Basic information History, Occurrence, and Uses Chemical Properties Uses Reactions Environmental Fate Safety Related Supplier
Vanadium Chemical Properties
- Melting point:1890 °C(lit.)
- Boiling point:3380 °C(lit.)
- Density 6.11 g/mL at 25 °C(lit.)
- vapor pressure 8 mm Hg ( 20 °C)
- storage temp. Storage temperature: no restrictions.
- solubility H2O: soluble
- form turnings
- Specific Gravity6.11
- color Silver-gray
- Resistivity24.8-26.0 μΩ-cm, 20°C
- Water Solubility insoluble H2O; reacts with hot H2SO4, HF, HNO3, aqua regia [MER06]
- Merck 13,9984
- Stability:Stable. Incompatible with strong acids, strong oxidizing agents.
- CAS DataBase Reference7440-62-2(CAS DataBase Reference)
- EPA Substance Registry SystemVanadium (7440-62-2)
Vanadium Usage And Synthesis
- History, Occurrence, and UsesVanadium was discovered in 1801 by Mexican mineralogist Manuel del Rio in a lead ore in Hidalgo, Mexico. He named it erythronium because of the red color its salts when heated with acids. However, del Rio’s discovery was mistakenly thought at that time to be a form of impure chromium. Swedish chemist Sefstrom in 1830 rediscovered this element detecting an unknown metal in the iron ores of Taberg, Sweden. He named it vanadium after the Scandinavian goddess Vanadis. Later in 1830, Wohler determined that del Rio’s erythronium and Sefstrom’s vanadium were the same element. Vanadium metal was prepared for the first time by Roscoe in 1867 in somewhat impure form, as a silvery-white powder, by reduction of vanadium chloride, VCl2, with hydrogen. Hunter and Jones in 1923 prepared the metal at 99.5% purity as a fine gray powder by thermal reduction of vanadium trichloride with sodium in a steel bomb.
Vanadium is added to steel for high resistance to oxidation and to stabilize carbide. Vanadium foil is used for cladding titanium to steel. Vanadium-gallium alloy is used in making superconductive magnets. An important compound of vanadium is pentoxide which has many commercial uses (See Vanadium Pentoxide).
- Chemical PropertiesVanadium typically exists in two forms in fresh water depending on the presence of oxidizing or reducing agents in the water. In the presence of reducing agents, vanadium is present as vanadyl compounds (VO2+ and VO(OH)+) and in the presence of oxidizing substances vanadium is found in the pentavalent form (V+5) as vanadate compounds such as H2VO4- and HVO42- (Holdway and Sprague, 1979). Vanadiumcompounds also combineswith particulatematter in fresh water with a particular affinity for humic acids (Ünsal, 1982).
- UsesVanadium is a naturally occurring element, and is the 22nd most abundant element found in geological formations. The initial discovery of vanadium occurred in 1801 by a Spanish chemist and mineralogist working as a teacher in Mexico, Andrés Manuel del Río. He described his analyses of lead ores and further chemical tests concluded that he had discovered a new element. He gave samples of his work to Alexander von Humboldt, who after consulting with a French chemist, was convinced that this new element was chromium.
Vanadium is also commonly used as a catalyst in the production of sulfuric acid and maleic acid anhydride—the latter compound is used in the synthesis of rubber polymers (Cheng et al., 2009). Vanadium pentoxide is used as a catalyst to oxidize sulfur dioxide (SO2) to anhydrous sulfur trioxide (SO3) followed by a reaction with water to generate sulfuric acid (H2SO4). Maleic acid anhydride is prepared by the vanadium pentoxide-catalyzed oxidation of benzene. More recently, vanadium pentoxide has been used as a selective reducing catalyst to reduce NO and NO2 emitted from diesel engines to nitrogen gas (N2) (Matthey, 2010). Other uses of vanadium compounds include the development of new batteries (e.g., vanadium flow and lithium–vanadium batteries), treatment of wastewater for nitrates, and as a colorant in ceramics and enamels.
- ReactionsVanadium forms four oxides: the light grey monoxide, VO or (V2O2); the blue black dioxide, VO2 (or V2O4); the black sesquioxide, V2O3; and the orangered pentoxide, V2O5. The oxides are formed when the metal is heated in air or oxygen. Vanadium combines with chlorine on heating. Three chlorides are known: the green dichloride, VCl2; the pink trichloride, VCl3; and the brownred tetrachloride, VCl4. The more stable tetrachloride is formed when the metal is heated with chlorine at 180°C. The metal also forms three fluorides in valence states +3, +4, and +5. They are the green trifluoride, VF3; a yellowishbrown tetrafluoride, VF4, and the white pentafluoride, VF5. When heated with bromine vapor vanadium forms the green-black tribromide, VBr3. Vanadium forms two iodides, a violet-rose diiodide, VI2, and a deliquescent triiodide, VI3.
