Vanadium redox battery

From Wikipedia, the free encyclopedia

Vanadium redox battery

Specific energy	10–20 Wh/kg (36–72 J/g)
Energy density	15–25 Wh/L (54–65 kJ/L)
Charge/discharge efficiency	75–80%<.
Time durability	20-30 years
Cycle durability	>12,000-20,000 cycles
Nominal cell voltage	1.15–1.55 V

Schematic design of a vanadium redox flow battery system

 

1 MW 4 MWh containerized vanadium flow battery owned by Avista Utilities and  manufactured by UniEnergy Technologies

 

A vanadium redox flow battery located at the University of New South Wales, Sydney, Australia

 

The vanadium redox battery (VRB), also known as the vanadium flow battery (VFB) or vanadium redox flow battery (VRFB), is a type of rechargeable flow battery that employs vanadium ions in different oxidation states to store chemical potential energy. The vanadium redox battery exploits the ability of vanadium to exist in solution in four different oxidation states, and uses this property to make a battery that has just one electroactive element instead of two. For several reasons, including their relative bulkiness, most vanadium batteries are currently used for grid energy storage, i.e., attached to power plants or electrical grids. 

The possibility of creating a vanadium flow battery was explored variously by Pissoort in the 1930s, NASA researchers in the 1970s, and Pellegri and Spaziante in the 1970s, but none of them were successful in demonstrating the technology. The first successful demonstration of the all-vanadium redox flow battery which employed vanadium in a solution of sulfuric acid in each half was by Maria Skyllas-Kazacos at the University of New South Wales in the 1980s. Her design used sulfuric acid electrolytes, and was patented by the University of New South Wales in Australia in 1986.

The main advantages of the vanadium redox battery are that it can offer almost unlimited energy capacity simply by using larger electrolyte storage tanks; it can be left completely discharged for long periods with no ill effects; if the electrolytes are accidentally mixed, the battery suffers no permanent damage; a single state of charge between the two electrolytes avoids the capacity degradation due to a single cell in non-flow batteries; the electrolyte is aqueous and inherently safe and non-flammable; and the generation 3 formulation using a mixed acid solution developed by the Pacific Northwest National Laboratory operates over a wider temperature range allowing for passive cooling. VRFBs can be used at depth of discharge (DOD) around 90% and more, i.e. deeper DODs than solid-state batteries (e.g. lithium-based and sodium-based batteries, which are usually specified with DOD=80%). In addition, VRFBs exhibit very long cycle lives: most producers specify cycle durability in excess of 15,000-20,000 charge/discharge cycles. These values are far beyond the cycle lives of solid-state batteries, which is usually in the order of 4,000-5,000 charge/discharge cycles. Consequently, the levelized cost of energy (LCOE, i.e. the system cost divided by the usable energy, the cycle life, and round-trip efficiency) of present VRFB systems is typically in the order of a few tens of $ cents or € cents, namely much lower than the LCOEs of equivalent solid-state batteries and close to the targets of $0.05 and €0.05, stated by the US Department of Energy and the European Commission Strategic Energy Technology (SET) Plan, respectively.

The main disadvantages with vanadium redox technology are a relatively poor energy-to-volume ratio in comparison with standard storage batteries (although the Generation 3 formulation has doubled the energy density  of the system), and the aqueous electrolyte makes the battery heavy and therefore only useful for stationary applications. Another disadvantage is the relatively high toxicity of oxides of vanadium.

Numerous companies and organizations involved in funding and developing vanadium redox batteries include Avalon Battery, Vionx (formerly Premium Power), UniEnergy Technologies and Ashlawn Energy in the United States; Renewable Energy Dynamics Technology in Ireland; Enerox GmbH (formerly Gildemeister energy storage) in Austria; Cellennium in Thailand; Rongke Power in China; Prudent Energy in China; Sumitomo in Japan; H2, Inc. in South Korea; redT in Britain, Australian Vanadium in Australia, and the now defunct Imergy (formerly Deeya). Lately, also several smaller size vanadium redox flow batteries were brought to market (for residential applications) mainly from StorEn Technologies (USA), Schmid Group, VoltStorage  and Volterion  (all three from Germany), VisBlue  (Denmark) or Pinflow energy storage  (Czechia).

