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gray metallic
General properties
Name, symbol, number molybdenum, Mo, 42
Element category transition metal
Group, period, block 65, d
Standard atomic weight 95.94g·mol−1
Electron configuration [Kr] 5s1 4d5
Electrons per shell 2, 8, 18, 13, 1 (Image)
Physical properties
Phase solid
Density (near r.t.) 10.28 g·cm−3
Liquid density at m.p. 9.33 g·cm−3
Melting point 2896 K, 2623 °C, 4753 °F
Boiling point 4912 K, 4639 °C, 8382 °F
Heat of fusion 37.48 kJ·mol−1
Heat of vaporization 617 kJ·mol−1
Specific heat capacity (25 °C) 24.06 J·mol−1·K−1
Vapor pressure
P/Pa 1 10 100 1 k 10 k 100 k
at T/K 2742 2994 3312 3707 4212 4879
Atomic properties
Oxidation states 6, 5, 4, 3, 2, 1[1], -1, -2
(strongly acidic oxide)
Electronegativity 2.16 (Pauling scale)
Ionization energies 1st: 684.3 kJ·mol−1
2nd: 1560 kJ·mol−1
3rd: 2618 kJ·mol−1
Atomic radius 139 pm
Covalent radius 154±5 pm
Crystal structure body-centered cubic
Magnetic ordering paramagnetic[2]
Electrical resistivity (20 °C) 53.4 nΩ·m
Thermal conductivity (300 K) 138 W·m−1·K−1
Thermal expansion (25 °C) 4.8 µm·m−1·K−1
Young's modulus 329 GPa
Shear modulus 126 GPa
Bulk modulus 230 GPa
Poisson ratio 0.31
Mohs hardness 5.5
Vickers hardness 1530 MPa
Brinell hardness 1500 MPa
CAS registry number 7439-98-7
Most stable isotopes
Main article: Isotopes of molybdenum
iso NA half-life DM DE (MeV) DP
92Mo 14.84% 92Mo is stable with 50 neutrons
93Mo syn 4×103 y ε - 93Nb
94Mo 9.25% 94Mo is stable with 52 neutrons
95Mo 15.92% 95Mo is stable with 53 neutrons
96Mo 16.68% 96Mo is stable with 54 neutrons
97Mo 9.55% 97Mo is stable with 55 neutrons
98Mo 24.13% 98Mo is stable with 56 neutrons
99Mo syn 65.94 h β 0.436, 1.214 99Tc
γ 0.74, 0.36,
100Mo 9.63% 7.8×1018 y ββ 3.04 100Ru

Molybdenum (pronounced /ˌmɒlɪbˈdiːnəm/ mol-ib-DEE-nəm, from Neo-Latin Molybdaenum, from Ancient Greek Μόλυβδος molybdos, meaning lead),[3] is a Group 6 chemical element with the symbol Mo and atomic number 42. The free element, which is a silvery metal, has the sixth-highest melting point of any element. It readily forms hard, stable carbides, and for this reason it is often used in high-strength steel alloys. Molybdenum does not occur as the free metal in nature, but rather in various oxidation states in minerals. Industrially molybdenum compounds are used in high pressure and high temperature applications, as pigments and catalysts.

Molybdenum minerals have long been known, but the element was "discovered" (in the sense of differentiating it as a new entity from minerals salts of other metals) in 1778 by Carl Wilhelm Scheele. The metal was first isolated in 1781 by Peter Jacob Hjelm.

Most molybdenum compounds have low water solubility, but the molybdate ion MoO 2−4 is soluble and will form if molybdenum-containing minerals are in contact with oxygen and water. Recent theories suggest that the release of oxygen by early life was important in removing molybdenum from minerals into a soluble form in the early oceans, where it was used as a catalyst by single-celled organisms. This sequence may have been important in the history of life, because molybdenum-containing enzymes then became the most important catalysts used by some bacteria to break into atoms the atmospheric molecular nitrogen, allowing biological nitrogen fixation. This, in turn allowed biologically driven nitrogen-fertilization of the oceans, and thus the development of more complex organisms.

At least 50 molybdenum-containing enzymes are now known in bacteria and animals, though only the bacterial and cyanobacterial enzymes are involved in nitrogen fixation. Due to the diverse functions of the remainder of the enzymes, molybdenum is a required element for life in higher organisms (eukariotes), though not in all bacteria.





In its pure form, molybdenum is silvery white metal with a Mohs hardness of 5.5. It has a melting point of 2,623 °C (4,753 °F); of the naturally occurring elements, only tantalum, osmium, rhenium, tungsten and carbon have higher melting points.[3] Molybdenum burns only at temperatures above 600 °C (1,112 °F).[4] It has one of the lowest coefficient of thermal expansion among commercially used metals.[5] Tensile strength of molybdenum wires increases about 3 times from about 10 to 30 GPa when their diameter decreases from ~50–100 nm to 10 nm.[6]


There are 35 known isotopes of molybdenum ranging in atomic mass from 83 to 117, as well as four metastable nuclear isomers. Seven isotopes occur naturally, with atomic masses of 92, 94, 95, 96, 97, 98 and 100. Of these naturally occurring isotopes, only molybdenum-92 and molybdenum-100 are unstable.[7] All unstable isotopes of molybdenum decay into isotopes of niobium, technetium and ruthenium.[8]

