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Rhenium

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Rhenium,  75Re
Rhenium single crystal bar and 1cm3 cube.jpg
Rhenium
Pronunciation/ˈriːniəm/ ​(REE-nee-əm)
Appearancesilvery-grayish
Standard atomic weight Ar, std(Re)186.207(1)[1]
Rhenium 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
Tc
↑
Re
↓
Bh
tungsten ← rhenium → osmium
Atomic number (Z)75
Groupgroup 7
Periodperiod 6
Blockd-block
Element category  Transition metal
Electron configuration[Xe] 4f14 5d5 6s2
Electrons per shell
2, 8, 18, 32, 13, 2
Physical properties
Phase at STPsolid
Melting point3459 K ​(3186 °C, ​5767 °F)
Boiling point5903 K ​(5630 °C, ​10,170 °F)
Density (near r.t.)21.02 g/cm3
when liquid (at m.p.)18.9 g/cm3
Heat of fusion60.43 kJ/mol
Heat of vaporization704 kJ/mol
Molar heat capacity25.48 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 3303 3614 4009 4500 5127 5954
Atomic properties
Oxidation states−3, −1, 0, +1, +2, +3, +4, +5, +6, +7 (a mildly acidic oxide)
ElectronegativityPauling scale: 1.9
Ionization energies
  • 1st: 760 kJ/mol
  • 2nd: 1260 kJ/mol
  • 3rd: 2510 kJ/mol
  • (more)
Atomic radiusempirical: 137 pm
Covalent radius151±7 pm
Color lines in a spectral range
Spectral lines of rhenium
Other properties
Natural occurrenceprimordial
Crystal structure ​hexagonal close-packed (hcp)
Hexagonal close packed crystal structure for rhenium
Speed of sound thin rod4700 m/s (at 20 °C)
Thermal expansion6.2 µm/(m·K)
Thermal conductivity48.0 W/(m·K)
Electrical resistivity193 nΩ·m (at 20 °C)
Magnetic orderingparamagnetic[2]
Magnetic susceptibility+67.6·10−6 cm3/mol (293 K)[3]
Young's modulus463 GPa
Shear modulus178 GPa
Bulk modulus370 GPa
Poisson ratio0.30
Mohs hardness7.0
Vickers hardness1350–7850 MPa
Brinell hardness1320–2500 MPa
CAS Number7440-15-5
History
Namingafter the river Rhine (German: Rhein)
DiscoveryMasataka Ogawa (1908)
First isolationMasataka Ogawa (1919)
Named byWalter Noddack, Ida Noddack, Otto Berg (1925)
Main isotopes of rhenium
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
185Re 37.4% stable
187Re 62.6% 4.12×1010 y β− 187Os
| references

Rhenium is a chemical element with the symbol Re and atomic number 75. It is a silvery-gray, heavy, third-row transition metal in group 7 of the periodic table. With an estimated average concentration of 1 part per billion (ppb), rhenium is one of the rarest elements in the Earth's crust. Rhenium has the third-highest melting point and highest boiling point of any stable element at 5903 K. Rhenium resembles manganese and technetium chemically and is mainly obtained as a by-product of the extraction and refinement of molybdenum and copper ores. Rhenium shows in its compounds a wide variety of oxidation states ranging from −1 to +7.

Discovered in 1908, rhenium was the second-last stable element to be discovered, it was named after the river Rhine in Europe.

Nickel-based superalloys of rhenium are used in the combustion chambers, turbine blades, and exhaust nozzles of jet engines; these alloys contain up to 6% rhenium, making jet engine construction the largest single use for the element. The second-most important use is as a catalyst: rhenium is an excellent catalyst for hydrogenation and isomerization, and is used for example in catalytic reforming of naphtha for use in gasoline (rheniforming process); because of the low availability relative to demand, rhenium is expensive, with price reaching an all-time high in 2008/2009 US$10,600 per kilogram (US$4,800 per pound). Due to increases in rhenium recycling and a drop in demand for rhenium in catalysts, the price of rhenium has dropped to US$2,844 per kilogram (US$1,290 per pound) as of July 2018.[4]

History[edit]

"Nipponium" redirects here. For element 113, see nihonium.