Operation

Diagram of a vanadium flow battery

 

A vanadium redox battery consists of an assembly of power cells in which the two electrolytes are separated by a proton exchange membrane. The electrodes in a VRB cell are carbon based; the most common types being carbon felt, carbon paper, carbon cloth, and graphite felt. Recently, carbon nanotube based electrodes have gained marked interest from the scientific community. Both electrolytes are vanadium-based, the electrolyte in the positive half-cells contains VO₂⁺ and VO²⁺ ions, the electrolyte in the negative half-cells, V³⁺ and V²⁺ ions. The electrolytes may be prepared by any of several processes, including electrolytically dissolving vanadium pentoxide (V₂O₅) in sulfuric acid (H₂SO₄). The solution remains strongly acidic in use. 

In vanadium flow batteries, both half-cells are additionally connected to storage tanks and pumps so that very large volumes of the electrolytes can be circulated through the cell. This circulation of liquid electrolytes is somewhat cumbersome and does restrict the use of vanadium flow batteries in mobile applications, effectively confining them to large fixed installations.

When the vanadium battery is being charged, the VO²⁺ ions in the positive half-cell are converted to VO₂⁺ ions when electrons are removed from the positive terminal of the battery. Similarly in the negative half-cell, electrons are introduced converting the V³⁺ ions into V²⁺. During discharge this process is reversed and results in a typical open-circuit voltage of 1.41 V at 25 °C. 

Other useful properties of vanadium flow batteries are their very fast response to changing loads and their extremely large overload capacities. Studies by the University of New South Wales have shown that they can achieve a response time of under half a millisecond for a 100% load change, and allowed overloads of as much as 400% for 10 seconds. The response time is mostly limited by the electrical equipment. Unless specifically designed for colder or warmer climates, most sulfuric acid-based vanadium batteries only work between about 10 and 40 °C. Below that temperature range, the ion-infused sulfuric acid crystallizes. Round trip efficiency in practical applications is around 65–75 %.

Proposed improvements

Second generation vanadium redox batteries (vanadium/bromine) may approximately double the energy density and increase the temperature range in which the battery can operate.

Specific energy and energy density

Current production vanadium redox batteries achieve a specific energy of about 20 Wh/kg (72 kJ/kg) of electrolyte. More recent research at UNSW indicates that the use of precipitation inhibitors can increase the density to about 35 Wh/kg (126 kJ/kg), with even higher densities made possible by controlling the electrolyte temperature. This specific energy is quite low compared to other rechargeable battery types (e.g., lead–acid, 30–40 Wh/kg (108–144 kJ/kg); and lithium ion, 80–200 Wh/kg (288–720 kJ/kg)).

Mechanisms of Electrode Permeation by Electrolyte

A number of research groups worldwide have reported capacity loss in VRFBs over prolonged periods of use. While several causes have been considered, the influence of electrode microstructure on cell electrochemistry within the electrode is poorly known. Electrolytic wetting of carbon electrodes in VRFBs is important for overcoming sources of degradation and applying appropriate operational procedures. Recently, it appears that electrolytic wetting behaviour within the electrode may be influenced by local concentration effects as well as capillary action. Rapid wetting or permeation may also leave behind undissolved gases which could cause electrode degradation.

Applications

The extremely large capacities possible from vanadium redox batteries make them well suited to use in large power storage applications such as helping to average out the production of highly variable generation sources such as wind or solar power, helping generators cope with large surges in demand or leveling out supply/demand at a transmission constrained region.

