Seaborgium (Sg)
transition-metalSolid
Peso atómico estándar
[271]Configuración electrónica
[Rn] 7s2 5f14 6d4Punto de fusión
N/DPunto de ebullición
N/DDensidad
3,5e+4 kg/m³Estados de oxidación
+3, +4, +5, +6Electronegatividad (Pauling)
N/DEnergía de ionización (1.ª)
7,8 eVAño de descubrimiento
1974Radio atómico
132 pmDetalles
Seaborgium is a synthetic transactinide element in group 6, below tungsten. All confirmed isotopes are radioactive and short-lived, so its chemistry is studied atom by atom rather than in bulk. Experiments show that seaborgium behaves broadly as a heavier homolog of molybdenum and tungsten, with a stable +6 oxidation state in suitable compounds, while relativistic effects modify details of its volatility and complex formation.
Seaborgium does not occur naturally in the Earth’s crust. In 1974, seaborgium was first synthesized by Albert Ghiorso and his team at the University of California in Berkeley using the nuclear reaction 249Cf (18O, 4n) 263Sg. The element is named for Glenn T. Seaborg (Fig. IUPAC.106.1), who synthesized a number of trans-uranium elements [634], [648].
Seaborgium has no commercial applications. However, 265Sg was one of the decay products used to confirm the synthesis of copernicium in a particle accelerator experiment.
Seaborgium is named after Glenn Seaborg.
Seaborgium was first produced by a team of scientists led by Albert Ghiorso working at the Lawrence Berkeley Laboratory in Berkeley, California, in 1974. They created seaborgium by bombarding atoms of californium-249 with ions of oxygen-18 using a machine called the Super-Heavy Ion Linear Accelerator. The collision produced atoms of seaborgium-263 and four free neutrons. Seaborgium-263 is an isotope of seaborgium with a half-life of about 1 second. Three months before the Berkeley group announced their discovery, a team of scientists working at the Joint Institute for Nuclear Research in Dubna, Russia, claimed to have produced seaborgium. Their method involved bombarding atoms of lead-207 and lead-208 with ions of chromium-54 with a device called a cyclotron. They believed that they had produced atoms of seaborgium-259. The Berkeley group's work was confirmed in 1993 and they were credited with the discovery. Seaborgium's most stable isotope, seaborgium-271, has a half-life of about 2.4 minutes. It decays into rutherfordium-267 through alpha decay or decays through spontaneous fission..
IIn June 1974, members of the Joint Institute for Nuclear Research in Dubna, U.S.S.R., reported their discovery of Element 106, which they reported to have synthesized. Glenn Seaborg was part of this group, and the element was named in his honor.
In September 1974, workers of the Lawrence Berkeley and Livermore Laboratories also claimed creation Element 106 "without any scientific doubt." The LBL and LLL Group used the Super HILAC to accelerate 18O ions onto a 249Cf target.
Element 106 was created by the reaction 249Cf(18O, 4N)263X, which decayed by alpha emission to rutherfordium, and then by alpha emission to nobelium, which in turn further decayed by alpha between daughter and granddaughter. The element so identified had alpha energies of 9.06 and 9.25 MeV with a half-life of 0.9 +/- 0.2 s.
At Dubna, 280-MeV ions of 54Cr from the 310-cm cyclotron were used to strike targets of 206Pb, 207Pb, and 208Pb, in separate runs. Foils exposed to a rotating target disc were used to detect spontaneous fission activities. The foils were etched and examined microscopically to detect the number of fission tracks and the half-life of the fission activity. Other experiments were made to aid in confirmation of the discovery.
No macroscopic sample of seaborgium has been prepared, and its visible appearance is unknown. Calculations usually treat it as a very dense metallic solid under ordinary conditions, but this remains a prediction rather than an observed bulk property.
Seaborgium has no practical use outside scientific research. Its isotopes are produced in heavy-ion fusion experiments to study nuclear stability, decay chains, and the chemical behavior of the heaviest group 6 element. The element is valuable mainly because single atoms can test periodic trends and relativistic chemical models near the end of the actinide and transactinide region.
