Nitrogen (N)
nonmetalGas
Peso atómico estándar
14,007 u [14,00643, 14,00728]Configuración electrónica
2s2.2p3Punto de fusión
-210 °CPunto de ebullición
-195,79 °CDensidad
1,2506 kg/m³Estados de oxidación
−3, −2, −1, 0, +1, +2, +3, +4, +5Electronegatividad (Pauling)
3,04Energía de ionización (1.ª)
14,53413 eVAño de descubrimiento
1772Radio atómico
65 pmDetalles
Nitrogen is a light nonmetal and the main constituent of Earth’s atmosphere as N₂. Its strong N≡N triple bond makes the element relatively inert at ordinary conditions, yet nitrogen chemistry is exceptionally rich once that bond is broken. It is essential in amino acids, nucleic acids, and many cofactors, and industrial fixation of N₂ underpins modern fertilizer production. Nitrogen commonly forms covalent compounds and spans oxidation states from −3 to +5.
Colourless, gaseous element which belongs to group 15 of the periodic table. Constitutes ~78% of the atmosphere and is an essential part of the ecosystem. Nitrogen for industrial purposes is acquired by the fractional distillation of liquid air. Chemically inactive, reactive generally only at high temperatures or in electrical discharges. It was discovered in 1772 by D. Rutherford.
The name derives from the Latin nitrum and Greek nitron for "native soda" and genes for "forming". Nitrogen was discovered by the Scottish physician and chemist Daniel Rutherford in 1772.
Nitrogen was discovered by the Scottish physician Daniel Rutherford in 1772. It is the fifth most abundant element in the universe and makes up about 78% of the earth's atmosphere, which contains an estimated 4,000 trillion tons of the gas. Nitrogen is obtained from liquefied air through a process known as fractional distillation.
From the Latin word nitrum, Greek Nitron, native soda; and genes, forming. Nitrogen was discovered by chemist and physician Daniel Rutherford in 1772. He removed oxygen and carbon dioxide from air and showed that the residual gas would not support combustion or living organisms. At the same time there were other noted scientists working on the problem of nitrogen. These included Scheele, Cavendish, Priestley, and others. They called it "burnt" or" dephlogisticated air," which meant air without oxygen.
Pure nitrogen is normally encountered as N₂, a colorless, odorless, tasteless gas. Liquid nitrogen is a colorless, very cold fluid that boils at 77 K at one atmosphere. Solid nitrogen is also colorless and exists in several low-temperature phases.
Most industrial nitrogen is used either as N₂ for inerting and blanketing or as fixed nitrogen after conversion to ammonia (NH₃). Gaseous N₂ protects reactive materials, purges pipelines and tanks, and provides controlled atmospheres for food packaging, electronics processing, and metal heat treatment. Liquid nitrogen is widely used as a cryogenic refrigerant for biological storage, laboratory cooling, and rapid freezing. Nitrogen is also a feedstock for nitric acid (HNO₃), fertilizers, explosives, and many polymers and pharmaceuticals.
The largest use of nitrogen is for the production of ammonia (NH3). Large amounts of nitrogen are combined with hydrogen to produce ammonia in a method known as the Haber process. Large amounts of ammonia are then used to create fertilizers, explosives and, through a process known as the Ostwald process, nitric acid (HNO3).
Nitrogen gas is largely inert and is used as a protective shield in the semiconductor industry and during certain types of welding and soldering operations. Oil companies use high pressure nitrogen to help force crude oil to the surface. Liquid nitrogen is an inexpensive cryogenic liquid used for refrigeration, preservation of biological samples and for low temperature scientific experimentation. Jefferson Lab's Frostbite Theater features videos of many basic liquid nitrogen experiments.
