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Vanadium - Wikipedia, the free encyclopedia /**/ /**/ if (wgNotice != '') document.writeln(wgNotice); Vanadium From Wikipedia, the free encyclopedia Jump to: navigation, search 23titanium ← vanadium → chromium-↑V↓Nb Periodic table - Extended periodic tableGeneralName, symbol, numbervanadium, V, 23Element categorytransition metalsGroup, period, block5, 4, dAppearancesilver-grey metal Standard atomic weight50.9415(1) g·mol−1Electron configuration[Ar] 3d3 4s2Electrons per shell2, 8, 11, 2Physical propertiesPhasesolidDensity (near r.t.)6.0 g·cm−3Liquid density at m.p.5.5 g·cm−3Melting point2183 K(1910 °C, 3470 °F)Boiling point3680 K(3407 °C, 6165 °F)Heat of fusion21.5 kJ·mol−1Heat of vaporization459 kJ·mol−1Specific heat capacity(25 °C) 24.89 J·mol−1·K−1Vapor pressureP/Pa1101001 k10 k100 kat T/K210122892523281431873679Atomic propertiesCrystal structurecubic body centeredOxidation states5, 4, 3, 2, 1 [1](amphoteric oxide)Electronegativity1.63 (Pauling scale)Ionization energies(more)1st: 650.9 kJ·mol−12nd: 1414 kJ·mol−13rd: 2830 kJ·mol−1Atomic radius135 pmAtomic radius (calc.)171 pmCovalent radius125 pmMiscellaneousMagnetic orderingparamagneticElectrical resistivity(20 °C) 197 nΩ·mThermal conductivity(300 K) 30.7 W·m−1·K−1Thermal expansion(25 °C) 8.4 µm·m−1·K−1Speed of sound (thin rod)(20 °C) 4560 m/sYoung's modulus128 GPaShear modulus47 GPaBulk modulus160 GPaPoisson ratio0.37Mohs hardness6.7CAS registry number7440-62-2Selected isotopesMain article: Isotopes of vanadiumisoNAhalf-lifeDMDE (MeV)DP48Vsyn15.9735 dε+β+4.012348Ti49Vsyn330 dε0.601949Ti50V0.25%1.5×1017yε2.208350Tiβ-1.036950Cr51V99.75%51V is stable with 28 neutronsReferencesThis box: view • talk • edit  The Pourbaix diagram for vanadium in water.Vanadium (IPA: /vəˈneɪdiəm/) is a chemical element that has the symbol V and atomic number 23. A soft and ductile element, vanadium naturally occurs in about 65 different minerals and is used mainly to produce certain alloys. It is one of the 26 elements found in most living organisms.Contents1 Notable characteristics2 Applications3 History4 Occurrence5 Isolation6 Compounds6.1 Toxicity of vanadium compounds6.2 Various oxidation states of vanadium ions7 Isotopes8 Precautions9 See also10 Footnotes11 References12 External links//[edit] Notable characteristicsVanadium is a soft and ductile, silver-grey metal. It has good resistance to corrosion by alkalis, sulfuric and hydrochloric acid. It oxidizes readily at about 933 K (660 °C). Vanadium has good structural strength and a low fission neutron cross section, making it useful in nuclear applications. Although a metal, it shares with chromium and manganese the property of having valency oxides with acid properties.Common oxidation states of vanadium include +2, +3, +4 and +5. A popular experiment with ammonium vanadate NH4VO3, reducing the compound with zinc metal, can demonstrate colorimetrically all four of these vanadium oxidation states. An oxidation state of +1 is rarely seen.[edit] ApplicationsApproximately 80% of vanadium produced is used as ferrovanadium or as a steel additive.[citation needed] Other uses:In such alloys asspecialty stainless steel, e.g. for use in surgical instruments and tools.rust resistant and high speed tool steels.mixed with aluminium in titanium alloys used in jet engines and high-speed airframesVanadium high-carbon steel alloys containing 0.15 to 0.25 percent vanadium to harden and toughen it are used in axles, bicycle frames, crankshafts, gears, and other critical components.It is an important carbide stabilizer in making steels.Because of its low fission neutron cross section, vanadium has nuclear applications.Vanadium foil is used in cladding titanium to steel.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 comon Nb3Sn and Nb3Ti.[1] The first A15 phase superconductur was also a vanadium compound. V3Si, which was disovered in 1952.[2]Vanadium pentoxide V2O5 is used as a catalyst in manufacturing sulfuric acid (via the contact process) and maleic anhydride. It is also used in making ceramics and glass manufacturing.Glass coated with vanadium dioxide VO2 can block infrared radiation (and not visible light) at a specific temperature.Electrical fuel cells and storage batteries such as vanadium redox batteries.Added to corundum to make simulated alexandrite jewelry.Vanadate electrochemical conversion coatings for protecting steel against rust and corrosionLithium vanadium oxide is 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.