Lutetium

Lutetium is a chemical element; it has 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 earth elements; it can also be classified as the first element of the sixth-period transition metals.[1]

Lutetium was independently discovered in 1907 by French scientist Georges Urbain, Austrian mineralogist Baron Carl Auer von Welsbach, and American chemist Charles James.[2] All of these researchers found lutetium as an impurity in 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 honoring the Latin name for Paris, Lutetia.[3] In 1949 the spelling 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.[4]

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 (2.6%) radioisotope 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[5] 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.[6]

## Contents

* 1 Characteristics
* 1.1 Physical properties
* 1.2 Chemical properties and compounds
* 1.3 Isotopes
* 2 History
* 3 Occurrence and production
* 4 Applications
* 4.1 Stable isotopes
* 4.2 Unstable isotopes
* 5 Precautions
* 6 See also
* 7 References

## Characteristics

### Physical properties

A lutetium atom has 71 electrons, arranged in the configuration [Xe] 4f145d16s2.[7] Lutetium is generally encountered in the +3 oxidation state, having lost its two outermost 6s and the single 5d-electron. The lutetium atom is the smallest among the lanthanide atoms, due to the lanthanide contraction,[8] and as a result lutetium has the highest density, melting point, and hardness of the lanthanides.[9] As lutetium's 4f orbitals are highly stabilized only the 5d and 6s orbitals are involved in chemical reactions and bonding;[10][11] thus it is characterized as a d-block rather than an f-block element,[12] and on this basis some consider it not to be a lanthanide at all, but a transition metal like its lighter congeners scandium and yttrium.[13][14]

### Chemical properties and compounds

Main article: Chemistry:Lutetium compounds

Lutetium's compounds almost always contain the element in the +3 oxidation state.[15] Aqueous solutions of most lutetium salts are colorless and form white crystalline solids upon drying, with the common exception of the iodide, which is brown. 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.[16]

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 it may be used to remove vapors of these compounds from closed atmospheres.[17] Similar observations are made during reaction between lutetium and water (slow when cold and fast when hot); lutetium hydroxide is formed in the reaction.[18] Lutetium metal is known to react with the four lightest halogens to form trihalides; except the fluoride they are soluble in water. [19]

Lutetium dissolves readily in weak acids[17] 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(H
2O)
8.2]3+.[20]

2 Lu + 3 H
2SO
4 → 2 Lu3+ \+ 3 SO2−
4 \+ 3 H

### Isotopes

Main article: Physics:Isotopes of lutetium

Lutetium occurs on the Earth in 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 3.70×1010 years; it makes up about 2.6% of natural lutetium.[21]

To date, 40 synthetic radioisotopes of the element have been characterized, ranging in mass number from 149 to 188; 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. 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. 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.[21] Experiments at the Facility for Rare Isotope Beams have reported lutetium-190 in fragments of platinum-198 colliding with a carbon target.[22]

The element also has 43 known nuclear isomers, of which the most stable of them are lutetium-177m3, with a half-life of 160.4 days, and lutetium-174m with a half-life of 142 days; longer than the ground states of all lutetium isotopes except 173-176.[21]

## History

Three scientists were involved in the discovery of lutetium:[23] French scientist Georges Urbain,[3] Austrian mineralogist Baron Carl Auer von Welsbach,[24] and American chemist Charles James.[25][26] They found lutetium as an impurity in ytterbia, which was thought by Swiss chemist Jean Charles Galissard de Marignac to consist entirely of ytterbium. Of the three, Urbain was the first to publish, followed by Welsbach; James was about to publish when he learned of Urbain's work, and thereafter gave up his claim and did not publish.[27] Despite staying out of the priority argument, James worked on a much larger scale and possessed the largest supply of lutetium at the time.[28]

Urbain and Welsbach proposed different names. Urbain chose neoytterbium for ytterbium and lutecium for the new element.[29] Welsbach chose aldebaranium and cassiopeium (after Aldebaran and Cassiopeia). Both authors accused the other man of publishing results based on their work.[30][31] 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 choice for a name, one derived from the Latin Lutetia (Paris).[32] This decision was based on the fact that the separation of lutetium from Marignac's ytterbium was first described by Urbain.[3][24] Welsbach had achieved the separation before Urbain, but Urbain had published 44 days earlier. Since Urbain was on the commission which made the decision, its objectivity could be questioned; furthermore, Welsbach protested that Urbain's spectral evidence was weak and argued that his rival's lutetium was very impure, but to no avail.[27] After Urbain's names were recognized, neoytterbium was reverted to ytterbium.[33]

