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Vanadium

Vanadium
23 ↑ V ↓ Nb titanium ← vanadium → chromium Ionization energies (more) 1st: 650.9 kJ·mol−1 2nd: 1414 kJ·mol−1 3rd: 2830 kJ·mol−1 Periodic table General Name, symbol, number Element category Group, period, block Appearance vanadium, V, 23 transition metal 5, 4, d blue-silver-grey metal Thermal expansion Speed of sound (thin rod) Young’s modulus [Ar] 3d3 4s2 2, 8, 11, 2 (Image) solid 6.0 g·cm−3 2183 K (1910 °C, 3470 °F) 3680 K (3407 °C, 6165 °F) 21.5 kJ·mol−1 459 kJ·mol−1 Shear modulus Bulk modulus Poisson ratio Mohs hardness CAS registry number Atomic radius Atomic radius (calc.) Covalent radius Magnetic ordering Electrical resistivity Thermal conductivity 135 pm 171 pm 125 pm paramagnetic (20 °C) 197 nΩ·m (300 K) 30.7 W·m−1·K−1 (25 °C) 8.4 µm·m−1·K−1 (20 °C) 4560 m/s 128 GPa 47 GPa 160 GPa 0.37 6.7 7440-62-2

Miscellaneous

Standard atomic weight Electron configuration Electrons per shell Phase Density (near r.t.) Melting point Boiling point Heat of fusion Heat of vaporization

50.9415(1) g·mol−1

Physical properties

Liquid density at m.p. 5.5 g·cm−3 iso
48V 49V 50V

Most stable isotopes Main article: Isotopes of vanadium NA syn syn 0.25% half-life DM DE
(MeV)

DP

15.9735 d ε+β+ 4.0123 48Ti 330 d ε β0.6019 49Ti 2.2083 50Ti 1.0369 50Cr 1.5×1017y ε

Specific heat capacity (25 °C) 24.89 J·mol−1·K−1 Vapor pressure P/Pa 1 10 100 1k 10 k 100 k at T/K 2101 2289 2523 2814 3187 3679 Atomic properties Crystal structure Oxidation states Electronegativity cubic body centered 5, 4, 3, 2, 1 (amphoteric oxide) 1.63 (Pauling scale)

51V

99.75% 51V is stable with 28 neutrons References

Vanadium (pronounced /vəˈneɪdiəm/) is the chemical element with the symbol V and atomic number 23. It is a soft, silvery grey, ductile transition metal. The formation of an oxide layer stabilizes the metal against oxidation. Andrés Manuel del Río discovered vanadium in 1801 by analyzing the mineral vanadinite, and named it erythronium. Four

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years later, however, he was convinced by other scientists that erythronium was identical to chromium. The element was rediscovered in 1831 by Nils Gabriel Sefström, who named it vanadium after the Norse goddess of beauty and fertility, Vanadis (Freya). Both names were attributed to the wide range of colors found in vanadium compounds. The element occurs naturally in about 65 different minerals and in fossil fuel deposits. It is produced in China and Russia from steel smelter slag; other countries produce it either from the flue dust of heavy oil, or as a byproduct of uranium mining. It is mainly used to produce specialty steel alloys such as high speed tool steels. The compound vanadium pentoxide is used as a catalyst for the production of sulfuric acid. Vanadium is found in many organisms, and is used by some life forms as an active center of enzymes.

Vanadium

1910 Model T be renamed "rionium" after del Río, but this suggestion was not followed.[3] The isolation of vanadium metal proved difficult. In 1831, Berzelius reported the production of the metal, but Henry Enfield Roscoe showed that Berzelius had in fact produced the nitride, vanadium nitride (VN). Roscoe eventually produced the metal in 1867 by reduction of vanadium(III) chloride, VCl3, with hydrogen.[4] In 1927, pure vanadium was produced by reducing vanadium pentoxide with calcium.[5] The first large scale industrial use of vanadium in steels was found in the chassis of the Ford Model T, inspired by French race cars. Vanadium steel allowed for reduced weight while simultaneously increasing tensile strength.[6]

