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| Atomic symbol: Al |
| Atomic number: 13 |
| Atomic weight: 26.98154 |
| Atomic volume: 10.0 cm3/mol |
| Density: 2.702 g/cm3 |
| Period Number: 3 |
| Group number: 13 |
| Group name: Metal |
| Element classification: Metal |
| Phase at room temperature: Solid |
| Melting Point: 933.57 K |
| Boiling point: 2740 K |
| Heat of fusion: 10.790 kJ/mol |
| Heat of vaporization: 293.40 kJ/mol |
| Ionization Energy: 5.986 eV |
| 1st ionization energy: 577.6 kJ/mole |
| 2nd ionization energy: 1816.6 kJ/mole |
| 3rd ionization energy: 2744.7 kJ/mole |
| Electronegativity: 1.61 |
| Electron affinity: 42.6 kJ/mole |
| Specific heat: 0.90 J/gK |
| Heat atomization: 326 kJ/mole atoms |
| Shells: 2,8,3 |
| Electron Shell Configuration: [Ne] 3s2 3p1 |
| Minimum oxidation number: 0 |
| Maximum oxidation number: 3 |
| Minimum common oxidation number: 0 |
| Maximum common oxidation no: 3 |
Appearance & Characteristics |
| Structure:: fcc: face-centered cubic |
| Color: silvery |
| Hardness: 2.8 mohs |
| Toxicity: ? |
| Characteristics: passivated: surface oxide |
| Uses: Al cans & foil,reflectors |
| Reaction with air: mild, w/ht =>Al2O3 |
| Reaction with 6M HCl: mild, =>H2, AlCl3 |
| Reaction with 15M HNO3: passivated |
| Reaction with 6M NaOH: mild, =>H2, [Al(OH)4]- |
| Number of isotopes: 1 |
| Oxide(s): Al2O3 |
| Hydride(s): AlH3 |
| Chloride(s): AlCl3Al2Cl6 |
| Atomic Radius: 143 pm |
| Ionic radius (1- ion): pm |
| Ionic radius (1+ ion): pm |
| Ionic radius (2- ion): pm |
| Ionic radius (2+ ion): pm |
| Ionic radius (3+ ion): 67.5 pm |
| Thermal conductivity: 237 J/m-sec-deg |
| Electrical conductivity: 376.676 1/mohm-cm |
| Polarizability: 8.3 A^3 |
| Source: Bauxite (oxide) |
| Relative abundance solar system: 4.929 log |
| Abundance earth's crust: 4.9 log |
| Estimated crustal abundance: 8.23×104 milligrams per kilogram |
| Estimated oceanic abundance: 2×10-3 milligrams per liter |
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(L. 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.
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 aluminum 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, 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.
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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.
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| 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 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. |
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.
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