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23 titaniumvanadiumchromium


Name, symbol, number vanadium, V, 23
Chemical seriestransition metals
Group, period, block 54, d
Appearancesilver-grey metal
Standard atomic weight 50.9415(1) g·mol−1
Electron configuration [Ar] 3d3 4s2
Electrons per shell 2, 8, 11, 2
Physical properties
Density (near r.t.)6.0 g·cm−3
Liquid density at m.p.5.5 g·cm−3
Melting point2183 K
(1910 °C, 3470 °F)
Boiling point3680 K
(3407 °C, 6165 °F)
Heat of fusion21.5 kJ·mol−1
Heat of vaporization459 kJ·mol−1
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
Crystal structurecubic body centered
Oxidation states5, 4, 3, 2, 1 [1]
(amphoteric oxide)
Electronegativity1.63 (Pauling scale)
Ionization energies
1st: 650.9 kJ·mol−1
2nd: 1414 kJ·mol−1
3rd: 2830 kJ·mol−1
Atomic radius135 pm
Atomic radius (calc.)171 pm
Covalent radius125 pm
Magnetic orderingparamagnetic
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 modulus128 GPa
Shear modulus47 GPa
Bulk modulus160 GPa
Poisson ratio0.37
Mohs hardness6.7
CAS registry number7440-62-2
Selected 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% V is stable with 28 neutrons
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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 certain minerals and is used mainly to produce certain alloys. It is one of the 26 elements found in most living organisms.


Notable characteristics

Vanadium 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. A +1 oxidation state is rarely seen.


Approximately 80% of vanadium produced is used as ferrovanadium or as a steel additive. Other uses:


Vanadium was originally discovered by Andrés Manuel del Río (a Spanish-born Mexican mineralogist) in Mexico City, in 1801. He called it "brown lead" (now named vanadinite). Through experimentation, its colors reminded him of chromium, so he named the element panchromium. 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.

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. 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. The name vanadium comes from Vanadis, a goddess in Scandinavian mythology, because the element has beautiful multicolored chemical compounds.

Biological role

In biology, a vanadium atom is an essential component of some enzymes, particularly the vanadium nitrogenase 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 reproduction.

Ten percent of the blood cell pigment of the sea cucumber is vanadium. Just as the horseshoe crab has blue blood rather than red blood (colored by iron in hemoglobin) because of copper in the hemocyanin pigment, the blood of the sea cucumber is yellow because of the vanadium in the vanabin pigment[1]. Nonetheless, there is no evidence that vanabins carry oxygen, in contrast to hemoglobin and hemocyanin.

A form of vanadium, vanadyl sulfate, seems to improve glucose control in people with type 2 diabetes.[2][3][4][5][6]

Mineral supplement in drinking water

Most continental waters show a vanadium concentration of less than 3 ppb. However, the groundwater of Mt. Fuji contains a very high concentration of vanadium—up to 150 ppb. This vanadium is solubilized from the basalt by the groundwater. The vanadium content in Mt. Fuji becomes higher at places nearer the summit and deeper in the ground. Recently this high-vanadium water of Mt. Fuji has been sold by many companies as an agent to cope with diabetes. However, there is no concrete evidence for its efficacy. The rainbow trout living in the Mt. Fuji water showed much higher accumulation of vanadium in kidneys and bone.


Vanadium 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. 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.


Vanadium 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.


Vanadium 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.

Vanadium(IV) chloride VCl4 is a soluble form of vanadium that is commonly used in the laboratory. V(IV) is the reduced form of V(V), and commonly occurs after anaerobic respiration by dissimilatory metal reducing bacteria. VCl4 reacts violently with water.

Toxicity of vanadium compounds

The 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).

Various oxidation states of vanadium ions

It is known that vanadium gets the oxidation states +2, +3, +4, +5. To observe the colours 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.


Main article: Isotopes of vanadium

Naturally 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.


Powdered 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.

See also


  • Los Alamos National Laboratory – Vanadium
  • High 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 JH. Carcinogenicity classification of vanadium pentoxide and inorganic vanadium compounds, the NTP study of carcinogenicity of inhaled vanadium pentoxide, and vanadium chemistry. Regul Toxicol Pharmacol 2007 Feb;47(1):110-4.
  • Gonzalez-Villalva A, Fortoul TI, Avila-Costa MR, et al. Thrombocytosis induced in mice after subacute and subchronic V2O5 inhalation. Toxicol Ind Health 2006 Apr;22(3):113-6.
  • Kobayashi K, Himeno S, Satoh M, et al. Pentavalent vanadium induces hepatic metallothionein through interleukin-6-dependent and -independent mechanisms. Toxicology 2006 Dec 7;228(2-3:162-170.
  • Ress NB, Chou BJ, Renne RA, et al. Carcinogenicity of inhaled vanadium pentoxide in F344/N rats and B6C3F1 mice. Toxicol Sci 2003 Aug;74(2):287-96.
  • Scibior A, Zaporowska H, Ostrowski J. Selected haematological and biochemical parameters of blood in rats after subchronic administration of vanadium and/or magnesium in drinking water. Arch Environ Contam Toxicol 2006 Aug;51(2):287-95.
  • Soazo M, Garcia GB. Vanadium exposure through lactation produces behavioral alterations and CNS myelin deficit in neonatal rats. Neurotoxicol Teratol 2007 Jul-Aug;29(4):503-10.
  • Worle-Knirsch JM, Kern K, Schleh C, et al. Nanoparticulate vanadium oxide potentiated vanadium toxicity in human lung cells. Environ Sci Technol 2007 Jan 1;41(1):331-6.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Vanadium". A list of authors is available in Wikipedia.
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