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Lutetium

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Lutetium,  71Lu
Lutetium sublimed dendritic and 1cm3 cube.jpg
General properties
Pronunciation /ljuːˈtiːʃiəm/ ​(lew-TEE-shee-əm)
Appearance silvery white
Standard atomic weight (Ar, standard) 174.9668(1)[1]
Lutetium 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
–
↑
Lu
↓
Lr
ytterbium ← lutetium → hafnium
Atomic number (Z) 71
Group group n/a
Period period 6
Element category   lanthanide, sometimes considered a transition metal
Block f-block
Electron configuration [Xe] 4f14 5d1 6s2
Electrons per shell
 2, 8, 18, 32, 9, 2
Physical properties
Phase at STP solid
Melting point 1925 K ​(1652 °C, ​3006 °F)
Boiling point 3675 K ​(3402 °C, ​6156 °F)
Density (near r.t.) 9.841 g/cm3
when liquid (at m.p.) 9.3 g/cm3
Heat of fusion ca. 22 kJ/mol
Heat of vaporization 414 kJ/mol
Molar heat capacity 26.86 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1906 2103 2346 (2653) (3072) (3663)
Atomic properties
Oxidation states 3, 2, 1 ​(a weakly basic oxide)
Electronegativity Pauling scale: 1.27
Ionization energies
  • 1st: 523.5 kJ/mol
  • 2nd: 1340 kJ/mol
  • 3rd: 2022.3 kJ/mol
Atomic radius empirical: 174 pm
Covalent radius 187±8 pm
Color lines in a spectral range
Other properties
Crystal structure ​hexagonal close-packed (hcp)
Hexagonal close packed crystal structure for lutetium
Thermal expansion poly: 9.9 µm/(m·K) (at r.t.)
Thermal conductivity 16.4 W/(m·K)
Electrical resistivity poly: 582 nΩ·m (at r.t.)
Magnetic ordering paramagnetic[2]
Young's modulus 68.6 GPa
Shear modulus 27.2 GPa
Bulk modulus 47.6 GPa
Poisson ratio 0.261
Vickers hardness 755–1160 MPa
Brinell hardness 890–1300 MPa
CAS Number 7439-94-3
History
Naming after Lutetia, Latin for: Paris, in the Roman era
Discovery Carl Auer von Welsbach and Georges Urbain (1906)
First isolation Carl Auer von Welsbach (1906)
Named by Georges Urbain (1906)
Main isotopes of lutetium
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
173Lu syn 1.37 y ε 173Yb
174Lu syn 3.31 y ε 174Yb
175Lu 97.401% stable
176Lu 2.599% 3.78×1010 y β− 176Hf
| references | in Wikidata

Lutetium is a chemical element with symbol Lu and atomic number 71. It is a silvery white metal, which resists corrosion in dry air, but not in moist air. Lutetium is the last element in the lanthanide series, and it is traditionally counted among the rare earths. Lutetium is sometimes considered the first element of the 6th-period transition metals, although lanthanum is more often considered as such.

Lutetium was independently discovered in 1907 by French scientist Georges Urbain, Austrian mineralogist Baron Carl Auer von Welsbach, and American chemist Charles James. All of these researchers found lutetium as an impurity in the mineral ytterbia, which was previously thought to consist entirely of ytterbium. The dispute on the priority of the discovery occurred shortly after, with Urbain and Welsbach accusing each other of publishing results influenced by the published research of the other; the naming honor went to Urbain, as he had published his results earlier. He chose the name lutecium for the new element, but in 1949 the spelling of element 71 was changed to lutetium. In 1909, the priority was finally granted to Urbain and his names were adopted as official ones; however, the name cassiopeium (or later cassiopium) for element 71 proposed by Welsbach was used by many German scientists until the 1950s.

Lutetium is not a particularly abundant element, although it is significantly more common than silver in the earth's crust. It has few specific uses. Lutetium-176 is a relatively abundant (2.5%) radioactive isotope with a half-life of about 38 billion years, used to determine the age of minerals and meteorites. Lutetium usually occurs in association with the element yttrium[citation needed] and is sometimes used in metal alloys and as a catalyst in various chemical reactions. 177Lu-DOTA-TATE is used for radionuclide therapy (see Nuclear medicine) on neuroendocrine tumours. Lutetium has the highest Brinell hardness of any lanthanide, at 890–1300 MPa.[3]

Characteristics[edit]

Physical properties[edit]

A lutetium atom has 71 electrons, arranged in the configuration [Xe] 4f145d16s2.[4] When entering a chemical reaction, the atom loses its two outermost electrons and the single 5d-electron. The lutetium atom is the smallest among the lanthanide atoms, due to the lanthanide contraction,[5] and as a result lutetium has the highest density, melting point, and hardness of the lanthanides.[6]

Chemical properties and compounds[edit]

See also: Category:Lutetium compounds.

