Chromium (Cr)
transition-metalSolid
Peso atómico estándar
51,9961 uConfiguración electrónica
[Ar] 3d5 4s1Punto de fusión
1906,85 °CPunto de ebullición
2670,85 °CDensidad
7150 kg/m³Estados de oxidación
−4, −2, −1, 0, +1, +2, +3, +4, +5, +6Electronegatividad (Pauling)
1,66Energía de ionización (1.ª)
6,76651 eVAño de descubrimiento
1797Radio atómico
140 pmDetalles
Chromium is a hard transition metal best known for forming adherent, protective oxide films and for giving many minerals and compounds strong colors. It occurs mainly in chromite ores and is an important alloying element in stainless and heat-resisting steels. Its chemistry spans several oxidation states, especially +3 and +6, with a sharp contrast between relatively stable Cr(III) compounds and strongly oxidizing, often toxic Cr(VI) species.
Chromium is used extensively in automobile trim as chromium metal because of its shiny finish and corrosion resistance.
The name derives from the Greek chroma for "colour", from the many coloured compounds of chromium. It was discovered in 1797 by the French chemist and pharmacist Nicolas-Louis Vauquelin, who also isolated chromium in 1798.
Chromium was discovered by Louis-Nicholas Vauquelin while experimenting with a material known as Siberian red lead, also known as the mineral crocoite (PbCrO4), in 1797. He produced chromium oxide (CrO3) by mixing crocoite with hydrochloric acid (HCl). Although he believed a method for isolating chromium didn't yet exist, Vauquelin was pleasantly surprised in 1798 to discover that he was able to obtain metallic chromium by simply heating chromium oxide in a charcoal oven. Today, chromium is primarily obtained by heating the mineral chromite (FeCr2O4) in the presence of aluminum or silicon.
From the Greek word chroma, color. Chromium is a steel-gray, lustrous, hard metal that takes a high polish. Discovered in 1797 by the Frenchman Louis Nicolas Vauquelin.
Pure chromium is a lustrous, silvery-gray metal with a high polish and a relatively high melting point. It is hard and brittle at room temperature, and its surface is rapidly passivated by a very thin oxide layer that resists further corrosion under many conditions.
The largest use of chromium is in ferrochrome for stainless steel, where chromium provides corrosion resistance by forming a passive surface film. It is also used in tool steels, superalloys, wear-resistant coatings, and hard chromium electroplating. Chromium compounds have been used in pigments, leather tanning, wood preservation, catalysts, and refractory materials, although several Cr(VI)-based uses have been restricted or replaced because of toxicity and environmental persistence.
Chromium is a blue-white metal that is hard, brittle and very corrosion resistant. Chromium can be polished to form a very shiny surface and is often plated to other metals to form a protective and attractive covering. Chromium is added to steel to harden it and to form stainless steel, a steel alloy that contains at least 10% chromium. Other chromium-steel alloys are used to make armor plate, safes, ball bearings and cutting tools.
Chromium forms many colorful compounds that have industrial uses. Lead chromate (PbCrO4), also known as chrome yellow, has been used as a yellow pigment in paints. Chromic oxide (Cr2O3), also known as chrome green, is the ninth most abundant compound in the earth's crust and is a widely used green pigment. Rubies and emeralds also owe their colors to chromium compounds. Potassium dichromate (K2Cr2O7) is used in the tanning of leather while other chromium compounds are used as mordants, materials which permanently fix dyes to fabrics. Chromium compounds are also used to anodize aluminum, a process which coats aluminum with a thick, protective layer of oxide. Chromite, chromium's primary ore, is used to make molds for the firing of bricks because of its high melting point, moderate thermal expansion and stable crystal structure.
Chromium is used to harden steel, manufacture stainless steel, and form many useful alloys. It is mostly used in plating to produce a hard, beautiful surface and to prevent corrosion. Chromium gives glass an emerald green color and is widely used as a catalyst.
The refractory industry uses chromite for forming bricks and shapes, as it has a high melting point, moderate thermal expansion, and stability of crystalline structure.
Isotopes in Earth/Planetary Science
Molecules, atoms, and ions of the stable isotopes of chromium possess slightly different physical and chemical properties, and they commonly will be fractionated during physical, chemical, and biological processes, giving rise to variations in isotopic abundances and in atomic weights. There are measureable variations in the isotopic abundances of chromium in natural terrestrial materials (Fig. IUPAC.24.1).