Isotopes in Biology
Isotopic fractionation can cause the isotope-amount ratio n(15N)/n(14N) to increase systematically through food chains through assimilation of nitrogen compounds in biomolecules such as proteins. When lower-order organisms are ingested by higher-order organisms, 15N may be selectively retained and 14N may be selectively excreted such that higher-order organisms tend to have higher n(15N)/n(14N) ratios than their food sources. Isotopic fractionation occurs as a result of assimilation, storage, and excretion of proteins and other nitrogen compounds. Biologists can use isotope-amount ratio n(15N)/n(14N) measurements to test hypotheses about predator-prey relations and detect disruptions to trophic structure of ecosystems that might be caused by toxic contaminants, invasive species, or harvesting of organisms. Similar principles are used to detect differences in diets among animals, including humans, both today and in the distant past [79] P. L. Koch, M. L. Fogel, N. Tuross. “Tracing the diets of fossil animals using stable isotopes”, in Stable Isotopes in Ecology and Environmental Science, K. Lajtha and R. H. Michener (Eds.), Blackwell Scientific Publications, Boston (1994)., [80] J. P. Montoya. “Nitrogen isotope fractionation in the modern ocean: implications for the sedimentary record”, in Carbon Cycling in the Glacial Ocean: Constraints on the Ocean’s Role in Global Change. NATO ASI Series (Series I: Global Environmental Change), R. Zahn, T. F. Pedersen, M. A. Kaminski, L. Labeyrie (Eds.), vol. 17. Springer, Berlin, Heidelberg (1994)., [81] R. E. M. Hedges, L. M. Reynard. J. Archaeolog. Sci.34, 1240 (2007)..
Artificially enriched 15N tracers are used to study movement and transformation of nitrogen in biological and environmental systems, such as the uptake and loss of nitrogen fertilizers by crops (Fig. IUPAC.7.1). A common experiment involves introducing an isotopically labeled compound into the environment and then analyzing various samples taken from the environment for the presence of the enriched isotope to determine where the labeled compound moved and whether it transformed into other compounds (Fig. IUPAC.7.2). Artificially enriched 15N is used to study uptake and dispersal of nitrogen in feed supplies used in food production industries such as aquaculture [82] M. A. Burford, N. P. Preston, P. M. Glibert, W. C. Dennison. Aquaculture206, 199 (2002)..
Isotopes in Earth/Planetary Science
The stable isotopes of nitrogen are subject to isotopic fractionation by physical, chemical, and biological processes. Variations in the isotope-amount ratio n(15N)/n(14N) are substantial (Fig. IUPAC.7.3) and commonly are used to study Earth-system processes, especially those related to biology because nitrogen is a major nutrient for growth [84] Stable Isotopes in Ecology and Environmental Science: 2nd Edition, ed. R. Michener and K. Lajtha, p. 566, Blackwell Publishing Ltd., Malden, MA (2007).. For example, isotope fractionation occurs when dissolved solutes, such as nitrate (NO3 -), are transformed to more reduced compounds (i.e. nitrogen gas) because nitrate with higher 14N abundances tends to be more readily broken down. This leaves the residual unreacted nitrate with a higher n(15N)/n(14N) ratio than the initial ratio prior to reaction. Changes in the isotopic composition of biologically reactive compounds can be used to detect such reactions in aquatic environments, which are important mechanisms for removing reactive contaminants like nitrate [85] J. Granger, D. M. Sigman, M. F. Lehmann, P. D. Tortell. Limnol. Oceanogr.53, 2533 (2008)., [86] A. Mariotti, A. Landreau, B. Simon. Limnol. Oceanogr.52, 1869 (1988)..
Variations in the isotope-amount ratio n(15N)/n(14N) are used to determine sources of nitrogen contamination in the atmosphere, oceans, groundwater, and rivers, where the isotopic composition of a contaminant molecule preserves evidence of the nitrogen sources and processes involved in its creation. An example is nitrate derived from artificial fertilizer, manure, power-plant emissions, or natural sources [87] T. H. E. Heaton. Chem. Geol.59, 87 (1986)., [88] C. Kendall, R. Aravena. “Nitrate isotopes in groundwater systems”, in Environmental Tracers in Subsurface Hydrology, P. G. Cook and A. L. Herczeg (Eds.), Kluwer Academic Publishers, Boston (2000)., [89] B. Mayer, E. W. Boyer, C. Goodale, N. A. Jaworski, N. Van Breemen, R. W. Howarth, S. P. Seitzinger, G. Billen, K. Lajtha, K. J. Nadelhoffer, D. Van Dam, L. J. Hetling, M. Nosal, K. Paustian. Biogeochemistry57 & 58, 171 (2002)..