Rhenium (Latin: Rhenus meaning: "Rhine")[5] was the second last-discovered of the elements that have a stable isotope (other new elements discovered in nature since then, such as francium, are radioactive);[6] the existence of a yet-undiscovered element at this position in the periodic table had been first predicted by Dmitri Mendeleev. Other calculated information was obtained by Henry Moseley in 1914.[7] In 1908, Japanese chemist Masataka Ogawa announced that he had discovered the 43rd element and named it nipponium (Np) after Japan (Nippon in Japanese). However, recent analysis indicated the presence of rhenium (element 75), not element 43,[8] although this reinterpretation has been questioned by Eric Scerri;[9] the symbol Np was later used for the element neptunium, and the name "nihonium", also named after Japan, along with symbol Nh, was later used for element 113. Element 113 was also discovered by a team of Japanese scientists and was named in respectful homage to Ogawa's work.[10]

Rhenium is generally considered to have been discovered by Walter Noddack, Ida Noddack, and Otto Berg in Germany. In 1925 they reported that they had detected the element in platinum ore and in the mineral columbite, they also found rhenium in gadolinite and molybdenite.[11] In 1928 they were able to extract 1 g of the element by processing 660 kg of molybdenite,[12] it was estimated in 1968 that 75% of the rhenium metal in the United States was used for research and the development of refractory metal alloys. It took several years from that point before the superalloys became widely used.[13][14]

Characteristics[edit]

Rhenium is a silvery-white metal with one of the highest melting points of all elements, exceeded by only tungsten and carbon, it also has one of the highest boiling points of all elements. It is also one of the densest, exceeded only by platinum, iridium and osmium. Rhenium has a hexagonal close-packed crystal structure, with lattice parameters a = 276.1 pm and c = 445.6 pm.[15]

Its usual commercial form is a powder, but this element can be consolidated by pressing and sintering in a vacuum or hydrogen atmosphere; this procedure yields a compact solid having a density above 90% of the density of the metal. When annealed this metal is very ductile and can be bent, coiled, or rolled.[16] Rhenium-molybdenum alloys are superconductive at 10 K; tungsten-rhenium alloys are also superconductive[17] around 4–8 K, depending on the alloy. Rhenium metal superconducts at 1.697±0.006 K.[18][19]

In bulk form and at room temperature and atmospheric pressure, the element resists alkalis, sulfuric acid, hydrochloric acid, dilute (but not concentrated) nitric acid, and aqua regia.

Isotopes[edit]

Main article: Isotopes of rhenium

Rhenium has one stable isotope, rhenium-185, which nevertheless occurs in minority abundance, a situation found only in two other elements (indium and tellurium). Naturally occurring rhenium is only 37.4% 185Re, and 62.6% 187Re, which is unstable but has a very long half-life (≈1010 years); this lifetime can be greatly affected by the charge state of rhenium atom.[20][21] The beta decay of 187Re is used for rhenium-osmium dating of ores; the available energy for this beta decay (2.6 keV) is one of the lowest known among all radionuclides. The isotope rhenium-186m is notable as being one of the longest lived metastable isotopes with a half-life of around 200,000 years. There are twenty-five other recognized radioactive isotopes of rhenium.[22]

Compounds[edit]

See also: Category:Rhenium compounds.

Rhenium compounds are known for all the oxidation states between −3 and +7 except −2; the oxidation states +7, +6, +4, and +2 are the most common.[23] Rhenium is most available commercially as salts of perrhenate, including sodium and ammonium perrhenates; these are white, water-soluble compounds.[24]

Halides and oxyhalides[edit]

The most common rhenium chlorides are ReCl6, ReCl5, ReCl4, and ReCl3.[25] The structures of these compounds often feature extensive Re-Re bonding, which is characteristic of this metal in oxidation states lower than VII. Salts of [Re2Cl8]2− feature a quadruple metal-metal bond. Although the highest rhenium chloride features Re(VI), fluorine gives the d0 Re(VII) derivative rhenium heptafluoride. Bromides and iodides of rhenium are also well known.