SiC grains are formed in very high-temperature events that occurred before the formation of the Solar System. The chemical and isotopic composition of certain elements in these grains, such as chromium, provides insights into the origin of the Solar System. The 54Cr nucleus is only produced by supernovae. Excess amounts of this isotope in the SiC grains (relative to terrestrial isotopic composition) in primitive meteorites suggest a heterogeneous distribution of 54Cr in the early Solar System and different sources of material to our Solar System [206] L. Qin, L. R. Nittler, C. M. O. D. Alexander, J. Wang, F. J. Stadermann, R. W. Carlson. Geochim. Cosmochim. Acta.75, 629 (2010).. The early solar nebula was divided into two components. One contained chromium depleted in the lighter isotopes and the other contained heavier chromium isotopes. Isotopic studies indicate these components formed a homogeneous mixture in the early Earth, but they separated during partitioning of the Earth’s core (Fig. IUPAC.24.1) [207] F. Moynier, Q. Z. Yin, E. Schauble. Science331, 1417 (2011)., [208] W. F. McDonough. Science331, 1397 (2011)..
Mobility and toxicity of chromium metal depend largely on the oxidation state of the element. Isotopes of chromium are fractionated by reduction-oxidation (redox) chemical reactions. The isotopic composition has been used to trace the origin of the element in the environment and provide information on reduction-oxidation chemical processes [209] A. S. Ellis, T. M. Johnson, T. D. Bullen. Science295, 2060 (2002)..
Isotopes in Medicine
Stable isotopes of chromium are used to investigate the metabolism of chromium (III), which is an essential nutrient. Chromium stable isotopes (53Cr and 54Cr) have been administered to patients and the relative metabolic activity of each isotope is measured to study insulin function in patients suffering from diabetes (a disease in which the body is unable to produce any or enough insulin, and/or is not able to properly use the insulin that it does produce, resulting in elevated levels of glucose in the blood) [210] H. M. Silver, M. A. Seebeck, R. M. Cowett, K. Y. Patterson, C. Veillon. J. Soc. Gynecol. Investig.4, 254 (1997).. 51Cr and 53Cr have been used to label red blood cells to determine blood volume and life-time of red blood cells in the body [210] H. M. Silver, M. A. Seebeck, R. M. Cowett, K. Y. Patterson, C. Veillon. J. Soc. Gynecol. Investig.4, 254 (1997)..
Chromium forms compounds in oxidation states from negative values in organometallic chemistry to +6, but +3 and +6 dominate common inorganic chemistry. Chromium(III) oxide, Cr₂O₃, is a stable green solid and an important pigment and refractory material. Chromium(VI) oxide, CrO₃, chromates such as potassium chromate, K₂CrO₄, and dichromates such as potassium dichromate, K₂Cr₂O₇, are strong oxidants. Chromium(II) chloride, CrCl₂, is a reducing Cr(II) salt used in specialized synthesis.
All compounds of chromium are colored. The most important chromates are those of sodium and potassium, the dichromates, and the potassium and ammonium chrome alums. The dichromates are used as oxidizing agents in quantitative analysis, also in tanning leather.
Other compounds are of industrial value; lead chromate is chrome yellow, a valued pigment. Chromium compounds are used in the textile industry as mordants, and by the aircraft and other industries for anodizing aluminum.
See more information at the Chromium compound page.
Metallic chromium is not highly reactive in bulk form, but dusts and fumes from welding, grinding, or plating operations can be hazardous. Soluble Cr(VI) compounds are toxic, corrosive, sensitizing, and carcinogenic by inhalation, and they require strict exposure control. Cr(III) compounds are generally less mobile and less toxic, although concentrated salts and fine powders still present chemical and occupational hazards.
Chromium compounds are toxic and should be handled with proper safeguards.
Chromium is a natural trace constituent of rocks, soils, and sediments, commonly associated with ultramafic rocks and chromite minerals. In the environment, Cr(III) tends to form insoluble hydroxides and complexes with organic matter, while Cr(VI) oxyanions are more mobile in oxygenated waters. Industrial releases from plating, tanning, pigment manufacture, and waste disposal have produced localized contamination where redox conditions control persistence and transport.