Artificially enriched 15N tracers have been used to determine rates of movement and natural remediation of nitrogen-bearing contaminants in aquifers and rivers [83] J. K. Böhlke, R. C. Antweiler, J. W. Harvey, A. E. Laursen, L. K. Smith, R. L. Smith, M. A. Voytek. Biogeochemistry93, 117 (2009)., [90] R. L. Smith, J. K. Böhlke, S. P. Garabedian, K. M. Revesz, T. Yoshinari. Water Resour. Res.40, 1 (2004)..
Isotopes in Forensic Science and Anthropology
Stable hydrogen, carbon, and nitrogen isotopic compositions are used to determine the origin of pseudoephedrine from seized methyl-amphetamine made from the pseudoephedrine (drug used as a nasal decongestant or as a stimulant) [91] H. Salouros, G. J. Sutton, J. Howes, D. B. Hibbert, M. Collins. Anal. Chem.85, 9400 (2013)..
Nitrogen forms many important compounds because it can make single, double, and triple bonds and adopt several oxidation states. Ammonia (NH₃) contains nitrogen in the −3 state and is both a base and a major industrial intermediate. Nitric acid (HNO₃), nitrate salts containing NO₃⁻, and nitrite salts containing NO₂⁻ are central to fertilizer, oxidation, and environmental chemistry. Nitrogen oxides such as nitric oxide (NO), nitrogen dioxide (NO₂), and nitrous oxide (N₂O) are chemically and atmospherically significant. Organic amines, amides, nitriles, azo compounds, and heterocycles form a large part of biological and synthetic chemistry.
Sodium nitrate (NaNO3) and potassium nitrate (KNO3) are formed by the decomposition of organic matter with compounds of these metals present. In certain dry areas of the world these saltpeters are found in quantity and are used as fertilizers. Other inorganic nitrogen compounds are nitric acid (HNO3), ammonia (NH3), the oxides (NO, NO2, N2O4, N2O), cyanides (CN-), etc.
The nitrogen cycle is one of the most important processes in nature for living organisms. Although nitrogen gas is relatively inert, bacteria in the soil are capable of “fixing” the nitrogen into a usable form (as a fertilizer) for plants. In other words, Nature has provided a method to produce nitrogen for plants to grow. Animals eat the plant material where the nitrogen has been incorporated into their system, primarily as protein. The cycle is completed when other bacteria convert the waste nitrogen compounds back to nitrogen gas. Nitrogen is crucial to life, as it is a component of all proteins.
See more information at the Nitrogen compound page.
N₂ is not toxic, but it is a serious asphyxiant because it can displace oxygen without warning by odor or irritation. Liquid nitrogen can cause severe cold burns and can rapidly generate large volumes of gas in confined spaces. Some nitrogen compounds are hazardous for unrelated reasons: ammonia (NH₃) is corrosive and irritating, nitric acid (HNO₃) is strongly corrosive and oxidizing, and nitrogen dioxide (NO₂) is a toxic inhalation hazard. Nitrate and nitrite exposure is regulated in drinking water and food contexts.
Atmospheric N₂ is a large reservoir, but most organisms cannot use it directly. Fixed nitrogen enters ecosystems through biological nitrogen fixation, lightning, industrial processes, and deposition from combustion-related nitrogen oxides. Microbial nitrification, denitrification, and anammox reactions return nitrogen among ammonium, nitrate, nitrite, nitrous oxide, and N₂. Excess reactive nitrogen can drive eutrophication, soil acidification, and formation of air pollutants, while nitrous oxide (N₂O) is a long-lived greenhouse gas.
Nitrogen gas is produced chiefly by cryogenic distillation of air, with pressure-swing adsorption and membrane separation used where lower purity or smaller-scale supply is sufficient. The largest economic value lies not in elemental N₂ itself but in nitrogen fixation, especially the Haber-Bosch synthesis of ammonia (NH₃) from N₂ and hydrogen. Fertilizer demand dominates fixed-nitrogen markets, followed by chemicals such as nitric acid (HNO₃) and urea (CO(NH₂)₂). Supply depends strongly on energy cost and hydrogen source; recycling occurs indirectly through manure management, wastewater treatment, and recovery or reuse of nitrogen-containing process streams.
Nitrogen gas (N2) makes up 78.1% of the Earth’s air, by volume. The atmosphere of Mars, by comparison, is only 2.6% nitrogen. From an exhaustible source in our atmosphere, nitrogen gas can be obtained by liquefaction and fractional distillation. Nitrogen is found in all living systems as part of the makeup of biological compounds.