Molybdenum-98 is the most abundant isotope, comprising 24.14% of all molybdenum. Molybdenum-100 has a half-life of about 1019 y and undergoes double beta decay into ruthenium-100. Molybdenum isotopes with mass numbers from 111 to 117 all have half-lives of approximately 150 ns.[7][8]

As also noted below, the most common isotopic molybdenum application involves molybdenum-99, which is a fission product. It is a parent radioisotope to the short-lived gamma-emitting daughter radioisotope technetium-99m, a nuclear isomer which is used in various imaging applications in medicine.[9]

Compounds and chemistry

Oxidation states
of molybdenum.[10]
−2 Na2[Mo2(CO)10]
0 Mo(CO)6
+1 Na[C6H6Mo]
+2 MoCl2
+3 Na3[Mo(CN)]6
+4 MoS2
+5 MoCl5
+6 MoF6
Keggin structure of the phosphomolybdate anion (P[Mo12O40]3−), an example of a polyoxometalate

Molybdenum is a transition metal with an electronegativity of 1.8 on the Pauling scale and an atomic mass of 95.94 g/mol.[11] It does not react with oxygen or water at room temperature. At elevated temperatures, molybdenum trioxide is formed:[12]

2 Mo + 3 O2 → 2 MoO3

Molybdenum has several oxidation states, the most stable being +4 and +6 (bolded in the table). The chemistry and the compounds show more similarity to those of tungsten than that of chromium. An example is the instability of molybdenum(III) and tungsten(III) compounds compared to the stability of the chromium(III) compounds. The highest oxidation state is common in the molybdenum(VI) oxide MoO3 while the normal sulfur compound is molybdenum disulfide MoS2.[13]

Molybdenum(VI) oxide is soluble in strong alkaline water, forming molybdates (MoO42−). Molybdates are weaker oxidants than chromates, but they show a similar tendency to form complex oxyanions by condensation at lower pH values, such as [Mo7O24]6− and [Mo8O26]4−. Polymolybdates can incorporate other ions into their structure, forming polyoxometalates.[14] The dark-blue phosphorus-containing heteropolymolybdate P[Mo12O40]3− is used for the spectroscopic detection of phosphorus.[15] The broad range of oxidation states of molybdenum is reflected in various molybdenum chlorides:[13]

The structure of the MoCl2 is composed of Mo6Cl84+ clusters with four chloride ions to compensate the charge.[13]

Like chromium and some other transition metals, molybdenum is able to form quadruple bonds, such as in Mo2(CH3COO)4. This compound can be transformed into Mo2Cl84− which also has a quadruple bond.[13]

The oxidation state 0 is possible with carbon monoxide as ligand, such as in molybdenum hexacarbonyl, Mo(CO)6.[13]


Molybdenite—the principal ore from which molybdenum is now extracted—was previously known as molybdena. Molybdena was confused with and often implemented as though it were graphite. Even when the two ores were distinguishable, molybdena was thought to be a lead ore.[5] In 1754, Bengt Andersson Qvist examined the mineral and determined that it did not contain lead.[16]

It was not until 1778 that Swedish chemist Carl Wilhelm Scheele realized molybdena was neither graphite nor lead.[17][18] He and other chemists then correctly assumed that it was the ore of a distinct new element, named molybdenum for the mineral in which it was discovered. Peter Jacob Hjelm successfully isolated molybdenum using carbon and linseed oil in 1781.[5][19] For a long time there was no industrial use for molybdenum. The French Schneider Electric company produced the first molybdenum-steel armor plates in 1894. Until World War I, most other armor factories also used molybdenum alloys. In World War I, some British tanks were protected by 75 mm (3 in) manganese plating, but this proved to be ineffective. The manganese plates were then replaced with 25 mm (1 in) molybdenum plating. These allowed for higher speed, greater maneuverability, and, despite being thinner, better protection.[5] The high demand for molybdenum in World War I and World War II and the steep decrease after the wars had a great influence on prices and production of molybdenum.


Molybdenum output in 2005
Lustrous, silvery, flat, hexagonal crystals in roughly parallel layers sit flowerlike on a rough, translucent crystalline piece of quartz.
Molybdenite on quartz

The world's largest producers of molybdenum materials are the United States, China, Chile, Peru and Canada.[5][20][21] Though molybdenum is found in such minerals as wulfenite (PbMoO4) and powellite (CaMoO4), the main commercial source of molybdenum is molybdenite (MoS2). Molybdenum is mined as a principal ore, and is also recovered as a byproduct of copper and tungsten mining.[3] Large mines in Colorado (such as the Henderson mine and the now-inactive Climax mine)[22] and in British Columbia yield molybdenite as their primary product, while many porphyry copper deposits such as the Bingham Canyon Mine in Utah and the Chuquicamata mine in northern Chile produce molybdenum as a byproduct of copper mining. The Knaben mine in southern Norway was opened in 1885, making it the first molybdenum mine. It remained open until 1973.[23]