The limited self-discharge characteristics of vanadium redox batteries make them useful in applications where the batteries must be stored for long periods of time with little maintenance while maintaining a ready state. This has led to their adoption in some military electronics, such as the sensor components of the GATOR mine system. Their ability to fully cycle and stay at 0% state of charge makes them suitable for solar + storage applications where the battery must start each day empty and fill up depending upon the load and weather. Lithium ion batteries, for example, are typically damaged when they are allowed to discharge below 20% state of charge, so they typically only operate between about 20% and 100%, meaning they are only using 80% of their nameplate capacity.

Their extremely rapid response times also make them superbly well suited to uninterruptible power supply (UPS) type applications, where they can be used to replace lead–acid batteries and even diesel generators. Also the fast response time makes them well-suited for frequency regulation. Economically neither the UPS or frequency regulation applications of the battery are currently sustainable alone, but rather the battery is able to layer these applications with other uses to capitalize on various sources of revenue. Also, these capabilities make vanadium redox batteries an effective "all-in-one" solution for microgrids that depend on reliable operations, frequency regulation and have a need for load shifting (from either high renewable penetration, a highly variable load or desire to optimize generator efficiency through time-shifting dispatch).

Largest vanadium grid batteries

A 200 MW, 800 MWh (4 hours) vanadium redox battery is under construction in China; it was expected to be completed by 2018 and its 250 kW/ 1MWh first stage was in operation in late 2018.

Vanadium

From Wikipedia, the free encyclopedia

Vanadium,  ₂₃V

Vanadium
Pronunciation	/vəˈneɪdiəm/ ​(və-NAY-dee-əm)
Appearance	blue-silver-grey metal
Standard atomic weight Ar, std(V)	50.9415(1)
Vanadium in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson – ↑ V ↓ Nb titanium ← vanadium → chromium
Atomic number (Z)	23
Group	group 5
Period	period 4
Block	d-block
Element category	transition metal
Electron configuration	[Ar] 3d3 4s2
Electrons per shell	2, 8, 11, 2
Physical properties
Phase at STP	solid
Melting point	2183 K ​(1910 °C, ​3470 °F)
Boiling point	3680 K ​(3407 °C, ​6165 °F)
Density (near r.t.)	6.0 g/cm3
when liquid (at m.p.)	5.5 g/cm3
Heat of fusion	21.5 kJ/mol
Heat of vaporization	444 kJ/mol
Molar heat capacity	24.89 J/(mol·K)
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	−3, −1, +1, +2, +3, +4, +5 (an amphoteric oxide)
Electronegativity	Pauling scale: 1.63
Ionization energies	1st: 650.9 kJ/mol 2nd: 1414 kJ/mol 3rd: 2830 kJ/mol (more)
Atomic radius	empirical: 134 pm
Covalent radius	153±8 pm
Spectral lines of vanadium
Other properties
Natural occurrence	primordial
Crystal structure	​body-centered cubic (bcc)
Speed of sound thin rod	4560 m/s (at 20 °C)
Thermal expansion	8.4 µm/(m·K) (at 25 °C)
Thermal conductivity	30.7 W/(m·K)
Electrical resistivity	197 nΩ·m (at 20 °C)
Magnetic ordering	paramagnetic
Magnetic susceptibility	+255.0·10−6 cm3/mol (298 K)
Young's modulus	128 GPa
Shear modulus	47 GPa
Bulk modulus	160 GPa
Poisson ratio	0.37
Mohs hardness	6.7
Vickers hardness	628–640 MPa
Brinell hardness	600–742 MPa
CAS Number	7440-62-2
History
Discovery	Andrés Manuel del Río (1801)
First isolation	Nils Gabriel Sefström (1830)
Named by	Nils Gabriel Sefström (1830)
Main isotopes of vanadium
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct 48V syn 16 d β+ 48Ti 49V syn 330 d ε 49Ti 50V 0.25% 1.5×1017 y ε 50Ti β− 50Cr 51V 99.75% stable

Vanadium is a chemical element with the symbol V and atomic number 23. It is a hard, silvery-grey, ductile, malleable transition metal. The elemental metal is rarely found in nature, but once isolated artificially, the formation of an oxide layer (passivation) somewhat stabilizes the free metal against further oxidation.