Like tungsten and molybdenum, with which it shares chemical similarities, rhenium forms a variety of oxyhalides; the oxychlorides are most common, and include ReOCl4, ReOCl3.

Oxides and sulfides[edit]

Perrhenic acid (H4Re2O9) adopts an unconventional structure.

The most common oxide is the volatile colourless Re2O7. Rhenium trioxide ReO3 adopts a perovskite-like structure. Other oxides include Re2O5, ReO2, and Re2O3.[25] The sulfides are ReS2 and Re2S7. Perrhenate salts can be converted to tetrathioperrhenate by the action of ammonium hydrosulfide.[26]

Other compounds[edit]

Rhenium diboride (ReB2) is a hard compound having the hardness similar to that of tungsten carbide, silicon carbide, titanium diboride or zirconium diboride.[27]

Organorhenium compounds[edit]

Main article: Organorhenium chemistry

Dirhenium decacarbonyl is the most common entry to organorhenium chemistry, its reduction with sodium amalgam gives Na[Re(CO)5] with rhenium in the formal oxidation state −1.[28] Dirhenium decacarbonyl can be oxidised with bromine to bromopentacarbonylrhenium(I):[29]

Re2(CO)10 + Br2 → 2 Re(CO)5Br

Reduction of this pentacarbonyl with zinc and acetic acid gives pentacarbonylhydridorhenium:[30]

Re(CO)5Br + Zn + HOAc → Re(CO)5H + ZnBr(OAc)

Methylrhenium trioxide ("MTO"), CH3ReO3 is a volatile, colourless solid has been used as a catalyst in some laboratory experiments. It can be prepared by many routes, a typical method is the reaction of Re2O7 and tetramethyltin:

Re2O7 + (CH3)4Sn → CH3ReO3 + (CH3)3SnOReO3

Analogous alkyl and aryl derivatives are known. MTO catalyses for the oxidations with hydrogen peroxide. Terminal alkynes yield the corresponding acid or ester, internal alkynes yield diketones, and alkenes give epoxides. MTO also catalyses the conversion of aldehydes and diazoalkanes into an alkene.[31]

Nonahydridorhenate[edit]

Structure of ReH2−
9.

A distinctive derivative of rhenium is nonahydridorhenate, originally thought to be the rhenide anion, Re−, but actually containing the ReH2−
9 anion in which the oxidation state of rhenium is +7.

Occurrence[edit]

Molybdenite

Rhenium is one of the rarest elements in Earth's crust with an average concentration of 1 ppb;[25] other sources quote the number of 0.5 ppb making it the 77th most abundant element in Earth's crust.[32] Rhenium is probably not found free in nature (its possible natural occurrence is uncertain), but occurs in amounts up to 0.2%[25] in the mineral molybdenite (which is primarily molybdenum disulfide), the major commercial source, although single molybdenite samples with up to 1.88% have been found.[33] Chile has the world's largest rhenium reserves, part of the copper ore deposits, and was the leading producer as of 2005,[34] it was only recently that the first rhenium mineral was found and described (in 1994), a rhenium sulfide mineral (ReS2) condensing from a fumarole on Kudriavy volcano, Iturup island, in the Kuril Islands.[35] Kudriavy discharges up to 20–60 kg rhenium per year mostly in the form of rhenium disulfide.[36][37] Named rheniite, this rare mineral commands high prices among collectors.[38]

Production[edit]

Ammonium perrhenate

Commercial rhenium is extracted from molybdenum roaster-flue gas obtained from copper-sulfide ores; some molybdenum ores contain 0.001% to 0.2% rhenium.[25][33] Rhenium(VII) oxide and perrhenic acid readily dissolve in water; they are leached from flue dusts and gasses and extracted by precipitating with potassium or ammonium chloride as the perrhenate salts, and purified by recrystallization.[25] Total world production is between 40 and 50 tons/year; the main producers are in Chile, the United States, Peru, and Poland.[39] Recycling of used Pt-Re catalyst and special alloys allow the recovery of another 10 tons per year. Prices for the metal rose rapidly in early 2008, from $1000–$2000 per kg in 2003–2006 to over $10,000 in February 2008;[40][41] the metal form is prepared by reducing ammonium perrhenate with hydrogen at high temperatures:[24]