Molybdenum is the 54th most abundant element in the Earth's crust and the 25th most abundant element in the oceans, with an average of 10 parts per billion; it is the 42nd most abundant element in the Universe.[4][5] The Russian Luna 24 mission discovered a molybdenum-bearing grain (1 × 0.6 µm) in a pyroxene fragment taken from Mare Crisium on the Moon.[24]


The molybdenite is first heated to a temperature of 700 °C (1,292 °F) and the sulfide is oxidized into molybdenum(VI) oxide by air:[13]

2 MoS2 + 7 O2 → 2 MoO3 + 4 SO2

The oxidized ore is then either heated to 1,100 °C (2,010 °F) to sublimate the oxide, or leached with ammonia which reacts with the molybdenum(VI) oxide to form water-soluble molybdates:

MoO3 + 2 NH4OH → (NH4)2(MoO4) + H2O

Copper, an impurity in molybdenite, is less soluble in ammonia. To completely remove it from the solution, it is precipitated with hydrogen sulfide.[13]

Pure molybdenum is produced by reduction of the oxide with hydrogen, while the molybdenum for steel production is reduced by the aluminothermic reaction with addition of iron to produce ferromolybdenum. A common form of ferromolybdenum contains 60% molybdenum.[5][13]

Molybdenum has a value of approximately $30,000 per tonne as of August 2009. It maintained a price at or near $10,000 per tonne from 1997 through 2003, and reached, due to increased demand, a peak of $103,000 per tonne in June 2005.[25] In 2008 the London Metal Exchange announced that molybdenum would be traded as a commodity on the exchange.[26]


Three helical loops of cylindrical molybdenum disilicide incandesce a vivid orange from heat.
MoSi2 heating element

The ability of molybdenum to withstand extreme temperatures without significantly expanding or softening makes it useful in applications that involve intense heat, including the manufacture of aircraft parts, electrical contacts, industrial motors and filaments.[5][27] Molybdenum is also used in alloys for its high corrosion resistance and weldability.[4][20] Molybdenum contributes corrosion resistance to type 316 stainless steel by lattice strain, increasing the energy required to dissolve out iron atoms from the surface. Most high-strength steel alloys contain 0.25% to 8% molybdenum.[3] Despite such small portions, more than 43,000 tonnes of molybdenum are used as an alloying agent each year in stainless steels, tool steels, cast irons and high-temperature superalloys.[4]

Because of its lower density and more stable price, molybdenum is used instead of tungsten.[4] An example is the 'M' series of high-speed steels such as M2, M4 and M42 as substitution for the 'T' steel series. Molybdenum can be implemented both as an alloying agent and as a flame-resistant coating for other metals. Although its melting point is 2,623 °C (4,753 °F), molybdenum rapidly oxidizes at temperatures above 760 °C (1,400 °F) making it better-suited for use in vacuum environments.[27]

Other molybdenum based alloys have only limited applications. Because of the corrosion resistance against molten zinc, molybdenum and the molybdenum tungsten alloy (70%/30%) are used for piping, stirrers and pump impellers which come into contact with molten zinc.[28]

Molybdenum-99 is a parent radioisotope to the daughter radioisotope technetium-99m, which is used in many medical procedures.[29]

Molybdenum disulfide (MoS2) is used as a solid lubricant and a high-pressure high-temperature (HPHT) antiwear agent. It forms strong films on metallic surfaces and is a common additive to HPHT greases—in case of a catastrophic grease failure, thin layer of molybdenum prevents contact of the lubricated parts.[30] Molybdenum disilicide (MoSi2) is an electrically conducting ceramic with primary use in heating elements operating at temperatures above 1500 °C in air.[31]

Molybdenum trioxide (MoO3) is used as an adhesive between enamels and metals.[17] Lead molybdate (wulfenite) co-precipitated with lead chromate and lead sulfate is a bright-orange pigment used with ceramics and plastics.[32]

Molybdenum powder is used as a fertilizer for some plants, such as cauliflower.[4] It is also used in NO, NO2, NOx analyzers in power plants for pollution controls. At 350 °C (662 °F) the element acts as a catalyst for NO2/NOx to form only NO molecules for consistent readings by infrared light.[33] Ammonium heptamolybdate is used in biological staining procedures.

Biological role


The most important use of the molybdenum in living organisms is as a metal heteroatom at the active site in certain enzymes. In nitrogen fixation in certain bacteria, the nitrogenase enzyme, which is involved in the terminal step of reducing molecular nitrogen, usually contains molybdenum in the active site (though replacement of Mo with iron or vanadium is also known). The structure of the catalytic center of the enzyme is similar to that in iron-sulfur proteins, it incorporates a Fe4S3 and MoFe3S3 clusters.[34]

In 2008, evidence was reported that a scarcity of molybdenum in the Earth's early oceans was a limiting factor in the further evolution of eukaryotic life (which includes all plants and animals) as eukaryotes cannot fix nitrogen and must acquire it from prokaryotic bacteria.[35][36][37] The scarcity of molybdenum resulted from the relative lack of oxygen in the early ocean. Oxygen dissolved in seawater helps dissolve molybdenum from minerals on the sea bottom. However, although oxygen may promote nitrogen fixation via making molybdenum available in water, it also directly poisons these nitrogenase enzymes, so that organisms which continued to fix nitrogen in aerobic conditions were required to isolate their nitrogen-fixing enzymes in heterocysts, or similar structures.