History
Vanadium was originally discovered by Andrés Manuel del Río, a Spanish-born Mexican mineralogist, in 1801. Del Río extracted the element from a sample of Mexican "brown lead" ore, later named vanadinite. He found that its salts exhibit a wide variety of colors, and as a result he named the element panchromium (Greek: all colors). Later, Del Río renamed the element erythronium as most of its salts turned red upon heating. In 1805, the French chemist Hippolyte Victor Collet-Descotils, backed by del Río’s friend, Baron Alexander von Humboldt, incorrectly declared that del Río’s new element was only an impure sample of chromium. Del Río accepted the Collet-Descotils’ statement, and retracted his claim.[1] In 1831, the Swedish chemist, Nils Gabriel Sefström, rediscovered the element in a new oxide he found while working with iron ores. Later same year, Friedrich Wöhler confirmed del Río’s earlier work.[2] Sefström choose a name beginning with V, which had not yet been assigned to any element yet. He called the element vanadium after Vanadis (another name for Freya, the Norse goddess of beauty and fertility), because of the many beautifully colored chemical compounds it produces.[2] In 1831, the geologist George William Featherstonhaugh suggested that vanadium should

Characteristics
Vanadium is a soft, ductile, silver-grey metal. It has good resistance to corrosion and it is stable against alkalis, sulfuric and hydrochloric acids.[7] It is oxidized in air at about 933 K (660 °C, 1220 °F), although an oxide layer forms even at room temperature.

Isotopes
Naturally occurring vanadium is composed of one stable isotope 51V and one radioactive isotope 50V. The latter has a half-life of 1.5×1017 years and a natural abundance 0.25%. 51V has a nuclear spin of 7/2 which is useful for NMR spectroscopy.[8] A number of 24 artificial radioisotopes have been characterized, ranging in mass number from 40 to 65. The most stable of these isotopes are 49V with a half-life of 330 days, and 48V with a half-life of 15.9735 days. All of the remaining

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radioactive isotopes have half-lives shorter than an hour, most of which are below 10 seconds. At least 4 isotopes have metastable excited states.[8] Electron capture is the main decay mode for isotopes lighter than the 51V. For the heavier ones, the most common mode is beta decay. The electron capture reactions lead to the formation of element 22 (titanium) isotopes, while for beta decay, it leads to element 24 (chromium) isotopes.

Vanadium

Chemistry and compounds
See also: Category:Vanadium compounds

Metavanadate chains The vanadium redox battery utilizes these oxidation states; conversions of these oxidation states is illustrated by the reduction of a strongly acidic solution of a vanadium(V) compound with zinc dust. The initial yellow color characteristic of the vanadate ion, VO43−, is replaced by the blue color of [VO(H2O)5]2+, followed by the green color of [V(H2O)6]3+ and then violet, due to [V(H2O)6]2+.[7] The most commercially important compound is vanadium pentoxide, which is used as a catalyst for the production of sulfuric acid.[7] This compound oxidizes sulfur dioxide (SO2) to the trioxide (SO3). In this redox reaction, sulfur is oxidized from +4 to +6, and vanadium is reduced from +5 to +3: V2O5 + 2 SO2 → V2O3 + 2 SO3 The catalyst is regenerated by oxidation with air: V2O 3 + O 2 → V 2O 5

Vanadium(V) oxide is a catalyst in the Contact process for producing sulfuric acid The chemistry of vanadium is noteworthy for the accessibility of four adjacent oxidation states. The common oxidation states of vanadium are +2 (lilac), +3 (green), +4 (blue) and +5 (yellow). Vanadium(II) compounds are reducing agents, and vanadium(V) compounds are oxidizing agents. Vanadium(IV) compounds often exist as vanadyl derivatives which contain the VO2+ center.[7] Ammonium vanadate(V) (NH4VO3) can be successively reduced with elemental zinc to obtain the different colors of vanadium in these four oxidation states. Lower oxidation states occur in compounds such as V(CO)6,[V(CO)6]- and substituted derivatives.[7]

Oxy and oxo compounds
The oxyanion chemistry of vanadium(V) is complex. The vanadate ion, VO43−, is present in dilute solutions at high pH. On

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Vanadium

A ball-and-stick model of VO(acac)2 The Pourbaix diagram for vanadium in water.[9] acidification, HVO42- and H2VO4- are formed, analogous to HPO42- and H2PO4-. The acid dissociation constants for the vanadium and phosphorus series are remarkably similar. In more concentrated solutions many polyvanadates are formed. Chains, rings and clusters involving tetrahedral vanadium, analogous to the polyphosphates, are known. In addition, clusters such as the decavanadates V10O284− and HV10O283−, which predominate at pH 4-6, are formed in which compound is octahedral about vanadium.[7] The correspondence between vanadate and phosphate chemistry can be attributed to the similarity in size and charge of phosphorus(V) and vanadium(V). Orthovanadate VO43− is used in protein crystallography[10] to study the biochemistry of phosphate.[11] coordination numbers higher than 6, as is the case in [V(CN)7]4−. Thirdly, the vanadyl ion, VO2+, is featured in many complexes of vanadium(IV) such as vanadyl acetylacetonate (V(=O)(acac)2). In this complex, the vanadium is 5-coordinate, square pyramidal, meaning that a sixth ligand, such as pyridine, may be attached, though the association constant of this process is small. Many 5-coordinate vanadyl complexes have a trigonal bypyramidal geometry, such as [12] VO(Cl2(NMe3)2.

