Cobalt (Co)
transition-metalSolid
Peso atómico estándar
58,933194 uConfiguración electrónica
[Ar] 4s2 3d7Punto de fusión
1494,85 °CPunto de ebullición
2926,85 °CDensidad
8860 kg/m³Estados de oxidación
−3, −1, 0, +1, +2, +3, +4, +5Electronegatividad (Pauling)
1,88Energía de ionización (1.ª)
7,88101 eVAño de descubrimiento
1735Radio atómico
135 pmDetalles
Cobalt is a hard transition metal of group 9, best known for stable high-temperature alloys, magnetic materials, rechargeable battery cathodes, and intensely colored blue pigments. It occurs in nature chiefly as a minor constituent of sulfide and arsenide minerals and is commonly recovered with copper or nickel. Chemically it is dominated by the +2 and +3 oxidation states, with coordination chemistry that includes biologically important corrinoids.
Cobalt is a brittle, hard metal, resembling iron and nickel in appearance. It has a metallic permeability of about two thirds that of iron. Cobalt tends to exist as a mixture of two allotropes over a wide temperature range. The transformation is sluggish and accounts in part for the wide variation in reported data on physical properties of cobalt.
The name derives from the German Kobold for "evil spirits" or "goblins", who were superstitiously thought to cause trouble for miners because the mineral contained arsenic that injured their health and the metallic ores did not yield metals when treated with the normal methods. Cobalt was discovered in 1735 by the Swedish chemist Georg Brandt.
Cobalt was discovered by Georg Brandt, a Swedish chemist, in 1739. Brandt was attempting to prove that the ability of certain minerals to color glass blue was due to an unknown element and not to bismuth, as was commonly believed at the time. Cobalt's primary ores are cobaltite (CoAsS) and erythrite (Co3(AsO4)2). Cobalt is usually recovered as a byproduct of mining and refining nickel, silver, lead, copper and iron.
From the German word Kobald, goblin or evil spirit; also from the Greek cobalos, mine. George Brandt discovered cobalt in 1735.
Pure cobalt is a lustrous, silvery gray metal with a faint bluish cast. It is hard, relatively brittle compared with many structural metals, and ferromagnetic near room temperature. Finely divided cobalt has a much larger reactive surface and can behave differently from compact metal.
Cobalt is used in superalloys for turbine blades and other hot, highly stressed components, where it helps retain strength and resist corrosion. It is a key constituent of some permanent magnets and magnetic recording alloys. Large quantities are used in lithium-ion battery cathode materials, especially layered oxides containing lithium, cobalt, nickel, manganese, or aluminum. Cobalt compounds are also used as catalysts, driers for paints and inks, and blue ceramic and glass colorants. The radioisotope cobalt-60 is used as a gamma-ray source for sterilization, radiography, and radiotherapy.
Although cobalt is used in electroplating to give objects an attractive surface that resists oxidation, it is more widely used to form alloys. Alnico, an alloy consisting of aluminum, nickel and cobalt is used to make powerful permanent magnets. Stellite alloys, which contain cobalt, chromium and tungsten, are used to make high-speed and high temperature cutting tools and dyes. Cobalt is also used to make alloys for jet engines and gas turbines, magnetic steels and some types of stainless steels.
Cobalt-60, a radioactive isotope of cobalt, is an important source of gamma rays and is used to treat some forms of cancer and as a medical tracer. Cobalt-60 has a half-life of 5.27 years and decays into nickel-60 through beta decay.
Cobalt compounds have been used for centuries to color porcelain, glass, pottery, tile and enamel. Some of these compounds are known as: cobalt blue, ceruleum, new blue, smalt, cobalt yellow and cobalt green. In addition to being used as a dye, cobalt is also important to human nutrition as it is an essential part of vitamin B12.
It is alloyed with iron, nickel and other metals to make Alnico, an alloy of unusual magnetic strength with many important uses. Stellite alloys, containing cobalt, chromium, and tungsten, are used for high-speed, heavy-duty, high temperature cutting tools, and for dies.