Skeletal structure of a molybdopterin with a single molybdenum atom bound to both of the thiolate groups
The molybdenum cofactor (pictured) contains an organic complex called molybdopterin, which binds an oxidized molybdenum through adjacent sulfur (or occasionally selenium) atoms.

Though molybdenum forms compounds with various organic molecules, including carbohydrates and amino acids, it is transported throughout the human body as MoO 2−4.[38] At least 50 molybdenum-containing enzymes were known by 2002, mostly in bacteria, and their number is increasing with every year;[39][40] those enzymes include aldehyde oxidase, sulfite oxidase and xanthine oxidase.[5] In some animals, and in humans, the oxidation of xanthine to uric acid, a process of purine catabolism, is catalyzed by xanthine oxidase, a molybdenum-containing enzyme. The activity of xanthine oxidase is directly proportional to the amount of molybdenum in the body. However, an extremely high concentration of molybdenum reverses the trend and can act as an inhibitor in both purine catabolism and other processes. Molybdenum concentrations also affect protein synthesis, metabolism and growth.[38]

In animals and plants these enzymes use molybdenum bound at the active site in a tricyclic molybdenum cofactor. All molybdenum-using enzymes so far identified in nature use this cofactor, save for the phylogenetically ancient nitrogenases, which fix nitrogen in some bacteria and cyanobacteria.[41] Molybdenum enzymes in plants and animals catalyze the oxidation and sometimes reduction of certain small molecules, as part of the regulation of nitrogen, sulfur and carbon cycles.[42]

Human dietary intake and deficiency

The human body contains about 0.07 mg of molybdenum per kilogram of weight.[43] It occurs in higher concentrations in the liver and kidneys and in lower concentrations in the vertebrae.[4] Molybdenum is also present within human tooth enamel and may help preventing its decay.[44] Pork, lamb and beef liver each have approximately 1.5 parts per million of molybdenum. Other significant dietary sources include green beans, eggs, sunflower seeds, wheat flour, lentils and cereal grain.[5]

The average daily intake of molybdenum varies between 0.12 and 0.24 mg, but it depends on the molybdenum content of the food.[45] Acute toxicity has not been seen in humans, and the toxicity depends strongly on the chemical state. Studies on rats show a median lethal dose (LD50) as low as 180 mg/kg for some Mo compounds.[46] Although human toxicity data is unavailable, animal studies have shown that chronic ingestion of more than 10 mg/day of molybdenum can cause diarrhea, growth retardation, infertility, low birth weight and gout; it can also affect the lungs, kidneys and liver.[45][47] Sodium tungstate is a competitive inhibitor of molybdenum. Dietary tungsten reduces the concentration of molybdenum in tissues.[4]

Dietary molybdenum deficiency from low soil concentration of molybdenum has been associated with increased rates of esophageal cancer in a geographical band from northern China to Iran.[48][49] Compared to the United States, which has a greater supply of molybdenum in the soil, people living in these areas have about 16 times greater risk for esophageal squamous cell carcinoma.[50]

Molybdenum deficiency has also been reported as a consequence of non-molybdenum supplmented total parenteral nutrition (complete intravenous feeding) for long periods of time. It results in high blood levels of sulfite and urate, in much the same way as molybdenum cofactor deficiency. However, presumably since pure molybdenum deficiency from this mechanism is seen primarily in adults, the neurological consequences have not been as marked as for the congenital cofactor deficiency.

Related diseases

A congenital molybdenum cofactor deficiency disease, seen in infants, results in interference with the ability of the body to use molybdenum in enzymes. It causes high levels of sulphite and urate, and neurological damage.[51][52]. The cause is inability of the body to synthesize molybdenum cofactor, a heterocyclic molecule which binds molybdenum at the active site in all known human enzymes which use molybdenum.

Copper-molybdenum antagonism

High levels of molybdenum can interfere with the body's uptake of copper, producing copper deficiency. Molybdenum prevents plasma proteins from binding to copper, and it also increases the amount of copper that is excreted in urine. Ruminants that consume high amounts of molybdenum develop symptoms including diarrhea, stunted growth, anemia and achromotrichia (loss of hair pigment). These symptoms can be alleviated by the administration of more copper into the system, both in dietary form and by injection.[53] The condition can be aggravated by excess sulfur.[4]

Copper reduction or deficiency can also be deliberately induced for therapeutic purposes by the compound ammonium tetrathiomolybdate, in which the bright red anion tetrathiomolybdate is the copper-chelating agent. Tetrathiomolybdate was first used therapeutically in the treatment of copper toxicosis in animals. It was then introduced as a treatment in Wilson's disease, a hereditary copper metabolism disorder in humans; it acts both by competing with copper absorption in the bowel and by increasing excretion. It has also been found to have an inhibitory effect on angiogenesis, potentially via the inhibition of copper ion dependent membrane translocation process invovling a non-classical secretion pathway.[54]. This makes it an interesting investigatory treatment for cancer, age-related macular degeneration, and other diseases featuring excessive blood vessel deposition.[55][56]


