Lutetium (Lu)
lanthanideSolid
Peso atómico estándar
174,9668 uConfiguración electrónica
[Xe] 6s2 4f14 5d1Punto de fusión
1662,85 °CPunto de ebullición
3401,85 °CDensidad
9840 kg/m³Estados de oxidación
0, +1, +2, +3Electronegatividad (Pauling)
1,27Energía de ionización (1.ª)
5,425871 eVAño de descubrimiento
1907Radio atómico
175 pmDetalles
Lutetium is a dense, silvery lanthanide and the last element of the 4f series. In chemistry it is almost exclusively trivalent, with a filled 4f shell in Lu³⁺ and a relatively small ionic radius compared with other lanthanides. It occurs with the rare-earth elements in minerals such as monazite and xenotime, but is one of the least abundant lanthanides. Its main technological value lies in specialized scintillators, catalysts, and medical radioisotopes rather than in bulk structural use.
Lutetium occurs in very small amounts in nearly all minerals containing yttrium, and is present in monazite to the extent of about 0.003%, which is a commercial source. The pure metal has been isolated only in recent years and is one of the most difficult to prepare. It can be prepared by the reduction of anhydrous LuCl3 or LuF3 by an alkali or alkaline earth metal. The metal is silvery white and relatively stable in air. 176Lu occurs naturally (2.6%) with 175Lu (97.4%). It is radioactive with a half-life of about 3 x 1010 years.
The name derives from Lutetia, the ancient name for the city of Paris. The discovery of lutetium is credited to the French chemist Georges Urbain in 1907 although it had been separated earlier and independently by the Austrian chemist Carl Auer (Baron von Welsbach) from an ytterbium sample.
Von Welsbach had named the element cassiopeium after the constellation Cassiopeia. However, because Urbain published his results before Auer, his name for the element was adopted by IUPAC in 1949.
The mineral gadolinite ((Ce, La, Nd, Y)2FeBe2Si2O10), discovered in a quarry near the town of Ytterby, Sweden, has been the source of a great number of rare earth elements. In 1843, Carl Gustaf Mosander, a Swedish chemist, was able to separate gadolinite into three materials, which he named yttria, erbia and terbia. As might be expected considering the similarities between their names and properties, scientists soon confused erbia and terbia and, by 1877, had reversed their names. What Mosander called erbia is now called terbia and visa versa. In 1878 Jean Charles Galissard de Marignac, a Swiss chemist, discovered that erbia was itself composed of two components. One component was named ytterbia by Marignac while the other component retained the name erbia. Marignac believed that ytterbia was a compound of a new element, which he named ytterbium. Other chemists produced and experimented with ytterbium in an attempt to determine some of it's properties. Unfortunately, different scientists obtained different results from the same experiments. While some scientists believed that these inconsistent results were caused by poor procedures or faulty equipment, Georges Urbain, a French chemist, believed that ytterbium wasn't an element at all, but a mixture of two elements. In 1907, Urbain was able to separate ytterbium into two elements. Urbain named one of the elements neoytterbium (new ytterbium) and the other element lutecium. Carl Auer von Welsbach, an Austrian chemist working independently of Urbain, reached the same conclusions at nearly the same time. Welsbach chose the names albebaranium and cassiopium for these elements. Urbain was eventually credited with the discovery of the elements and won the right to name them, although chemists later changed the name neoytterbium back to ytterbium and changed the spelling of lutecium to lutetium. Today, lutetium is primarily obtained through an ion exchange process from monazite sand ((Ce, La, Th, Nd, Y)PO4), a material rich in rare earth elements.
Lutetia is the ancient name for Paris. In 1907, Urbain described a process by which Marignac's ytterbium (1879) could be separated into the two elements, ytterbium (neoytterbium) and lutetium. These elements were identical with "aldebaranium" and "cassiopeium," independently discovered at this time. The spelling of the element was changed from lutecium to lutetium in 1949.
Pure lutetium is a bright silvery metal that tarnishes slowly in air. It is relatively hard and dense for a lanthanide, and can be cut or machined as a reactive metal under suitable conditions. Macroscopic metal is available, but usually only in small quantities because separation is costly.
The largest practical uses of lutetium are specialized. Lutetium oxyorthosilicate, Lu₂SiO₅, and related cerium-doped crystals are important scintillators in positron emission tomography and other radiation detectors. Lutetium compounds are used as catalysts or catalyst supports in some petroleum refining and organic reactions. The radioisotope ¹⁷⁷Lu is used in targeted radiopharmaceutical therapy, where its beta emission and accompanying gamma rays are useful for treatment and imaging dosimetry. Metallic lutetium itself has few direct applications.
Lutetium is one of the most difficult elements to prepare and has no large scale practical uses, although some of its radioactive isotopes can be used as a catalyst in the cracking of petroleum products and a catalyst in some hydrogenation and polymerization processes.