Cobalt is also used in other magnetic steels and stainless steels, and in alloys used in jet turbines and gas turbine generators. The metal is used in electroplating because of its appearance, hardness, and resistance to oxidation.
Cobalt salts have been used for centuries to produce brilliant and permanent blue colors in porcelain, glass, pottery, tiles, and enamels. It is the principal ingredient in Sevre's and Thenard's blue. A solution of the chloride is used as a sympathetic ink. Cobalt carefully used in the form of the chloride, sulfate, acetate, or nitrate has been found effective in correcting a certain mineral deficiency disease in animals.
Soils should contain 0.13 to 0.30 ppm of cobalt for proper animal nutrition.
Isotopes in Industry
60Co (with a half-life of 5.27 years) is used to irradiate food sources as a method of preserving food (Fig. IUPAC.27.1). The gamma radiation from 60Co kills bacteria and other organisms that cause disease and spoilage of food (see Fig. IUPAC.27.1). The use of radioactive compounds for preserving food is not always viewed positively. Some individuals are concerned that harmful compounds will be produced during the irradiation process. However, there is no evidence to support the claim that irradiation is dangerous for food preservation [108] World Nuclear Association. Radioisotopes in Industry: Industrial Uses of Radioisotopes, World Nuclear Association (2014), Feb. 24; http://www.world-nuclear.org/info/inf56.html.. Many medical products today are sterilized using gamma rays from a 60Co source. This technique of sterilization is generally much cheaper and more effective than steam-heat sterilization because it is a cold process. For example, it can be performed on packaged items, such as disposable syringes. This sterilization technique is applicable to a wide range of heat-sensitive items, such as powders, ointments, and solutions, as well as biological preparations, such as bone, nerve, skin, etc., used in tissue grafts [108] World Nuclear Association. Radioisotopes in Industry: Industrial Uses of Radioisotopes, World Nuclear Association (2014), Feb. 24; http://www.world-nuclear.org/info/inf56.html..
60Co is also used in industrial radiography to detect structural flaws in metal parts. The radiation can penetrate metals and the X-ray pattern produced by the radiating material can provide information on its strength, composition, and other properties [108] World Nuclear Association. Radioisotopes in Industry: Industrial Uses of Radioisotopes, World Nuclear Association (2014), Feb. 24; http://www.world-nuclear.org/info/inf56.html.. Because of the above property, 60Co is also used in leveling devices and thickness gauges used to test welds and castings [108] World Nuclear Association. Radioisotopes in Industry: Industrial Uses of Radioisotopes, World Nuclear Association (2014), Feb. 24; http://www.world-nuclear.org/info/inf56.html..
Isotopes in Medicine
60Co is a radioactive metal isotope that is used in cancer treatments by radiotherapy. When 60Co undergoes radioactive decay, high-energy gamma rays (energies of 1.17 MeV and 1.33 MeV) are emitted and have been used in brachytherapy to treat various types of cancer. Brachytherapy (brachy is Greek meaning “short distance”) is a method of radiation treatment in which sealed sources are used to deliver a radiation dose at a distance of up to a few centimeters by surface, intracavitary (insertion of the radioactive isotope in a body cavity), or interstitial (between cells) application [75] J. Peterson, M. McDonell, L. Haroun, F. Monette, R. D. Hildebrand, A. Taboas. Radiological and Chemical Fact Sheets to Support Health Risk Analyses for Contaminated Areas, Prepared by Argonne National Laboratory Environmental Science Division in collaboration with U.S. Department of Energy, Richland Operations Office and Chicago Operations Office (2014), Feb. 22; http://www.remm.nlm.gov/ANL_ContaminantFactSheets_All_070418.pdf.. 60Co is used as a source of high-energy ionizing gamma radiation that can be directed to cancer cells from a device outside the body (external radiotherapy).
60Co (and sometimes 57Co and 58Co, with half-lives of 0.75 year and 71 days, respectively) is the key component of the Schilling test, which is a method for determining whether a patient’s body is making and using vitamin B12 properly. The cobalt isotope is used to label cobalt in vitamin B12 to monitor how the body processes this essential vitamin [224] B. R. Krynyckyi, L. S. Zuckier. J. Nucl. Med.36, 1659 (1995)..