Lutetium's compounds always contain the element in the oxidation state +3. Aqueous solutions of most lutetium salts are colorless and form white crystalline solids upon drying, with the common exception of the iodide. The soluble salts, such as nitrate, sulfate and acetate form hydrates upon crystallization. The oxide, hydroxide, fluoride, carbonate, phosphate and oxalate are insoluble in water.[7]

Lutetium metal is slightly unstable in air at standard conditions, but it burns readily at 150 °C to form lutetium oxide. The resulting compound is known to absorb water and carbon dioxide, and may be used to remove vapors of these compounds from closed atmospheres.[8] Similar observations are made during reaction between lutetium and water (slow when cold and fast when hot); lutetium hydroxide is formed in the reaction.[9] Lutetium metal is known to react with the four lightest halogens to form trihalides; all of them (except the fluoride) are soluble in water.

Lutetium dissolves readily in weak acids[8] and dilute sulfuric acid to form solutions containing the colorless lutetium ions, which are coordinated by between seven and nine water molecules, the average being [Lu(H2O)8.2]3+.[10]

2 Lu + 3 H2SO4 → 2 Lu3+ + 3 SO2–
4 + 3 H2↑

Isotopes[edit]

Main article: Isotopes of lutetium

Lutetium occurs on the Earth in form of two isotopes: lutetium-175 and lutetium-176. Out of these two, only the former is stable, making the element monoisotopic. The latter one, lutetium-176, decays via beta decay with a half-life of 3.78×1010 years; it makes up about 2.5% of natural lutetium.[11] To date, 32 synthetic radioisotopes of the element have been characterized, ranging in mass from 149.973 (lutetium-150) to 183.961 (lutetium-184); the most stable such isotopes are lutetium-174 with a half-life of 3.31 years, and lutetium-173 with a half-life of 1.37 years.[11] All of the remaining radioactive isotopes have half-lives that are less than 9 days, and the majority of these have half-lives that are less than half an hour.[11] Isotopes lighter than the stable lutetium-175 decay via electron capture (to produce isotopes of ytterbium), with some alpha and positron emission; the heavier isotopes decay primarily via beta decay, producing hafnium isotopes.[11]

The element also has 42 nuclear isomers, with masses of 150, 151, 153–162, 166–180 (not every mass number corresponds to only one isomer). The most stable of them are lutetium-177m, with half-life of 160.4 days and lutetium-174m, with half-life of 142 days; this is longer than half-lives of the ground states of all radioactive lutetium isotopes, except only for lutetium-173, 174, and 176.[11]

History[edit]

Lutetium, derived from the Latin Lutetia (Paris), was independently discovered in 1907 by French scientist Georges Urbain, Austrian mineralogist Baron Carl Auer von Welsbach, and American chemist Charles James.[12][13] They found it as an impurity in ytterbia, which was thought by Swiss chemist Jean Charles Galissard de Marignac to consist entirely of ytterbium.[14] The scientists proposed different names for the elements: Urbain chose neoytterbium and lutecium,[15] whereas Welsbach chose aldebaranium and cassiopeium (after Aldebaran and Cassiopeia).[16] Both of these articles accused the other man of publishing results based on those of the author.

The International Commission on Atomic Weights, which was then responsible for the attribution of new element names, settled the dispute in 1909 by granting priority to Urbain and adopting his names as official ones, based on the fact that the separation of lutetium from Marignac's ytterbium was first described by Urbain;[14] after Urbain's names were recognized, neoytterbium was reverted to ytterbium. Until the 1950s, some German-speaking chemists called lutetium by Welsbach's name, cassiopeium; in 1949, the spelling of element 71 was changed to lutetium. The reason for this was that Welsbach's 1907 samples of lutetium had been pure, while Urbain's 1907 samples only contained traces of lutetium.[17] This later misled Urbain into thinking that he had discovered element 72, which he named celtium, which was actually very pure lutetium. The later discrediting of Urbain's work on element 72 led to a reappraisal of Welsbach's work on element 71, so that the element was renamed to cassiopeium in German-speaking countries for some time.[17] Charles James, who stayed out of the priority argument, worked on a much larger scale and possessed the largest supply of lutetium at the time.[18] Pure lutetium metal was first produced in 1953.[18]