Vanadium combines with other nonmetals at elevated temperatures forming binary compounds. Such compounds include nitride, VN; carbide VC, and the sulfides, VS (or V2S2), V2S3, and V2S5.
Vanadium reacts with fused caustic soda and caustic potash to form water soluble vanadates with liberation of hydrogen. The metal, however, is stable in alkaline solutions.
- Environmental FateNatural sources of vanadium in soil come from minerals (over 50 known minerals containing vanadium; Box 37.2) and from the atmospheric deposition of marine aerosols and particulate matter of volcanic origin. Vanadium is not typically mined for directly but is recovered while mining for other minerals. In addition, anthropogenic sources of vanadium also find their way into soil primarily fromthe deposition of particulatematter from fossil fuel combustion sources (e.g., coal- and oil-fueled power plants). Themovement of vanadiumin soil is heavilypH dependent since most vanadium minerals are not soluble in neutral water.
The presence of vanadium in the atmosphere is primarily in the form of compounds bound to particulate matter as gaseous species of vanadium do not exist at ambient temperatures. Examples of vanadium compounds bound to particulate matter include vanadium pentoxide (V2O5), but most measurements of vanadium bound to particles is measured as elemental vanadium and is not speciated to specific compounds or minerals. Vanadium-enriched particles can dry deposit, as do particles in general, as well as be rained out with particles either acting as condensation nuclei or being absorbed directly into water droplets.
- Chemical PropertiesVanadium is a soft, ductile, silver-gray metal. It has good resistance to corrosion by alkalis, sulfuric and hydrochloric acid, and salt water. Vanadium metal, sheet, strip, foil, bar, wire, and tubing are used in industries. It is used in high-temperature service, in the production of rust-resistant, high-speed tools, and is an important carbide stabilizer in making steels. In fact, most vanadium is used as an additive to improve steels. Vanadium steel is especially strong and hard, with improved resistance to shock. Vanadium pentoxide (V2O5) is perhaps vanadium’s most useful compound. It is used as a mordant—a material that permanently fi xes dyes to fabrics. Vanadium pentoxide is used as a catalyst in chemical reactions and in the manufacture of ceramics. Vanadium pentoxide can also be mixed with gallium to form superconductive magnets.
- Chemical PropertiesVanadium is a light-gray or silver-white, ductile solid, lustrous powder, or fused hard lump. Insoluble in water; resistant to corrosion, but soluble in nitric, hydrofluoric, and concentrated sulfuric acids; attacked by alkali, forming water-soluble vanadates. Acts as either a metal or a nonmetal and forms a variety of complex compounds.
- Physical propertiesVanadium is a silvery whitish-gray metal that is somewhat heavier than aluminum, butlighter than iron. It is ductile and can be worked into various shapes. It is like other transitionmetals in the way that some electrons from the next-to-outermost shell can bond with otherelements. Vanadium forms many complicated compounds as a result of variable valences. Thisattribute is responsible for the four oxidation states of its ions that enable it to combine withmost nonmetals and to at times even act as a nonmetal. Vanadium’s melting point is 1890°C,its boiling point is 3380°C, and its density is 6.11 g/cm3.
- IsotopesThere are 27 isotopes of vanadium. Only vanadium-51 is stable and makes up99.75% of the total vanadium on Earth. The other 0.25% of the vanadium found onEarth is from the radioisotope vanadium-50, which has such a lon+17years that it is considered stable. The other radioactive isotopes have half-lives rangingfrom 150 nanoseconds to one year.
- Origin of NameNamed after the Scandinavian mythological goddess Vanadis because of the many colors exhibited by vanadium’s compounds.
- OccurrenceVanadium is not found in its pure state. Small amounts of vanadium can be found inphosphate rocks and some iron ores. Most of it is recovered from two minerals: vanadinite,which is a compound of lead and chlorine plus some vanadium oxide, and carnotite, a mineral containing uranium, potassium, and an oxide of vanadium. Because of its four oxidationstates and its ability to act as both a metal and a nonmetal, vanadium is known to chemicallycombine with over 55 different elements.Vanadium’s principal ores are roscoelite, patronite, vanadinite, and carnotite, which arefound in the states of Idaho, Montana, Arkansas, and Arizona as well as in Mexico and Peru.It is also a by-product from the production of phosphate ores.