57Co delivers the smallest radiation dose of all the cobalt isotopes. As a result, it has been used in the past for imaging and estimating organ size and location and in evaluating tumors of the head and neck [75] J. Peterson, M. McDonell, L. Haroun, F. Monette, R. D. Hildebrand, A. Taboas. Radiological and Chemical Fact Sheets to Support Health Risk Analyses for Contaminated Areas, Prepared by Argonne National Laboratory Environmental Science Division in collaboration with U.S. Department of Energy, Richland Operations Office and Chicago Operations Office (2014), Feb. 22; http://www.remm.nlm.gov/ANL_ContaminantFactSheets_All_070418.pdf., [99] World Nuclear Association. Radioisotopes in Medicine, World Nuclear Association (2014), Feb. 23; http://www.world-nuclear.org/info/inf55.html., [225] Royal Society of Chemistry. Cobalt, Royal Society of Chemistry (2017), Feb. 26; http://www.rsc.org/periodic-table/element/27/cobalt., [226] US Environmental Protection Agency. Cobalt, US Environmental Protection Agency (2017), Feb. 26; https://www.epa.gov/radiation/radionuclide-basics-cobalt-60., [227] Washington State Department of Health. Cobalt-60, Washington State Department of Health (2014), Feb. 26; http://www.doh.wa.gov/Portals/1/Documents/Pubs/320-078_co60_fs.pdf..
Cobalt commonly forms cobalt(II) compounds such as cobalt(II) oxide (CoO), cobalt(II) chloride (CoCl₂), and cobalt(II) sulfate (CoSO₄). Cobalt(III) is strongly stabilized in many coordination compounds, including hexaamminecobalt(III) chloride ([Co(NH₃)₆]Cl₃), and in oxides used in battery electrodes such as lithium cobalt oxide (LiCoO₂). Mixed-valence cobalt oxides include cobalt(II,III) oxide (Co₃O₄). The element also forms carbonyls, notably dicobalt octacarbonyl (Co₂(CO)₈), and complex corrinoid chemistry in vitamin B₁₂ derivatives.
See more information at the Cobalt compound page.
Cobalt is an essential trace element only as part of vitamin B₁₂, but soluble cobalt salts, metal dusts, and some cobalt-containing powders can be harmful by inhalation, ingestion, or skin contact. Industrial exposure may cause respiratory sensitization, dermatitis, and other toxic effects. Cobalt metal powder can present fire or dust hazards. Cobalt-60 is radioactive and hazardous because it emits penetrating gamma radiation; its risks are isotope-specific and depend on activity and shielding.
Exposure to cobalt (metal fumes and dust) should be limited to 0.05 mg/m3 (8-hour time-weighted average 40-hour week).
Cobalt is a trace element in soils, waters, and living systems. It is released naturally by weathering of rocks and minerals and also through mining, smelting, combustion residues, and disposal of cobalt-bearing products. In soils and sediments it can adsorb to iron and manganese oxides or occur in sulfide-rich phases, which affects mobility. It is nutritionally important for organisms that require vitamin B₁₂, but elevated bioavailable concentrations can be toxic.
Cobalt is produced mainly as a by-product of copper and nickel mining, so supply is tied to markets and operations whose primary product is usually another metal. Ores are processed by flotation, leaching, solvent extraction, precipitation, and refining to metal, salts, or battery-grade intermediates. Demand is strongly influenced by rechargeable batteries, superalloys, catalysts, and hard metals. Supply concentration, by-product dependence, and processing capacity make substitution and recycling important. Recycling recovers cobalt from spent batteries, superalloy scrap, and cemented carbides, but collection and chemistry vary by product type.
Cobalt occurs in the minerals cobaltite, smaltite, and erythrite, and is often associated with nickel, silver, lead, copper, and iron ores, from which it is most frequently obtained as a by-product. It is also present in meteorites.