Molybdenum dusts and fumes, as can be generated by mining or metalworking, can be toxic, especially if ingested (including dust trapped in the sinuses and later swallowed).[46] Low levels of prolonged exposure can cause irritation to the eyes and skin. Direct inhalation or ingestion of molybdenum and its oxides should be avoided.[57][58] OSHA regulations specify the maximum permissible molybdenum exposure in an 8-hour day as 5 mg/m3. Chronic exposure to 60 to 600 mg/m3 can cause symptoms including fatigue, headaches and joint pains.[59]


  1. ^ "Molybdenum: molybdenum(I) fluoride compound data". Retrieved 2007-12-10.  
  2. ^ Magnetic susceptibility of the elements and inorganic compounds, in Handbook of Chemistry and Physics 81th edition, CRC press.
  3. ^ a b c d editor-in-chief David R. Lide. (1994). "Molybdenum". in Lide, David R.. CRC Handbook of Chemistry and Physics. 4. Chemical Rubber Publishing Company. p. 18. ISBN 0849304741.  
  4. ^ a b c d e f g h i edited by Glenn D. Considine. (2005). "Molybdenum". in Considine, Glenn D.. Van Nostrand's Encyclopedia of Chemistry. New York: Wiley-Interscience. pp. 1038–1040. ISBN 9780471615255.  
  5. ^ a b c d e f g h i j Emsley, John (2001). Nature's Building Blocks. Oxford: Oxford University Press. pp. 262–266. ISBN 0198503415.  
  6. ^ Shpak, Anatoly P; Kotrechko, Sergiy O; Mazilova, Tatjana I; Mikhailovskij, Igor M (2009). "Inherent tensile strength of molybdenum nanocrystals" (free-download pdf). Science and Technology of Advanced Materials 10: 045004. doi:10.1088/1468-6996/10/4/045004.  
  7. ^ a b Audi, Georges (2003). "The NUBASE Evaluation of Nuclear and Decay Properties". Nuclear Physics A (Atomic Mass Data Center) 729: 3–128. doi:10.1016/j.nuclphysa.2003.11.001.  
  8. ^ a b editor-in-chief, David R. Lide. (2006). Lide, David R.. ed. CRC Handbook of Chemistry and Physics. 11. CRC. pp. 87–88. ISBN 0849304873.  
  9. ^ Armstrong, John T. (2003). "Technetium". Chemical & Engineering News. Retrieved 2009-07-07.  
  10. ^ Schmidt, Max (1968). "VI. Nebengruppe" (in German). Anorganische Chemie II.. Wissenschaftsverlag. pp. 119–127.  
  11. ^ "Properties of Molybdenum". Integral Scientist Periodic Table. Qivx, Inc.. 2003. Retrieved 2007-06-10.  
  12. ^ Winter, Mark. "Chemistry". Molybdenum. The University of Sheffield. Retrieved 2007-06-10.  
  13. ^ a b c d e f g h Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985). Lehrbuch der Anorganischen Chemie (91–100 ed.). Walter de Gruyter. pp. 1096–1104. ISBN 3-11-007511-3.  
  14. ^ Pope, Michael T.; Müller, Achim (1997). "Polyoxometalate Chemistry: An Old Field with New Dimensions in Several Disciplines". Angewandte Chemie International Edition 30: 34. doi:10.1002/anie.199100341.  
  15. ^ ed. by Nollet, Leo M.L. (2000). Handbook of water analysis. New York, NY: Marcel Dekker. pp. 280–288. ISBN 9780824784331.  
  16. ^ Van der Krogt, Peter (2006-01-10). "Molybdenum". Elementymology & Elements Multidict. Retrieved 2007-05-20.  
  17. ^ a b Gagnon, Steve. "Molybdenum". Jefferson Science Associates, LLC. Retrieved 2007-05-06.  
  18. ^ Scheele, C. W. K. (1779). "Versuche mit Wasserbley;Molybdaena". Svenska vetensk. Academ. Handlingar 40: 238.  
  19. ^ Hjelm, P. J. (1788). "Versuche mit Molybdäna, und Reduction der selben Erde". Svenska vetensk. Academ. Handlingar 49: 268.  
  20. ^ a b "Molybdenum Statistics and Information". U.S. Geological Survey. 2007-05-10. Retrieved 2007-05-10.  
  21. ^ Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics. 4. Chemical Rubber Publishing Company. pp. 22–23. ISBN 0849304873.  
  22. ^ Coffman, Paul B. (1937). "The Rise of a New Metal: The Growth and Success of the Climax Molybdenum Company". The Journal of Business of the University of Chicago 10: 30. doi:10.1086/232443.  
  23. ^ Langedal, M (1997). "Dispersion of tailings in the Knabena—Kvina drainage basin, Norway, 1: Evaluation of overbank sediments as sampling medium for regional geochemical mapping". Journal of Geochemical Exploration 58: 157. doi:10.1016/S0375-6742(96)00069-6.  
  24. ^ Jambor, J.L. et al. (2002). "New mineral names" (free download pdf). American Mineralogist 87: 181.  
  25. ^ "Dynamic Prices and Charts for Molybdenum". InfoMine Inc.. 2007. Retrieved 2007-05-07.  
  26. ^ "LME to launch minor metals contracts in H2 2009". London Metal Exchange. 4 September 2008. Retrieved 28 July 2009.  
  27. ^ a b "Molybdenum". Pty. Limited. 2007. Retrieved 2007-05-06.  
  28. ^ Cubberly, W. H.; Bakerjian, Ramon (1989). Tool and manufacturing engineers handbook. Society of Manufacturing Engineers. p. 421. ISBN 9780872633513.  
  29. ^ Gottschalk, A (1969). "Technetium-99m in clinical nuclear medicine". Annual review of medicine 20: 131–40. doi:10.1146/ PMID 4894500.  
  30. ^ Winer, W. (1967). "Molybdenum disulfide as a lubricant: A review of the fundamental knowledge". Wear 10: 422. doi:10.1016/0043-1648(67)90187-1.  