Andrés Manuel del Río discovered compounds of vanadium in 1801 in Mexico by analyzing a new lead-bearing mineral he called "brown lead", and presumed its qualities were due to the presence of a new element, which he named erythronium (derived from "ἐρυθρόν", greek word for "red") since upon heating most of the salts turned red. Four years later, he was (erroneously) convinced by other scientists that erythronium was identical to chromium. Chlorides of vanadium were generated in 1830 by Nils Gabriel Sefström who thereby proved that a new element was involved, which he named "vanadium" after the Scandinavian goddess of beauty and fertility, Vanadís (Freyja). 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. In 1867 Henry Enfield Roscoe obtained the pure element.

Vanadium occurs naturally in about 65 minerals and in fossil fuel deposits. It is produced in China and Russia from steel smelter slag. Other countries produce it either from magnetite directly, 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. The vanadium redox battery for energy storage may be an important application in the future.

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.

History

Vanadium was discovered by Andrés Manuel del Río, a Spanish-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") because most of the salts turned red upon heating. In 1805, 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 Collet-Descotils' statement and retracted his claim.

In 1831, Swedish chemist Nils Gabriel Sefström rediscovered the element in a new oxide he found while working with iron ores. Later that year, Friedrich Wöhler confirmed del Río's earlier work. Sefström chose a name beginning with V, which had not yet been assigned to any element. He called the element vanadium after Old Norse Vanadís (another name for the Norse Vanr goddess Freyja, whose attributes include beauty and fertility), because of the many beautifully colored chemical compounds it produces. In 1831, the geologist George William Featherstonhaugh suggested that vanadium should be renamed "rionium" after del Río, but this suggestion was not followed.

The Model T used vanadium steel in its chassis.

 

The isolation of vanadium metal was difficult. In 1831, Berzelius reported the production of the metal, but Henry Enfield Roscoe showed that Berzelius had produced the nitride, vanadium nitride (VN). Roscoe eventually produced the metal in 1867 by reduction of vanadium(II) chloride, VCl₂, with hydrogen. In 1927, pure vanadium was produced by reducing vanadium pentoxide with calcium.

The first large-scale industrial use of vanadium was in the steel alloy chassis of the Ford Model T, inspired by French race cars. Vanadium steel allowed reduced weight while increasing tensile strength (ca. 1905).^[8] For the first decade of the 20^th century, most vanadium ore was mined by American Vanadium Company from the Minas Ragra in Peru. Later the demand for uranium rose, leading to increased mining of that metal's ores. One major uranium ore was carnotite, which also contains vanadium. Thus, vanadium became available as a by-product of uranium production. Eventually uranium mining began to supply a large share of the demand for vanadium.

German chemist Martin Henze discovered vanadium in the hemovanadin proteins found in blood cells (or coelomic cells) of Ascidiacea (sea squirts) in 1911.

Characteristics

High-purity (99.95%) vanadium cuboids, ebeam remelted and macro-etched

 

Vanadium is a medium-hard, ductile, steel-blue metal. It is electrically conductive and thermally insulating. Some sources describe vanadium as "soft", perhaps because it is ductile, malleable, and not brittle. Vanadium is harder than most metals and steels. It has good resistance to corrosion and it is stable against alkalis and sulfuric and hydrochloric acids. It is oxidized in air at about 933 K (660 °C, 1220 °F), although an oxide passivation 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 of 0.25%. ⁵¹V has a nuclear spin of ​⁷⁄₂, which is useful for NMR spectroscopy. Twenty-four 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. The remaining radioactive isotopes have half-lives shorter than an hour, most below 10 seconds. At least four isotopes have metastable excited states. Electron capture is the main decay mode for isotopes lighter than 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 beta decay leads to element 24 (chromium) isotopes.