Chromium is produced chiefly by mining chromite ore and reducing it to ferrochrome for steelmaking. South Africa, Kazakhstan, India, Turkey, and several other countries are important sources of chromite, so supply is tied to ore quality, energy costs, and metallurgical capacity. Demand is dominated by stainless steel production, with smaller markets for chemicals, refractories, and plating. Recycling occurs mainly through stainless steel and alloy scrap, which returns chromium to steel production and reduces dependence on primary ore.
The principal ore is chromite, which is found in Zimbabwe, Russia, New Zealand, Turkey, Iran, Albania, Finland, Democratic Republic of Madagascar, and the Phillippines. The metal is usually produced by reducing the oxide with aluminum.
Chromium is a minor but widespread element in the cosmos, made mainly in massive stars and supernova nucleosynthesis near the iron peak. It is present in the Sun, meteorites, and rocky planetary materials. Isotopic ratios of chromium in meteorites are used in cosmochemistry to trace early Solar System reservoirs and nucleosynthetic contributions.
- The name chromium comes from the Greek word for color, reflecting its vividly colored compounds.
- Ruby owes its red color to trace Cr³⁺ substituting for aluminum in corundum.
- Chrome plating can be decorative, but engineering hard chrome is used mainly for wear resistance.
- Passivation by chromium oxide is the key reason stainless steel does not behave like ordinary carbon steel.
- Lead chromate, PbCrO₄, was once a major yellow pigment but is now restricted in many applications.
- Chromium metal is usually traded through ferrochrome rather than as pure metal.
Imágenes
Propiedades
Físicas
- Radio atómico (empírico)
- 140 pm Comparar Radio atómico (empírico) de todos los elementos →
- Radio covalente
- 139 pm Comparar Radio covalente de todos los elementos →
- Radio de van der Waals
- 189 pm Comparar Radio de van der Waals de todos los elementos →
- Radio metálico
- 119 pm Comparar Radio metálico de todos los elementos →
- Densidad
- 7150 kg/m³ Comparar Densidad de todos los elementos →
- Volumen molar
- 0,00723 L/mol
- Fase en CNPT
- Sólido Comparar Fase en CNPT de todos los elementos →
- Punto de fusión
- 1906,85 °C Comparar Punto de fusión de todos los elementos →
- Punto de ebullición
- 2670,85 °C Comparar Punto de ebullición de todos los elementos →
- Conductividad térmica
- 93,9 W/(m·K) Comparar Conductividad térmica de todos los elementos →
- Capacidad calorífica específica
- 0,449 J/(g·K) Comparar Capacidad calorífica específica de todos los elementos →
- Capacidad calorífica molar
- 23,35 J/(mol·K) Comparar Capacidad calorífica molar de todos los elementos →
- Estructura cristalina
- Cúbica centrada en el cuerpo Comparar Estructura cristalina de todos los elementos →
Químicas
- Electronegatividad (Pauling)
- 1,66 Comparar Electronegatividad (Pauling) de todos los elementos →
- Electronegatividad (Allen)
- 1,65
- Afinidad electrónica
- 0,675 eV
- Energía de ionización (1.ª)
- 6,76651 eV Comparar Energía de ionización (1.ª) de todos los elementos →
- Energía de ionización (2.ª)
- 16,486362 eV Comparar Energía de ionización (2.ª) de todos los elementos →
- Energía de ionización (3.ª)
- 30,959107 eV Comparar Energía de ionización (3.ª) de todos los elementos →
- Energía de ionización (4.ª)
- 49,160169 eV Comparar Energía de ionización (4.ª) de todos los elementos →
- Energía de ionización (5.ª)
- 69,460239 eV Comparar Energía de ionización (5.ª) de todos los elementos →