  31. ^ Moulson, A. J.; Herbert, J. M. (2003). Electroceramics: materials, properties, applications. John Wiley and Sons. p. 141. ISBN 0471497487.  
  32. ^ International Molybdenum Association
  33. ^ Lal, S.; Patil, R. S. (2001). Environmental Monitoring and Assessment 68: 37–50. doi:10.1023/A:1010730821844.  
  34. ^ Dos Santos, Patricia C.; Dean, Dennis R. (2008). "A newly discovered role for iron-sulfur clusters". PNAS 105 (33): 11589–11590. doi:10.1073/pnas.0805713105. PMID 18697949.  
  35. ^ Scott, C; Lyons, T. W.; Bekker, A.; Shen, Y.; Poulton, S. W.; Chu, X.; Anbar, A. D. (2008). "Tracing the stepwise oxygenation of the Proterozoic ocean". Nature 452 (7186): 456–460. doi:10.1038/nature06811. PMID 18368114.  
  36. ^ "International team of scientists discover clue to delay of life on Earth". Retrieved 2008-10-25.  
  37. ^ "Scientists uncover the source of an almost 2 billion year delay in animal evolution". Retrieved 2008-10-25.  
  38. ^ a b Mitchell, Phillip C. H. (2003). "Overview of Environment Database". International Molybdenum Association. Retrieved 2007-05-05.  
  39. ^ Enemark, John H. et al. (2004). "Synthetic Analogues and Reaction Systems Relevant to the Molybdenum and Tungsten Oxotransferases". Chem. Rev. 104 (2): 1175–1200. doi:10.1021/cr020609d. PMID 14871153.  
  40. ^ Mendel, RR; Bittner, F (2006). "Cell biology of molybdenum.". Biochimica et biophysica acta 1763 (7): 621–635. doi:10.1016/j.bbamcr.2006.03.013. PMID 16784786.  
  41. ^ [1] Structure, synthesis, empirical formula for the di-sulfhydryl. Accessed Nov. 16, 2009.
  42. ^ Kisker, C.; Schindelin, H.; Baas, D.; Rétey, J.; Meckenstock, R.U; Kroneck, P.M.H (1999). "A structural comparison of molybdenum cofactor-containing enzymes". FEMS Microbiol. Rev. 22 (5): 503–521. doi:10.1111/j.1574-6976.1998.tb00384.x. PMID 9990727.  
  43. ^ Holleman, Arnold F.; Wiberg, Egon (2001). Inorganic chemistry. Academic Press. p. 1384. ISBN 0123526515.  
  44. ^ Curzon, M. E. J.; Kubota, J.; Bibby, B.G. (1971). "Environmental Effects of Molybdenum on Caries" (PDF). Journal of Dental Research 50: 74–77. doi:10.1177/00220345710500013401 (inactive 2009-09-29).  
  45. ^ a b Coughlan, M. P. (1983). "The role of molybdenum in human biology". Journal of Inherited Metabolic Disease 6: 70–77. doi:10.1007/BF01811327. PMID 6312191.  
  46. ^ a b "Risk Assessment Information System: Toxicity Summary for Molybdenum". Oak Ridge National Laboratory. Retrieved 2008-04-23.  
  47. ^ Barceloux‌, Donald G.; Barceloux, Donald (1999). "Molybdenum". Clinical Toxicology 37 (2): 231–237. doi:10.1081/CLT-100102422. PMID 10382558.  
  48. ^ Yang, Chung S. (1980). "Research on Esophageal Cancer in China: a Review". Cancer Research 40: 2633.  
  49. ^ Nouri, Mohsen; Chalian, Hamid; Bahman, Atiyeh; Mollahajian, Hamid; Ahmadi-Faghih, Mohammadamin; Fakheri, Hafez; Soroush, Ahmadreza (2008). "Nail Molybdenum and Zinc Contents in Populations with Low and Moderate Incidence of Esophageal Cancer". Archives of Iranian Medicine 11: 392.  
  50. ^ Taylor, Philip R.; Li, Bing; Dawsey, Sanford M.; Li, Jun-Yao; Yang, Chung S.; Guo, Wande; Blot, William J. (1994). "Prevention of Esophageal Cancer: The Nutrition Intervention Trials in Linxian, China". Cancer Research 54 (7 Suppl): 2029s-2031s. PMID 8137333.  
  51. ^ Smolinsky, B. et al. (2008). "Splice-specific Functions of Gephyrin in Molybdenum Cofactor Biosynthesis" (free text). Journal of Biological Chemistry 283 (25): 17370. doi:10.1074/jbc.M800985200. PMID 18411266.  
  52. ^ Reiss, J. (2000). "Genetics of molybdenum cofactor deficiency". Human Genetics 106 (2): 157. doi:10.1007/s004390051023. PMID 10746556.  
  53. ^ Suttle, N. F. (1974). "Recent studies of the copper-molybdenum antagonism". Proceedings of the Nutrition Society (CABI Publishing) 33 (3): 299–305. doi:10.1079/PNS19740053. PMID 4617883.  
  54. ^ Nickel, W (2003). "The Mystery of nonclassical protein secretion, a current view on cargo proteins and potential export routes". Eur. J. Biochem. 270: 2109–2119. doi:10.1046/j.1432-1033.2003.03577.x.  
  55. ^ Brewer GJ, Hedera P, Kluin KJ et al. (2003). "Treatment of Wilson disease with ammonium tetrathiomolybdate: III. Initial therapy in a total of 55 neurologically affected patients and follow-up with zinc therapy". Arch Neurol 60 (3): 379–85. doi:10.1001/archneur.60.3.379. PMID 12633149.  
  56. ^ A phase I trial of thiomolybdate as an chemotherapeutic agent in humans. Accessed Nov. 8 2009.
  57. ^ "Material Safety Data Sheet - Molybdenum". The REMBAR Company, Inc.. 2000-09-19. Retrieved 2007-05-13.  
  58. ^ "Material Safety Data Sheet - Molybdenum Powder". CERAC, Inc.. 1994-02-23. Retrieved 2007-10-19.  
  59. ^ "NIOSH Documentation for ILDHs Molybdenum". National Institute for Occupational Safety and Health. 1996-08-16. Retrieved 2007-05-31.  