Occurrence and production[edit]

Monazite

Found with almost all other rare-earth metals but never by itself, lutetium is very difficult to separate from other elements. Its principal commercial source is as a by-product from the processing of the rare earth phosphate mineral monazite (Ce,La,...)PO4, which has concentrations of only 0.0001% of the element,[8] not much higher than the abundance of lutetium in the Earth crust of about 0.5 mg/kg. No lutetium-dominant minerals are currently known.[19] The main mining areas are China, United States, Brazil, India, Sri Lanka and Australia. The world production of lutetium (in the form of oxide) is about 10 tonnes per year.[18] Pure lutetium metal is very difficult to prepare. It is one of the rarest and most expensive of the rare earth metals with the price about US$10,000 per kilogram, or about one-fourth that of gold.[20][21]

Crushed minerals are treated with hot concentrated sulfuric acid to produce water-soluble sulfates of rare earths. Thorium precipitates out of solution as hydroxide and is removed. After that the solution is treated with ammonium oxalate to convert rare earths into their insoluble oxalates. The oxalates are converted to oxides by annealing. The oxides are dissolved in nitric acid that excludes one of the main components, cerium, whose oxide is insoluble in HNO3. Several rare earth metals, including lutetium, are separated as a double salt with ammonium nitrate by crystallization. Lutetium is separated by ion exchange. In this process, rare-earth ions are sorbed onto suitable ion-exchange resin by exchange with hydrogen, ammonium or cupric ions present in the resin. Lutetium salts are then selectively washed out by suitable complexing agent. Lutetium metal is then obtained by reduction of anhydrous LuCl3 or LuF3 by either an alkali metal or alkaline earth metal.[7]

2 LuCl3 + 3 Ca → 2 Lu + 3 CaCl2

Applications[edit]

Because of production difficulty and high price, lutetium has very few commercial uses, especially since it is rarer than most of the other lanthanides but is chemically not very different. However, stable lutetium can be used as catalysts in petroleum cracking in refineries and can also be used in alkylation, hydrogenation, and polymerization applications.[22]

Lutetium aluminium garnet (Al5Lu3O12) has been proposed for use as a lens material in high refractive index immersion lithography.[23] Additionally, a tiny amount of lutetium is added as a dopant to gadolinium gallium garnet (GGG), which is used in magnetic bubble memory devices.[24] Cerium-doped lutetium oxyorthosilicate (LSO) is currently the preferred compound for detectors in positron emission tomography (PET).[25][26] Lutetium aluminium garnet (LuAG) is used as a phosphor in LED light bulbs.[27][28]

Aside from stable lutetium, its radioactive isotopes have several specific uses. The suitable half-life and decay mode made lutetium-176 used as a pure beta emitter, using lutetium which has been exposed to neutron activation, and in lutetium–hafnium dating to date meteorites.[29] The synthetic isotope lutetium-177 bound to octreotate (a somatostatin analogue), is used experimentally in targeted radionuclide therapy for neuroendocrine tumors.[30] Indeed, lutetium-177 is seeing increasing use as a radionuclide, in neuroendrocine tumor therapy and bone pain palliation.[31][32] Research indicates that lutetium-ion atomic clocks could provide greater accuracy than any existing atomic clock.[33]

Lutetium tantalate (LuTaO4) is the densest known stable white material (density 9.81 g/cm3)[34] and therefore is an ideal host for X-ray phosphors.[35][36] The only denser white material is thorium dioxide, with density of 10 g/cm3, but the thorium it contains is radioactive.

Precautions[edit]

Like other rare-earth metals, lutetium is regarded as having a low degree of toxicity, but its compounds should be handled with care nonetheless: for example, lutetium fluoride inhalation is dangerous and the compound irritates skin.[8] Lutetium nitrate may be dangerous as it may explode and burn once heated. Lutetium oxide powder is toxic as well if inhaled or ingested.[8]

Similarly to the other rare-earth metals, lutetium has no known biological role, but it is found even in humans, concentrating in bones, and to a lesser extent in the liver and kidneys.[18] Lutetium salts are known to occur together with other lanthanide salts in nature; the element is the least abundant in the human body of all lanthanides.[18] Human diets have not been monitored for lutetium content, so it is not known how much the average human takes in, but estimations show the amount is only about several micrograms per year, all coming from tiny amounts taken by plants. Soluble lutetium salts are mildly toxic, but insoluble ones are not.[18]

See also[edit]