Organometallic compounds
Organometallic chemistry of vanadium is well developed, but organometallic compounds are of minor commercial significance. Vanadocene dichloride is a versatile starting reagent and even finds minor applications in organic chemistry.[13] Vanadium carbonyl, V(CO)6, is a rare example of a metal carbonyl containing an unpaired electron, but which exists without dimerization. The addition of an electron yields V(CO)6− (isoelectronic with Cr(CO)6), which may be further reduced with sodium in liquid ammonia to yield V(CO)53− (isoelectronic with Fe(CO)5).[14][15]

Halide compounds
Several halides are known for oxidation states +2, +3 and +4. VCl4 is the most important commercially. This liquid is mainly used as a catalyst for polymerization of dienes.

Coordination compounds
Vanadium’s early position in the transition metal series lead to three rather unusual features of the coordination chemistry of vanadium. Firstly, metallic vanadium has the electronic configuration [Ar]4s23d3, so compounds of vanadium are relatively electronpoor. Consequently, most binary compounds are Lewis acids (electron pair acceptors); examples are all the halides forming octahedral adducts with the formula VXnL6-n (X = halide; L = other ligand). Secondly, the vanadium ion is rather large and can achieve

Occurrence
See also: Category:Vanadate minerals Metallic vanadium is not found in nature, but is known to exist in about 65 different minerals. Economically significant examples include patronite (VS4),[16] vanadinite (Pb5(VO4)3Cl), and carnotite (K2(UO2)2(VO4)2·3H2O). Much of the world’s vanadium production is sourced from vanadium-bearing magnetite found in ultramafic gabbro bodies. Vanadium is mined mostly in South Africa, north-western China,

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Vanadium
in use, in all of which vanadium is produced as a byproduct of other processes.[21] Purification of vanadium is possible by the crystal bar process developed by Anton Eduard van Arkel and Jan Hendrik de Boer in 1925. It involves the formation of the metal iodide, in this example vanadium(III) iodide, and the subsequent decomposition to yield pure metal.[22] 2 V + 3 I2 2 VI3

Vanadinite and eastern Russia. In 2007 these three countries mined more than 95 % of the 58,600 tonnes of produced vanadium.[17] Vanadium is also present in bauxite and in fossil fuel deposits such as crude oil, coal, oil shale and tar sands. In crude oil, concentrations up to 1200 ppm have been reported. When such oil products are burned, the traces of vanadium may initiate corrosion in motors and boilers.[18] An estimated 110,000 tonnes of vanadium per year are released into the atmosphere by burning fossil fuels.[19] Vanadium has also been detected spectroscopically in light from the Sun and some other stars.[20]

Applications

Production
Most vanadium is used as ferrovanadium as an additive to improve steels. Ferrovanadium is produced directly by reducing a mixture of vanadium oxide, iron oxides and iron in an electric furnace. Vanadium-bearing magnetite iron ore is the main source for the production of vanadium.[21] The vanadium ends up in pig iron produced from vanadium bearing magnetite. During steel production, oxygen is blown into the pig iron, oxidizing the carbon and most of the other impurities, forming slag. Depending on the used ore, the slag contains up to 25% of vanadium.[21] Vanadium metal is obtained via a multistep process that begins with the roasting of crushed ore with NaCl or Na2CO3 at about 850 °C to give sodium metavanadate (NaVO3). An aqueous extract of this solid is acidified to give "red cake", a polyvanadate salt, which is reduced with calcium metal. As an alternative for small scale production, vanadium pentoxide is reduced with hydrogen or magnesium. Many other methods are also

Tool made from vanadium steel

Alloys
Approximately 85% of vanadium produced is used as ferrovanadium or as a steel additive.[21] The considerable increase of strength in steel containing small amounts of vanadium was discovered in the beginning of 20th century,[23] and from that time vanadium steel was used for applications in axles, bicycle frames, crankshafts, gears, and other critical components. Vanadium forms stable nitrides and carbides, resulting in a significant increase in the strength of the steel. There are two groups of vanadium containing steel alloy groups. Vanadium high-carbon steel alloys containing 0.15 to 0.25 percent vanadium and high speed tool steels (HSS) with a vanadium content ranges from 1 % to 5 %. For high speed tool steels, a hardness above HRC 60 can be achieved. HSS steel is used in surgical instruments and tools.[24] Vanadium stabilizes the beta form of titanium and increases the strength and

