Lutetium

Template:Infobox 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 6th-period transition metals.<ref name="finally">Template:Cite journal</ref>

Lutetium was independently discovered in 1907 by French scientist Georges Urbain, Austrian mineralogist Baron Carl Auer von Welsbach, and American chemist Charles James.<ref name=":0">Template:Cite web</ref> 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, but 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.<ref>Template:Cite web</ref>

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<ref>Template:Cite web</ref> 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.<ref>Template:Cite book</ref>

Characteristics

Physical properties

A lutetium atom has 71 electrons, arranged in the configuration [Xe] 4f¹⁴5d¹6s².<ref name="Cotton">Template:Greenwood&Earnshaw</ref> 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,<ref>Template:Cotton&Wilkinson5th</ref> and as a result lutetium has the highest density, melting point, and hardness of the lanthanides.<ref name="Parker">Template:Cite book</ref> As lutetium's 4f orbitals are highly stabilized only the 5d and 6s orbitals are involved in chemical reactions and bonding;<ref name=jensenlaw>Template:Cite web</ref><ref>Template:Cite journal</ref> thus it is characterized as a d-block rather than an f-block element,<ref name="Jensen2015">Template:Cite journal</ref> 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.<ref>Template:Cite web</ref><ref>Template:Cite book</ref>

Chemical properties and compounds

Template:Category see also Lutetium's compounds almost always contain the element in the +3 oxidation state.<ref>Template:Cite web</ref> 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.<ref name="patnaik" />

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.<ref name="aaaaaa">Template:Cite book</ref> Similar observations are made during reaction between lutetium and water (slow when cold and fast when hot); lutetium hydroxide is formed in the reaction.<ref name="ffff">Template:Cite web</ref> Lutetium metal is known to react with the four lightest halogens to form trihalides; except the fluoride they are soluble in water. Template:Citation needed

Lutetium dissolves readily in weak acids<ref name="aaaaaa" /> 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 Template:Chem2.<ref name="Persson2010">Template:Cite journal</ref>

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Oxidation states

Lutetium is usually found in the +3 oxidation state, like most other lanthanides. However, it can also be in the 0, +1 and +2 states as well.

Isotopes

Template:Main 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 Template:Val; it makes up about 2.5% of natural lutetium.Template:NUBASE2020 To date, 40 synthetic radioisotopes of the element have been characterized, ranging in mass number from 149 to 190;Template:NUBASE2020<ref name=PRL132.7>Template:Cite journal</ref> 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.Template:NUBASE2020 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.Template:NUBASE2020 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.Template:NUBASE2020

The element also has 43 known nuclear isomers, with masses of 150, 151, 153–162, and 166–180 (not every mass number corresponds to only one isomer). The most stable of them are lutetium-177m, with a half-life of 160.4 days, and lutetium-174m, with a half-life of 142 days; these are longer than the half-lives of the ground states of all radioactive lutetium isotopes except lutetium-173, 174, and 176.Template:NUBASE2020

History

The discovery of lutetium was intertwined with that of ytterbium and thulium. Three scientists were involved in all three elements:<ref>Template:Cite book</ref> French scientist Georges Urbain,<ref name="1st">Template:Cite journal</ref> Austrian mineralogist Baron Carl Auer von Welsbach,<ref name="Deu">Template:Cite journal 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.)</ref> and American chemist Charles James.<ref name=JamesPrimary>Template:Cite journal 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.</ref><ref>Template:Cite web</ref> They found lutetium as an impurity in ytterbia, which was thought by Swiss chemist Jean Charles Galissard de Marignac to consist entirely of ytterbium.

Urbain and Welsbach proposed different names. Urbain chose neoytterbium for ytterbium and lutecium for the new element.<ref name="Fra">Template:Cite journal</ref> Welsbach chose aldebaranium and cassiopeium (after Aldebaran and Cassiopeia). Both authors accused the other man of publishing results based on their work.<ref name="Weeks">Template:Cite book</ref><ref name="XVI">Template:Cite journal</ref><ref name="Beginnings">Template:Cite journal</ref><ref name="Virginia">Template:Cite journal</ref><ref name="Marshall">Template:Cite journal</ref> 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). This decision was based on the fact that the separation of lutetium from Marignac's ytterbium was first described by Urbain;<ref name="1st" /> after Urbain's names were recognized, neoytterbium was reverted to ytterbium.<ref>Template:Cite journal</ref>

The controversy did not end. Confusion over element 72, Zirconium lead x-ray spectroscopic studies that suggested Welsbach's 1907 samples of lutetium had been pure, while Urbain's 1907 samples only contained traces of lutetium.<ref name="rare-earth-handbook">Template:Cite book</ref> 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.<ref name="Emsley240">Template:Cite book</ref> Pure lutetium metal was first produced in 1953.<ref name="Emsley240" />

Occurrence and production

File:Monazit - Mosambik, O-Afrika.jpg

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 (Template:Chem, which has concentrations of only 0.0001% of the element,<ref name="aaaaaa" /> 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. <ref>Template:Cite web</ref> 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.<ref name="Emsley240" /> 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.<ref>Template:Cite news</ref><ref>Template:Cite book</ref>

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.<ref name="patnaik">Template:Cite book</ref>

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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.<ref name=PillaiKnapp/>

Applications

Small quantities of lutetium have many speciality uses.

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.<ref>Template:RubberBible86th</ref>

Lutetium aluminium garnet (Template:Chem2) has been proposed for use as a lens material in high refractive index immersion lithography.<ref>Template:Cite book</ref> Additionally, a tiny amount of lutetium is added as a dopant to gadolinium gallium garnet, which was used in magnetic bubble memory devices.<ref>Template:Cite journal</ref> Cerium-doped lutetium oxyorthosilicate is currently the preferred compound for detectors in positron emission tomography (PET).<ref>Template:Cite book</ref><ref>Template:Cite journal</ref> Lutetium aluminium garnet (LuAG) is used as a phosphor in light-emitting diode light bulbs.<ref>Template:Cite web</ref><ref>Template:Cite journal</ref>

Lutetium tantalate (LuTaO₄) is the densest known stable white material (density 9.81 g/cm³)<ref name="lu1">Template:Cite journal</ref> and therefore is an ideal host for X-ray phosphors.<ref>Template:Cite book</ref><ref name="appl">Template:Cite book</ref> 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.<ref>Template:Cite journal</ref>

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.<ref>Template:Cite book</ref>

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.<ref name=PillaiKnapp>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.</ref> The synthetic isotope lutetium-177 bound to octreotate (a somatostatin analogue), is used experimentally in targeted radionuclide therapy for neuroendocrine tumors.<ref>Template:Cite book</ref> Lutetium-177 is used as a radionuclide in neuroendocrine tumor therapy and bone pain palliation.<ref>Template:Cite journal</ref><ref>Template:Cite journal</ref>

Lutetium (¹⁷⁷Lu) vipivotide tetraxetan is a therapy for prostate cancer, FDA approved in 2022.<ref>Template:Cite journal</ref>

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.<ref name="aaaaaa" /> Lutetium nitrate may be dangerous as it may explode and burn once heated. Lutetium oxide powder is toxic as well if inhaled or ingested.<ref name="aaaaaa" />

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.<ref name="Emsley240" /> 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.<ref name="Emsley240" /> 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.<ref name="Emsley240" />