The controversy died down after 1910, only to be reignited with the discovery of element 72. Urbain claimed in 1911 to have discovered a new rare earth named celtium and identified it as element 72. However, Niels Bohr had demonstrated from his quantum theory that element 72 had to be a group 4 element and not a rare earth, and based on an idea by Fritz Paneth, Bohr's friend George de Hevesy worked with Dirk Coster to search for it in zirconium minerals. This they succeeded in doing, discovering hafnium in 1923. This discovery announcement, being in direct conflict with Urbain's celtium, ignited a controversy on element 72 throughout the 1920s; the resulting investigations on the nature of Urbain's celtium, since it was not the same as hafnium, reopened the case on element 71.[34]

The physicists Hans M. Hansen and Sven Werner, at Bohr's Copenhagen institute, found in 1923 that Welsbach's 1907 samples of cassiopeium had been pure element 71, while Urbain's 1907 lutecium samples only contained traces of element 71 and his 1911 samples identified as celtium were actually pure element 71 – confirming Welsbach's criticism.[27][34] The Copenhagen physicists then started a campaign to re-award priority for element 71 to Welsbach and replace the name lutetium with cassiopeium, writing to Welsbach in 1923 of their intentions. This campaign encountered success in the physics literature, but in spite of strong German and Scandinavian support for cassiopeium, lutetium remained embedded in most of the chemical literature, with the International Commission on Atomic Weights in 1930 accepting that element 72 was hafnium but using lutetium for element 71.[27]

In 1949, it was decided by the International Union of Pure and Applied Chemistry to recommend the name lutetium, since cassiopeium by then was only used in German and sometimes Dutch, and it was a difficult name to adapt to other languages. It was nonetheless clarified that this was not intended as a statement on priority. Urbain's spelling lutecium was changed to lutetium, in order to derive the name from Latin Lutetia instead of French Lutèce.[35] Pure lutetium metal was first produced in 1953.[28]

## Occurrence and production

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,[17] 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.[36] 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.[28] 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.[37][38]

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 adsorbed 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.[16]

2 LuCl
3 \+ 3 Ca → 2 Lu + 3 CaCl

177Lu is produced by neutron activation of 176Lu or by indirectly by neutron activation of 176Yb followed by beta decay. The 6.693-day half-life allows transport from the production reactor to the point of use without significant loss in activity.[39]

## Applications

There are few commercial uses specific to natural lutetium, and all of them involve small quantities.

### Stable isotopes

Stable lutetium can be used as catalysts in petroleum cracking in refineries and can also be used in alkylation, hydrogenation, and polymerization applications.[40]

Lutetium aluminium garnet (Al
5Lu

12) has been proposed for use as a lens material in high refractive index immersion lithography.[41] Additionally, a tiny amount of lutetium is added as a dopant to gadolinium gallium garnet, which was used in magnetic bubble memory devices.[42] Cerium-doped lutetium oxyorthosilicate is currently the preferred compound for detectors in positron emission tomography (PET).[43][44] Lutetium aluminium garnet (LuAG) is used as a phosphor in light-emitting diode light bulbs.[45][46]

Lutetium tantalate (LuTaO4) is the densest known stable white material (density 9.81 g/cm3)[47] and therefore is an ideal host for X-ray phosphors.[48][49] The only denser white material is thorium dioxide, with density of 10 g/cm3, but the thorium it contains is radioactive.

Lutetium is also a compound of several scintillating materials, which convert X-rays to visible light. It is part of LYSO, LuAG and lutetium iodide scintillators.

Research indicates that lutetium-ion atomic clocks could provide greater accuracy than any existing atomic clock.[50]

### Unstable isotopes

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.[51]

The isotope 177Lu emits low-energy beta particles and gamma rays and has a half-life around 7 days, positive characteristics for commercial applications, especially in therapeutic nuclear medicine.[39] The synthetic isotope lutetium-177 bound to octreotate (a somatostatin analogue), is used experimentally in targeted radionuclide therapy for neuroendocrine tumors.[52] Lutetium-177 is used as a radionuclide in neuroendocrine tumor therapy and bone pain palliation.[53][54]

Lutetium (177Lu) vipivotide tetraxetan is a therapy for prostate cancer, FDA approved in 2022.[55]

## Precautions

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.[17] Lutetium nitrate may be dangerous as it may explode and burn once heated. Lutetium oxide powder is toxic as well if inhaled or ingested.[17]

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.[28] 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.[28] 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 absorbed by plants. Soluble lutetium salts are mildly toxic, but insoluble ones are not.[28]