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Vanadium
oxide of vanadium, vanadium dioxide VO2, is used in the production of glass coatings, which blocks infrared radiation (and not visible light) at a specific temperature.[34] Vanadium oxide can be used to induce color centers in corundum to creat simulated alexandrite jewelry, although alexandrite in nature is a chrysoberyl.[35] The possibility to use vanadium redox couples in both half-cells, thereby eliminating the problem of cross contamination by diffusion of ions across the membrane is the advantage of vanadium redox rechargeable batteries.[36] Vanadate can be used for protecting steel against rust and corrosion by electrochemical conversion coating.[37] Lithium vanadium oxide has been proposed for use as a high energy density anode for lithium ion batteries, at 745 Wh/l when paired with a lithium cobalt oxide cathode.[38] It has ben proposed by some researchers that a small amount, 40 to 270 ppm, of vanadium in Wootz steel and Damascus steel, significantly improves the strength of the material, although it is unclear what the source of the vanadium was.[39]

Vanadium temperature stability of titanium. Mixed with aluminium in titanium alloys it is used in jet engines and high-speed airframes. One of the common alloys is Ti 6Al 4V a titanium alloy with 6% aluminium and 4% of vanadium.[25]

Biological role

Other uses
Vanadium is compatible with iron and titanium, therefore vanadium foil is used in cladding titanium to steel.[26] The moderate thermal neutron-capture cross-section and the short half-life of the isotopes produced by neutron capture makes vanadium a suitable material for the inner structure of a fusion reactor.[27][28] Several vanadium alloys show superconducting behaviour. The first A15 phase superconductor was a vanadium compound, V3Si, which was discovered in 1952.[29] Vanadium-gallium tape is used in superconducting magnets (17.5 teslas or 175,000 gauss). The structure of the superconducting A15 phase of V3Ga is similar to that of the more common Nb3Sn and Nb3Ti.[30] The most common oxide of vanadium Vanadium pentoxide, V2O5, is used as a catalyst in manufacturing sulfuric acid by the contact process[31] and as an oxidizer in maleic anhydride production.[32] Vanadium pentoxide is also used in making ceramics.[33] Another

Ascidiacea contain vanadium. Vanadium plays a very limited role in biology. A vanadium-containing nitrogenase is used by some nitrogen-fixing micro-organisms. Vanadium is essential to ascidians or sea squirts in vanadium chromagen proteins. The concentration of vanadium in their blood is more than 100 times higher than the concentration of vanadium in the seawater around them. Rats and chickens are also known to require vanadium in very small amounts and deficiencies result in reduced growth and impaired

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Vanadium
35 mg/m3 of vanadium be considered immediately dangerous to life and health. This is the exposure level of a chemical that is likely to cause permanent health problems or death.[54] Vanadium compounds are poorly absorbed through the gastrointestinal system. Inhalation exposures to vanadium and vanadium compounds result primarily in adverse effects on the respiratory system.[55][56][57] Quantitative data are, however, insufficient to derive a subchronic or chronic inhalation reference dose. Other effects have been reported after oral or inhalation exposures on blood parameters,[58][59] on liver,[60] on neurological development in rats,[61] and other organs.[62] There is little evidence that vanadium or vanadium compounds are reproductive toxins or teratogens. Vanadium pentoxide was reported to be carcinogenic in male rats and male and female mice by inhalation in an NTP study,[63] although the interpretation of the results has recently been disputed.[64] Vanadium has not been classified as to carcinogenicity by the U.S. EPA.[65]

Amanita muscaria contains amavadine. reproduction.[40] Vanadium is a relatively controversial dietary supplement, primarily for increasing insulin sensitivity[41] and bodybuilding. Whether it works for the latter purpose has not been proven, and there is some evidence that athletes who take it are merely experiencing a placebo effect.[42] Vanadyl sulfate may improve glucose control in people with type 2 diabetes.[43][44][45][46][47] Ten percent of the blood cell pigment of the sea cucumber is vanadium. Just as the horseshoe crab has blue blood due to copper in hemocyanin, and land animals have red blood from the iron in hemoglobin, the blood of the sea cucumber is yellow because of the vanadium in the vanabin pigment.[48] Nonetheless, there is no evidence that vanabins carry oxygen, in contrast to hemoglobin and hemocyanin.[49] Several species of macrofungi, namely Amanita muscaria and related species, accumulate vanadium (up to 500 mg/ kg in dry weight). Vanadium is present in the coordination complex, amavadine,[50] in fungal fruit-bodies. However, the biological importance of the accumulation process is unknown.[51][52]