Important ore deposits are found in Zaire, Morocco, and Canada. The U.S. Geological Survey has announced that the bottom of the north central Pacific Ocean may have cobalt-rich deposits at relatively shallow depths in water close to the the Hawaiian Islands and other U.S. Pacific territories.
Cobalt is far less abundant than iron and nickel but is a normal product of stellar nucleosynthesis. Stable cobalt is represented in nature by ⁵⁹Co, while radioactive cobalt isotopes can be produced in supernovae, cosmic-ray interactions, and neutron activation. In meteorites and planetary materials, cobalt tends to follow siderophile and chalcophile behavior, associating with metal and sulfide phases.
- Natural cobalt is essentially monoisotopic, consisting of stable ⁵⁹Co.
- The name comes from miners’ terms for troublesome ores that yielded toxic arsenic fumes.
- Cobalt blue pigments were valued long before cobalt was isolated as a metal.
- Cobalt remains ferromagnetic at temperatures above ordinary ambient conditions.
- Vitamin B₁₂ contains cobalt in a corrin ring, not as free cobalt metal.
Imágenes
Propiedades
Físicas
- Radio atómico (empírico)
- 135 pm Comparar Radio atómico (empírico) de todos los elementos →
- Radio covalente
- 126 pm Comparar Radio covalente de todos los elementos →
- Radio de van der Waals
- 192 pm Comparar Radio de van der Waals de todos los elementos →
- Radio metálico
- 116 pm Comparar Radio metálico de todos los elementos →
- Densidad
- 8860 kg/m³ Comparar Densidad de todos los elementos →
- Volumen molar
- 0,0067 L/mol
- Fase en CNPT
- Sólido Comparar Fase en CNPT de todos los elementos →
- Punto de fusión
- 1494,85 °C Comparar Punto de fusión de todos los elementos →
- Punto de ebullición
- 2926,85 °C Comparar Punto de ebullición de todos los elementos →
- Conductividad térmica
- 100 W/(m·K) Comparar Conductividad térmica de todos los elementos →
- Capacidad calorífica específica
- 0,421 J/(g·K) Comparar Capacidad calorífica específica de todos los elementos →
- Capacidad calorífica molar
- 24,81 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)
- 1,88 Comparar Electronegatividad (Pauling) de todos los elementos →
- Electronegatividad (Allen)
- 1,84
- Afinidad electrónica
- 0,661 eV
- Energía de ionización (1.ª)
- 7,88101 eV Comparar Energía de ionización (1.ª) de todos los elementos →
- Energía de ionización (2.ª)
- 17,084459 eV Comparar Energía de ionización (2.ª) de todos los elementos →
- Energía de ionización (3.ª)
- 33,500115 eV Comparar Energía de ionización (3.ª) de todos los elementos →
- Energía de ionización (4.ª)
- 51,270176 eV Comparar Energía de ionización (4.ª) de todos los elementos →
- Energía de ionización (5.ª)
- 79,500274 eV Comparar Energía de ionización (5.ª) de todos los elementos →
- Estados de oxidación
- −3, −1, 0, +1, +2, +3, +4, +5 Comparar Estados de oxidación de todos los elementos →
- Electrones de valencia
- 9 Comparar Electrones de valencia de todos los elementos →
- Configuración electrónica
- [Ar] 4s2 3d7
Termodinámicas
- Calor de fusión
- 0,1677981 eV Comparar Calor de fusión de todos los elementos →
- Calor de vaporización
- 3,886614 eV Comparar Calor de vaporización de todos los elementos →
- Calor de sublimación
- 4,40172 eV
- Calor de atomización
- 4,40172 eV
- Entalpía de atomización
- 4,422449 eV
Nucleares
- Protones
- 27 Comparar Protones de todos los elementos →
- Neutrones
- 32 Comparar Neutrones de todos los elementos →
- Isótopos conocidos
- 32 Comparar Isótopos conocidos de todos los elementos →
- Isótopos estables
- 1 Comparar Isótopos estables de todos los elementos →
- Isótopo más estable
- Co-59
- Año de descubrimiento
- 1735
Abundancia
- Abundancia (corteza terrestre)
- 25 mg/kg Comparar Abundancia (corteza terrestre) de todos los elementos →
- Abundancia (océano)
- 2 × 10−5 mg/L Comparar Abundancia (océano) de todos los elementos →
Estructura cristalina
- Constante de red a
- 251 pm
Estructura electrónica
- Electrones por capa
- 2, 8, 15, 2 Comparar Electrones por capa de todos los elementos →
Identificadores
- Número CAS
- 7440-48-4 Comparar Número CAS de todos los elementos →
- Símbolo del término
- 4F9/2
- InChI
- InChI=1S/Co
- Clave InChI
- GUTLYIVDDKVIGB-UHFFFAOYSA-N
Configuración electrónica Medido
Co: 3d⁷ 4s²[Ar] 3d⁷ 4s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁷ 4s²Modelo 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 |
|---|---|---|---|
| 59 Estable | 58,93319429 ± 0,00000056 | 100,0000% | Estable |
Fase / Estado
Motivo: 1469,8 °C por debajo del punto de fusión (1494,85 °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 27. Ordenado por carga del ion (ascendente).