Chemistry

From left: [V(H₂O)₆]²⁺ (lilac), [V(H₂O)₆]³⁺ (green), [VO(H₂O)₅]²⁺ (blue) and [VO(H₂O)₅]³⁺ (yellow).

 

The chemistry of vanadium is noteworthy for the accessibility of the four adjacent oxidation states 2–5. In aqueous solution, vanadium forms metal aquo complexes of which the colours are lilac [V(H₂O)₆]²⁺, green [V(H₂O)₆]³⁺, blue [VO(H₂O)₅]²⁺, yellow VO₃⁻. 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.

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.

The most commercially important compound is vanadium pentoxide. It is used as a catalyst for the production of sulfuric acid. This compound oxidizes sulfur dioxide (SO
₂) to the trioxide (SO
₃). In this redox reaction, sulfur is oxidized from +4 to +6, and vanadium is reduced from +5 to +4:

V₂O₅ + SO₂ → 2 VO₂ + SO₃

The catalyst is regenerated by oxidation with air:

4 VO₂ + O₂ → 2 V₂O₅

Similar oxidations are used in the production of maleic anhydride, phthalic anhydride, and several other bulk organic compounds.

The vanadium redox battery utilizes all four oxidation states: one electrode uses the +5/+4 couple and the other uses the +3/+2 couple. Conversion of these oxidation states is illustrated by the reduction of a strongly acidic solution of a vanadium(V) compound with zinc dust or amalgam. The initial yellow color characteristic of the pervanadyl ion [VO₂(H₂O)₄]⁺ is replaced by the blue color of [VO(H₂O)₅]²⁺, followed by the green color of [V(H₂O)₆]³⁺ and then the violet color of [V(H₂O)₆]²⁺.

Oxyanions

The decavanadate structure

 

In aqueous solution, vanadium(V) forms an extensive family of oxyanions. The interrelationships in this family are described by the predominance diagram, which shows at least 11 species, depending on pH and concentration. The tetrahedral orthovanadate ion, VO³⁻
₄, is the principal species present at pH 12-14. Similar in size and charge to phosphorus(V), vanadium(V) also parallels its chemistry and crystallography. Orthovanadate VO³⁻
₄ is used in protein crystallography to study the biochemistry of phosphate. The tetrathiovanadate [VS₄]³⁻ is analogous to the orthovanadate ion.

At lower pH values, the monomer [HVO₄]²⁻ and dimer [V₂O₇]⁻ are formed, with the monomer predominant at vanadium concentration of less than c. 10⁻²M (pV > 2, where pV is equal to the minus value of the logarithm of the total vanadium concentration/M). The formation of the divanadate ion is analogous to the formation of the dichromate ion. As the pH is reduced, further protonation and condensation to polyvanadates occur: at pH 4-6 [H₂VO₄]⁻ is predominant at pV greater than ca. 4, while at higher concentrations trimers and tetramers are formed. Between pH 2-4 decavanadate predominates, its formation from orthovanadate is represented by this condensation reaction:

10 [VO₄]³⁻ + 24 H⁺ → [V₁₀O₂₈]⁶⁻ + 12 H₂O

In decavanadate, each V(V) center is surrounded by six oxide ligands. Vanadic acid, H₃VO₄ exists only at very low concentrations because protonation of the tetrahedral species [H₂VO₄]⁻ results in the preferential formation of the octahedral [VO₂(H₂O)₄]⁺ species. In strongly acidic solutions, pH<2 .="" sub="">2

(H₂O)₄]⁺ is the predominant species, while the oxide V₂O₅ precipitates from solution at high concentrations. The oxide is formally the acid anhydride of vanadic acid. The structures of many vanadate compounds have been determined by X-ray crystallography. 

The Pourbaix diagram for vanadium in water

 

The Pourbaix diagram for vanadium in water, which shows the redox potentials between various vanadium species in different oxidation states, is also complex.