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## References

1. ↑ Scerri, E. (2012). "Mendeleev's Periodic Table Is Finally Completed and What To Do about Group 3?". Chemistry International 34 (4). doi:10.1515/ci.2012.34.4.28. http://www.iupac.org/publications/ci/2012/3404/ud.html.
2. ↑ "Lutetium Element Facts / Chemistry". https://www.chemicool.com/elements/lutetium.html.
3. ↑ 3.0 3.1 3.2 Urbain, Georges (4 November 1907). "Un nouvel élément: le lutécium, résultant du dédoublement de l'ytterbium de Marignac". C. R. Acad. Sci. 145: 759-762. https://gallica.bnf.fr/ark:/12148/bpt6k3099v/f759.item.
4. ↑ Ghosh, Joydeep (25 May 2018). "History of Lutetium". Chemistry Learner. https://www.chemistrylearner.com/lutetium.html.
5. ↑ "lutetium - Dictionary Definition". https://www.vocabulary.com/dictionary/lutetium.
6. ↑ Samsonov, G. V., ed (1968). "Mechanical Properties of the Elements". Handbook of the physicochemical properties of the elements. New York, USA: IFI-Plenum. pp. 387–446. doi:10.1007/978-1-4684-6066-7_7. ISBN 978-1-4684-6066-7. http://ihtik.lib.ru/2011.08_ihtik_nauka-tehnika/2011.08_ihtik_nauka-tehnika_3560.rar.
7. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1223. ISBN 978-0-08-037941-8.
8. ↑ Cotton, F. Albert; Wilkinson, Geoffrey (1988), Advanced Inorganic Chemistry (5th ed.), New York: Wiley-Interscience, pp. 776, 955, ISBN 0-471-84997-9
9. ↑ Parker, Sybil P. (1984). Dictionary of Scientific and Technical Terms (3rd ed.). New York: McGraw-Hill.
10. ↑ Jensen, William B. (2000). "The Periodic Law and Table". http://www.che.uc.edu/jensen/W. B. Jensen/Reprints/081. Periodic Table.pdf.
11. ↑ Krinsky, Jamin L.; Minasian, Stefan G.; Arnold, John (2010-12-08). "Covalent Lanthanide Chemistry Near the Limit of Weak Bonding: Observation of (CpSiMe3)3Ce−ECp* and a Comprehensive Density Functional Theory Analysis of Cp3Ln−ECp (E = Al, Ga)". Inorganic Chemistry (American Chemical Society (ACS)) 50 (1): 345–357. doi:10.1021/ic102028d. ISSN 0020-1669. PMID 21141834.
12. ↑ Jensen, William B. (2015). "The positions of lanthanum (actinium) and lutetium (lawrencium) in the periodic table: an update". Foundations of Chemistry 17: 23–31. doi:10.1007/s10698-015-9216-1. https://link.springer.com/article/10.1007/s10698-015-9216-1. Retrieved 28 January 2021.
13. ↑ Winter, Mark (1993–2022). "WebElements". The University of Sheffield and WebElements Ltd, UK. https://www.webelements.com/.
14. ↑ Cowan, Robert D. (1981). The Theory of Atomic Structure and Spectra. University of California Press. p. 598. ISBN 978-0-520-90615-0.
15. ↑ "Lutetium". Encyclopedia Britannica. https://www.britannica.com/science/lutetium.
16. ↑ 16.0 16.1 Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. p. 510. ISBN 978-0-07-049439-8. https://books.google.com/books?id=Xqj-TTzkvTEC&pg=PA243. Retrieved 2009-06-06.
17. ↑ 17.0 17.1 17.2 17.3 17.4 Krebs, Robert E. (2006). The history and use of our earth's chemical elements: a reference guide. Greenwood Publishing Group. pp. 303–304. ISBN 978-0-313-33438-2. https://archive.org/details/historyuseourear00kreb_356.
18. ↑ "Chemical reactions of Lutetium". Webelements. https://www.webelements.com/lutetium/chemistry.html.
19. ↑ "Lutetium (Lu)". EBSCO Research Starters. https://www.ebsco.com/research-starters/earth-and-atmospheric-sciences/lutetium-lu.
20. ↑ 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.
21. ↑ 21.0 21.1 21.2 Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties". Chinese Physics C 45 (3). doi:10.1088/1674-1137/abddae. https://www-nds.iaea.org/amdc/ame2020/NUBASE2020.pdf.
22. ↑ Tarasov, O. B.Expression error: Unrecognized word "et". (2024). "Observation of New Isotopes in the Fragmentation of 198Pt at FRIB". Physical Review Letters 132 (7). doi:10.1103/PhysRevLett.132.072501. PMID 38427880. Bibcode: 2024PhRvL.132g2501T.
