titanium ← vanadium → chromium - ↑ V ↓ Nb 23V Periodic table Appearance blue-silver-grey metal General properties Name, symbol, number vanadium, V, 23 Pronunciation /vəˈneɪdiəm/ və-NAY-dee-əm Element category transition metal Group, period, block 5, 4, d Standard atomic weight 50.9415g·mol−1 Electron configuration Ar 3d3 4s2 Electrons per shell 2, 8, 11, 2 (Image) Physical properties Phase solid Density (near r.t.) 6.0 g·cm−3 Liquid density at m.p. 5.5 g·cm−3 Melting point 2183 K, 1910 °C, 3470 °F Boiling point 3680 K, 3407 °C, 6165 °F Heat of fusion 21.5 kJ·mol−1 Heat of vaporization 459 kJ·mol−1 Specific heat capacity (25 °C) 24.89 J·mol−1·K−1 Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 2101 2289 2523 2814 3187 3679 Atomic properties Oxidation states 5, 4, 3, 2, 1, -1 (amphoteric oxide) Electronegativity 1.63 (Pauling scale) Ionization energies (more) 1st: 650.9 kJ·mol−1 2nd: 1414 kJ·mol−1 3rd: 2830 kJ·mol−1 Atomic radius 134 pm Covalent radius 153±8 pm Miscellanea Crystal structure body-centered cubic Magnetic ordering paramagnetic Electrical resistivity (20 °C) 197 nΩ·m Thermal conductivity (300 K) 30.7 W·m−1·K−1 Thermal expansion (25 °C) 8.4 µm·m−1·K−1 Speed of sound (thin rod) (20 °C) 4560 m/s Young's modulus 128 GPa Shear modulus 47 GPa Bulk modulus 160 GPa Poisson ratio 0.37 Mohs hardness 6.7 CAS registry number 7440-62-2 Most stable isotopes Main article: Isotopes of vanadium iso NA half-life DM DE (MeV) DP 48V syn 15.9735 d ε+β+ 4.0123 48Ti 49V syn 330 d ε 0.6019 49Ti 50V 0.25% 1.5×1017y ε 2.2083 50Ti β− 1.0369 50Cr 51V 99.75% 51V is stable with 28 neutrons v · d · e Vanadium ( /vəˈneɪdiəm/ və-NAY-dee-əm) is a chemical element with the symbol V and atomic number 23. It is a soft, silvery gray, ductile transition metal. The formation of an oxide layer stabilizes the metal against oxidation. The element is found only in chemically combined form in nature. Andrés Manuel del Río discovered vanadium in 1801 by analyzing a new lead-bearing mineral he called "brown lead," and named the new element erythronium (Greek for "red") since, upon heating, most of its salts turned from their initial color to red. Four 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 Scandinavian goddess of beauty and fertility, Vanadis (Freya). Both names were attributed to the wide range of colors found in vanadium compounds. Del Rio's lead mineral was later renamed vanadinite for its vanadium content. 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 most important industrial vanadium compound, vanadium pentoxide, is used as a catalyst for the production of sulfuric acid. Large amounts of vanadium ions are found in a few organisms, possibly as a toxin. The oxide and some other salts of vanadium have moderate toxicity. Particularly in the ocean, vanadium is used by some life forms as an active center of enzymes, such as the vanadium bromoperoxidase of some ocean algae. Vanadium is probably a micronutrient in mammals, including humans, but its precise role in this regard is unknown. Contents 1 History 2 Creation 3 Characteristics 3.1 Isotopes 3.2 Chemistry and compounds 3.2.1 Oxy and oxo compounds 3.2.2 Halide compounds 3.2.3 Coordination compounds 3.2.4 Organometallic compounds 4 Occurrence 5 Production 6 Applications 6.1 Alloys 6.2 Other uses 7 Biological role 7.1 Bromoperoxidases in algae 7.2 Vanabins in tunicates and ascidians 7.3 Nitrogen fixation 7.4 Fungi 7.5 Mammals and birds 8 Safety 9 References 10 Further reading 11 External links 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: παγχρώμιο "all colors"). Later, Del Río renamed the element erythronium (Greek: ερυθρός "red") 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 that same year, Friedrich Wöhler confirmed del Río's earlier work.2 Sefström chose a name beginning with V, which had not been assigned to any element yet. He called the element vanadium after Old Norse Vanadís (another name for the Norse Vanr goddess Freyja, whose facets include connections to 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 be renamed "rionium" after del Río, but this suggestion was not followed.3 The Model T made use of vanadium steel in its chassis. 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(II) chloride, VCl2, 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 Creation The stable form of vanadium is created in supernovas via the r-process.7 Characteristics Vanadium is a soft, ductile, silver-gray metal. It has good resistance to corrosion and it is stable against alkalis, sulfuric and hydrochloric acids.8 It is oxidized in air at about 933 K (660 °C, 1220 °F), although an oxide layer forms even at room temperature. Isotopes Main article: Isotopes of vanadium 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.9 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 16.0 days. All of the remaining radioactive isotopes have half-lives shorter than an hour, most of which are below 10 seconds. At least 4 isotopes have metastable excited states.9 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. Chemistry and compounds See also Category: Vanadium compounds Oxidation states of vanadium, from left +2 (lilac), +3 (green), +4 (blue) and +5 (yellow). 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.8 Metavanadate chains 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.8