2 NH4ReO4 + 7 H2 → 2 Re + 8 H2O + 2 NH3

Applications[edit]

The Pratt & Whitney F-100 engine uses rhenium-containing second-generation superalloys

Rhenium is added to high-temperature superalloys that are used to make jet engine parts, using 70% of the worldwide rhenium production.[42] Another major application is in platinum–rhenium catalysts, which are primarily used in making lead-free, high-octane gasoline.[43]

Alloys[edit]

The nickel-based superalloys have improved creep strength with the addition of rhenium; the alloys normally contain 3% or 6% of rhenium.[44] Second-generation alloys contain 3%; these alloys were used in the engines for the F-15 and F-16, whereas the newer single-crystal third-generation alloys contain 6% of rhenium; they are used in the F-22 and F-35 engines.[43][45] Rhenium is also used in the superalloys, such as CMSX-4 (2nd gen) and CMSX-10 (3rd gen) that are used in industrial gas turbine engines like the GE 7FA. Rhenium can cause superalloys to become microstructurally unstable, forming undesirable TCP (topologically close packed) phases. In 4th- and 5th-generation superalloys, ruthenium is used to avoid this effect. Among others the new superalloys are EPM-102 (with 3% Ru) and TMS-162 (with 6% Ru),[46] as well as TMS-138[47] and TMS-174.[48][49]

CFM International CFM56 jet engine still with blades made with 3% rhenium

For 2006, the consumption is given as 28% for General Electric, 28% Rolls-Royce plc and 12% Pratt & Whitney, all for superalloys, whereas the use for catalysts only accounts for 14% and the remaining applications use 18%.[42] In 2006, 77% of the rhenium consumption in the United States was in alloys;[43] the rising demand for military jet engines and the constant supply made it necessary to develop superalloys with a lower rhenium content. For example, the newer CFM International CFM56 high-pressure turbine (HPT) blades will use Rene N515 with a rhenium content of 1.5% instead of Rene N5 with 3%.[50][51]

Rhenium improves the properties of tungsten. Tungsten-rhenium alloys are more ductile at low temperature, allowing them to be more easily machined; the high-temperature stability is also improved. The effect increases with the rhenium concentration, and therefore tungsten alloys are produced with up to 27% of Re, which is the solubility limit.[52] Tungsten-rhenium wire was originally created in efforts to develop a wire that was more ductile after recrystallization; this allows the wire to meet specific performance objectives, including superior vibration resistance, improved ductility, and higher resistivity.[53] One application for the tungsten-rhenium alloys is X-ray sources; the high melting point of both elements, together with their high atomic mass, makes them stable against the prolonged electron impact.[54] Rhenium tungsten alloys are also applied as thermocouples to measure temperatures up to 2200 °C.[55]

The high temperature stability, low vapor pressure, good wear resistance and ability to withstand arc corrosion of rhenium are useful in self-cleaning electrical contacts. In particular, the discharge occurring during the switching oxidizes the contacts. However, rhenium oxide Re2O7 has poor stability (sublimes at ~360 °C) and therefore is removed during the discharge.[42]

Rhenium has a high melting point and a low vapor pressure similar to tantalum and tungsten. Therefore, rhenium filaments exhibit a higher stability if the filament is operated not in vacuum, but in oxygen-containing atmosphere;[56] those filaments are widely used in mass spectrometers, in ion gauges[57] and in photoflash lamps in photography.[58]

Catalysts[edit]

Rhenium in the form of rhenium-platinum alloy is used as catalyst for catalytic reforming, which is a chemical process to convert petroleum refinery naphthas with low octane ratings into high-octane liquid products. Worldwide, 30% of catalysts used for this process contain rhenium;[59] the olefin metathesis is the other reaction for which rhenium is used as catalyst. Normally Re2O7 on alumina is used for this process.[60] Rhenium catalysts are very resistant to chemical poisoning from nitrogen, sulfur and phosphorus, and so are used in certain kinds of hydrogenation reactions.[16][61][62]