Vanadium(V) forms various peroxo complexes, most notably in the active site of the vanadium-containing bromoperoxidase enzymes. The species VO(O)₂(H₂O)₄⁺ is stable in acidic solutions. In alkaline solutions, species with 2, 3 and 4 peroxide groups are known; the last forms violet salts with the formula M₃V(O₂)₄ nH₂O (M= Li, Na, etc.), in which the vanadium has an 8-coordinate dodecahedral structure.

Halide derivatives

Twelve binary halides, compounds with the formula VX_n (n=2..5), are known. VI₄, VCl₅, VBr₅, and VI₅ do not exist or are extremely unstable. In combination with other reagents, VCl₄ is used as a catalyst for polymerization of dienes. Like all binary halides, those of vanadium are Lewis acidic, especially those of V(IV) and V(V). Many of the halides form octahedral complexes with the formula VX_nL_6−n (X= halide; L= other ligand). 

Many vanadium oxyhalides (formula VO_mX_n) are known. The oxytrichloride and oxytrifluoride (VOCl₃ and VOF₃) are the most widely studied. Akin to POCl₃, they are volatile, adopt tetrahedral structures in the gas phase, and are Lewis acidic.

Coordination compounds

A ball-and-stick model of VO₅(C₅H₇)₂

 

Complexes of vanadium(II) and (III) are relatively exchange inert and reducing. Those of V(IV) and V(V) are oxidants. Vanadium ion is rather large and some complexes achieve coordination numbers greater than 6, as is the case in [V(CN)₇]⁴⁻. Oxovanadium(V) also forms 7 coordinate coordination complexes with tetradentate ligands and peroxides and these complexes are used for oxidative brominations and thioether oxidations. The coordination chemistry of V⁴⁺ is dominated by the vanadyl center, VO²⁺, which binds four other ligands strongly and one weakly (the one trans to the vanadyl center). An example is vanadyl acetylacetonate (V(O)(O₂C₅H₇)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 bipyramidal geometry, such as VOCl₂(NMe₃)₂. The coordination chemistry of V⁵⁺ is dominated by the relatively stable dioxovanadium coordination complexes which are often formed by aerial oxidation of the vanadium(IV) precursors indicating the stability of the +5 oxidation state and ease of interconversion between the +4 and +5 states.

Organometallic compounds

Organometallic chemistry of vanadium is well developed, although it has mainly only academic significance. Vanadocene dichloride is a versatile starting reagent and even finds some applications in organic chemistry. Vanadium carbonyl, V(CO)₆, is a rare example of a paramagnetic metal carbonyl. Reduction yields V(CO)⁻
₆ (isoelectronic with Cr(CO)₆), which may be further reduced with sodium in liquid ammonia to yield V(CO)³⁻
₅ (isoelectronic with Fe(CO)₅).

Occurrence

Vanadinite

Universe

The cosmic abundance of vanadium in the universe is 0.0001%, making the element nearly as common as copper or zinc. Vanadium is detected spectroscopically in light from the Sun and sometimes in the light from other stars.

Earth's crust

Vanadium is the 20th most abundant element in the earth's crust; metallic vanadium is rare in nature (known as the mineral vanadium, native vanadium), but vanadium compounds occur naturally in about 65 different minerals. 

At the beginning of the 20th century a large deposit of vanadium ore was discovered. For several years this patrónite (VS₄) deposit was a economically significant source for vanadium ore. With the production of radium in the 1910s and 1920s from carnotite (K₂(UO₂)₂(VO₄)₂·3H₂O) vanadium became available as a side product of radium and uranium production. Vanadinite (Pb₅(VO₄)₃Cl) and other vanadium bearing minerals are only mined in exceptional cases. With the rising demand, much of the world's vanadium production is now sourced from vanadium-bearing magnetite found in ultramafic gabbro bodies. If this titanomagnetite is used to produce iron, most of the vanadium goes to the slag, and is extracted from it.

Vanadium is mined mostly in South Africa, north-western China, and eastern Russia. In 2013 these three countries mined more than 97% of the 79,000 tonnes of produced vanadium.