External links

1911 encyclopedia

Up to date as of January 14, 2010

From LoveToKnow 1911

MOLYBDENUM [[[symbol]], Mo; atomic weight, 96 (0=16)] a metallic chemical element. The name is derived from Gr. yOXv13Sos, lead, and was originally employed to denote many substances containing or resembling lead; ultimately the term was applied to graphite and to molybdenum sulphide. The difference between these two latter substances was first pointed out by Cronstedt, and in 1778 C. Scheele prepared molybdic acid from the sulphide. Molybdenum occurs in nature chiefly as the minerals molybdenite (MoS 2) and wulfenite (PbMo04), and more rarely as molybdic ochre (Moos) and ilsemannite; it also occurs in many iron ores. The metal may be obtained by heating the trioxide with carbon in the electric furnace (H. Moissan, Comptes rendus, 1893, 116, p. 1225), or by the Goldschmidt method (Rosenheim and Braun, Zeit. anorg. Chem., 1905, p. 311) or by dissociating the tetraand pentachloride in a graphite crucible with an electric current below 1330° (J. N. Pring and W. Fielding, Jour. Chem. Soc., 1909, 95, p. 1 497). It forms a grey coloured powder of specific gravity 9.01; it is malleable, and not as hard as glass. It is rapidly oxidized on heating to a temperature of 500°-600° C., and also when fused with nitre or potassium chlorate. It is soluble in dilute nitric acid, and in concentrated sulphuric acid; in the XVIII. 2 2 a latter case with the formation of a blue solution which on heating ,becomes colourless, molybdenum trioxide being formed with the liberation of sulphur dioxide.