Since only a few atoms of seaborgium have ever been made, there are currently no uses for seaborgium outside of basic scientific research.
Seaborgium chemistry is known from rapid radiochemical experiments with individual atoms. The +6 oxidation state is the best established, consistent with group 6 chemistry. Volatile oxyhalides such as seaborgium oxychloride, SgO₂Cl₂, have been investigated by gas chromatography and compared with molybdenum oxychloride, MoO₂Cl₂, and tungsten oxychloride, WO₂Cl₂. Aqueous studies indicate formation of anionic oxo and oxofluoride complexes, but only fleeting trace quantities have been observed.
See more information at the Seaborgium compound page.
The safety properties of seaborgium are dominated by radioactivity, not chemical toxicity. The few atoms made in laboratories decay by alpha emission or spontaneous fission, depending on the isotope. External exposure from produced quantities is negligible, but accelerator targets, recoil products, and contaminated equipment are handled with radiological controls appropriate for heavy-ion nuclear research.
Seaborgium has no confirmed natural occurrence and no environmental cycle. Any atoms produced in a laboratory decay rapidly to other nuclides and are confined to experimental apparatus. Its environmental chemistry has not been observed directly, and ordinary ecological behavior cannot be assigned to an element produced only atom by atom.
Seaborgium has no commodity market, industrial supply chain, or recoverable inventory. It is made only in specialized accelerator facilities by bombarding heavy actinide targets with lighter ions, producing at most a few atoms at a time. The cost is therefore tied to nuclear research infrastructure, target preparation, beam time, and detection systems rather than to mining, refining, or commercial demand. Recycling in the usual materials sense is not applicable.
Made by bombarding californium-249 with oxygen-18.
Seaborgium is not expected to persist naturally in the universe because its known isotopes have very short half-lives. It may be formed transiently in extreme nuclear reactions, but any such atoms would decay quickly. It is not a significant constituent of stars, planets, meteorites, or interstellar material.
- Seaborgium was the first element named after a living person at the time the name was approved.
- Its chemistry must be measured before the atom decays, often within seconds.
- Gas-phase experiments compare seaborgium directly with molybdenum and tungsten compounds.
- Several seaborgium isotopes are identified through decay chains ending in better-known nuclei.
- Only atom-at-a-time chemistry is possible with present production methods.
Imágenes
Propiedades
Físicas
- Radio atómico (empírico)
- 132 pm Comparar Radio atómico (empírico) de todos los elementos →
- Densidad
- 3,5 × 104 kg/m³ Comparar Densidad de todos los elementos →
Químicas
- Afinidad electrónica
- 0,85 eV
- Energía de ionización (1.ª)
- 7,8 eV Comparar Energía de ionización (1.ª) de todos los elementos →
- Energía de ionización (2.ª)
- 17,100059 eV Comparar Energía de ionización (2.ª) de todos los elementos →
- Energía de ionización (3.ª)
- 25,800089 eV Comparar Energía de ionización (3.ª) de todos los elementos →
- Energía de ionización (4.ª)
- 35,500122 eV Comparar Energía de ionización (4.ª) de todos los elementos →
- Energía de ionización (5.ª)
- 47,200162 eV Comparar Energía de ionización (5.ª) de todos los elementos →
- Estados de oxidación
- +3, +4, +5, +6 Comparar Estados de oxidación de todos los elementos →
- Electrones de valencia
- 6 Comparar Electrones de valencia de todos los elementos →
- Configuración electrónica
- [Rn] 7s2 5f14 6d4
Termodinámicas
N/D
Nucleares
- Protones
- 106 Comparar Protones de todos los elementos →
- Neutrones
- 163 Comparar Neutrones de todos los elementos →
- Isótopos conocidos
- 16 Comparar Isótopos conocidos de todos los elementos →
- Isótopos estables
- 0 Comparar Isótopos estables de todos los elementos →
- Número másico (isótopo más estable)
- 271
- Isótopo más estable
- Sg-269
- Año de descubrimiento
- 1974
Abundancia
N/D
Estructura cristalina
N/D
Estructura electrónica
- Electrones por capa
- 2, 8, 18, 32, 32, 12, 2 Comparar Electrones por capa de todos los elementos →
Identificadores
- Número CAS
- 54038-81-2 Comparar Número CAS de todos los elementos →
- Símbolo del término
- 0
- InChI
- InChI=1S/Sg
- Clave InChI
- VAOUCABZIBBBJH-UHFFFAOYSA-N
Configuración electrónica Predicho
Sg: 5f¹⁴ 6d⁴ 7s²[Rn] 5f¹⁴ 6d⁴ 7s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 5f¹⁴ 6d⁴ 7s²Modelo 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
No hay isótopos estables.