- Estados de oxidación
- −4, −2, −1, 0, +1, +2, +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
- [Ar] 3d5 4s1
Termodinámicas
- Calor de fusión
- 0,21246826 eV Comparar Calor de fusión de todos los elementos →
- Calor de vaporización
- 3,518682 eV Comparar Calor de vaporización de todos los elementos →
- Calor de sublimación
- 4,119811 eV
- Calor de atomización
- 4,119811 eV
- Entalpía de atomización
- 4,119604 eV
Nucleares
- Protones
- 24 Comparar Protones de todos los elementos →
- Neutrones
- 28 Comparar Neutrones de todos los elementos →
- Isótopos conocidos
- 30 Comparar Isótopos conocidos de todos los elementos →
- Isótopos estables
- 3 Comparar Isótopos estables de todos los elementos →
- Isótopo más estable
- Cr-52
- Año de descubrimiento
- 1797
Abundancia
- Abundancia (corteza terrestre)
- 102 mg/kg Comparar Abundancia (corteza terrestre) de todos los elementos →
- Abundancia (océano)
- 3 × 10−4 mg/L Comparar Abundancia (océano) de todos los elementos →
Estructura cristalina
- Constante de red a
- 288 pm
Estructura electrónica
- Electrones por capa
- 2, 8, 13, 1 Comparar Electrones por capa de todos los elementos →
Identificadores
- Número CAS
- 7440-47-3 Comparar Número CAS de todos los elementos →
- Símbolo del término
- 7S3
- InChI
- InChI=1S/Cr
- Clave InChI
- VYZAMTAEIAYCRO-UHFFFAOYSA-N
Configuración electrónica Medido
Cr: 3d⁵ 4s¹[Ar] 3d⁵ 4s¹1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹Modelo 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 |
|---|---|---|---|
| 52 Estable | 51,94050623 ± 0,00000063 | 83,7890% | Estable |
| 53 Estable | 52,94064815 ± 0,00000062 | 9,5010% | Estable |
| 54 Estable | 53,93887916 ± 0,00000061 | 2,3650% | Estable |
Fase / Estado
Motivo: 1881,8 °C por debajo del punto de fusión (1906,85 °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 24. Ordenado por carga del ion (ascendente).
Líneas disponibles ?
| Ion | Carga | Total de líneas | Probabilidades de transición | Designaciones de los niveles |
|---|---|---|---|---|
| Cr I | 0 | 4369 | 527 | 4369 |
| Cr II | +1 | 5370 | 92 | 5370 |
| Cr III | +2 | 136 | 0 | 0 |
| Cr IV | +3 | 188 | 102 | 102 |
| Cr V | +4 | 193 | 104 | 193 |
| Cr VI | +5 | 102 | 26 | 102 |
| Cr VII | +6 | 143 | 4 | 143 |
| Cr VIII | +7 | 36 | 9 | 36 |
| Cr IX | +8 | 58 | 18 | 58 |
| Cr X | +9 | 75 | 46 | 75 |
Niveles disponibles ?
| Ion | Carga | Niveles |
|---|---|---|
| Cr I | 0 | 659 |
| Cr II | +1 | 914 |
| Cr III | +2 | 215 |
| Cr IV | +3 | 155 |
| Cr V | +4 | 47 |
| Cr VI | +5 | 63 |
| Cr VII | +6 | 66 |
| Cr VIII | +7 | 34 |
| Cr IX | +8 | 49 |
| Cr X | +9 | 39 |
Radios iónicos
| Carga | Coordinación | Espín | Radio |
|---|---|---|---|
| +2 | 6 | low | 73 pm |
| +2 | 6 | high | 80 pm |
| +3 | 6 | N/D | 61.5 pm |
| +4 | 4 | N/D | 41 pm |
| +4 | 6 | N/D | 55.00000000000001 pm |
| +5 | 4 | N/D | 34.5 pm |
| +5 | 6 | N/D | 49 pm |
| +5 | 8 | N/D | 56.99999999999999 pm |
| +6 | 4 | N/D | 26 pm |
| +6 | 6 | N/D | 44 pm |
Compuestos
Isótopos (3)
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración | Modo de desintegración | |
|---|---|---|---|---|---|
| 52 Estable | 51,94050623 ± 0,00000063 | 83,7890% ± 0,0180% | Estable | stable | |
| 53 Estable | 52,94064815 ± 0,00000062 | 9,5010% ± 0,0170% | Estable | stable | |
| 54 Estable | 53,93887916 ± 0,00000061 | 2,3650% ± 0,0070% | Estable | stable |
Líneas espectrales
Se muestran 50 de 2531. De forma predeterminada, solo se muestran las líneas espectrales con intensidad medida.