The vanadium redox battery utilizes these oxidation states; conversion 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, VO3− 4, is replaced by the blue color of [VO(H2O)52+, followed by the green color of [V(H2O)63+ and then violet, due to [V(H2O)62+.8 The most commercially important compound is vanadium pentoxide, which is used as a catalyst for the production of sulfuric acid.8 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: V2O3 + O2 → V2O5 Oxy and oxo compounds The Pourbaix diagram for vanadium in water.10 The oxyanion chemistry of vanadium(V) is complex. The vanadate ion, VO3− 4, is present in dilute solutions at high pH. On acidification, HVO2− 4 and H2VO− 4 are formed, analogous to HPO2− 4 and H2PO− 4. 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 V10O4− 28 and HV10O3− 28, which predominate at pH 4-6, are formed in which compound is octahedral about vanadium.8 The correspondence between vanadate and phosphate chemistry can be attributed to the similarity in size and charge of phosphorus(V) and vanadium(V). Orthovanadate VO3− 4 is used in protein crystallography11 to study the biochemistry of phosphate.12 Vanadium also forms various peroxo- complexes when treated with hydrogen peroxide. For instance, the yellow oxovanadium(V) ion VO+ 2 in acidic hydrogen peroxide solution forms the brick red peroxovanadium(V) ion, VO(O2)2+.13 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 A ball-and-stick model of VO(acac)2 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 electron-poor. 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 coordination numbers higher than 6, as is the case in [V(CN)74−. 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 VOCl2(NMe3)2.14 Organometallic compounds Main article: Organovanadium chemistry 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.15 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)3− 6 (isoelectronic with Fe(CO)5).1617 Occurrence See also Category: Vanadate minerals Vanadinite Metallic vanadium is not found in nature, but is known to exist in about 65 different minerals. Economically significant examples include patronite (VS4),18 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, and eastern Russia. In 2007 these three countries mined more than 95 % of the 58,600 tonnes of produced vanadium.19