[2]Used to make lacrosse shaftsPossibly used to make Wootz steel and Damascus steel.[edit] HistoryVanadium (named after Vanadis, another name for Freya, the Scandinavian goddess of fertility) was originally discovered by Andrés Manuel del Río (a Spanish-born Mexican mineralogist) in Mexico City, in 1801. He discovered the element after being sent a sample of "brown lead" ore (now named vanadinite). Through experimentation, he found it to form salts with a wide variety of colors, so he named the element panchromium (Greek: all colors). He later renamed this compound erythronium, since most of the salts turned red when heated. The French chemist Hippolyte Victor Collet-Descotils incorrectly declared that del Río's new element was only impure chromium. Del Río thought himself to be mistaken and accepted the statement of the French chemist that was also backed by del Río's friend Baron Alexander von Humboldt.[3]In 1831, Sefström of Sweden rediscovered vanadium in a new oxide he found while working with some iron ores and later that same year Friedrich Wöhler confirmed del Río's earlier work.[4] Later, George William Featherstonhaugh, one of the first US geologists, suggested that the element should be named "rionium" after del Río, but this never happened.Metallic vanadium was isolated by Henry Enfield Roscoe in 1867, who reduced vanadium(III) chloride VCl3 with hydrogen.[5] The name vanadium comes from Vanadis, a goddess in Scandinavian mythology, because the element has beautiful multicolored chemical compounds.[4]Vanadium is mined mostly in South Africa, Namibia, Botswana, Zimbabwe, Zambia, north west China, the Great Plains of USA, eastern Russia and Kazakhstan.[edit] Occurrence VanadiniteVanadium is never found unbound in nature but it does occur in about 65 different minerals among which are patronite VS4, vanadinite Pb5(VO4)3Cl, and carnotite K2(UO2)2(VO4)2.3H2O.By far the greatest proportion of the world's vanadium production is sourced from vanadium-bearing magnetite found in ultramafic gabbro bodies. From these ores vanadium can be calcined to form ferrovanadium, or can be recovered from the vanadium steel smelting process which is widely used in Russia and China.Vanadium is also present in bauxite, and in carbon containing deposits such as crude oil, coal, oil shale and tar sands. Vanadium has also been detected spectroscopically in light from the Sun and some other stars.Much of the vanadium metal being produced is now made by calcium reduction of V2O5 in a pressure vessel. Vanadium is usually recovered as a by-product or co-product, and so world resources of the element are not really indicative of available supply.See also category:vanadate minerals.[edit] IsolationVanadium is available commercially and production of a sample in the laboratory is not normally required. Commercially, routes leading to metallic vanadium as main product are not usually required as enough is produced as byproduct in other processes.In industry, heating of vanadium ore or residues from other processes with salt NaCl or sodium carbonate Na2CO3 at about 850°C gives sodium vanadate NaVO3. This is dissolved in water and acidified to give a red solid which in turn is melted to form a crude form of vanadium pentoxide V2O5. Reduction of vanadium pentoxide with calcium gives pure vanadium. An alternative suitable for small scales is the reduction of vanadium pentachloride VCl5 with hydrogen or magnesium. Many other methods are also in use.Industrially, most vanadium is used as an additive to improve steels. Rather than proceed via pure vanadium metal it is often sufficient to react the crude of vanadium pentoxide V2O5 with crude iron. This produces ferrovanadium suitable for further work.