References
[1] Pedro Cintas (2004). "The Road to Chemical Names and Eponyms: Discovery, Priority, and Credit". Angewandte Chemie International Edition 43 (44): 5888 – 5894. doi:10.1002/anie.200330074. [2] ^ Sefström, N. G. (1831). "Ueber das Vanadin, ein neues Metall, gefunden im Stangeneisen von Eckersholm, einer Eisenhütte, die ihr Erz von Taberg in Småland bezieht". Annalen der Physik und Chemie 97 (1): 43–49. doi:10.1002/ andp.18310970103. [3] Featherstonhaugh, George William (1831). The Monthly American Journal of Geology and Natural Science: 69. [4] Henry E. Roscoe (1869 – 1870). "Researches on Vanadium.--Part II.". Proceedings of the Royal Society of London 18: 37–42. doi:10.1098/ rspl.1869.0012. http://www.jstor.org/ stable/112705. [5] Marden, J. W.; Rich, M. N. (1927). "Vanadium". Industrial and Engineering Chemistry 19 (7): 786–788. doi:10.1021/ ie50211a012. [6] Betz, Frederick (2003). Managing Technological Innovation: Competitive

Safety
All vanadium compounds should be considered to be toxic. Tetravalent VOSO4 has been reported to be over 5 times more toxic than trivalent V2O3.[53] The Occupational Safety and Health Administration (OSHA) has set an exposure limit of 0.05 mg/m3 for vanadium pentoxide dust and 0.1 mg/m3 for vanadium pentoxide fumes in workplace air for an 8-hour workday, 40-hour work week.[54] The National Institute for Occupational Safety and Health (NIOSH) has recommended that

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Advantage from Change. Wiley-IEEE. pp. 158–159. ISBN 0471225630. http://books.google.com/ books?id=KnpGtu-R77UC&pg=PA158. [7] ^ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils; (1985). "Vanadium" (in German). Lehrbuch der Anorganischen Chemie (91–100 ed.). Walter de Gruyter. pp. 1071–1075. ISBN 3110075113. [8] ^ Georges, Audi (2003). "The NUBASE Evaluation of Nuclear and Decay Properties". Nuclear Physics A (Atomic Mass Data Center) 729: 3–128. doi:10.1016/j.nuclphysa.2003.11.001. [9] Al-Kharafi, F. M.; Badawy, W. A. (1997). "Electrochemical behaviour of vanadium in aqueous solutions of different pH". Electrochimica Acta 42 (4): 579–586. doi:10.1016/S0013-4686(96)00202-2. [10] Sinning, Irmgard (2004). "The power of vanadate in crystallographic investigations of phosphoryl transfer enzymes". FEBS letters 577 (3): 315–321. doi:10.1016/ j.febslet.2004.10.022. [11] Seargeant, Lorne E.; Stinson, Robert A. (1979). "Inhibition of Human Alkaline Phosphatases by Vanadate". Biochemical Journal 181: 247–250. [12] Greenwood, Norman N.; Earnshaw, A. (1997), Chemistry of the Elements (2nd ed.), Oxford: Butterworth-Heinemann, ISBN 0-7506-3365-4 Chapter 22 [13] G. Wilkinson and J.G. Birmingham (1954). "Bis-cyclopentadienyl Compounds of Ti, Zr, V, Nb and Ta". Journal of the American Chemical Society 76 (17): 4281–4284. doi:10.1021/ ja01646a008. [14] Bellard, S.; Rubinson, K. A.; Sheldrick, G. M. (1979). "Crystal and molecular structure of vanadium hexacarbonyl". Acta Crystallographica B35: 271–274. doi:10.1107/S0567740879003332. [15] Elschenbroich, C.; Salzer A. (1992). Organometallics : A Concise Introduction. Wiley-VCH. ISBN 3527281657. [16] "mineralogical data about Patrónite". mindata.org. http://www.mindat.org/ min-3131.html. Retrieved on 2009-01-19. [17] Magyar, Michael J.. "Mineral Commodity Summaries 2008: Vanadium". United States Geological Survey. http://minerals.usgs.gov/minerals/pubs/