Líneas disponibles ?
| Ion | Carga | Total de líneas | Probabilidades de transición | Designaciones de los niveles |
|---|---|---|---|---|
| Co I | 0 | 420 | 338 | 338 |
| Co II | +1 | 3168 | 2761 | 3168 |
| Co III | +2 | 2064 | 1957 | 2064 |
| Co IV | +3 | 9 | 0 | 0 |
| Co V | +4 | 55 | 0 | 0 |
| Co VIII | +7 | 165 | 150 | 165 |
| Co IX | +8 | 48 | 19 | 48 |
| Co X | +9 | 22 | 5 | 22 |
Niveles disponibles ?
| Ion | Carga | Niveles |
|---|---|---|
| Co I | 0 | 330 |
| Co II | +1 | 482 |
| Co III | +2 | 288 |
| Co IV | +3 | 297 |
| Co V | +4 | 268 |
| Co VI | +5 | 180 |
| Co VII | +6 | 65 |
| Co VIII | +7 | 73 |
| Co IX | +8 | 40 |
| Co X | +9 | 31 |
Radios iónicos
| Carga | Coordinación | Espín | Radio |
|---|---|---|---|
| +2 | 4 | high | 57.99999999999999 pm |
| +2 | 5 | N/D | 67 pm |
| +2 | 6 | low | 65 pm |
| +2 | 6 | high | 74.5 pm |
| +2 | 8 | N/D | 90 pm |
| +3 | 6 | low | 54.50000000000001 pm |
| +3 | 6 | high | 61 pm |
| +4 | 4 | N/D | 40 pm |
| +4 | 6 | high | 53 pm |
Compuestos
Isótopos (1)
Cobalt-60, an artificial isotope, is an important gamma ray source, and is extensively used as a tracer and a radiotherapeutic agent.
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración | Modo de desintegración | |
|---|---|---|---|---|---|
| 59 Estable | 58,93319429 ± 0,00000056 | 100,0000% | Estable | stable |
Líneas espectrales
Se muestran 50 de 738. De forma predeterminada, solo se muestran las líneas espectrales con intensidad medida.