Stable lutetium nuclides, which emit pure beta radiation after thermal neutron activation, can be used as catalysts in cracking, alkylation, hydrogenation, and polymerization. Virtually no other commercial uses have been found yet for lutetium.
Isotopes in Biology
176Lu (with a half-life of 3.73×1010 years) is used in labeling experiments to quantify absolute protein abundance (absolute quantities of proteins in a cell) and examine the extent of synthesis of proteins under specific biological conditions [500] C. Rappel, D. Schaumloöffel. Anal. Chem.81, 385 (2009).. 175Lu has been used as a yield tracer in inductively coupled plasma mass spectrometry (ICP-MS) determination of plutonium in urine [500] C. Rappel, D. Schaumloöffel. Anal. Chem.81, 385 (2009)..
Isotopes in Medicine
177Lu (with a half-life of 160 h) has potential for use as an isotope for radioimmunotherapy for the treatment of small, soft tumors and for imaging purposes (Fig. IUPAC.71.1) [501] N. H. Bander, M. I. Milowsky, D. M. Nanus, L. Kostakoglu, S. Vallabhajosula, S. J. Goldsmith. J. Clin. Oncol.23, 4591 (2005)..
Lutetium chemistry is dominated by the +3 oxidation state. Common compounds include lutetium oxide, Lu₂O₃, a refractory sesquioxide; lutetium chloride, LuCl₃; lutetium fluoride, LuF₃; and lutetium nitrate, Lu(NO₃)₃. Lu³⁺ forms colorless or weakly colored salts because the 4f shell is filled and gives little visible absorption. Organometallic and coordination compounds are known, including cyclopentadienyl complexes, but they are mainly used in research or as specialized catalysts. Stable lower oxidation states are not characteristic under ordinary conditions.
See more information at the Lutetium compound page.
Lutetium metal dust can present fire and irritation hazards typical of reactive rare-earth metals. Soluble lutetium salts should be handled as toxic laboratory chemicals, although lutetium has no known biological role and its ordinary compounds are not among the most acutely hazardous rare-earth salts. The main isotope-specific hazard is radiological: ¹⁷⁷Lu and other radioactive isotopes require shielding, contamination control, and regulated handling. Stable natural lutetium is not significantly radioactive for practical purposes, despite containing long-lived ¹⁷⁶Lu.
While lutetium, like other rare-earth metals, is thought to have a low toxicity rating, it should be handled with care until more information is available.
Lutetium is dispersed in the crust with other heavy rare-earth elements and is concentrated only weakly by normal geological processes. It is released from minerals mainly through weathering or mining and processing of rare-earth ores. In natural waters Lu³⁺ is strongly complexed, adsorbed to particles, or incorporated into sediments, so dissolved concentrations are very low. It has no recognized biological function, and ecological effects are chiefly a concern near rare-earth mining, refining, or waste streams.
Lutetium is obtained as a minor component during separation of mixed rare-earth concentrates, especially from xenotime, ion-adsorption clays, and some monazite-derived streams. Its supply is constrained less by absolute geological scarcity than by the difficulty of separating adjacent lanthanides with very similar chemistry and by the limited volume of heavy rare-earth processing. Demand is modest but high-value, led by scintillator materials, research chemicals, catalysts, and medical isotope production chains. Recycling is limited and mostly tied to recovery from specialized crystals or process residues rather than broad consumer products.
Found with ytterbium in gadolinite and xenotime. Usually obtained from monazite sand which is ofter 50% rare earth by weight and 0.003% lutetium.
Lutetium is a rare heavy element in cosmic terms. Its stable isotope ¹⁷⁵Lu and long-lived ¹⁷⁶Lu are produced by neutron-capture processes in evolved stars and supernova-related environments, with details depending on s-process and r-process histories. In planetary materials it follows lithophile rare-earth behavior and is useful in isotope geochemistry, especially through the ¹⁷⁶Lu–¹⁷⁶Hf decay system.
- Lutetium was the last naturally occurring lanthanide to be identified as a separate element.
- The name derives from Lutetia, the Latin name for Paris.
- Lu³⁺ is the smallest common trivalent lanthanide ion.
- Natural lutetium is mostly ¹⁷⁵Lu, with a small fraction of long-lived ¹⁷⁶Lu.
- The ¹⁷⁶Lu–¹⁷⁶Hf system is used to date rocks and study mantle evolution.
- Lutetium is often placed under yttrium in periodic tables, but its group placement has been historically debated.