Nitrogen is a common light element made mainly through stellar nucleosynthesis in the carbon-nitrogen-oxygen cycle and later stellar processing. In the Solar System it is concentrated in volatile reservoirs, including planetary atmospheres, ices, and organic material. Titan’s dense atmosphere is mostly N₂, and nitrogen-bearing ices and organics occur in comets and outer Solar System bodies.
- The strength of the N₂ triple bond is why air is chemically stable despite abundant oxygen.
- Liquid nitrogen expands greatly on warming, making sealed containers dangerous.
- Most nitrogen atoms in human tissue have passed through microbial or industrial fixation.
- Nitrous oxide (N₂O) is chemically distinct from the toxic brown gas nitrogen dioxide (NO₂).
- Nitrogen can form catenated compounds, but N–N single bonds are usually much weaker than the N≡N bond in N₂.
Imágenes
Propiedades
Físicas
- Radio atómico (empírico)
- 65 pm Comparar Radio atómico (empírico) de todos los elementos →
- Radio covalente
- 71 pm Comparar Radio covalente de todos los elementos →
- Radio de van der Waals
- 155 pm Comparar Radio de van der Waals de todos los elementos →
- Densidad
- 1,2506 kg/m³ Comparar Densidad de todos los elementos →
- Volumen molar
- 0,0173 L/mol
- Fase en CNPT
- Gas Comparar Fase en CNPT de todos los elementos →
- Punto de fusión
- -210 °C Comparar Punto de fusión de todos los elementos →
- Punto de ebullición
- -195,79 °C Comparar Punto de ebullición de todos los elementos →
- Conductividad térmica
- 0,026 W/(m·K) Comparar Conductividad térmica de todos los elementos →
- Capacidad calorífica específica
- 1,04 J/(g·K) Comparar Capacidad calorífica específica de todos los elementos →
- Capacidad calorífica molar
- 29,124 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)
- 3,04 Comparar Electronegatividad (Pauling) de todos los elementos →
- Electronegatividad (Allen)
- 3,066
- Afinidad electrónica
- -0,07 eV (valor negativo: se predice que el átomo no capta un electrón adicional)
- Energía de ionización (1.ª)
- 14,53413 eV Comparar Energía de ionización (1.ª) de todos los elementos →
- Energía de ionización (2.ª)
- 29,601352 eV Comparar Energía de ionización (2.ª) de todos los elementos →
- Energía de ionización (3.ª)
- 47,445463 eV Comparar Energía de ionización (3.ª) de todos los elementos →
- Energía de ionización (4.ª)
- 77,473767 eV Comparar Energía de ionización (4.ª) de todos los elementos →
- Energía de ionización (5.ª)
- 97,890437 eV Comparar Energía de ionización (5.ª) de todos los elementos →
- Estados de oxidación
- −3, −2, −1, 0, +1, +2, +3, +4, +5 Comparar Estados de oxidación de todos los elementos →
- Electrones de valencia
- 5 Comparar Electrones de valencia de todos los elementos →
- Configuración electrónica
- 2s2.2p3
Termodinámicas
- Punto triple (temperatura)
- -209,999 °C
- Punto triple (presión)
- 1,252e+4 Pa
- Punto crítico (temperatura)
- -146,958 °C
- Punto crítico (presión)
- 3,3958e+6 Pa
- Calor de fusión
- 0,00373115 eV Comparar Calor de fusión de todos los elementos →
- Calor de vaporización
- 0,05762554 eV Comparar Calor de vaporización de todos los elementos →
- Calor de atomización
- 4,899 eV
- Entalpía de atomización
- 4,896512 eV
Nucleares
- Protones
- 7 Comparar Protones de todos los elementos →
- Neutrones
- 7 Comparar Neutrones de todos los elementos →
- Isótopos conocidos
- 16 Comparar Isótopos conocidos de todos los elementos →
- Isótopos estables
- 2 Comparar Isótopos estables de todos los elementos →
- Isótopo más estable
- N-14
- Año de descubrimiento
- 1772
Abundancia
- Abundancia (corteza terrestre)
- 19 mg/kg Comparar Abundancia (corteza terrestre) de todos los elementos →
- Abundancia (océano)
- 0,5 mg/L Comparar Abundancia (océano) de todos los elementos →
Estructura cristalina
- Constante de red a
- 403,9 pm
Estructura electrónica
- Electrones por capa
- 2, 5 Comparar Electrones por capa de todos los elementos →
Identificadores
- Número CAS
- 7727-37-9 Comparar Número CAS de todos los elementos →
- Símbolo del término
- 4S°3/2
- InChI
- InChI=1S/N
- Clave InChI
- QJGQUHMNIGDVPM-UHFFFAOYSA-N
Configuración electrónica Medido
N: 2s² 2p³[He] 2s² 2p³1s² 2s² 2p³Modelo 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 |
|---|---|---|---|
| 14 Estable | 14,00307400443 ± 0,0000000002 | 99,6360% | Estable |
| 15 Estable | 15,00010889888 ± 0,00000000064 | 0,3640% | Estable |
Fase / Estado
Motivo: 220,8 °C por encima del punto de ebullición (-195,79 °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
Densidad
En condiciones estándar
Estimada mediante la ley de los gases ideales a la T actual
Avanzado
Espectros atómicos
Líneas disponibles ?