| Longitud de onda (nm) | Intensidad | Estado de ionización | Tipo | Transición | Exactitud | Fuente | |
|---|---|---|---|---|---|---|---|
| 389.4073 nm | 7900 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d8.(3F).4p y 2G* | Medida | NIST | |
| 384.5461 nm | 6900 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d8.(3F).4p y 2G* | Medida | NIST | |
| 399.5302 nm | 6000 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d8.(3F).4p y 4G* | Medida | NIST | |
| 512.92021 nm | 5800 | Co II | emission | 3d7.(4F).4d e 5H → 3d7.(4F<9/2>).4f 2[15/2]* | Medida | NIST | |
| 387.3114 nm | 5500 | Co I | emission | 3p6.3d8.(3F).4s b 4F → 3p6.3d7.(4F).4s.4p.(3P*) z 4D* | Medida | NIST | |
| 412.1311 nm | 4400 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d7.(4F).4s.4p.(3P*) z 2G* | Medida | NIST | |
| 516.315 nm | 4100 | Co II | emission | 3d7.(4F).4d e 3H → 3d7.(4F<7/2>).4f 2[13/2]* | Medida | NIST | |
| 521.43464 nm | 3900 | Co II | emission | 3d7.(4F).4d e 5H → 3d7.(4F<9/2>).4f 2[15/2]* | Medida | NIST | |
| 505.07089 nm | 3800 | Co II | emission | 3d7.(4F).4d e 5G → 3d7.(4F<9/2>).4f 2[13/2]* | Medida | NIST | |
| 517.06829 nm | 3200 | Co II | emission | 3d7.(4F).4d e 5H → 3d7.(4F<7/2>).4f 2[13/2]* | Medida | NIST | |
| 387.3955 nm | 2800 | Co I | emission | 3p6.3d8.(3F).4s b 4F → 3p6.3d7.(4F).4s.4p.(3P*) z 4D* | Medida | NIST | |
| 411.8767 nm | 2800 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d7.(4F).4s.4p.(3P*) z 2G* | Medida | NIST | |
| 519.95128 nm | 2800 | Co II | emission | 3d7.(4F).4d e 3H → 3d7.(4F<5/2>).4f 2[11/2]* | Medida | NIST | |
| 513.56812 nm | 2700 | Co II | emission | 3d7.(4F).4d e 5H → 3d7.(4F<5/2>).4f 2[11/2]* | Medida | NIST | |
| 509.92115 nm | 2500 | Co II | emission | 3d7.(4F).4d e 3G → 3d7.(4F<7/2>).4f 2[11/2]* | Medida | NIST | |
| 523.11044 nm | 2300 | Co II | emission | 3d7.(4F).4d e 3H → 3d7.(4F<3/2>).4f 2[9/2]* | Medida | NIST | |
| 496.41682 nm | 2200 | Co II | emission | 3d7.(4F).4d f 5F → 3d7.(4F<9/2>).4f 2[11/2]* | Medida | NIST | |
| 505.7416 nm | 1700 | Co II | emission | 3d7.(4F).4d e 5G → 3d7.(4F<9/2>).4f 2[11/2]* | Medida | NIST | |
| 393.5959 nm | 1500 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d8.(3F).4p y 4F* | Medida | NIST | |
| 384.2046 nm | 1400 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d7.(4F).4s.4p.(3P*) z 2D* | Medida | NIST | |
| 509.52694 nm | 1400 | Co II | emission | 3d7.(4F).4d e 3G → 3d7.(4F<5/2>).4f 2[9/2]* | Medida | NIST | |
| 510.75362 nm | 1400 | Co II | emission | 3d7.(4F).4d e 5G → 3d7.(4F<7/2>).4f 2[9/2]* | Medida | NIST | |
| 506.70997 nm | 1200 | Co II | emission | 3d7.(4F).4d e 5P → 3d7.(4F<9/2>).4f 2[3/2]* | Medida | NIST | |
| 396.31 nm | 1100 | Co II | emission | 3d7.(4F).5p 5F* → 3d7.(4F).6d 5G | Medida | NIST | |
| 496.23566 nm | 1100 | Co II | emission | 3d7.(4F).4d f 5F → 3d7.(4F<9/2>).4f 2[9/2]* | Medida | NIST | |
| 517.6949 nm | 1100 | Co II | emission | 3d7.(4F).4d e 5G → 3d7.(4F<9/2>).4f 2[13/2]* | Medida | NIST | |
| 657.13038 nm | 1100 | Co II | emission | 3d7.(4F).5p 5G* → 3d7.(4F).5d 5H | Medida | NIST | |