Imágenes
Propiedades
Físicas
- Radio atómico (empírico)
- 175 pm Comparar Radio atómico (empírico) de todos los elementos →
- Radio covalente
- 187 pm Comparar Radio covalente de todos los elementos →
- Radio de van der Waals
- 221 pm Comparar Radio de van der Waals de todos los elementos →
- Densidad
- 9840 kg/m³ Comparar Densidad de todos los elementos →
- Volumen molar
- 0,0178 L/mol
- Fase en CNPT
- Sólido Comparar Fase en CNPT de todos los elementos →
- Punto de fusión
- 1662,85 °C Comparar Punto de fusión de todos los elementos →
- Punto de ebullición
- 3401,85 °C Comparar Punto de ebullición de todos los elementos →
- Capacidad calorífica específica
- 0,154 J/(g·K) Comparar Capacidad calorífica específica de todos los elementos →
- Capacidad calorífica molar
- 26,86 J/(mol·K) Comparar Capacidad calorífica molar de todos los elementos →
- Estructura cristalina
- Hexagonal compacta Comparar Estructura cristalina de todos los elementos →
Químicas
- Electronegatividad (Pauling)
- 1,27 Comparar Electronegatividad (Pauling) de todos los elementos →
- Electronegatividad (Allen)
- 1,09
- Afinidad electrónica
- 0,346 eV
- Energía de ionización (1.ª)
- 5,425871 eV Comparar Energía de ionización (1.ª) de todos los elementos →
- Energía de ionización (2.ª)
- 14,130049 eV Comparar Energía de ionización (2.ª) de todos los elementos →
- Energía de ionización (3.ª)
- 20,959472 eV Comparar Energía de ionización (3.ª) de todos los elementos →
- Energía de ionización (4.ª)
- 45,249156 eV Comparar Energía de ionización (4.ª) de todos los elementos →
- Energía de ionización (5.ª)
- 66,80023 eV Comparar Energía de ionización (5.ª) de todos los elementos →
- Estados de oxidación
- 0, +1, +2, +3 Comparar Estados de oxidación de todos los elementos →
- Electrones de valencia
- 3 Comparar Electrones de valencia de todos los elementos →
- Configuración electrónica
- [Xe] 6s2 4f14 5d1
Termodinámicas
- Calor de fusión
- 0,18759393 eV Comparar Calor de fusión de todos los elementos →
- Calor de vaporización
- 3,679328 eV Comparar Calor de vaporización de todos los elementos →
- Calor de sublimación
- 4,435923 eV
- Calor de atomización
- 4,435923 eV
- Entalpía de atomización
- 4,431777 eV
Nucleares
- Protones
- 71 Comparar Protones de todos los elementos →
- Neutrones
- 104 Comparar Neutrones de todos los elementos →
- Isótopos conocidos
- 39 Comparar Isótopos conocidos de todos los elementos →
- Isótopos estables
- 1 Comparar Isótopos estables de todos los elementos →
- Isótopo más estable
- Lu-175
- Año de descubrimiento
- 1907
Abundancia
- Abundancia (corteza terrestre)
- 0,8 mg/kg Comparar Abundancia (corteza terrestre) de todos los elementos →
- Abundancia (océano)
- 1,5 × 10−7 mg/L Comparar Abundancia (océano) de todos los elementos →
Estructura cristalina
- Constante de red a
- 351 pm
Estructura electrónica
- Electrones por capa
- 2, 8, 18, 32, 9, 2 Comparar Electrones por capa de todos los elementos →
Identificadores
- Número CAS
- 7439-94-3 Comparar Número CAS de todos los elementos →
- Símbolo del término
- 2D3/2
- InChI
- InChI=1S/Lu
- Clave InChI
- OHSVLFRHMCKCQY-UHFFFAOYSA-N
Configuración electrónica Medido
Lu: 4f¹⁴ 5d¹ 6s²[Xe] 4f¹⁴ 5d¹ 6s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹ 6s²Modelo atómico
Los isótopos cambian el número de neutrones, la masa y la estabilidad, pero no la configuración electrónica de un átomo neutro.
Modelo atómico esquemático, no a escala.
Huella atómica
Espectro de emisión / absorción
Distribución isotópica
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración |
|---|---|---|---|
| 175 Estable | 174,9407752 ± 0,000002 | 97,4010% | Estable |
Fase / Estado
Motivo: 1637,8 °C por debajo del punto de fusión (1662,85 °C)
Esquemático, no a escala
Puntos de transición de fase
Energías de transición
Energía necesaria para fundir 1 mol en el punto de fusión
Energía necesaria para vaporizar 1 mol en el punto de ebullición
Energía necesaria para sublimar 1 mol en el punto de sublimación
Densidad
En condiciones estándar
En condiciones estándar
Espectros atómicos
Se muestran 10 de 71. Ordenado por carga del ion (ascendente).