23. ↑ Marshall, James L. Marshall; Marshall, Virginia R. Marshall (2015). "Rediscovery of the elements: The Rare Earths–The Confusing Years". The Hexagon: 72–77. http://www.chem.unt.edu/~jimm/REDISCOVERY 7-09-2018/Hexagon Articles/rare earths II.pdf. Retrieved 30 December 2019.
24. ↑ 24.0 24.1 Welsbach, Carl A. von (1908). "Die Zerlegung des Ytterbiums in seine Elemente". Monatshefte für Chemie 29 (2): 181–225, 191. doi:10.1007/BF01558944. http://babel.hathitrust.org/cgi/pt?id=mdp.39015036977471;view=1up;seq=193. 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.)
25. ↑ James, C. (1907). "A new method for the separation of the yttrium earths". Journal of the American Chemical Society 29 (4): 495–499. doi:10.1021/ja01958a010. Bibcode: 1907JAChS..29..495J. https://books.google.com/books?id=TrhMAAAAYAAJ&pg=PA495. 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.
26. ↑ "Separation of Rare Earth Elements by Charles James". National Historic Chemical Landmarks. American Chemical Society. http://www.acs.org/content/acs/en/education/whatischemistry/landmarks/earthelements.html.
27. ↑ 27.0 27.1 27.2 27.3 Kragh, Helge (1996). "Chapter 5. Elements No. 70, 71 and 72: Discoveries and Controversies". in Evans, C. H.. Episodes from the History of the Rare Earth Elements. Kluwer Academic Publishers. pp. 67–90. ISBN 978-94-010-6614-3.
28. ↑ 28.0 28.1 28.2 28.3 28.4 28.5 Emsley, John (2001). Nature's building blocks: an A-Z guide to the elements. Oxford University Press. pp. 240–242. ISBN 978-0-19-850341-5. https://books.google.com/books?id=Yhi5X7OwuGkC&pg=PA241.
29. ↑ 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. https://zenodo.org/record/1859372.
30. ↑ Weeks, Mary Elvira (1956). The discovery of the elements (6th ed.). Easton, PA: Journal of Chemical Education. https://archive.org/details/discoveryoftheel002045mbp.
31. ↑ Weeks, Mary Elvira (1932). "The discovery of the elements: XVI. The rare earth elements". Journal of Chemical Education 9 (10): 1751-1773. doi:10.1021/ed009p1751. Bibcode: 1932JChEd...9.1751W.
32. ↑ Clarke, F. W.; Ostwald, W.; Thorpe, T. E.; Urbain, G. (1909-01-01). "REPORT OF THE INTERNATIONAL COMMITTEE ON ATOMIC WEIGHTS. 1909.". Journal of the American Chemical Society 31 (1): 1–6. doi:10.1021/ja01931a001. ISSN 0002-7863. https://doi.org/10.1021/ja01931a001.
33. ↑ Skelton, Alasdair; Thornton, Brett F. (2017). "Iterations of ytterbium". Nature Chemistry 9 (4): 402. doi:10.1038/nchem.2755. PMID 28338694. Bibcode: 2017NatCh...9..402S. https://www.nature.com/articles/nchem.2755. Retrieved 31 January 2024.
34. ↑ 34.0 34.1 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. https://books.google.com/books?id=8SstnPFSzb0C&pg=PA66. Retrieved 2013-04-25.
35. ↑ Jensen, K. A. (1953). "Chapter 5. Problems of an International Chemical Nomenclature". Chemical Nomenclature. American Chemical Society. pp. 38–48.
36. ↑ Hudson Institute of Mineralogy (1993–2018). "Mindat.org". https://www.mindat.org/.
37. ↑ Hedrick, James B.. "Rare-Earth Metals". USGS. https://minerals.usgs.gov/minerals/pubs/commodity/rare_earths/740798.pdf.
38. ↑ 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. Society for Mining, Metallurgy and Exploration. pp. 769–792. http://www.rareelementresources.com/i/pdf/RareEarths-CastorHedrickIMAR7.pdf.
39. ↑ 39.0 39.1 MR Pillai, Ambikalmajan, and Furn F Russ Knapp. "Evolving important role of lutetium-177 for therapeutic nuclear medicine." Current radiopharmaceuticals 8.2 (2015): 78-85.
40. ↑ Lide, D. R., ed (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
41. ↑ Wei, Yayi; Brainard, Robert L. (2009). Advanced Processes for 193-NM Immersion Lithography. SPIE Press. p. 12. ISBN 978-0-8194-7557-2. https://books.google.com/books?id=Sx39H8XR1FcC&pg=PA12.