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commodity/vanadium/ mcs-2008-vanad.pdf. Retrieved on 2009-01-15. [18] Pearson, C. D.; Green J. B. (1993). "Vanadium and nickel complexes in petroleum resid acid, base, and neutral fractions". Energy Fuels 7 (3): 338. doi:10.1021/ef00039a001. [19] Anke, Manfred (2004). "Vanadium - An element both essential and toxic to plants, animals and humans?". Anal. Real Acad. Nac. Farm. 70: 961–999. http://www.ranf.com/pdf/anales/2004/ 0406.pdf. [20] Cowley, C. R.; Elste, G. H.; Urbanski, J. L. (1978). "Vanadium abundances in early A stars". Astronomical Society of the Pacific 90: 536–542. doi:10.1086/ 130379. Bibcode: 1978PASP...90..536C. [21] ^ Moskalyk, R. R.; Alfantazi, A. M. (2003). "Processing of vanadium: a review". Minerals Engineering 16 (9, September 2003): 793–805. doi:10.1016/ S0892-6875(03)00213-9. [22] Carlson, O. N.; Owen, C. V. (1961). "Preparation of High-Purity Vanadium Metals by the Iodide Refining Process". Journal of the Electrochemical Society 108 (1): 88–93. doi:10.1149/1.2428019. [23] Chandler, Harry (1998). Metallurgy for the Non-metallurgist. ASM International. pp. 6–7. ISBN 9780871706522. http://books.google.de/ books?id=arupok8PTBEC. [24] Davis, Joseph R. (1995). Tool Materials: Tool Materials. ASM International. ISBN 9780871705457. http://books.google.de/ books?id=Kws7x68r_aUC&pg=PA11. [25] Peters, Manfred; Leyens, C. (2002). "Metastabile β-Legierungen". Titan und Titanlegierungen. Wiley-VCH. pp. 23–24. ISBN 9783527305391. http://books.google.de/ books?id=sxdR882jQpYC&pg=PA23. [26] Lositskii, N. T.; Grigor’ev A. A.; Khitrova, G. V. (1966). "Welding of chemical equipment made from two-layer sheet with titanium protective layer (review of foreign literature)". Chemical and Petroleum Engineering 2 (12): 854–856. doi:10.1007/BF01146317. [27] Matsui, H.; Fukumoto, K.; Smith, D. L.; Chung, Hee M.; Witzenburg, W. van; Votinov, S. N. (1996). "Status of vanadium alloys for fusion reactors". Journal of Nuclear Materials 233–237

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(1): 92–99. doi:10.1016/ S0022-3115(96)00331-5. [28] "Vanadium Data Sheet". Allegheny Technologies – Wah Chang. http://www.wahchang.com/pages/ products/data/pdf/Vanadium.pdf. Retrieved on 2009-01-16. [29] Hardy, George F.; Hulm, John K. (1953). "Superconducting Silicides and Germanides". Physical Reviews 89: 884–884. doi:10.1103/PhysRev.89.884. [30] Markiewicz, W.; Mains, E.; Vankeuren, R.; Wilcox, R.; Rosner, C.; Inoue, H.; Hayashi, C.; Tachikawa, K. (1977). "A 17.5 Tesla superconducting concentric Nb3Sn and V3Ga magnet system". IEEE Transactions on Magnetics 13 (1): 35–37. doi:10.1109/ TMAG.1977.1059431. [31] Eriksen, K. M.; Karydis, D. A.; Boghosian, S.; Fehrmann, R. (1995). "Deactivation and Compound Formation in SulfuricAcid Catalysts and Model Systems". Journal of Catalysis 155 (1): 32–42. doi:10.1006/jcat.1995.1185. [32] Abon, Michel; Volta, Jean-Claude (1997). "Vanadium phosphorus oxides for nbutane oxidation to maleic anhydride". Applied Catalysis A: General 157: 173–193. doi:10.1016/ S0926-860X(97)00016-1. [33] Lide, David R. (2004). "vanadium". CRC Handbook of Chemistry and Physics. Boca Raton: CRC Press. pp. 4–34. ISBN 9780849304859. [34] Manning, Troy D.; Parkin,Ivan P.; Clark, Robin J. H.; Sheel, David; Pemble, Martyn E.; Vernadou, Dimitra (2002). "Intelligent window coatings: atmospheric pressure chemical vapour deposition of vanadium oxides". Journal of Materials Chemistry 12: 2936–2939. doi:10.1039/b205427m. [35] White, Willam B.; Roy, Rustum; McKay, Chrichton (1962). "The Alexandrite Effect: And Optical Study". American Mineralogist 52: 867–871. http://www.minsocam.org/ammin/AM52/ AM52_867.pdf. [36] Joerissen, Ludwig; Garche, Juergen; Fabjan, Ch.; Tomazic G. (2004). "Possible use of vanadium redox-flow batteries for energy storage in small grids and standalone photovoltaic systems". Journal of Power Sources 127: 98–104. doi:10.1016/j.jpowsour.2003.09.066.

