nm | 15 | Al II | emission | 3s.5p 3P* → 3s.9s 3S | Medida | NIST | |
| 452.919 nm | 14 | Al III | emission | 2p6.4p 2P* → 2p6.4d 2D | Medida | NIST | |
| 451.257 nm | 13 | Al III | emission | 2p6.4p 2P* → 2p6.4d 2D | Medida | NIST | |
| 669.6018 nm | 13 | Al I | emission | 3s2.4s 2S → 3s2.5p 2P* | Medida | NIST |
Propiedades ampliadas
Radios covalentes (ampliados)
- Radio covalente (Pyykkö)
- 126 pm
- Radio covalente (Pyykkö, enlace doble)
- 113 pm
- Radio covalente (Pyykkö, enlace triple)
- 111 pm
- Radio covalente (Bragg)
- 135 pm
Radios de van der Waals
- Truhlar
- 184 pm
- Batsanov
- 210 pm
- Alvarez
- 225 pm
- UFF
- 449,9 pm
- MM3
- 236 pm
- Dreiding
- 439 pm
Radios atómicos y metálicos
- Radio atómico (Rahm)
- 239 pm
- Radio metálico (C12)
- 143 pm
Escalas de numeración
- Mendeleev
- 82
- Pettifor
- 80
- Glawe
- 78
Escalas de electronegatividad
- Ghosh
- 0
- Miedema
- 4
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 3
Polarizabilidad y dispersión
- Polarizabilidad dipolar
- 57,8 a.u.
- Polarizabilidad dipolar (incert.)
- 1 a.u.
- C₆
- 528 Ha·Bohr6
- C₆ (Gould–Bučko)
- 520 Ha·Bohr6
Parámetros de Miedema
- Volumen molar de Miedema
- 10 cm3/mol
- Densidad electrónica de Miedema
- 3
Riesgo de suministro y economía
- Concentración de la producción
- 31
- Riesgo relativo de suministro
- 5
- Distribución de las reservas
- 26
- Estabilidad política (principal productor)
- 75
- Estabilidad política (país con mayores reservas)
- 5
Transiciones de fase y alótropos
| Punto de fusión | 933,47 K |
| Punto de ebullición | 2792,15 K |
| Punto crítico (temperatura) | 6700,15 K |
Categorías de estados de oxidación
Datos de referencia avanzados
Constantes de apantallamiento (5)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0,409 |
| 2 | p | 4,0366 |
| 2 | s | 4,7864 |
| 3 | p | 8,9344 |
| 3 | s | 8,8828 |
Detalle de los radios cristalinos (3)
| Carga | CN | Espín | rcrystal (pm) | Origen |
|---|---|---|---|---|
| 3 | IV | 53 | ||
| 3 | V | 62 | ||
| 3 | VI | 67,5 | from r^3 vs V plots, |
Modos de desintegración de los isótopos (51)
| Isótopo | Modo | Intensidad |
|---|---|---|
| 21 | p | — |
| 22 | B+ | 100% |
| 22 | B+p | 55% |
| 22 | 2p | 1,1% |
| 22 | B+A | 0% |
| 23 | B+ | 100% |
| 23 | B+p | 1,2% |
| 24 | B+ | 100% |
| 24 | B+A | 0% |
| 24 | B+p | 0% |
Factores de dispersión de rayos X (504)
| Energía (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 3,1199 |
| 10,1617 | — | 3,05822 |
| 10,3261 | — | 2,99776 |
| 10,4931 | — | 2,9385 |
| 10,6628 | — | 2,88041 |
| 10,8353 | — | 2,82347 |
| 11,0106 | — | 2,76766 |
| 11,1886 | — | 2,722 |
| 11,3696 | — | 2,69148 |
| 11,5535 | — | 2,66129 |
Datos adicionales
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
8.23×104 milligrams per kilogram
Referencias (1)
- [5] Aluminum https://education.jlab.org/itselemental/ele013.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
2×10-3 milligrams per liter
Referencias (1)
- [5] Aluminum https://education.jlab.org/itselemental/ele013.html
Sources
Sources of this element.
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.
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 also found in granite and in many other common minerals.
Referencias (1)
- [6] Aluminum https://periodic.lanl.gov/13.shtml
Referencias
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Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Aluminum.
The element property data was retrieved from publications.