[edit] CompoundsVanadium pentoxide V2O5 is used as a catalyst principally in the production of sulfuric acid. It is the source of vanadium used in the manufacture of ferrovanadium. It can be used as a dye and color-fixer.Vanadyl sulfate VOSO4, also called vanadium(IV) sulfate oxide hydrate, is used as a relatively controversial dietary supplement, primarily for increasing insulin sensitivity and body-building. 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.Anhydrous VCl4 is a liquid at room temperature and reacts violently with water; it can be used, in conjunction with an appropriate nitrogen compound, for vapour deposition of hard VN layers [3]. Vanadium pentafluoride is an extremely powerful fluorinating agent, capable of perfluorinating chloroalkanes [4], and has been proposed (eg [5]) as a safe and economical substitute for XeF2(Xenon difluoride)); it is also liquid at room temperature.Orthovanadate VO43- is used in biochemistry as a phosphate analogue; in protein crystallography it can be used to make phosphate binding sites very visible in electron density.Vanadium forms polyoxometalate cluster compounds, including V10 O24.[edit] Toxicity of vanadium compoundsThe toxicity of vanadium depends on its physico-chemical state; particularly on its valence state and solubility. Tetravalent VOSO4 has been reported to be more than 5 times as toxic as trivalent V2O3 (Roschin, 1967). Vanadium compounds are poorly absorbed through the gastrointestinal system. Inhalation exposures to vanadium and vanadium compounds result primarily in adverse effects to the respiratory system (Sax, 1984; ATSDR, 1990; Ress et al., 2003; Worle-Knirsch et al., 2007). Quantitative data are, however, insufficient to derive a subchronic or chronic inhalation reference dose. Other effects have been reported on blood parameters after oral or inhalation exposures (Scibior et al., 2006; Gonzalez-Villalva et al., 2006), on liver (Kobayashi et al., 2006), neurological development in rats (Soaso and Garcia, 2007), and other organs.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 (Ress et al., 2003), although the interpretation of the results has recently been disputed (Duffus, 2007). Vanadium has not been classified as to carcinogenicity by the U.S. EPA (1991a).[6][edit] Various oxidation states of vanadium ionsIt is known that vanadium gets the oxidation states +2, +3, +4, +5. To observe the colors of these states, ammonium metavanadate (NH4VO3) can be used as a starting agent. It must be acidified beforehand so dioxovanadium(V) ion, VO2+ (yellow +5 oxidation number) is produced. In alkaline medium, the stable form of vanadium(V) state is VO3-.Adding zinc powder and concentrated hydrochloric acid continuously, VO2+ is reduced into blue VO2+.It can be seen that during the reaction, the mixture is green in colour as the original yellow of the +5 state and the blue of the +4 are present.Continuously adding Zn powder and concentrated HCl, blue VO2+ is reduced to green V3+. V3+ is then reduced to violet V2+ by Zn powder and concentrated HCl again.See also Vanadium compounds.See also Vanadium(V) oxide.[edit] IsotopesMain article: Isotopes of vanadiumNaturally occurring vanadium is composed of one stable isotope 51V and one radioactive isotope 50V with a half-life of 1.5×1017 years. 24 artificial radioisotopes have been characterized (in the range of mass number between 40 and 65) with the most stable being 49V with a half-life of 330 days, and 48V with a half-life of 15.9735 days. All of the remaining radioactive isotopes have half-lives shorter than an hour, the majority of them below 10 seconds. In 4 isotopes, metastable excited states were found (including 2 metastable states for 60V).The primary decay mode before the most abundant stable isotope 51V is electron capture. The next most common mode is beta decay. The primary decay products before 51V are element 22 (titanium) isotopes and the primary products after are element 24 (chromium) isotopes.[edit] PrecautionsPowdered metallic vanadium is a fire hazard, and unless known otherwise, all vanadium compounds should be considered highly toxic. Generally, the higher the oxidation state of vanadium, the more toxic the compound is. The most dangerous compound is vanadium pentoxide.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.The National Institute for Occupational Safety and Health (NIOSH) has recommended that 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.