- CharacteristicsVanadium is an excellent alloy metal with iron that produces hard, strong, corrosion-resistant steel that resists most acids and alkali. It is even more resistant to seawater corrosion thanis stainless steel. Vanadium is difficult to prepare in a pure form in large amounts. Impureforms seem to work as well as a very pure form of the metal when used as an alloy. Whenworked as a metal, it must be heated in an inert atmosphere because it will readily oxidize.
- HistoryVanadium was first discovered by del Rio in 1801. Unfortunately, a French chemist incorrectly declared that del Rio’s new element was only impure chromium; del Rio thought himself to be mistaken and accepted the French chemist’s statement. The element was rediscovered in 1830 by Sefstrom, who named the element in honor of the Scandinavian goddess Vanadis because of its beautiful multicolored compounds. It was isolated in nearly pure form by Roscoe, in 1867, who reduced the chloride with hydrogen. Vanadium of 99.3 to 99.8% purity was not produced until 1927. Vanadium is found in about 65 different minerals among which carnotite, roscoelite, vanadinite, and patronite are important sources of the metal. Vanadium is also found in phosphate rock and certain iron ores, and is present in some crude oils in the form of organic complexes. It is also found in small percentages in meteorites. Commercial production from petroleum ash holds promise as an important source of the element. China, South Africa, and Russia supply much of the world’s vanadium ores. High-purity ductile vanadium can be obtained by reduction of vanadium trichloride with magnesium or with magnesium–sodium mixtures. Much of the vanadium metal being produced is now made by calcium reduction of V2O5 in a pressure vessel, an adaptation of a process developed by McKechnie and Seybolt. Natural vanadium is a mixture of two isotopes, 50V (0.25%) and 51V (99.75%). 50V is slightly radioactive, having a long half-life. Twenty other unstable isotopes are recognized. Pure vanadium is a bright white metal, and is soft and ductile. It has good corrosion resistance to alkalis, sulfuric and hydrochloric acid, and salt water, but the metal oxidizes readily above 660°C. The metal has good structural strength and a low-fission neutron cross section, making it useful in nuclear applications. Vanadium is used in producing rust-resistant, spring, and high-speed tool steels. It is an important carbide stabilizer in making steels. About 80% of the vanadium now produced is used as ferrovanadium or as a steel additive. Vanadium foil is used as a bonding agent in cladding titanium to steel. Vanadium pentoxide is used in ceramics and as a catalyst. It is also used in producing a superconductive magnet with a field of 175,000 gauss. Vanadium and its compounds are toxic and should be handled with care. Ductile vanadium is commercially available. Vanadium metal (99.7%) costs about $3/g.
- UsesThe major use of vanadium is as an alloying metal to make a strong and corrosion-resistant form of steel that is well suited for structures such as nuclear reactors. It does not absorbneutrons or become “stretched” by heat and stress, as does normal stainless steel, thus makingvanadium ideal for the construction of nuclear reactors.Some of its compounds, particularly the oxides, are used in chemical industries as catalyststo speed up organic chemical reactions. The yellow-brown vanadium pentoxide (V2O5) is usedas a catalyst to facilitate the production of sulfuric acid by the contact process. Vanadium pentoxide is also used as a photographic developer, to dye textiles, and in the production of artificialrubber. When combined with glass, it acts as a filter against ultraviolet rays from sunlight.
- DefinitionA silvery transition element occurring in complex ores in small quantities. It is used in alloy steels. Vanadium forms compounds with oxidation states +5, +4, +3, and +2. It forms colored ions. Symbol: V; m.p. 1890°C; b.p. 3380°C; r.d. 6.1 (20°C); p.n. 23; r.a.m. 50.94.
- DefinitionSymbol V. A silverywhite metallic transition element; a.n. 23; r.a.m. 50.94; r.d. 5.96; m.p. 1890°C; b.p. 3380°C. It occurs in a number of complex ores, including vanadinite (Pb5Cl(VO4)3) and carnotite (K2(ClO2)2(VO4)2). The pure metal can be obtained by reducing the oxide with calcium. The element is used in a large number of alloy steels. Chemically, it reacts with nonmetals at high temperatures but is not affected by hydrochloric acid or alkalis. It forms a range of complexes with oxidation states from +2 to +5. Vanadium was discovered in 1801 by Andrés del Rio (1764–1849), who allowed himself to be persuaded that what he had discovered was an impure form of chromium. The element was rediscovered and named by Nils Sefström (1787–1854) in 1880.