Vanadium is also present in bauxite and in deposits of 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, traces of vanadium may cause corrosion in engines and boilers. An estimated 110,000 tonnes of vanadium per year are released into the atmosphere by burning fossil fuels.

Water

The vanadyl ion is abundant in seawater, having an average concentration of 30 nM. Some mineral water springs also contain the ion in high concentrations. For example, springs near Mount Fuji contain as much as 54 μg per liter.

Production

Vacuum sublimed vanadium dendritic crystals (99.9%)

 

Crystal-bar vanadium, showing different textures and surface oxidation; 99.95%-pure cube for comparison

 

Vanadium metal is obtained by a multistep process that begins with roasting crushed ore with NaCl or Na₂CO₃ at about 850 °C to give sodium metavanadate (NaVO₃). An aqueous extract of this solid is acidified to produce "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 used, in all of which vanadium is produced as a byproduct of other processes. 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:

2 V + 3 I₂ ⇌ 2 VI₃

Ferrovanadium chunks

 

Most vanadium is used as a steel alloy called ferrovanadium. Ferrovanadium is produced directly by reducing a mixture of vanadium oxide, iron oxides and iron in an electric furnace. The vanadium ends up in pig iron produced from vanadium-bearing magnetite. Depending on the ore used, the slag contains up to 25% of vanadium.

Applications

Tool made from vanadium steel

Alloys

Approximately 85% of the vanadium produced is used as ferrovanadium or as a steel additive. The considerable increase of strength in steel containing small amounts of vanadium was discovered in the early 20th century. Vanadium forms stable nitrides and carbides, resulting in a significant increase in the strength of steel. 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 steel alloys. Vanadium high-carbon steel alloys contain 0.15% to 0.25% vanadium, and high-speed tool steels (HSS) have a vanadium content of 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. Powder-metallurgic alloys contain up to 18% percent vanadium. The high content of vanadium carbides in those alloys increases wear resistance significantly. One application for those alloys is tools and knives.

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, high-speed airframes and dental implants. The most common alloy for seamless tubing is Titanium 3/2.5 containing 2.5% vanadium, the titanium alloy of choice in the aerospace, defense, and bicycle industries. Another common alloy, primarily produced in sheets, is Titanium 6AL-4V, a titanium alloy with 6% aluminium and 4% vanadium.

Several vanadium alloys show superconducting behavior. The first A15 phase superconductor was a vanadium compound, V₃Si, which was discovered in 1952. 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.

It has been proposed that a small amount, 40 to 270 ppm, of vanadium in Wootz steel and Damascus steel significantly improved the strength of the product, though the source of the vanadium is unclear.

Other uses

Vanadium(V) oxide is a catalyst in the contact process for producing sulfuric acid

 

Vanadium compounds are used extensively as catalysts; for example, the most common oxide of vanadium, vanadium pentoxide V₂O₅, is used as a catalyst in manufacturing sulfuric acid by the contact process and as an oxidizer in maleic anhydride production. Vanadium pentoxide is used in ceramics. Vanadium is an important component of mixed metal oxide catalysts used in the oxidation of propane and propylene to acrolein, acrylic acid or the ammoxidation of propylene to acrylonitrile. In service, the oxidation state of vanadium changes dynamically and reversibly with the oxygen and the steam content of the reacting feed mixture. 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. Vanadium oxide can be used to induce color centers in corundum to create simulated alexandrite jewelry, although alexandrite in nature is a chrysoberyl.

The Vanadium redox battery, a type of flow battery, is an electrochemical cell consisting of aqueous vanadium ions in different oxidation states. Batteries of the type were first proposed in the 1930s and developed commercially from the 1980s onwards. Cells use +5 and +2 formal oxidization state ions. Vanadium redox batteries are used commercially for grid energy storage. 

Vanadate can be used for protecting steel against rust and corrosion by conversion coating. Vanadium foil is used in cladding titanium to steel because it is compatible with both iron and titanium. 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.