Molybdenum combines with oxygen to form many oxides, the most important of which are: the monoxide, MoO.n (H 2 O), the sesquioxide, M0203, the dioxide, MoO 2, and the trioxide, MoO 3. Molybdenum monoxide, MoO.n(H 2 O), is a black powder obtained when the dichloride is boiled with concentrated potash solution. According to W. Muthmann and W. Nagel (Ber., 1898, 31, p. 2009), this oxide does not exist, the reaction leading to the formation of an hydroxide according to the equation: Mo 3 C1 4 (OH) 2 + 4KHO 3H 2 O = 3Mo(OH) 3 -l-4KBr+3H. Molybdenum sesquioxide, Mo 2 O 3, a black mass insoluble in acids, is formed by heating the corresponding hydroxide in vacuo, or by digesting the trioxide with zinc and hydrochloric acid. Molybdenum dioxide, Mo02, is formed by heating sodium trimolybdate, Na2M03010, to redness in a current of hydrogen (L. Svanberg and H. Struve, Jour. prak. Chem., 1848, 44, P. 301), or by long fusion of a mixture of ammonium molybdate, potassium carbonate, and boron trioxide (W. Muthmann, Ann., 1887, 238, p. 114). It forms quadratic prisms, having a violet reflex and insoluble in boiling hydrochloric acid. Molybdenum trioxide, Mo03, is prepared by oxidizing the metal or the sulphide by heating them in air, or with nitric acid. It is a white powder, which turns pale yellow on heating, and melts at a red heat. It sublimes in small rhombic tables or needles, and is slightly soluble in cold water, the solution possessing an acid reaction. Several hydrated forms of the oxide are known, and a colloidal variety may be obtained by the dialysis of a strong hydrochloric acid solution of sodium molybdate. Molybdenum trioxide, like chromium trioxide, is an acidic oxide, and forms salts known as molybdates. The normal molybdates show a tendency to pass into polymolybdates. The molybdates are also capable of combining with other oxides (such as phosphorus and arsenic pentoxides) yielding very complex salts. The ordinary ammonium molybdate, used as a test reagent for phosphates, is a salt of composition (NH4)10M012041; it has been examined physicochemically by J. Sand and F. Eisenlohr (Abst. J.C.S., 1907, ii. pp. 178, 179). The molybdates may be recognized by the fact that they give a white precipitate on the addition of hydrochloric or nitric acids to their solutions, and that with reducing agents (zinc and sulphuric acid) they give generally a blue coloration which turns to a green and finally to a brown colour.

Molybdenum combines with the halogen elements in varying proportions, forming with chlorine a di-, tri-, tetraand penta-chloride, and similar compounds with bromine and iodine. Molybdenum dichloride (MoC1 2) 3 or Cl 4 Mo 3 C1 2 (chlormolybdenum chloride), is prepared (together with some tetrachloride) by heating the trichloride in a stream of carbon dioxide (C. W. Blomstrand, Jour. f. prak.Chem.,1857, 71, P. 449; 1861, 82, P. 433). It is a yellow amorphous powder which is soluble in dilute alkalis, the solution on acidification giving an hydroxide, C1 4 Mo 3 (OH) 2, which is soluble in nitric acid, and does not give a reaction with silver nitrate. The molecular weight determinations of W. Muthmann and W. Nagel (Ber., 1898, 31, p. 2009) show the salt to possess the composition Mo 3 C1 6. Molybdenum trichloride, MoC1 31 is obtained when the pentachloride is heated to a temperature of about 250° C. in a current of hydrogen. It forms red crusts, is insoluble in cold water, but is decomposed by boiling water. It is easily soluble in hot nitric acid. Molybdenum pentachloride, MoC1 5r is obtained when molybdenum is gently heated in dry chlorine (L. P. Liechti and B. Kempe, Ann., 1873, 16 9, p. 345). It is a dark-coloured crystalline solid which melts at 194° C. and boils at 268° C. It fumes in moist air and deliquesces gradually. It is occasionally used as a chlorine carrier. It is soluble in absolute alcohol and in ether. Molybdenum disulphide, MoS 2, is found as the mineral molybdenite, and may be prepared by heating the trioxide with sulphur or sulphuretted hydrogen. It is a black crystalline powder, resembling graphite in appearance. It is readily oxidized by nitric acid, and when strongly heated_ in a current of hydrogen is reduced to the metallic condition. Molybdenum trisulphide, MoS3, is obtained by saturating a solution of an alkaline molybdate with sulphuretted hydrogen and adding a mineral acid. It is a brown powder which on heating in air loses sulphur and leaves a residue of the disulphide. A tetrasulphide, MoS 4, has also been described.

Many varying values have been given for the atomic weight of molybdenum. J. J. Berzelius (Pogg. Ann., 1826, 8, p. 23), by converting lead molybdate into lead nitrate, obtained the value 95. 2; while J. B. A. Dumas (Ann., 1860, 113, p. 32), by converting the trioxide into the metal, obtained the value 95.65. K. Seubert and W. Pollard (Zeit. anorg. Chem., 18 95, 8, p. 434) using this second method obtained the value 96.28; whilst E. F. Smith and P. Maas (Zeit. anorg. Chem., 18 94, 5, p. 280), by heating pure sodium molybdate in hydrochloric acid and estimating the amount of sodium chloride formed, obtained the value 96.087.

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Simple English

[[File:|thumb|crystaline molybdenum and a 1cm3 cube]] Molybdenum is a chemical element. It has the chemical symbol Mo. It has the atomic number 42. The name Molybdenum is from the Greek meaning "leadlike". The color of pure molybdenum is silvery-white. It does not occur naturally, and is made from molybdenite.[1]


It is used in alloys with other metals like stainless steel. It helps to make metal stronger, especially in high temperatures, and makes it less likely to rust.[2] This makes it good for use in high speed tools, such as drills and saw blades.[2] It is used in aircraft and missile parts, as well as in nuclear reactors.[1] It is also not toxic, so it is used in making metal bowls for use in making food, medicines and other chemicals.[2]


Molybdenum was used for many years before it was identified in 1778 by Swedish scientist, Carl Wilhelm Scheele. In 1782, Peter Jacob Hjelm was able to separate it into a dark powder he called "molybdenum".[3] It was first mined in 1916 at Climax, near Leadville, in Colorado.[4]



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