| Ion | Carga | Total de líneas | Probabilidades de transición | Designaciones de los niveles |
|---|---|---|---|---|
| N I | 0 | 1309 | 1287 | 1287 |
| N II | +1 | 809 | 786 | 786 |
| N III | +2 | 1378 | 1359 | 1359 |
| N IV | +3 | 536 | 531 | 531 |
| N V | +4 | 442 | 402 | 433 |
| N VI | +5 | 91 | 90 | 91 |
| N VII | +6 | 137 | 137 | 137 |
Niveles disponibles ?
| Ion | Carga | Niveles |
|---|---|---|
| N I | 0 | 381 |
| N II | +1 | 197 |
| N III | +2 | 347 |
| N IV | +3 | 292 |
| N V | +4 | 151 |
| N VI | +5 | 148 |
| N VII | +6 | 149 |
Radios iónicos
| Carga | Coordinación | Espín | Radio |
|---|---|---|---|
| -3 | 4 | N/D | 146 pm |
| +3 | 6 | N/D | 16 pm |
| +5 | 6 | N/D | 13 pm |
Compuestos
Isótopos (2)
| Número másico | Masa atómica (u) | Abundancia natural | Periodo de semidesintegración | Modo de desintegración | |
|---|---|---|---|---|---|
| 14 Estable | 14,00307400443 ± 0,0000000002 | 99,6360% ± 0,0200% | Estable | stable | |
| 15 Estable | 15,00010889888 ± 0,00000000064 | 0,3640% ± 0,0200% | Estable | stable |
Líneas espectrales
Se muestran 50 de 731. De forma predeterminada, solo se muestran las líneas espectrales con intensidad medida.
| Longitud de onda (nm) | Intensidad | Estado de ionización | Tipo | Transición | Exactitud | Fuente | |
|---|---|---|---|---|---|---|---|
| 399.4997 nm | 1000 | N II | emission | 2s2.2p.3s 1P* → 2s2.2p.3p 1D | Medida | NIST | |
| 746.8312 nm | 900 | N I | emission | 2s2.2p2.(3P).3s 4P → 2s2.2p2.(3P).3p 4S* | Medida | NIST | |
| 463.0539 nm | 870 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Medida | NIST | |
| 500.515 nm | 870 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Medida | NIST | |
| 567.956 nm | 870 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Medida | NIST | |
| 744.2298 nm | 785 | N I | emission | 2s2.2p2.(3P).3s 4P → 2s2.2p2.(3P).3p 4S* | Medida | NIST | |
| 648.205 nm | 750 | N II | emission | 2s2.2p.3s 1P* → 2s2.2p.3p 1P | Medida | NIST | |
| 661.056 nm | 750 | N II | emission | 2s2.2p.3p 1D → 2s2.2p.3d 1F* | Medida | NIST | |
| 575.2499 nm | 700 | N I | emission | 2s2.2p2.(3P).3p 4P* → 2s2.2p2.(3P).5d 4D | Medida | NIST | |
| 742.3641 nm | 685 | N I | emission | 2s2.2p2.(3P).3s 4P → 2s2.2p2.(3P).3p 4S* | Medida | NIST | |
| 444.703 nm | 650 | N II | emission | 2s2.2p.3p 1P → 2s2.2p.3d 1D* | Medida | NIST | |
| 500.1474 nm | 650 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Medida | NIST | |
| 566.663 nm | 650 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Medida | NIST | |
| 594.165 nm | 650 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Medida | NIST | |
| 460.1478 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Medida | NIST | |
| 464.3086 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Medida | NIST | |
| 500.7328 nm | 550 | N II | emission | 2s2.2p.3p 3S → 2s2.2p.3d 3P* | Medida | NIST | |
| 504.5099 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3S | Medida | NIST | |
| 567.602 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Medida | NIST | |
| 593.178 nm | 550 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Medida | NIST | |
| 395.5851 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 1D | Medida | NIST | |
| 460.7153 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Medida | NIST | |