Proposed

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. Vanadium phosphates have been proposed as the cathode in the lithium vanadium phosphate battery, another type of lithium-ion battery.

Biological role

Vanadium is more important in marine environments than terrestrial.

Active site of the enzyme vanadium bromoperoxidase, which produces the preponderance of naturally-occurring organobromine compounds.

 

Tunicates such as this bluebell tunicate contain vanadium as vanabin.

 

Amanita muscaria contains amavadin.

Vanadoenzymes

A number of species of marine algae produce vanadium bromoperoxidase as well as the closely related chloroperoxidase (which may use a heme or vanadium cofactor) and iodoperoxidases. The bromoperoxidase produces an estimated 1–2 million tons of bromoform and 56,000 tons of bromomethane annually. Most naturally occurring organobromine compounds are produced by this enzyme, catalyzing the following reaction (R-H is hydrocarbon substrate):

R-H + Br⁻ + H₂O₂ → R-Br + H₂O + OH⁻

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.

Vanadium accumulation in tunicates and ascidians

Vanadium is essential to ascidians and tunicates, where it is stored in the highly acidified vacuoles of certain blood cell types, designated "vanadocytes". Vanabins (vanadium binding proteins) have been identified in the cytoplasm of such cells. The concentration of vanadium in the blood of ascidians is as much as ten million times higher than the surrounding seawater, which normally contains 1 to 2 µg/l. The function of this vanadium concentration system and these vanadium-bearing proteins is still unknown, but the vanadocytes are later deposited just under the outer surface of the tunic where they may deter predation.

Fungi

Amanita muscaria and related species of macrofungi accumulate vanadium (up to 500 mg/kg in dry weight). Vanadium is present in the coordination complex amavadin in fungal fruit-bodies. The biological importance of the accumulation is unknown. Toxic or peroxidase enzyme functions have been suggested.

Mammals

Deficiencies in vanadium result in reduced growth in rats. The U.S. Institute of Medicine has not confirmed that vanadium is an essential nutrient for humans, so neither a Recommended Dietary Intake nor an Adequate Intake have been established. Dietary intake is estimated at 6 to 18 µg/day, with less than 5% absorbed. The Tolerable Upper Intake Level (UL) of dietary vanadium, beyond which adverse effects may occur, is set at 1.8 mg/day.

Research

Vanadyl sulfate as a dietary supplement has been researched as a means of increasing insulin sensitivity or otherwise improving glycemic control in people who are diabetic. Some of the trials had significant treatment effects, but were deemed as being of poor study quality. The amounts of vanadium used in these trials (30 to 150 mg) far exceeded the safe upper limit. The conclusion of the systemic review was "There is no rigorous evidence that oral vanadium supplementation improves glycaemic control in type 2 diabetes. The routine use of vanadium for this purpose cannot be recommended."

In astrobiology, it has been suggested that discrete vanadium accumulations on Mars could be a potential microbial biosignature, when used in conjunction with Raman spectroscopy and morphology.

Safety

All vanadium compounds should be considered toxic. Tetravalent VOSO₄ has been reported to be at least 5 times more toxic than trivalent V₂O₃. 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, that is, likely to cause permanent health problems or death.

Vanadium compounds are poorly absorbed through the gastrointestinal system. Inhalation of vanadium and vanadium compounds results primarily in adverse effects on the respiratory system. 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, liver, neurological development, and other organs in rats. 

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 in male and female mice by inhalation in an NTP study, although the interpretation of the results has recently been disputed. The carcinogenicity of vanadium has not been determined by the United States Environmental Protection Agency.

Vanadium traces in diesel fuels are the main fuel component in high temperature corrosion. During combustion, vanadium oxidizes and reacts with sodium and sulfur, yielding vanadate compounds with melting points as low as 530 °C, which attack the passivation layer on steel and render it susceptible to corrosion. The solid vanadium compounds also abrade engine components.