| Longitud de onda (nm) | Intensidad | Estado de ionización | Tipo | Transición | Exactitud | Fuente | |
|---|---|---|---|---|---|---|---|
| 540.978408 nm | 8500 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 534.57965 nm | 5100 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 529.827202 nm | 3540 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 435.17622 nm | 3500 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 534.83147 nm | 3200 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 434.450128 nm | 3100 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 433.944609 nm | 2600 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 526.415341 nm | 2600 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 464.616212 nm | 2400 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 529.669109 nm | 2100 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 391.915844 nm | 2030 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 433.755701 nm | 1900 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 740.01798 nm | 1900 | Cr I | emission | 3d5.(6S).4p z 7P* → 3d5.(6S).5s e 7S | Medida | NIST | |
| 465.215743 nm | 1750 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 435.962444 nm | 1420 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 437.127465 nm | 1400 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 735.58903 nm | 1400 | Cr I | emission | 3d5.(6S).4p z 7P* → 3d5.(6S).5s e 7S | Medida | NIST | |
| 461.612404 nm | 1360 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 390.875593 nm | 1310 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 449.685195 nm | 1300 | Cr I | emission | 3d5.(6S).4s a 5S → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 524.756509 nm | 1250 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 460.074835 nm | 1190 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 433.971051 nm | 1120 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 462.617342 nm | 1100 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 435.104951 nm | 1080 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 438.4975 nm | 1060 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5F* | Medida | NIST | |
| 526.571497 nm | 1050 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 452.64538 nm | 960 | Cr I | emission | 3d5.(4G).4s a 5G → 3d5.(4G).4p z 5G* | Medida | NIST | |
| 454.595302 nm | 930 | Cr I | emission | 3d5.(6S).4s a 5S → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 532.832346 nm | 930 | Cr I | emission | 3d5.(6S).4p z 7P* → 3d5.(6S).4d e 7D | Medida | NIST | |
| 388.32867 nm | 910 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 392.86372 nm | 880 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 388.521354 nm | 810 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 746.23079 nm | 800 | Cr I | emission | 3d5.(6S).4p z 7P* → 3d5.(6S).5s e 7S | Medida | NIST | |
| 453.073802 nm | 770 | Cr I | emission | 3d5.(4G).4s a 5G → 3d5.(4G).4p z 5G* | Medida | NIST | |
| 388.679508 nm | 740 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 392.102067 nm | 740 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 394.148757 nm | 720 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 697.83983 nm | 640 | Cr I | emission | 3d4.(5D).4s.4p.(3P*) y 7P* → 3d5.(6S).4d e 7D | Medida | NIST | |
| 396.3684 nm | 620 | Cr I | emission | 3d5.(4G).4s a 5G → 3d5.(4G).4p y 5H* | Medida | NIST | |
| 453.569676 nm | 600 | Cr I | emission | 3d5.(4G).4s a 5G → 3d5.(4G).4p z 5G* | Medida | NIST | |
| 390.290908 nm | 590 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) z 5D* | Medida | NIST | |
| 455.864413 nm | 590 | Cr II | emission | 3d5 b 4F → 3d4.(5D).4p z 4D* | Medida | NIST | |
| 461.335727 nm | 590 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 396.974253 nm | 570 | Cr I | emission | 3d5.(4G).4s a 5G → 3d5.(4G).4p y 5H* | Medida | NIST | |
| 458.004789 nm | 560 | Cr I | emission | 3d5.(6S).4s a 5S → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST | |
| 530.074563 nm | 530 | Cr I | emission | 3d4.4s2 a 5D → 3d5.(6S).4p z 5P* | Medida | NIST | |
| 397.665859 nm | 520 | Cr I | emission | 3d5.(4G).4s a 5G → 3d5.(4G).4p y 5H* | Medida | NIST | |
| 454.04987 nm | 500 | Cr I | emission | 3d5.(4G).4s a 5G → 3d5.(4G).4p z 5G* | Medida | NIST | |
| 459.139098 nm | 490 | Cr I | emission | 3d4.4s2 a 5D → 3d4.(5D).4s.4p.(3P*) y 5P* | Medida | NIST |
Propiedades ampliadas
Radios covalentes (ampliados)
- Radio covalente (Pyykkö)
- 122 pm
- Radio covalente (Pyykkö, enlace doble)
- 111 pm
- Radio covalente (Pyykkö, enlace triple)
- 103 pm
- Radio covalente (Bragg)
- 140 pm
Radios de van der Waals
- Batsanov
- 205 pm
- Alvarez
- 245 pm
- UFF
- 302,3 pm
- MM3
- 225 pm
Radios atómicos y metálicos
- Radio atómico (Rahm)
- 233 pm
- Radio metálico (C12)
- 128 pm
Escalas de numeración
- Mendeleev
- 51
- Pettifor
- 57
- Glawe
- 55
Escalas de electronegatividad
- Ghosh
- 0
- Miedema
- 5
- Gunnarsson–Lundqvist
- 4
- Robles–Bartolotti
- 2
Polarizabilidad y dispersión
- Polarizabilidad dipolar
- 83 a.u.