| 462.1393 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Medida | NIST | |
| 480.3287 nm | 450 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3D* | Medida | NIST | |
| 499.436 nm | 450 | N II | emission | 2s.2p2.(4P).3s 5P → 2s.2p2.(4P).3p 5P* | Medida | NIST | |
| 501.0621 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3S | Medida | NIST | |
| 549.5655 nm | 450 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3P* | Medida | NIST | |
| 568.621 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Medida | NIST | |
| 571.077 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Medida | NIST | |
| 391.9001 nm | 360 | N II | emission | 2s2.2p.3p 1P → 2s2.2p.3d 1P* | Medida | NIST | |
| 461.3868 nm | 360 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Medida | NIST | |
| 500.2703 nm | 360 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3S | Medida | NIST | |
| 501.6381 nm | 360 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Medida | NIST | |
| 502.5659 nm | 360 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Medida | NIST | |
| 592.781 nm | 360 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Medida | NIST | |
| 637.962 nm | 360 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 1P | Medida | NIST | |
| 648.2699 nm | 360 | N I | emission | 2s2.2p2.(3P).3p 4D* → 2s2.2p2.(3P).4d 4F | Medida | NIST | |
| 460.374 nm | 350 | N V | emission | 1s2.3s 2S → 1s2.3p 2P* | Medida | NIST | |
| 648.4808 nm | 325 | N I | emission | 2s2.2p2.(3P).3p 4D* → 2s2.2p2.(3P).4d 4F | Medida | NIST | |
| 648.3753 nm | 300 | N I | emission | 2s2.2p2.(3P).3p 4D* → 2s2.2p2.(3P).4d 4F | Medida | NIST | |
| 383.8374 nm | 285 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.4s 3P* | Medida | NIST | |
| 422.7736 nm | 285 | N II | emission | 2s2.2p.3p 1D → 2s2.2p.4s 1P* | Medida | NIST | |
| 478.8138 nm | 285 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3D* | Medida | NIST | |
| 489.5117 nm | 285 | N II | emission | 2s.2p3 1D* → 2s2.2p.3p 1P | Medida | NIST | |
| 498.7376 nm | 285 | N II | emission | 2s2.2p.3p 3S → 2s2.2p.3d 3P* | Medida | NIST | |
| 553.5347 nm | 285 | N II | emission | 2s.2p2.(4P).3s 5P → 2s.2p2.(4P).3p 5D* | Medida | NIST | |
| 574.73 nm | 285 | N II | emission | 2s2.2p.3s 1P* → 2s2.2p.3p 3D | Medida | NIST | |
| 594.024 nm | 285 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Medida | NIST | |
| 595.239 nm | 285 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Medida | NIST | |
| 616.775 nm | 285 | N II | emission | 2s2.2p.3d 3F* → 2s2.2p.4p 3D | Medida | NIST |
Propiedades ampliadas
Radios covalentes (ampliados)
- Radio covalente (Pyykkö)
- 71 pm
- Radio covalente (Pyykkö, enlace doble)
- 60 pm
- Radio covalente (Pyykkö, enlace triple)
- 54 pm
- Radio covalente (Bragg)
- 65 pm
Radios de van der Waals
- Bondi
- 155 pm
- Batsanov
- 160 pm
- Alvarez
- 166 pm
- UFF
- 366 pm
- MM3
- 193 pm
- Dreiding
- 366,21 pm
- Rowland–Taylor
- 164 pm
Radios atómicos y metálicos
- Radio atómico (Rahm)
- 179 pm
- Radio metálico (C12)
- 53 pm
Escalas de numeración
- Mendeleev
- 93
- Pettifor
- 100
- Glawe
- 88
Escalas de electronegatividad
- Ghosh
- 0
- Miedema
- 7
- Gunnarsson–Lundqvist
- 7
- Robles–Bartolotti
- 6
Polarizabilidad y dispersión
- Polarizabilidad dipolar
- 7,4 a.u.