[edit] See alsoVanadium compoundsVanadium mineralsVanadate minerals[edit] Footnotes^ 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. ^ Hardy, George F.; Hulm, John K. (1953). "Superconducting Silicides and Germanides". Physical Reviews 89: 884 - 884. doi:10.1103/PhysRev.89.884. ^ 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. ^ a b N. G. Sefström (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. ^ Henry E. Roscoe (1869 – 1870). "Researches on Vanadium.--Part II.". Proceedings of the Royal Society of London 18: 37–42, http://www.jstor.org/stable/112705. ^ Opreskos, Dennis M. (1991). "Toxicity Summary for VANADIUM". Retrieved on 2008-11-08.[edit] ReferencesLos Alamos National Laboratory – VanadiumHigh vanadium content in Mt.Fuji groundwater and its relevance to the ancient biosphere by Tatsuo Hamada in Vanadium in Environment. Part 1: Chemistry and Biochemistry. Edited by Jerome O. Nriagu. Page 97-123. 1998. John Wilen & Sons, Inc.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. Gonzalez-Villalva, A.; et al.. "Thrombocytosis induced in mice after subacute and subchronic V2O5 inhalation". Toxicology and Industrial Health 22 (3): 113–116. doi:10.1191/0748233706th250oa. Kobayashi, K.; et al. (2006). "Pentavalent vanadium induces hepatic metallothionein through interleukin-6-dependent and -independent mechanisms". Toxicology 228 (2–3): 162–170. doi:10.1016/j.tox.2006.08.022. Ress, N. B.; et al. (2003). "Carcinogenicity of inhaled vanadium pentoxide in F344/N rats and B6C3F1 mice". Toxicological Sciences 74 (2): 287–296. doi:10.1093/toxsci/kfg136. 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. 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. Wörle-Knirsch, Jörg M.; et al. (2007). "Nanoparticulate Vanadium Oxide Potentiated Vanadium Toxicity in Human Lung Cells". Environ. Sci. Technol. 41 (1): 331–336. doi:10.1021/es061140x. [edit] External links Wikimedia Commons has media related to: Vanadium Look up vanadium inWiktionary, the free dictionary.WebElements.com – VanadiumMineral Information Institute – VanadiumATSDR – ToxFAQs: VanadiumThe Vanadium Redox Battery was invented at The University of New South WalesVanadium general infosOxidation States of Vanadium, with video demostration and electrode potentials relevantRedox chemistry quoted Vanadium as illustrationsThe (REACH) Vanadium ConsortiumComprehensive Data on Vanadiumv • d • ePeriodic tableH HeLiBe BCNOFNeNaMg AlSiPSClArKCa ScTiVCrMnFeCoNiCuZnGaGeAsSeBrKrRbSr YZrNbMoTcRuRhPdAgCdInSnSbTeIXeCsBaLaCePrNdPmSmEuGdTbDyHoErTmYbLuHfTaWReOsIrPtAuHgTlPbBiPoAtRnFrRaAcThPaUNpPuAmCmBkCfEsFmMdNoLrRfDbSgBhHsMtDsRgUubUutUuqUupUuhUusUuoUueUbn Alkali metalsAlkaline earth metalsLanthanoidsActinoidsTransition metalsOther metalsMetalloidsOther nonmetalsHalogensNoble gasesRetrieved from "http://en.wikipedia.org/wiki/Vanadium" Categories: Chemical elements | Dietary minerals | Transition metals | VanadiumHidden categories: All articles with unsourced statements | Articles with unsourced statements since September 2008 Views Article Discussion Edit this page History Personal tools Log in / create account if (window.isMSIE55) fixalpha(); Navigation Main page Contents Featured content Current events Random article Search Interaction About Wikipedia Community portal Recent changes Contact Wikipedia Donate to Wikipedia Help Toolbox What links here Related changesUpload fileSpecial pages Printable version Permanent linkCite this page Languages Afrikaans العربية Asturianu বাংলা Беларуская Bosanski Български Català Česky Corsu Cymraeg Dansk Deutsch Eesti Ελληνικά Español Esperanto Euskara فارسی Français Furlan Gaelg Galego 한국어 Հայերեն हिन्दी Hrvatski Ido Bahasa Indonesia Íslenska Italiano עברית Basa Jawa ಕನ್ನಡ Kiswahili Kreyòl ayisyen Kurdî / كوردی Latina Latviešu Lëtzebuergesch Lietuvių Lojban Magyar മലയാളം मराठी Nederlands 日本語 Norsk (bokmål) Norsk (nynorsk) Occitan O'zbek ਪੰਜਾਬੀ Polski Português Română Runa Simi Русский Sicilianu Simple English Slovenčina Slovenščina Српски / Srpski Srpskohrvatski / Српскохрватски Suomi Svenska தமிழ் ไทย Tiếng Việt Türkçe Українська 中文   This page was last modified on 2 December 2008, at 15:13. 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