Other uses[edit]

The isotopes 188Re and 186Re are radioactive and are used for treatment of liver cancer, they both have similar penetration depth in tissue (5 mm for 186Re and 11 mm for 188Re), but 186Re has advantage of longer lifetime (90 hours vs. 17 hours).[63][64]

188Re is also being used experimentally in a novel treatment of pancreatic cancer where it is delivered by means of the bacterium Listeria monocytogenes.[65]

Related by periodic trends, rhenium has a similar chemistry to that of technetium; work done to label rhenium onto target compounds can often be translated to technetium; this is useful for radiopharmacy, where it is difficult to work with technetium – especially the 99m isotope used in medicine – due to its expense and short half-life.[63][66]

Precautions[edit]

Very little is known about the toxicity of rhenium and its compounds because they are used in very small amounts. Soluble salts, such as the rhenium halides or perrhenates, could be hazardous due to elements other than rhenium or due to rhenium itself.[67] Only a few compounds of rhenium have been tested for their acute toxicity; two examples are potassium perrhenate and rhenium trichloride, which were injected as a solution into rats; the perrhenate had an LD50 value of 2800 mg/kg after seven days (this is very low toxicity, similar to that of table salt) and the rhenium trichloride showed LD50 of 280 mg/kg.[68]

References[edit]