- Polarizabilidad dipolar (incert.)
- 0,2 a.u.
- C₆
- 24,2 Ha·Bohr6
- C₆ (Gould–Bučko)
- 25,7 Ha·Bohr6
Afinidad química
- Afinidad protónica
- 342,2 kJ/mol
- Basicidad en fase gaseosa
- 318,7 kJ/mol
Parámetros de Miedema
- Volumen molar de Miedema
- 4,1 cm3/mol
- Densidad electrónica de Miedema
- 4
Transiciones de fase y alótropos
| Punto de fusión | 63,15 K |
| Punto de ebullición | 77,35 K |
| Punto crítico (temperatura) | 126,19 K |
| Punto crítico (presión) | 3,4 MPa |
| Punto triple (temperatura) | 63,15 K |
| Punto triple (presión) | 12,52 kPa |
Categorías de estados de oxidación
Datos de referencia avanzados
Constantes de apantallamiento (3)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0,3349 |
| 2 | p | 3,166 |
| 2 | s | 3,1526 |
Detalle de los radios cristalinos (4)
| Carga | CN | Espín | rcrystal (pm) | Origen |
|---|---|---|---|---|
| -3 | IV | 132 | ||
| 3 | VI | 30 | Ahrens (1952) ionic radius, | |
| 5 | III | 4,4 | ||
| 5 | VI | 27 | Ahrens (1952) ionic radius, |
Modos de desintegración de los isótopos (33)
| Isótopo | Modo | Intensidad |
|---|---|---|
| 10 | p | — |
| 11 | p | 100% |
| 12 | B+ | 100% |
| 12 | B+A | 1,9% |
| 13 | B+ | 100% |
| 16 | B- | 100% |
| 16 | B-A | 0% |
| 17 | B- | 100% |
| 17 | B-n | 95,1% |
| 17 | B-A | 0% |
Factores de dispersión de rayos X (503)
| Energía (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 0,67785 |
| 10,1617 | — | 0,68963 |
| 10,3261 | — | 0,70162 |
| 10,4931 | — | 0,71382 |
| 10,6628 | — | 0,72623 |
| 10,8353 | — | 0,73885 |
| 11,0106 | — | 0,7517 |
| 11,1886 | — | 0,76584 |
| 11,3696 | — | 0,78603 |
| 11,5535 | — | 0,80674 |
Datos adicionales
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
1.9×101 milligrams per kilogram
Referencias (1)
- [5] Nitrogen https://education.jlab.org/itselemental/ele007.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
5×10-1 milligrams per liter
Referencias (1)
- [5] Nitrogen https://education.jlab.org/itselemental/ele007.html
Sources
Sources of this element.
Nitrogen gas (N2) makes up 78.1% of the Earth’s air, by volume. The atmosphere of Mars, by comparison, is only 2.6% nitrogen. From an exhaustible source in our atmosphere, nitrogen gas can be obtained by liquefaction and fractional distillation. Nitrogen is found in all living systems as part of the makeup of biological compounds.
Referencias (1)
- [6] Nitrogen https://periodic.lanl.gov/7.shtml
Isotopes in Forensic Science and Anthropology
Information on the use of this element's isotopes in forensic science and anthropology.
Stable hydrogen, carbon, and nitrogen isotopic compositions are used to determine the origin of pseudoephedrine from seized methyl-amphetamine made from the pseudoephedrine (drug used as a nasal decongestant or as a stimulant) [91] H. Salouros, G. J. Sutton, J. Howes, D. B. Hibbert, M. Collins. Anal. Chem.85, 9400 (2013)..
Referencias (2)
- [91] H. Salouros, G. J. Sutton, J. Howes, D. B. Hibbert, M. Collins. Anal. Chem.85, 9400 (2013).
- [4] IUPAC Periodic Table of the Elements and Isotopes (IPTEI) https://doi.org/10.1515/pac-2015-0703
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 Nitrogen.
The element property data was retrieved from publications.