| 657.62238 nm | 1100 | Co II | emission | 3d7.(4F).5p 3G* → 3d7.(4F).5d 3H | Medida | NIST | |
| 502.59107 nm | 990 | Co II | emission | 3d7.(4F).4d e 5D → 3d7.(4F<7/2>).4f 2[11/2]* | Medida | NIST | |
| 399.79 nm | 970 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d8.(3F).4p * | Medida | NIST | |
| 512.9972 nm | 960 | Co II | emission | 3d7.(4F).4d e 3G → 3d7.(4F<3/2>).4f 2[9/2]* | Medida | NIST | |
| 743.9418 nm | 960 | Co II | emission | 3d7.(4F).5p 5D* → 3d7.(4F).6s 5F | Medida | NIST | |
| 637.37856 nm | 920 | Co II | emission | 3d7.(4F).5p 5F* → 3d7.(4F).5d 5G | Medida | NIST | |
| 495.82966 nm | 900 | Co II | emission | 3d7.(4F).4d f 5F → 3d7.(4F<9/2>).4f 2[11/2]* | Medida | NIST | |
| 502.25161 nm | 900 | Co II | emission | 3d7.(4F).4d e 3D → 3d7.(4F<3/2>).4f 2[7/2]* | Medida | NIST | |
| 642.58717 nm | 900 | Co II | emission | 3d7.(4F).5p 5F* → 3d7.(4F).5d 5F | Medida | NIST | |
| 510.45696 nm | 890 | Co II | emission | 3d7.(4F).4d e 5D → 3d7.(4F<5/2>).4f 2[9/2]* | Medida | NIST | |
| 502.36685 nm | 860 | Co II | emission | 3d7.(4F).4d f 5F → 3d7.(4F<9/2>).4f 2[9/2]* | Medida | NIST | |
| 620.5716 nm | 860 | Co II | emission | 3d7.(4F).5p 5D* → 3d7.(4F).5d 5F | Medida | NIST | |
| 409.2384 nm | 830 | Co I | emission | 3p6.3d8.(3F).4s a 2F → 3p6.3d7.(4F).4s.4p.(3P*) z 2F* | Medida | NIST | |
| 508.31892 nm | 780 | Co II | emission | 3d7.(4F).4d e 5D → 3d7.(4F<3/2>).4f 2[5/2]* | Medida | NIST | |
| 502.6664 nm | 680 | Co II | emission | 3d7.(4F).4d e 5G → 3d7.(4F<5/2>).4f 2[7/2]* | Medida | NIST | |
| 517.75201 nm | 680 | Co II | emission | 3d7.(4F).4d e 3H → 3d7.(4F<7/2>).4f 2[11/2]* | Medida | NIST | |
| 662.16287 nm | 680 | Co II | emission | 3d7.(4F).5p 3G* → 3d7.(4F).5d 3H | Medida | NIST | |
| 495.25711 nm | 670 | Co II | emission | 3d7.(4F).4d e 5G → 3d7.(4F<5/2>).4f 2[9/2]* | Medida | NIST | |
| 500.77152 nm | 640 | Co II | emission | 3d7.(4F).4d f 5F → 3d7.(4F<9/2>).4f 2[5/2]* | Medida | NIST | |
| 510.63945 nm | 640 | Co II | emission | 3d7.(4F).4d e 5D → 3d7.(4F<3/2>).4f 2[5/2]* | Medida | NIST | |
| 499.59719 nm | 600 | Co II | emission | 3d7.(4F).4d e 5H → 3d7.(4F<7/2>).4f 2[13/2]* | Medida | NIST | |
| 509.2051 nm | 600 | Co II | emission | 3d7.(4F).4d e 5D → 3d7.(4F<3/2>).4f 2[3/2]* | Medida | NIST | |
| 510.07741 nm | 600 | Co II | emission | 3d7.(4F).4d e 3G → 3d7.(4F<7/2>).4f 2[9/2]* | Medida | NIST |
Propiedades ampliadas
Radios covalentes (ampliados)
- Radio covalente (Pyykkö)
- 111 pm
- Radio covalente (Pyykkö, enlace doble)
- 103 pm
- Radio covalente (Pyykkö, enlace triple)
- 96 pm
- Radio covalente (Bragg)
- 137 pm
Radios de van der Waals
- Batsanov
- 200 pm
- Alvarez
- 240 pm
- UFF
- 287,2 pm
- MM3
- 223 pm
Radios atómicos y metálicos
- Radio atómico (Rahm)
- 233 pm
- Radio metálico (C12)
- 125 pm
Escalas de numeración
- Mendeleev
- 63
- Pettifor
- 64
- Glawe
- 70
Escalas de electronegatividad
- Ghosh
- 0
- Miedema
- 5
- Gunnarsson–Lundqvist
- 6
- Robles–Bartolotti
- 5
Polarizabilidad y dispersión
- Polarizabilidad dipolar
- 55 a.u.