References[edit]

  1. ^ Meija, J.; 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. ^ Samsonov, G. V., ed. (1968). "Mechanical Properties of the Elements". Handbook of the physicochemical properties of the elements. New York, USA: IFI-Plenum. doi:10.1007/978-1-4684-6066-7_7. ISBN 978-1-4684-6066-7. Archived from the original on 2015-04-02.
  4. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1223. ISBN 0-08-037941-9.
  5. ^ Cotton, F. Albert; Wilkinson, Geoffrey (1988), Advanced Inorganic Chemistry (5th ed.), New York: Wiley-Interscience, pp. 776, 955, ISBN 0-471-84997-9
  6. ^ Parker, Sybil P. (1984). Dictionary of Scientific and Technical Terms (3rd ed.). New York: McGraw-Hill.
  7. ^ a b Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. p. 510. ISBN 0-07-049439-8. Retrieved 2009-06-06.
  8. ^ a b c d e Krebs, Robert E. (2006). The history and use of our earth's chemical elements: a reference guide. Greenwood Publishing Group. pp. 303–304. ISBN 0-313-33438-2.
  9. ^ "Chemical reactions of Lutetium". Webelements. Retrieved 2009-06-06.
  10. ^ Persson, Ingmar (2010). "Hydrated metal ions in aqueous solution: How regular are their structures?". Pure and Applied Chemistry. 82 (10): 1901–1917. doi:10.1351/PAC-CON-09-10-22. ISSN 0033-4545.
  11. ^ a b c d e Georges, Audi; Bersillon, O.; Blachot, J.; Wapstra, A. H. (2003). "The NUBASE Evaluation of Nuclear and Decay Properties" (PDF). Nuclear Physics A. Atomic Mass Data Center. 729: 3–128. Bibcode:2003NuPhA.729....3A. doi:10.1016/j.nuclphysa.2003.11.001. Archived from the original (PDF) on 2016-01-17.
  12. ^ James, C. (1907). "A new method for the separation of the yttrium earths". Journal of the American Chemical Society. 29: 495–499. doi:10.1021/ja01958a010. In a footnote on page 498, James mentions that Carl Auer von Welsbach had announced " … the presence of a new element Er, γ, which is undoubtedly the same as here noted, … ." The article to which James refers is: C. Auer von Welsbach (1907) "Über die Elemente der Yttergruppe, (I. Teil)" (On the elements of the ytterbium group (1st part)), Monatshefte für Chemie und verwandte Teile anderer Wissenschaften (Monthly Journal for Chemistry and Related Fields of Other Sciences), 27 : 935-946.
  13. ^ "Separation of Rare Earth Elements by Charles James". National Historic Chemical Landmarks. American Chemical Society. Retrieved 2014-02-21.
  14. ^ a b Urbain, G. (1907). "Un nouvel élément: le lutécium, résultant du dédoublement de l'ytterbium de Marignac". Comptes Rendus. 145: 759–762.
  15. ^ Urbain, G. (1909). "Lutetium und Neoytterbium oder Cassiopeium und Aldebaranium -- Erwiderung auf den Artikel des Herrn Auer v. Welsbach". Monatshefte für Chemie. 31 (10): 1. doi:10.1007/BF01530262.
  16. ^ Welsbach, Carl A. von (1908). "Die Zerlegung des Ytterbiums in seine Elemente" [Resolution of ytterbium into its elements]. Monatshefte für Chemie. 29 (2): 181–225, 191. doi:10.1007/BF01558944. On page 191, Welsbach suggested names for the two new elements: "Ich beantrage für das an das Thulium, beziehungsweise Erbium sich anschließende, in dem vorstehenden Teile dieser Abhandlung mit Yb II bezeichnete Element die Benennung: Aldebaranium mit dem Zeichen Ad — und für das zweite, in dieser Arbeit mit Yb I bezeichnete Element, das letzte in der Reihe der seltenen Erden, die Benennung: Cassiopeïum mit dem Zeichen Cp." (I request for the element that is attached to thulium or erbium and that was denoted by Yb II in the above part of this paper, the designation "Aldebaranium" with the symbol Ad — and for the element that was denoted in this work by Yb I, the last in the series of the rare earths, the designation "Cassiopeïum" with the symbol Cp.)