  1. ^ Meija, Juris; et al. (2016). "Atomic weights of the elements 2013 (IUPAC Technical Report)". Pure and Applied Chemistry. 88 (3): 265–91. doi:10.1515/pac-2015-0305.
  2. ^ Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
  3. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  4. ^ https://apps.catalysts.basf.com/apps/eibprices/mp/YearlyCharts.aspx
  5. ^ Tilgner, Hans Georg (2000). Forschen Suche und Sucht (in German). Books on Demand. ISBN 978-3-89811-272-7.
  6. ^ "Rhenium: Statistics and Information". Minerals Information. United States Geological Survey. 2011. Retrieved 2011-05-25.
  7. ^ Moseley, Henry (1914). "The High-Frequency Spectra of the Elements, Part II". Philosophical Magazine. 27 (160): 703–713. doi:10.1080/14786440408635141. Archived from the original on 2010-01-22. Retrieved 2009-05-14.
  8. ^ Yoshihara, H. K. (2004). "Discovery of a new element 'nipponiumʼ: re-evaluation of pioneering works of Masataka Ogawa and his son Eijiro Ogawa". Spectrochimica Acta Part B Atomic Spectroscopy. 59 (8): 1305–1310. Bibcode:2004AcSpe..59.1305Y. doi:10.1016/j.sab.2003.12.027.
  9. ^ Eric Scerri, A tale of seven elements, (Oxford University Press 2013) ISBN 978-0-19-539131-2, p.109–114
  10. ^ Öhrström, Lars; Reedijk, Jan (28 November 2016). "Names and symbols of the elements with atomic numbers 113, 115, 117 and 118 (IUPAC Recommendations 2016)" (PDF). Pure Appl. Chem. 88 (12): 1225–1229. doi:10.1515/pac-2016-0501. Retrieved 22 April 2017.
  11. ^ Noddack, W.; Tacke, I.; Berg, O. (1925). "Die Ekamangane". Naturwissenschaften. 13 (26): 567–574. Bibcode:1925NW.....13..567.. doi:10.1007/BF01558746.
  12. ^ Noddack, W.; Noddack, I. (1929). "Die Herstellung von einem Gram Rhenium". Zeitschrift für Anorganische und Allgemeine Chemie (in German). 183 (1): 353–375. doi:10.1002/zaac.19291830126.
  13. ^ Committee On Technical Aspects Of Critical And Strategic Material, National Research Council (U.S.) (1968). Trends in usage of rhenium: Report. pp. 4–5.
  14. ^ Savitskiĭ, Evgeniĭ Mikhaĭlovich; Tulkina, Mariia Aronovna; Povarova, Kira Borisovna (1970). Rhenium alloys.
  15. ^ Liu, L. G.; Takahashi, T.; Bassett, W. A. (1970). "Effect of pressure and temperature on lattice parameters of rhenium". Journal of Physics and Chemistry of Solids. 31 (6): 1345–1351. Bibcode:1970JPCS...31.1345L. doi:10.1016/0022-3697(70)90138-1.
  16. ^ a b Hammond, C. R. (2004). "The Elements". Handbook of Chemistry and Physics (81st ed.). CRC press. ISBN 978-0-8493-0485-9.
  17. ^ Neshpor, V. S.; Novikov, V. I.; Noskin, V. A.; Shalyt, S. S. (1968). "Superconductivity of Some Alloys of the Tungsten-rhenium-carbon System". Soviet Physics JETP. 27: 13. Bibcode:1968JETP...27...13N.
  18. ^ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 12.60. ISBN 978-1439855119.
  19. ^ Daunt, J. G.; Lerner, E. "The Properties of Superconducting Mo-Re Alloys". Defense Technical Information Center. Archived from the original on 2017-02-06.
  20. ^ Johnson, Bill (1993). "How to Change Nuclear Decay Rates". math.ucr.edu. Retrieved 2009-02-21.
  21. ^ Bosch, F.; Faestermann, T.; Friese, J.; et al. (1996). "Observation of bound-state β− decay of fully ionized 187Re: 187Re-187Os Cosmochronometry". Physical Review Letters. 77 (26): 5190–5193. Bibcode:1996PhRvL..77.5190B. doi:10.1103/PhysRevLett.77.5190. PMID 10062738.
  22. ^ Audi, Georges; Bersillon, Olivier; Blachot, Jean; Wapstra, Aaldert Hendrik (2003), "The NUBASE evaluation of nuclear and decay properties", Nuclear Physics A, 729: 3–128, Bibcode:2003NuPhA.729....3A, doi:10.1016/j.nuclphysa.2003.11.001
  23. ^ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985). "Rhenium". Lehrbuch der Anorganischen Chemie (in German) (91–100 ed.). Walter de Gruyter. pp. 1118–1123. ISBN 978-3-11-007511-3.