Líneas disponibles ?
| Ion | Carga | Total de líneas | Probabilidades de transición | Designaciones de los niveles |
|---|---|---|---|---|
| Lu I | 0 | 133 | 44 | 108 |
| Lu II | +1 | 79 | 9 | 17 |
| Lu III | +2 | 64 | 0 | 0 |
| Lu IV | +3 | 100 | 0 | 0 |
| Lu V | +4 | 64 | 0 | 0 |
Niveles disponibles ?
| Ion | Carga | Niveles |
|---|---|---|
| Lu I | 0 | 234 |
| Lu II | +1 | 40 |
| Lu III | +2 | 29 |
| Lu IV | +3 | 62 |
| Lu V | +4 | 40 |
| Lu VI | +5 | 2 |
| Lu VII | +6 | 2 |
| Lu VIII | +7 | 2 |
| Lu IX | +8 | 2 |
| Lu X | +9 | 2 |
Radios iónicos
| Carga | Coordinación | Espín | Radio |
|---|---|---|---|
| +3 | 6 | N/D | 86.1 pm |
| +3 | 8 | N/D | 97.7 pm |
| +3 | 9 | N/D | 103.2 pm |
Compuestos
Isótopos (1)
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración | Modo de desintegración | |
|---|---|---|---|---|---|
| 175 Estable | 174,9407752 ± 0,000002 | 97,4010% ± 0,0130% | Estable | stable |
Propiedades ampliadas
Radios covalentes (ampliados)
- Radio covalente (Pyykkö)
- 162 pm
- Radio covalente (Pyykkö, enlace doble)
- 131 pm
- Radio covalente (Pyykkö, enlace triple)
- 131 pm
Radios de van der Waals
- Alvarez
- 274 pm
- UFF
- 364 pm
- MM3
- 265 pm
Radios atómicos y metálicos
- Radio atómico (Rahm)
- 270 pm
Escalas de numeración
- Mendeleev
- 41
- Pettifor
- 21
- Glawe
- 19
Escalas de electronegatividad
- Ghosh
- 0
- Miedema
- 3
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 2
Polarizabilidad y dispersión
- Polarizabilidad dipolar
- 137 a.u.
- Polarizabilidad dipolar (incert.)
- 7 a.u.
- C₆ (Gould–Bučko)
- 2020 Ha·Bohr6
Afinidad química
- Afinidad protónica
- 992 kJ/mol
- Basicidad en fase gaseosa
- 970,6 kJ/mol
Parámetros de Miedema
- Volumen molar de Miedema
- 17,77 cm3/mol
- Densidad electrónica de Miedema
- 2
Riesgo de suministro y economía
- Concentración de la producción
- 97
- Riesgo relativo de suministro
- 10
- Distribución de las reservas
- 50
- Estabilidad política (principal productor)
- 24
- Estabilidad política (país con mayores reservas)
- 24
Transiciones de fase y alótropos
| Punto de fusión | 1936,15 K |
| Punto de ebullición | 3675,15 K |
Categorías de estados de oxidación
Datos de referencia avanzados
Constantes de apantallamiento (14)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 1,3805 |
| 2 | p | 4,389 |
| 2 | s | 18,5502 |
| 3 | d | 13,5812 |
| 3 | p | 20,8337 |
| 3 | s | 21,4655 |
| 4 | d | 35,7108 |
| 4 | f | 40,0688 |
| 4 | p | 33,8096 |
| 4 | s | 32,7308 |
Detalle de los radios cristalinos (3)
| Carga | CN | Espín | rcrystal (pm) | Origen |
|---|---|---|---|---|
| 3 | VI | 100,1 | from r^3 vs V plots, | |
| 3 | VIII | 111,7 | from r^3 vs V plots, | |
| 3 | IX | 117,2 | from r^3 vs V plots, |
Modos de desintegración de los isótopos (53)
| Isótopo | Modo | Intensidad |
|---|---|---|
| 150 | p | 100% |
| 150 | B+ | — |
| 151 | p | — |
| 151 | B+ | — |
| 152 | B+ | 100% |
| 152 | B+p | 15% |
| 153 | A | — |
| 153 | B+ | — |
| 153 | p | 0% |
| 154 | B+ | — |
Factores de dispersión de rayos X (514)
| Energía (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 1,67493 |
| 10,1617 | — | 1,63824 |
| 10,3261 | — | 1,60236 |
| 10,4931 | — | 1,56726 |
| 10,6628 | — | 1,53293 |
| 10,8353 | — | 1,49935 |
| 11,0106 | — | 1,46651 |
| 11,1886 | — | 1,43538 |
| 11,3696 | — | 1,42424 |
| 11,5535 | — | 1,41319 |
Datos adicionales
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
8×10-1 milligrams per kilogram
Referencias (1)
- [5] Lutetium https://education.jlab.org/itselemental/ele071.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
1.5×10-7 milligrams per liter
Referencias (1)
- [5] Lutetium https://education.jlab.org/itselemental/ele071.html
Referencias
(9)
Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Lutetium.
The element property data was retrieved from publications.