- Polarizabilidad dipolar (incert.)
- 4 a.u.
- C₆
- 408 Ha·Bohr6
- C₆ (Gould–Bučko)
- 461 Ha·Bohr6
Afinidad química
- Afinidad protónica
- 742,7 kJ/mol
- Basicidad en fase gaseosa
- 719,8 kJ/mol
Parámetros de Miedema
- Volumen molar de Miedema
- 6,7 cm3/mol
- Densidad electrónica de Miedema
- 5
Riesgo de suministro y economía
- Concentración de la producción
- 67
- Riesgo relativo de suministro
- 8
- Distribución de las reservas
- 45
- Estabilidad política (principal productor)
- 3
- Estabilidad política (país con mayores reservas)
- 3
Transiciones de fase y alótropos
| Punto de fusión | 1768,15 K |
| Punto de ebullición | 3200,15 K |
Categorías de estados de oxidación
Datos de referencia avanzados
Constantes de apantallamiento (7)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0,6332 |
| 2 | p | 3,9076 |
| 2 | s | 7,595 |
| 3 | d | 15,1446 |
| 3 | p | 13,5654 |
| 3 | s | 12,6777 |
| 4 | s | 21,4236 |
Detalle de los radios cristalinos (9)
| Carga | CN | Espín | rcrystal (pm) | Origen |
|---|---|---|---|---|
| 2 | IV | HS | 72 | |
| 2 | V | 81 | calculated, | |
| 2 | VI | LS | 79 | from r^3 vs V plots, |
| 2 | VI | HS | 88,5 | from r^3 vs V plots, |
| 2 | VIII | 104 | ||
| 3 | VI | LS | 68,5 | from r^3 vs V plots, |
| 3 | VI | HS | 75 | |
| 4 | IV | 54 | ||
| 4 | VI | HS | 67 | from r^3 vs V plots, |
Modos de desintegración de los isótopos (57)
| Isótopo | Modo | Intensidad |
|---|---|---|
| 47 | p | — |
| 48 | p | — |
| 49 | p | — |
| 50 | B+ | 100% |
| 50 | B+p | 70,5% |
| 50 | 2p | — |
| 51 | B+ | 100% |
| 51 | B+p | 3,8% |
| 52 | B+ | 100% |
| 52 | B+p | — |
Factores de dispersión de rayos X (504)
| Energía (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 1,42071 |
| 10,1617 | — | 1,45925 |
| 10,3261 | — | 1,49884 |
| 10,4931 | — | 1,53949 |
| 10,6628 | — | 1,58125 |
| 10,8353 | — | 1,62415 |
| 11,0106 | — | 1,6682 |
| 11,1886 | — | 1,71345 |
| 11,3696 | — | 1,75993 |
| 11,5535 | — | 1,80767 |
Datos adicionales
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
2.5×101 milligrams per kilogram
Referencias (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
2×10-5 milligrams per liter
Referencias (1)
Sources
Sources of this element.
Cobalt occurs in the minerals cobaltite, smaltite, and erythrite, and is often associated with nickel, silver, lead, copper, and iron ores, from which it is most frequently obtained as a by-product. It is also present in meteorites.
Important ore deposits are found in Zaire, Morocco, and Canada. The U.S. Geological Survey has announced that the bottom of the north central Pacific Ocean may have cobalt-rich deposits at relatively shallow depths in water close to the the Hawaiian Islands and other U.S. Pacific territories.
Referencias (1)
- [6] Cobalt https://periodic.lanl.gov/27.shtml
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 Cobalt.
The element property data was retrieved from publications.