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.20 An estimated 110,000 tonnes of vanadium per year are released into the atmosphere by burning fossil fuels.21 Vanadium has also been detected spectroscopically in light from the Sun and some other stars.22 Production Ferrovanadium chunks Electrolytically refined vanadium dendritic crystals (99,9%) Most vanadium is used as an alloy called 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.23 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.23 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 in use, in all of which vanadium is produced as a byproduct of other processes.23 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.24 2 V + 3 I2 2 VI3 Applications Tool made from vanadium steel Highpure (99,95%) vanadium cuboids, ebeam remelted and macro etched Alloys Approximately 85% of vanadium produced is used as ferrovanadium or as a steel additive.23 The considerable increase of strength in steel containing small amounts of vanadium was discovered in the beginning of the 20th century. Vanadium forms stable nitrides and carbides, resulting in a significant increase in the strength of the steel.25 From that time on vanadium steel was used for applications in axles, bicycle frames, crankshafts, gears, and other critical components. There are two groups of vanadium containing steel alloy groups. Vanadium high-carbon steel alloys containing 0.15 to 0.25% 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.26 Vanadium stabilizes the beta form of titanium and increases the strength and 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 Titanium 6AL-4V, a titanium alloy with 6% aluminium and 4% vanadium.27 Other uses Vanadium(V) oxide is a catalyst in the contact process for producing sulfuric acid Vanadium is compatible with iron and titanium, therefore vanadium foil is used in cladding titanium to steel.28 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.2930 Several vanadium alloys show superconducting behavior. The first A15 phase superconductor was a vanadium compound, V3Si, which was discovered in 1952.31 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.32 The most common oxide of vanadium, vanadium pentoxide V2O5, is used as a catalyst in manufacturing sulfuric acid by the contact process33 and as an oxidizer in maleic anhydride production.34 Vanadium pentoxide is also used in making ceramics.35 Another 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.36 Vanadium oxide can be used to induce color centers in corundum to create simulated alexandrite jewelry, although alexandrite in nature is a chrysoberyl.37 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.38 Vanadate can be used for protecting steel against rust and corrosion by electrochemical conversion coating.39 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.40 It has been 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.41 Biological role

Vanadium plays a very limited role in biology, and is more important in ocean environments than on land. Ascidiacea (sea squirts) contain vanadium as vanabin. Tunicates such as this bluebell tunicate contain vanadium as vanabin. Amanita muscaria contains amavadin. Bromoperoxidases in algae Organobromine compounds in a number of species of marine algae are generated by the action of a vanadium dependent bromoperoxidase. This is a haloperoxidase in algae which requires bromide and is an absolutely vanadium-dependent enzyme. Most organobromine compounds in the sea ultimately arise via the action of this vanadium bromoperoxidase.42 Vanabins in tunicates and ascidians German chemist Martin Henze discovered vanadium in the blood cells (or coelomic cells) of Ascidiacea (sea squirts) in 1911 43 where it is essential to ascidians and tunicates, as vanabins (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. Vanadium has been reported in high concentrations in holothurian (sea cucumber) blood,44 however other researchers have been unable to reproduce these results.45 There is no evidence that hemovanadin carries oxygen, in contrast to hemoglobin and hemocyanin, which may also be present in these organisms.46 Nitrogen fixation A vanadium nitrogenase is used by some nitrogen-fixing micro-organisms, such as Azotobacter. In this role vanadium replaces more common molybdenum or iron, and gives the nitrogenase slightly different properties.47 Fungi 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, amavadin,48 in fungal fruit-bodies. However, the biological importance of the accumulation process is unknown.4950 Toxin functions or peroxidase enzyme functions have been suggested. Mammals and birds Rats and chickens are also known to require vanadium in very small amounts and deficiencies result in reduced growth and impaired reproduction.51 Vanadium is a relatively controversial dietary supplement, primarily for increasing insulin sensitivity52 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.53 Vanadyl sulfate may improve glucose control in people with type 2 diabetes.5455565758 In addition, decavanadate and oxovanadates are species that potentially have many biological activities and that have been successfully used as tools in the comprehension of several biochemical processes.59 Safety All vanadium compounds should be considered to be toxic. Tetravalent VOSO4 has been reported to be over 5 times more toxic than trivalent V2O3.60 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.61 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.61 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.626364 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,6566 on liver,67 on neurological development in rats,68 and other organs.69 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.70 Vanadium has not been classified as to carcinogenicity by the United States Environmental Protection Agency.71