- Production MethodsWorld resources of vanadium exceed 63 million tons. Vanadium occurs in deposits of phosphate rock, titaniferous magnetite, and uraniferous sandstone and siltstone, in which it constitutes less than 2% of the host rock. Signi?cant amounts are also present in bauxite and carboniferous materials,suchascoal,crudeoil,oilshale,andtarsands(19).
Vanadium is usually recovered as a by-product or a coproduct during the extraction of other compounds, such as iron, titanium, phosphate, or petroleum. It is extracted from carnotite, phosphate rock deposits, titaniferous magnetites, and vanadiferous clays. A process called salt roasting during the initial stage of extraction produces the oxide concentrate. The ores, petroleum residues, iodide thermal decomposition products, and slags formed during ferrovanadate production are crushed, dried, ?nely ground, mixed with a sodium salt, and roasted. The hot ore, containing sodium metavanadate, precipitates as a red cake, is then mixedwithsulfuricacid,andtheresultantprecipitateisdried to form vanadium pentoxide. The vanadium pentoxide can then be processed further to form the required vanadium compound. Pure vanadium is dif?cult to obtain as it tends to be readily contaminated with other elements. Methods to extract pure vanadium include iodide re?ning, electrolytic re?ning in a fused salt, and electrotransport. The highest purity vanadium has been puri?ed by the electrotransport technique. High-purity ductile vanadium can be obtainedbyreductionofvanadiumchloridewithmagnesium or with magnesium-sodium mixtures. Much of thevanadium metal is now produced by calcium reduction of V2O5 in a pressure vessel.
- Air & Water ReactionsNot oxidized by air and not appreciably affected by moisture at ordinary temperatures. Some hydrogen gas may be created however this would proceed slowly under ambient conditions. Insoluble in water.
- Reactivity ProfileVANADIUM is a reducing agent. Finely divided form favors rapid or explosive reactions with oxidizing agents such as air or oxygen. Reacts exothermically with compounds having active hydrogen atoms (such as acids and water) to form flammable hydrogen gas and caustic products. The reactions are much less vigorous than the similar reactions of alkali metals. Can catalyze polymerization reactions in several classes of organic compounds; these polymerizations sometimes proceed rapidly or even explosively. Vanadium is used as a catalyst in the production of synthetic rubber and sulfuric acid.
- HazardVanadium powder, dust, and most of its oxide compounds are explosive when exposedto heat and air. They are also toxic when inhaled. Vanadium chloride compounds are strongirritants to the skin and poisonous when ingested.
Many of its compounds must be stored in a dry, oxygen-free atmosphere or in containersof inert gas. Protective clothing and goggles should be worn when handling vanadium, as wellas with most of the other transition elements.
- Health HazardExposures to high levels of vanadium cause harmful health effects. The major effects from breathing high levels of vanadium are on the lungs, throat, and eyes. Workers who breathe vanadium for short and long periods show lung irritation, coughing, wheezing, chest pain, runny nose, and sore throat. Prolonged period of exposures to respirable dusts and vanadium fume have caused potential symptoms of toxicity among occupational workers. The symptoms of poisoning include, but are not limited to, irritation of the eyes and throat, green tongue, metallic taste, sore throat, cough, drowsiness, wheezing, bronchitis, abdominal cramps, nausea, vomiting, diarrhea, respiratory distress, pulmonary edema, bronchial damage, epistaxis (bloody nose), eczema, conjunctivitis, headache, dry mouth, dizziness, nervousness, insomnia, and tremor. It is not classifi able as a human carcinogen. Vanadium is a natural component of fuel oil, and workers have developed vanadium poisoning during cleaning operations on oil-fi red furnaces.
- Agricultural UsesVanadium (V) is a silvery-white, metallic, transition
element of Group 5 of the Periodic Table and
exhibits a range of valencies from +2 to +5. The ores
containing vanadium include vanadite and carnotite.
The pure metal, formed by the reduction of vanadium
oxide with calcium, is generally used as an alloying
element for steel and iron. Several vanadium compounds
are used as oxidation catalysts. They are also used as
coloring agents in the ceramic industry.
Vanadium comes under the category of beneficial elements which are non-essential but beneficial to plant growth. It is a very useful nutrient for the green alga Scenedesmus, but the exact amount of vanadium needed for the growth of higher plants is yet to be established.
Vanadium may replace molybdenum to some extent in nitrogen fixation by micro-organisms such as Azotobacter and Rhizobium. An increase in growth due to vanadium is seen in asparagus, rice, lettuce, barley and corn. It has also been speculated that vanadium may function in biological oxidation-reduction reactions.