  24. ^ a b Glemser, O. (1963) "Ammonium Perrhenate" in Handbook of Preparative Inorganic Chemistry, 2nd ed., G. Brauer (ed.), Academic Press, NY., Vol. 1, pp. 1476–85.
  25. ^ a b c d e f Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  26. ^ Goodman, J. T.; Rauchfuss, T. B. (2002). Tetraethylammonium-tetrathioperrhenate [Et4N] [ReS4]. Inorganic Syntheses. 33. pp. 107–110. doi:10.1002/0471224502.ch2. ISBN 9780471208259.
  27. ^ Qin, Jiaqian; He, Duanwei; Wang, Jianghua; Fang, Leiming; Lei, Li; Li, Yongjun; Hu, Juan; Kou, Zili; Bi, Yan (2008). "Is Rhenium Diboride a Superhard Material?". Advanced Materials. 20 (24): 4780–4783. doi:10.1002/adma.200801471.
  28. ^ Breimair, Josef; Steimann, Manfred; Wagner, Barbara; Beck, Wolfgang (1990). "Nucleophile Addition von Carbonylmetallaten an kationische Alkin-Komplexe [CpL2M(η2-RC≡CR)]+ (M = Ru, Fe): μ-η1:η1-Alkin-verbrückte Komplexe". Chemische Berichte. 123: 7. doi:10.1002/cber.19901230103.
  29. ^ Schmidt, Steven P.; Trogler, William C.; Basolo, Fred (1990). Pentacarbonylrhenium Halides. Inorganic Syntheses. 28. pp. 154–159. doi:10.1002/9780470132593.ch42. ISBN 978-0-470-13259-3.
  30. ^ Michael A. Urbancic; John R. Shapley (1990). Pentacarbonylhydridorhenium. Inorganic Syntheses. 28. pp. 165–168. doi:10.1002/9780470132593.ch43. ISBN 978-0-470-13259-3.
  31. ^ Hudson, A. (2002) “Methyltrioxorhenium” in Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons: New York, ISBN 9780470842898, doi:10.1002/047084289X.
  32. ^ Emsley, John (2001). "Rhenium". Nature's Building Blocks: An A-Z Guide to the Elements. Oxford, England, UK: Oxford University Press. pp. 358–360. ISBN 978-0-19-850340-8.
  33. ^ a b Rouschias, George (1974). "Recent advances in the chemistry of rhenium". Chemical Reviews. 74 (5): 531. doi:10.1021/cr60291a002.
  34. ^ Anderson, Steve T. "2005 Minerals Yearbook: Chile" (PDF). United States Geological Survey. Retrieved 2008-10-26.
  35. ^ Korzhinsky, M. A.; Tkachenko, S. I.; Shmulovich, K. I.; Taran Y. A.; Steinberg, G. S. (2004-05-05). "Discovery of a pure rhenium mineral at Kudriavy volcano". Nature. 369 (6475): 51–52. Bibcode:1994Natur.369...51K. doi:10.1038/369051a0.
  36. ^ Kremenetsky, A. A.; Chaplygin, I. V. (2010). "Concentration of rhenium and other rare metals in gases of the Kudryavy Volcano (Iturup Island, Kurile Islands)". Doklady Earth Sciences. 430 (1): 114. Bibcode:2010DokES.430..114K. doi:10.1134/S1028334X10010253.
  37. ^ Tessalina, S.; Yudovskaya, M.; Chaplygin, I.; Birck, J.; Capmas, F. (2008). "Sources of unique rhenium enrichment in fumaroles and sulphides at Kudryavy volcano". Geochimica et Cosmochimica Acta. 72 (3): 889. Bibcode:2008GeCoA..72..889T. doi:10.1016/j.gca.2007.11.015.
  38. ^ "The Mineral Rheniite". Amethyst Galleries.
  39. ^ Magyar, Michael J. (January 2012). "Rhenium" (PDF). Mineral Commodity Summaries. U.S. Geological Survey. Retrieved 2013-09-04.
  40. ^ "MinorMetal prices". minormetals.com. Retrieved 2008-02-17.
  41. ^ Harvey, Jan (2008-07-10). "Analysis: Super hot metal rhenium may reach "platinum prices"". Reuters India. Retrieved 2008-10-26.
  42. ^ a b c Naumov, A. V. (2007). "Rhythms of rhenium". Russian Journal of Non-Ferrous Metals. 48 (6): 418–423. doi:10.3103/S1067821207060089.
  43. ^ a b c Magyar, Michael J. (April 2011). "2009 Mineral Yearbook: Rhenium" (PDF). United States Geological Survey.
  44. ^ Bhadeshia, H. K. D. H. "Nickel Based Superalloys". University of Cambridge. Archived from the original on 2006-08-25. Retrieved 2008-10-17.
  45. ^ Cantor, B.; Grant, Patrick Assender Hazel (2001). Aerospace Materials: An Oxford-Kobe Materials Text. CRC Press. pp. 82–83. ISBN 978-0-7503-0742-0.
  46. ^ Bondarenko, Yu. A.; Kablov, E. N.; Surova, V. A.; Echin, A. B. (2006). "Effect of high-gradient directed crystallization on the structure and properties of rhenium-bearing single-crystal alloy". Metal Science and Heat Treatment. 48 (7–8): 360. Bibcode:2006MSHT...48..360B. doi:10.1007/s11041-006-0099-6.