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[37] Guan, H.; Buchheit R. G. (2004). "Corrosion Protection of Aluminum Alloy 2024-T3 by Vanadate Conversion Coatings". Corrosion 60 (3): 284–296. [38] Kariatsumari, Koji (February 2008). "LiIon Rechargeable Batteries Made Safer". Nikkei Business Publications, Inc.. http://techon.nikkeibp.co.jp/article/ HONSHI/20080129/146549/. Retrieved on 10-12-2008. [39] Verhoeven, J. D.; Pendray, A. H.; Dauksch, W. E. (1998). "The key role of impurities in ancient damascus steel blades". Journal of the Minerals, Metals and Materials Society 50 (9): 58–64. doi:10.1007/s11837-998-0419-y. [40] Schwarz, Klaus; Milne, David B. (1971). "Growth Effects of Vanadium in the Rat". Science 174 (4007): 426–428. doi:10.1126/science.174.4007.426. PMID 5112000. http://www.jstor.org/stable/ 1731776. [41] Yeh, Gloria Y.; Eisenberg, David M.; Kaptchuk, Ted J.; Phillips, Russell S. (2003). "Systematic Review of Herbs and Dietary Supplements for Glycemic Control in Diabetes". Diabetes Care 26: 1277–1294. doi:10.2337/ diacare.26.4.1277. PMID 12663610. http://care.diabetesjournals.org/cgi/ content/full/26/4/1277. [42] Talbott,, Shawn M.; Hughes, Kerry (2007). "Vanadium". The Health Professional’s Guide to Dietary Supplements. Lippincott Williams & Wilkins. pp. 419–422. ISBN 9780781746724. http://books.google.com/ books?id=hV2_TdmoDo8C&pg=PA419. [43] Halberstam, M, et al. (1996). "Oral vanadyl sulfate improves insulin sensitivity in NIDDM but not in obese nondiabetic subjects.". Diabetes 45: 659–66. doi:10.2337/diabetes.45.5.659. PMID 8621019. [44] Boden, G, et al. (1996;). "Effects of vanadyl sulfate on carbohydrate and lipid metabolism in patients with non-insulin dependent diabetes mellitus.". Metabolism 45: 1130–5. doi:10.1016/ S0026-0495(96)90013-X. [45] Goldfine, AB, et al. (2000). "Metabolic effects of vanadyl sulfate in humans with non-insulin-dependent diabetes mellitus: in vivo and in vitro studies.". Metabolism

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49: 400–10. doi:10.1016/ S0026-0495(00)90418-9. [46] Badmaev, V, et al. (1999). "Vanadium: a review of its potential role in the fight against diabetes.". Altern Complement Med. 5: 273–291. doi:10.1089/ acm.1999.5.273. [47] Goldwaser, I, et al. (1999). "L-Glutamic Acid gamma -Monohydroxamate. A Potentiator of Vanadium-Evoked Glucose Metabolism in vitro and in vivo". J Biol Chem 274: 26617–26624. doi:10.1074/ jbc.274.37.26617. PMID 10473627. [48] Natkin, Michael (2007). "Blood Color". Science Facts. Soak (Source Of All Knowledge). http://www.soak.com/topic/ sciencefacts/article/tshow/98556/ blood+color. Retrieved on 2007-11-16. [49] Rehder, Dieter (1992). "Structure and function of vanadium compounds in living organisms". BioMetals 5 (1): 3–12. doi:10.1007/BF01079691. [50] Kneifel, Helmut; Bayer, Ernst (1997). "Determination of the Structure of the Vanadium Compound, Amavadine, from Fly Agaric". Angewandte Chemie International Edition in English 12 (6): 508. ISSN 10.1002/anie.197305081. [51] Falandysz, J.; Kunito, T., Kubota, R.; Lipka, K.; Mazur, A.; Falandysz, Justyna J.; Tanabe, S. (2007). "Selected elements in fly agaric Amanita muscaria". Journal of Environmental Science and Health, Part A 42 (11): 1615–1623. doi:10.1080/ 10934520701517853. [52] Berry, Robert E.; Armstrong, Elaine M.; Beddoes, Roy L.; Collison, David; Ertok, Nigar; Helliwell, Madeleine; Garner, David (1999). "The Structural Characterization of Amavadin". Angew. Chem. Int. Ed. 38 (6): 795–797. doi:10.1002/ (SICI)1521-3773(19990315)38:6<795::AIDANIE795>3.0.CO;2-7. [53] Roschin, A. V. (1967). "Toxicology of vanadium compounds used in modern industry". Gig Sanit. (Water Res.) 32: 26–32. [54] ^ "Occupational Safety and Health Guidelines for Vanadium Pentoxide". Occupational Safety and Health Administration. http://www.osha.gov/ SLTC/healthguidelines/ vanadiumpentoxidedust/ recognition.html. Retrieved on 2009-01-29.