Vanadium traces in diesel fuels present a corrosion hazard; it is the main fuel component influencing high temperature corrosion. During combustion, it oxidizes and reacts with sodium and sulfur, yielding vanadate compounds with melting points down to 530 °C, which attack the passivation layer on steel, rendering it susceptible to corrosion. The solid vanadium compounds also cause abrasion of engine components. References ^ Cintas, Pedro (2004). "The Road to Chemical Names and Eponyms: Discovery, Priority, and Credit". Angewandte Chemie International Edition 43 (44): 5888. doi:10.1002/anie.200330074. PMID 15376297.  ^ a b 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: 43. doi:10.1002/andp.18310970103.  ^ Featherstonhaugh, George William (1831). The Monthly American Journal of Geology and Natural Science: 69.  ^ Roscoe, Henry E. 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Journal Inorganic Biochemistry 103: 536–546. doi:10.1016/j.jinorgbio.2008.11010.  ^ Roschin, A. V. (1967). "Toxicology of vanadium compounds used in modern industry". Gig Sanit. (Water Res.) 32 (6): 26–32. PMID 5605589.  ^ a b "Occupational Safety and Health Guidelines for Vanadium Pentoxide". Occupational Safety and Health Administration. http://www.osha.gov/SLTC/healthguidelines/vanadiumpentoxidedust/recognition.html. Retrieved 2009-01-29.  ^ Sax, N. I. (1984). Dangerous Properties of Industrial Materials, 6th ed.. Van Nostrand Reinhold Company. pp. 2717–2720.  ^ a b 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. PMID 12773761.  ^ 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. 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Neurotoxicology and Teratology 29 (4): 503–510. doi:10.1016/j.ntt.2007.03.001. PMID 17493788.  ^ Barceloux, Donald G.; Barceloux, Donald (1999). "Vanadium". Clinical Toxicology 37 (2): 265–278. doi:10.1081/CLT-100102425. PMID 10382561.  ^ 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. PMID 17030368.  ^ Opreskos, Dennis M. (1991). "Toxicity Summary for Vanadium". Oak Ridge National Laboratory. http://rais.ornl.gov/tox/profiles/old/vanadium_f_V1.htm. Retrieved 2008-11-08. dead link Further reading Slebodnick, Carla et al. (1999). "Modeling the Biological Chemistry of Vanadium: Structural and Reactivity Studies Elucidating Biological Function". In Hill, Hugh A.O. et al.. Metal sites in proteins and models: phosphatases, Lewis acids, and vanadium. Springer. ISBN 9783540655534. http://books.google.com/books?id=ZF5aNOeHd5sC&pg=PA51.  External links Wikimedia Commons has media related to: Vanadium Look up vanadium in Wiktionary, the free dictionary. The periodic table of videos videos of the chemistry of the elements WebElements.com – Vanadium ATSDR – ToxFAQs: Vanadium The periodic table of videos: Vanadium v · d · e  Vanadium compounds

VBr3 · VC · V(CO)6 · VCl2 · VCl3 · VCl4 · VF3 · VF4 · VI3 · VN · VO · VO2 · VOCl3 · VOF3 · V2O3 · V2O5 · V2(SO4)3 v · d · e Periodic table H   He Li Be   B C N O F Ne Na Mg   Al Si P S Cl Ar K Ca   Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr   Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases Unknown chem. properties Large version 

VBr3 · VC · V(CO)6 · VCl2 · VCl3 · VCl4 · VF3 · VF4 · VI3 · VN · VO · VO2 · VOCl3 · VOF3 · V2O3 · V2O5 · V2(SO4)3 v · d · e Periodic table H   He Li Be   B C N O F Ne Na Mg   Al Si P S Cl Ar K Ca   Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr   Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases Unknown chem. properties Large version 

VBr3 · VC · V(CO)6 · VCl2 · VCl3 · VCl4 · VF3 · VF4 · VI3 · VN · VO · VO2 · VOCl3 · VOF3 · V2O3 · V2O5 · V2(SO4)3 v · d · e Periodic table H   He Li Be   B C N O F Ne Na Mg   Al Si P S Cl Ar K Ca   Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr   Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases Unknown chem. properties Large version 

VBr3 · VC · V(CO)6 · VCl2 · VCl3 · VCl4 · VF3 · VF4 · VI3 · VN · VO · VO2 · VOCl3 · VOF3 · V2O3 · V2O5 · V2(SO4)3 v · d · e Periodic table H   He Li Be   B C N O F Ne Na Mg   Al Si P S Cl Ar K Ca   Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr   Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uus Uuo Alkali metals Alkaline earth metals Lanthanides Actinides Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases Unknown chem. properties Large version