  17. ^ a b Thyssen, Pieter; Binnemans, Koen (2011). "Accommodation of the Rare Earths in the Periodic Table: A Historical Analysis". In Gschneider, Karl A., Jr.; Bünzli, Jean-Claude; Pecharsky, Vitalij K. Handbook on the Physics and Chemistry of Rare Earths. Amsterdam: Elsevier. p. 63. ISBN 978-0-444-53590-0. OCLC 690920513. Retrieved 2013-04-25.
  18. ^ a b c d e f Emsley, John (2001). Nature's building blocks: an A-Z guide to the elements. Oxford University Press. pp. 240–242. ISBN 0-19-850341-5.
  19. ^ Hudson Institute of Mineralogy (1993–2018). "Mindat.org". www.mindat.org. Retrieved 14 January 2018.
  20. ^ Hedrick, James B. "Rare-Earth Metals" (PDF). USGS. Retrieved 2009-06-06.
  21. ^ Castor, Stephen B.; Hedrick, James B. (2006). "Rare Earth Elements". In Jessica Elzea Kogel, Nikhil C. Trivedi and James M. Barker. Industrial Minerals and Rocks (PDF). Society for Mining, Metallurgy and Exploration. pp. 769–792. Archived from the original on 2009-10-07.
  22. ^ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
  23. ^ Wei, Yayi; Brainard, Robert L. (2009). Advanced Processes for 193-NM Immersion Lithography. SPIE Press. p. 12. ISBN 0-8194-7557-2.
  24. ^ Nielsen, J. W.; Blank, S. L.; Smith, D. H.; Vella-Coleiro, G. P.; Hagedorn, F. B.; Barns, R. L.; Biolsi, W. A. (1974). "Three garnet compositions for bubble domain memories". Journal of Electronic Materials. 3 (3): 693–707. Bibcode:1974JEMat...3..693N. doi:10.1007/BF02655293.
  25. ^ Wahl, R. L. (2002). "Instrumentation". Principles and Practice of Positron Emission Tomography. Philadelphia: Lippincott: Williams and Wilkins. p. 51.
  26. ^ Daghighian, F.; Shenderov, P.; Pentlow, K. S.; Graham, M. C.; Eshaghian, B.; Melcher, C. L.; Schweitzer, J. S. (1993). "Evaluation of cerium doped lutetium oxyorthosilicate (LSO) scintillation crystals for PET". IEEE Transactions on Nuclear Science. 40 (4): 1045–1047. Bibcode:1993ITNS...40.1045D. doi:10.1109/23.256710.
  27. ^ Bush, Steve (14 March 2014). "Discussing LED lighting phosphors". Electronic Weekly. Retrieved 26 January 2017.
  28. ^ Simard-Normandin, Martine (2011). "A19 LED bulbs: What's under the frosting?". EE Times (July 18): 44–45. ISSN 0192-1541.
  29. ^ Muriel Gargaud; Hervé Martin; Philippe Claeys (2007). Lectures in Astrobiology. Springer. p. 51. ISBN 3-540-33692-3.
  30. ^ Sigel, Helmut (2004). Metal complexes in tumor diagnosis and as anticancer agents. CRC Press. p. 98. ISBN 0-8247-5494-8.
  31. ^ Balter, H.; Trindade, V.; Terán, M.; Gaudiano, J.; Ferrando, R.; Paolino, A.; Rodriguez, G.; Hermida, J.; De Marco, E.; Oliver, P. (2015). "177Lu-Labeled Agents for Neuroendocrine Tumor Therapy and Bone Pain Palliation in Uruguay". Current Radiopharmaceuticals. PMID 25771367.
  32. ^ Carollo, A.; Papi, S.; Chinol, M. (2015). "Lutetium-177 Labeled Peptides: The European Institute of Oncology Experience". Current Radiopharmaceuticals. PMID 25771368.
  33. ^ Arnold, K.J.; Kaewuam, R.; Roy, A.; Tan, T.R.; Barrett, M.D. (2018). "Blackbody radiation shift assessment for a lutetium ion clock". Nature Communications. Bibcode:2018NatCo...9.1650A. doi:10.1038/s41467-018-04079-x.
  34. ^ Blasse, G.; Dirksen, G.; Brixner, L.; Crawford, M. (1994). "Luminescence of materials based on LuTaO4". Journal of Alloys and Compounds. 209: 1–2. doi:10.1016/0925-8388(94)91069-3.
  35. ^ Shionoya, Shigeo (1998). Phosphor handbook. CRC Press. p. 846. ISBN 0-8493-7560-6.
  36. ^ Gupta, C. K.; Krishnamurthy, Nagaiyar (2004). Extractive metallurgy of rare earths. CRC Press. p. 32. ISBN 0-415-33340-7.

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