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[55] Sax, N. I. (1984). Dangerous Properties of Industrial Materials, 6th ed.. Van Nostrand Reinhold Company. pp. 2717–2720. [56] N. B. Ress, B. J. Chou, R. A. Renne, J. A. Dill, R. A. Miller, J. H. Roycroft, J. R. Hailey, J. K. Haseman and J. R. Bucher (2003). "Carcinogenicity of Inhaled Vanadium Pentoxide in F344/N Rats and B6C3F1 Mice". Toxicological Sciences 74: 2876–296. doi:10.1093/toxsci/ kfg136. PMID 12773761. [57] Jörg M. Wörle-Knirsch, Katrin Kern, Carsten Schleh, Christel Adelhelm, Claus Feldmann, and Harald F. Krug (2007). "Nanoparticulate Vanadium Oxide Potentiated Vanadium Toxicity in Human Lung Cells". Environ. Sci. Technol. 41: 331–336. doi:10.1021/es061140x. [58] Ścibior, A.; Zaporowska, H.; Ostrowski, J. (2006). "Selected haematological and biochemical parameters of blood in rats after subchronic administration of vanadium and/or magnesium in drinking water". Archives of Environmental Contamination and Toxicology 51 (2): 287–295. doi:10.1007/ s00244-005-0126-4. [59] Gonzalez-Villalva, A.; et al. (2006). "Thrombocytosis induced in mice after subacute and subchronic V2O5 inhalation". Toxicology and Industrial Health 22 (3): 113–116. doi:10.1191/ 0748233706th250oa. PMID 16716040. [60] Kazuo Kobayashia, Seiichiro Himeno, Masahiko Satoh, Junji Kuroda, Nobuo Shibata, Yoshiyuki Seko and Tatsuya Hasegawa (2006,). "Pentavalent vanadium induces hepatic metallothionein through interleukin-6-dependent and independent mechanisms". Toxicology 228: 162–170. doi:10.1016/ j.tox.2006.08.022. [61] Soazo, Marina; Garcia, Graciela Beatriz (2007). "Vanadium exposure through lactation produces behavioral alterations and CNS myelin deficit in neonatal rats". Neurotoxicology and Teratology 29 (4): 503–510. doi:10.1016/j.ntt.2007.03.001. [62] Barceloux, Donald G.; Barceloux, Donald (1999). "Vanadium". Clinical Toxicology 37 (2): 265–278. doi:10.1081/ CLT-100102425. [63] Ress, N. B.; et al. (2003). "Carcinogenicity of inhaled vanadium

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pentoxide in F344/N rats and B6C3F1 mice". Toxicological Sciences 74 (2): 287–296. doi:10.1093/toxsci/kfg136. PMID 12773761. [64] Duffus, J. H. (2007). "Carcinogenicity classification of vanadium pentoxide and inorganic vanadium compounds, the NTP study of carcinogenicity of inhaled vanadium pentoxide, and vanadium chemistry". Regulatory Toxicology and Pharmacology 47 (1): 110–114. doi:10.1016/j.yrtph.2006.08.006. [65] Opreskos, Dennis M. (1991). "Toxicity Summary for Vanadium". Oak Ridge

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National Laboratory. http://rais.ornl.gov/ tox/profiles/old/vanadium_f_V1.htm. Retrieved on 2008-11-08.

External links
• The periodic table of videos videos of the chemistry of the elements • Los Alamos National Laboratory – Vanadium • WebElements.com – Vanadium • ATSDR – ToxFAQs: Vanadium

Retrieved from "http://en.wikipedia.org/wiki/Vanadium" Categories: Chemical elements, Dietary minerals, Transition metals, Vanadium, Biology and pharmacology of chemical elements This page was last modified on 19 May 2009, at 12:06 (UTC). All text is available under the terms of the GNU Free Documentation License. (See Copyrights for details.) Wikipedia® is a registered trademark of the Wikimedia Foundation, Inc., a U.S. registered 501(c)(3) taxdeductible nonprofit charity. Privacy policy About Wikipedia Disclaimers

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