42. ↑ 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. doi:10.1007/BF02655293. Bibcode: 1974JEMat...3..693N.
43. ↑ Wahl, R. L. (2002). "Instrumentation". Principles and Practice of Positron Emission Tomography. Philadelphia: Lippincott: Williams and Wilkins. p. 51.
44. ↑ 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. doi:10.1109/23.256710. Bibcode: 1993ITNS...40.1045D.
45. ↑ Bush, Steve (14 March 2014). "Discussing LED lighting phosphors". Electronic Weekly. http://www.electronicsweekly.com/news/products/led/discussing-led-lighting-phosphors-2014-03/.
46. ↑ Simard-Normandin, Martine (2011). "A19 LED bulbs: What's under the frosting?". EE Times (July 18): 44–45. ISSN 0192-1541.
47. ↑ Blasse, G.; Dirksen, G.; Brixner, L.; Crawford, M. (1994). "Luminescence of materials based on LuTaO4". Journal of Alloys and Compounds 209 (1–2): 1–2. doi:10.1016/0925-8388(94)91069-3.
48. ↑ Shionoya, Shigeo (1998). Phosphor handbook. CRC Press. p. 846. ISBN 978-0-8493-7560-6. https://books.google.com/books?id=lWlcJEDukRIC&pg=PA846.
49. ↑ Gupta, C. K.; Krishnamurthy, Nagaiyar (2004). Extractive metallurgy of rare earths. CRC Press. p. 32. ISBN 978-0-415-33340-5. https://books.google.com/books?id=F0Bte_XhzoAC&pg=PA32.
50. ↑ 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 9 (1): 1650. doi:10.1038/s41467-018-04079-x. PMID 29695720. Bibcode: 2018NatCo...9.1650A.
51. ↑ Muriel Gargaud; Hervé Martin; Philippe Claeys (2007). Lectures in Astrobiology. Springer. p. 51. ISBN 978-3-540-33692-1. https://books.google.com/books?id=3uYmP0K5PXEC&pg=PA52.
52. ↑ Sigel, Helmut (2004). Metal complexes in tumor diagnosis and as anticancer agents. CRC Press. p. 98. ISBN 978-0-8247-5494-5. https://books.google.com/books?id=ZtRdbUNbPn8C&pg=PA98.
53. ↑ Balter, H.; Trindade, V.; Terán, M.; Gaudiano, J.; Ferrando, R.; Paolino, A.; Rodriguez, G.; Hermida, J. et al. (2015). "177Lu-Labeled Agents for Neuroendocrine Tumor Therapy and Bone Pain Palliation in Uruguay". Current Radiopharmaceuticals 9 (1): 85–93. doi:10.2174/1874471008666150313112620. PMID 25771367.
54. ↑ Carollo, A.; Papi, S.; Chinol, M. (2015). "Lutetium-177 Labeled Peptides: The European Institute of Oncology Experience". Current Radiopharmaceuticals 9 (1): 19–32. doi:10.2174/1874471008666150313111633. PMID 25771368.
55. ↑ Fallah, Jaleh; Agrawal, Sundeep; Gittleman, Haley; Fiero, Mallorie H.; Subramaniam, Sriram; John, Christy; Chen, Wei; Ricks, Tiffany K. et al. (1 May 2023). "FDA Approval Summary: Lutetium Lu 177 Vipivotide Tetraxetan for Patients with Metastatic Castration-Resistant Prostate Cancer". Clinical Cancer Research 29 (9): 1651–1657. doi:10.1158/1078-0432.CCR-22-2875. PMID 36469000.

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Periodic table

|  | 1 | 2 |  | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | 16 | 17 | 18

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1 | H |  | He
2 | Li | Be |  | B | C | N | O | F | Ne
3 | Na | Mg |  | Al | Si | P | S | Cl | Ar
4 | K | Ca |  | Sc | Ti | V | Cr | Mn | Fe | Co | Ni | Cu | Zn | Ga | Ge | As | Se | Br | Kr
5 | Rb | Sr |  | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd | Ag | Cd | In | Sn | Sb | Te | I | Xe
6 | Cs | Ba | La | Ce | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg | Tl | Pb | Bi | Po | At | Rn
7 | Fr | Ra | Ac | Th | Pa | U | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og

| Alkali metal | Alkaline earth metal | Lan­thanide | Actinide | Transition metal | Post-​transition metal | Metalloid | Reactive nonmetal | Noble gas

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Lutetium compounds

* Al5Lu3O12
* LuCl3
* LuBr3
* Lu2O3
* LuTaO4
* C52H72LuN5O14 (motexafin lutetium)

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