- Polarizabilidad dipolar (incert.)
- 12 a.u.
- C₆
- 602 Ha·Bohr6
- C₆ (Gould–Bučko)
- 709 Ha·Bohr6
Afinidad química
- Afinidad protónica
- 791,3 kJ/mol
- Basicidad en fase gaseosa
- 768,4 kJ/mol
Parámetros de Miedema
- Volumen molar de Miedema
- 7,23 cm3/mol
- Densidad electrónica de Miedema
- 5
Riesgo de suministro y economía
- Concentración de la producción
- 37
- Riesgo relativo de suministro
- 6
- Distribución de las reservas
- 46
- Estabilidad política (principal productor)
- 44
- Estabilidad política (país con mayores reservas)
- 62
Transiciones de fase y alótropos
| Punto de fusión | 2180,15 K |
| Punto de ebullición | 2944,15 K |
Categorías de estados de oxidación
Datos de referencia avanzados
Constantes de apantallamiento (7)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0,5862 |
| 2 | p | 3,9248 |
| 2 | s | 7,0162 |
| 3 | d | 14,2434 |
| 3 | p | 12,534 |
| 3 | s | 11,6322 |
| 4 | s | 18,8668 |
Detalle de los radios cristalinos (10)
| Carga | CN | Espín | rcrystal (pm) | Origen |
|---|---|---|---|---|
| 2 | VI | LS | 87 | estimated, |
| 2 | VI | HS | 94 | from r^3 vs V plots, |
| 3 | VI | 75,5 | from r^3 vs V plots, | |
| 4 | IV | 55 | ||
| 4 | VI | 69 | from r^3 vs V plots, | |
| 5 | IV | 48,5 | from r^3 vs V plots, | |
| 5 | VI | 63 | estimated, from r^3 vs V plots, | |
| 5 | VIII | 71 | ||
| 6 | IV | 40 | ||
| 6 | VI | 58 | calculated, |
Modos de desintegración de los isótopos (52)
| Isótopo | Modo | Intensidad |
|---|---|---|
| 41 | p | — |
| 42 | B+ | 100% |
| 42 | B+p | 94,4% |
| 42 | 2p | — |
| 43 | B+ | 100% |
| 43 | B+p | 79,3% |
| 43 | 2p | 11,6% |
| 43 | 3p | 0,1% |
| 43 | B+A | — |
| 44 | B+ | 100% |
Factores de dispersión de rayos X (751)
| Energía (eV) | f₁ | f₂ |
|---|---|---|
| 0,42 | -0,0076 | 0,02756 |
| 0,46 | -0,01 | 0,03022 |
| 0,5 | -0,0123 | 0,03301 |
| 0,54 | -0,0148 | 0,03586 |
| 0,58 | -0,0176 | 0,03897 |
| 0,62 | -0,0202 | 0,04225 |
| 0,66 | -0,0225 | 0,04515 |
| 0,7 | -0,0257 | 0,04771 |
| 0,74 | -0,0292 | 0,05056 |
| 0,78 | -0,0332 | 0,05331 |
Datos adicionales
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
1.02×102 milligrams per kilogram
Referencias (1)
- [5] Chromium https://education.jlab.org/itselemental/ele024.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
3×10-4 milligrams per liter
Referencias (1)
- [5] Chromium https://education.jlab.org/itselemental/ele024.html
Sources
Sources of this element.
The principal ore is chromite, which is found in Zimbabwe, Russia, New Zealand, Turkey, Iran, Albania, Finland, Democratic Republic of Madagascar, and the Phillippines. The metal is usually produced by reducing the oxide with aluminum.
Referencias (1)
- [6] Chromium https://periodic.lanl.gov/24.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 Chromium.
The element property data was retrieved from publications.