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración |
|---|---|---|---|
| 263 Radiactivo | 263,11829 ± 0,0001 | N/D | 940 ms |
| 259 Radiactivo | 259,1144 ± 0,00013 | N/D | 402 ms |
| 266 Radiactivo | 266,12198 ± 0,00026 | N/D | 390 ms |
| 261 Radiactivo | 261,115949 ± 0,00002 | N/D | 183 ms |
| 264 Radiactivo | 264,11893 ± 0,0003 | N/D | 78 ms |
Fase / Estado
No hay datos disponibles sobre la fase o el estado
Espectros atómicos
Se muestran 10 de 95. Ordenado por carga del ion (ascendente).
Niveles disponibles ?
| Ion | Carga | Niveles |
|---|---|---|
| Sg I | 0 | 2 |
| Sg II | +1 | 2 |
| Sg III | +2 | 2 |
| Sg IV | +3 | 2 |
| Sg V | +4 | 2 |
| Sg VI | +5 | 2 |
| Sg VII | +6 | 2 |
| Sg VIII | +7 | 2 |
| Sg IX | +8 | 2 |
| Sg X | +9 | 2 |
No hay datos disponibles sobre la fase o el estado
Compuestos
Isótopos (5)
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración | Modo de desintegración | |
|---|---|---|---|---|---|
| 263 Radiactivo | 263,11829 ± 0,0001 | N/D | 940 ms | α =87±0.8%SF =13±0.8% | |
| 259 Radiactivo | 259,1144 ± 0,00013 | N/D | 402 ms | α ≈100%SF ?β+ ? | |
| 266 Radiactivo | 266,12198 ± 0,00026 | N/D | 390 ms | SF>90% | |
| 261 Radiactivo | 261,115949 ± 0,00002 | N/D | 183 ms | α =98.1±0.4%β+ =1.3±0.3%SF =0.6±0.2% | |
| 264 Radiactivo | 264,11893 ± 0,0003 | N/D | 78 ms | SF>80% α ? |
Propiedades ampliadas
Radios covalentes (ampliados)
- Radio covalente (Pyykkö)
- 143 pm
- Radio covalente (Pyykkö, enlace doble)
- 128 pm
- Radio covalente (Pyykkö, enlace triple)
- 121 pm
Escalas de numeración
- Mendeleev
- 54
Polarizabilidad y dispersión
- Polarizabilidad dipolar
- 40 a.u.
- Polarizabilidad dipolar (incert.)
- 4 a.u.
Categorías de estados de oxidación
Datos de referencia avanzados
Modos de desintegración de los isótopos (32)
| Isótopo | Modo | Intensidad |
|---|---|---|
| 258 | SF | 100% |
| 258 | A | — |
| 259 | A | 100% |
| 259 | SF | — |
| 259 | B+ | — |
| 260 | SF | 71% |
| 260 | A | 29% |
| 261 | A | 98,1% |
| 261 | B+ | 1,3% |
| 261 | SF | 0,6% |
Datos adicionales
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
Not Applicable
Referencias (1)
- [5] Seaborgium https://education.jlab.org/itselemental/ele106.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
Not Applicable
Referencias (1)
- [5] Seaborgium https://education.jlab.org/itselemental/ele106.html
Referencias
(8)
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 Seaborgium.