  47. ^ "Fourth generation nickel base single crystal superalloy" (PDF).
  48. ^ Koizumi, Yutaka; et al. "Development of a Next-Generation Ni-base Single Crystal Superalloy" (PDF). Proceedings of the International Gas Turbine Congress, Tokyo November 2–7, 2003.
  49. ^ Walston, S.; Cetel, A.; MacKay, R.; O'Hara, K.; Duhl, D.; Dreshfield, R. "Joint Development of a Fourth Generation Single Crystal Superalloy" (PDF). Archived from the original (PDF) on 2006-10-15.
  50. ^ Fink, Paul J.; Miller, Joshua L.; Konitzer, Douglas G. (2010). "Rhenium reduction—alloy design using an economically strategic element". JOM. 62 (1): 55. Bibcode:2010JOM....62a..55F. doi:10.1007/s11837-010-0012-z.
  51. ^ Konitzer, Douglas G. (September 2010). "Design in an Era of Constrained Resources". Archived from the original on 2011-07-25. Retrieved 2010-10-12.
  52. ^ Lassner, Erik; Schubert, Wolf-Dieter (1999). Tungsten: properties, chemistry, technology of the element, alloys, and chemical compounds. Springer. p. 256. ISBN 978-0-306-45053-2.
  53. ^ "Tungsten-Rhenium - Union City Filament". Union City Filament. Retrieved 2017-04-05.
  54. ^ Cherry, Pam; Duxbury, Angela (1998). Practical radiotherapy physics and equipment. Cambridge University Press. p. 55. ISBN 978-1-900151-06-1.
  55. ^ Asamoto, R.; Novak, P. E. (1968). "Tungsten-Rhenium Thermocouples for Use at High Temperatures". Review of Scientific Instruments. 39 (8): 1233. Bibcode:1968RScI...39.1233A. doi:10.1063/1.1683642.
  56. ^ Blackburn, Paul E. (1966). "The Vapor Pressure of Rhenium". The Journal of Physical Chemistry. 70: 311–312. doi:10.1021/j100873a513.
  57. ^ Earle, G. D.; Medikonduri, R.; Rajagopal, N.; Narayanan, V.; Roddy, P. A. (2005). "Tungsten-Rhenium Filament Lifetime Variability in Low Pressure Oxygen Environments". IEEE Transactions on Plasma Science. 33 (5): 1736–1737. Bibcode:2005ITPS...33.1736E. doi:10.1109/TPS.2005.856413.
  58. ^ Ede, Andrew (2006). The chemical element: a historical perspective. Greenwood Publishing Group. ISBN 978-0-313-33304-0.
  59. ^ Ryashentseva, Margarita A. (1998). "Rhenium-containing catalysts in reactions of organic compounds". Russian Chemical Reviews. 67 (2): 157–177. Bibcode:1998RuCRv..67..157R. doi:10.1070/RC1998v067n02ABEH000390.
  60. ^ Mol, Johannes C. (1999). "Olefin metathesis over supported rhenium oxide catalysts". Catalysis Today. 51 (2): 289–299. doi:10.1016/S0920-5861(99)00051-6.
  61. ^ Angelidis, T. N.; Rosopoulou, D. Tzitzios V. (1999). "Selective Rhenium Recovery from Spent Reforming Catalysts". Ind. Eng. Chem. Res. 38 (5): 1830–1836. doi:10.1021/ie9806242.
  62. ^ Burch, Robert (1978). "The Oxidation State of Rhenium and Its Role in Platinum-Rhenium" (PDF). Platinum Metals Review. 22 (2): 57–60.
  63. ^ a b Dilworth, Jonathan R.; Parrott, Suzanne J. (1998). "The biomedical chemistry of technetium and rhenium". Chemical Society Reviews. 27: 43–55. doi:10.1039/a827043z.
  64. ^ "The Tungsten-188 and Rhenium-188 Generator Information". Oak Ridge National Laboratory. 2005. Archived from the original on 2008-01-09. Retrieved 2008-02-03.
  65. ^ Baker, Monya (22 April 2013). "Radioactive bacteria attack cancer". Nature.
  66. ^ Colton, R.; Peacock R. D. (1962). "An outline of technetium chemistry". Quarterly Reviews, Chemical Society. 16 (4): 299–315. doi:10.1039/QR9621600299.
  67. ^ Emsley, J. (2003). "Rhenium". Nature's Building Blocks: An A-Z Guide to the Elements. Oxford, England, UK: Oxford University Press. pp. 358–361. ISBN 978-0-19-850340-8.
  68. ^ Haley, Thomas J.; Cartwright, Frank D. (1968). "Pharmacology and toxicology of potassium perrhenate and rhenium trichloride". Journal of Pharmaceutical Sciences. 57 (2): 321–323. doi:10.1002/jps.2600570218. PMID 5641681.

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