Vanadium stimulates growth and nitrogenase activity in Anabaena variabilis in the absence of molybdenum. Low concentrations of vanadium are beneficial for the optimal growth of micro-organisms and higher plants. Generally, the concentration of vanadium in plants is about 1 ppm.
- Industrial usesVanadium is a member of the d-block metals and belongs to group 5 of the periodic table of elements. Vanadium can be found in the earth s crust in numerous minerals and is isolated from ores mostly as a by-product. Its main application is in the steel industry, where it is used as an alloy in combination with iron. Vanadium pentaoxide is also being used as a catalyst for the production of sulfuric acid. The metal vanadium has very similar properties to titanium. Therefore, it is not surprising that its metallocene, vanadium dichloride, was also subjected to research as a potential anticancer agent. Vanadium is an essential trace metal in the human body, but still very little is known about its biological function. Vanadium is mainly found in its ionic state bound to proteins.
- Safety ProfileAn inhalation hazard. Poison by subcutaneous route. Questionable carcinogen with experimental tumorigenic data. Flammable in dust form from heat, flame, or sparks. Violent reaction with BrF3, Cl2, lithium, nitryl fluoride, oxidants. When heated to decomposition it emits toxic fumes of VOx. See also VANADIUM COMPOUNDS.
- Potential ExposureVanadium is used as a catalyst in the production of synthetic rubber and sulfuric acid. Most of the vanadium produced is used in ferrovanadium and of this the majority is used in high speed and other alloy steels with only small amounts in tool or structural steels. It is usually combined with chromium, nickel, manganese, boron, and tungsten in steel alloys.
- Veterinary Drugs and TreatmentsVanadium supplementation may be useful in the adjunctive treatment of diabetes mellitus, particularly in cats. There is controversy whether or not this treatment is beneficial.
- CarcinogenicityThe results of 2-year NTP inhalation study on F344/N rats (at concentrations of 0, 5, 1, or 2mg/m3) and B6C3F1 mice (at concentrations of 1, 2, or 4mg/m3)exposedfor6hperdayfor5daysperweekindicate clear evidence of carcinogenic activity of vanadium pentoxide based on the occurrence of alveolar/bronchiolar neoplasms. Exposure to V2O5 caused a spectrum of nonneoplastic lesions in the respiratory tract (nose, larynx, and lung), including alveolar and bronchiolar epithelium hyperplasia, in?ammation, ?brosis, and alveolar histiocytosis of the lung in male and female rats and mice, and an unusual squamous metaplasia of the lung in male and female rats. Hyperplasiaofthebronchiallymphnodesoccurredinfemale mice. In a 16-day inhalation study in rat, alveolar and bronchiolar epithelial hyperplasia was observed in most rats exposed to 2 or 4mg/m3 V2O5 on days 6 and 13.
- ShippingUN3285 Vanadium compound, n.o.s., Hazard Class: 6.1; Labels: 6.1-Poisonous materials, Technical Name Required. This number includes vanadium fume or dust.
- Purification MethodsClean the metal by rapid exposure consecutively to HNO3, HCl, HF, de-ionised water and reagent grade acetone, then dry it in a vacuum desiccator. [Brauer in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol II pp 1252-1255 1965.]
- IncompatibilitiesDust may form explosive mixture with air. Dust, fume, and powders are a strong reducing agent; incompatible with oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions. Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides, bromine trifluoride, lithium, nitryl fluoride, chlorine trifluoride.
- VANADIUM (IV) SULFATE OXIDE HYDRATE,VANADIUM (IV) OXYSULFATE, HYDROUS Vanadium(V) oxide VANADIUM OXALATE VANADIUM OXALATE VANADIUM SILICATE VANADIUM OXIDE VANADIUM OXYTRICHLORIDE VANADIUM OXIDE VANADIUM SELENIDE VANADIUM OXIDE VANADIUM N-BUTOXIDE VANADIUM OXYFLUORIDE,VANADIUM OXYTRIFLUORIDE 2,4-PENTANEDIONE, VANADIUM(III) DERIVATIVE VANADIUM OCTAETHYLPORPHINE OXIDE,2,3,7,8,12,13,17,18-OCTAETHYL-21H,23H-PORPHINE VANADIUM(IV) OXIDE ) VANADIUM PENTOXIDE POWDER VANADIUM NAPHTHENATE OXIDE VANADIUM OXIDE TRIS(METHOXYETHOXIDE) VANADIUM (IV,V) OXIDE,VANADIUM OXIDE
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