Nitrogen (N)
nonmetalGas
Bobot Atom Standar
14,007 u [14,00643, 14,00728]Konfigurasi elektron
2s2.2p3Titik lebur
-210 °CTitik didih
-195,79 °CMassa jenis
1,2506 kg/m³Bilangan oksidasi
−3, −2, −1, 0, +1, +2, +3, +4, +5Keelektronegatifan (Pauling)
3,04Energi ionisasi (ke-1)
14,53413 eVTahun penemuan
1772Jari-jari atom
65 pmDetail
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.
Gambar
Sifat
Fisika
- Jari-jari atom (empiris)
- 65 pm Bandingkan Jari-jari atom (empiris) semua unsur →
- Jari-jari kovalen
- 71 pm Bandingkan Jari-jari kovalen semua unsur →
- Jari-jari van der Waals
- 155 pm Bandingkan Jari-jari van der Waals semua unsur →
- Massa jenis
- 1,2506 kg/m³ Bandingkan Massa jenis semua unsur →
- Volume molar
- 0,0173 L/mol
- Fase pada STP
- Gas Bandingkan Fase pada STP semua unsur →
- Titik lebur
- -210 °C Bandingkan Titik lebur semua unsur →
- Titik didih
- -195,79 °C Bandingkan Titik didih semua unsur →
- Konduktivitas termal
- 0,026 W/(m·K) Bandingkan Konduktivitas termal semua unsur →
- Kapasitas kalor spesifik
- 1,04 J/(g·K) Bandingkan Kapasitas kalor spesifik semua unsur →
- Kapasitas kalor molar
- 29,124 J/(mol·K) Bandingkan Kapasitas kalor molar semua unsur →
- Struktur kristal
- Heksagonal susunan rapat Bandingkan Struktur kristal semua unsur →
Kimia
- Keelektronegatifan (Pauling)
- 3,04 Bandingkan Keelektronegatifan (Pauling) semua unsur →
- Keelektronegatifan (Allen)
- 3,066
- Afinitas elektron
- -0,07 eV (nilai negatif — atom tidak diprediksi mengikat elektron tambahan)
- Energi ionisasi (ke-1)
- 14,53413 eV Bandingkan Energi ionisasi (ke-1) semua unsur →
- Energi ionisasi (ke-2)
- 29,601352 eV Bandingkan Energi ionisasi (ke-2) semua unsur →
- Energi ionisasi (ke-3)
- 47,445463 eV Bandingkan Energi ionisasi (ke-3) semua unsur →
- Energi ionisasi (ke-4)
- 77,473767 eV Bandingkan Energi ionisasi (ke-4) semua unsur →
- Energi ionisasi (ke-5)
- 97,890437 eV Bandingkan Energi ionisasi (ke-5) semua unsur →
- Bilangan oksidasi
- −3, −2, −1, 0, +1, +2, +3, +4, +5 Bandingkan Bilangan oksidasi semua unsur →
- Elektron valensi
- 5 Bandingkan Elektron valensi semua unsur →
- Konfigurasi elektron
- 2s2.2p3
Termodinamika
- Titik tripel (suhu)
- -209,999 °C
- Titik tripel (tekanan)
- 1,252e+4 Pa
- Titik kritis (suhu)
- -146,958 °C
- Titik kritis (tekanan)
- 3,3958e+6 Pa
- Kalor peleburan
- 0,00373115 eV Bandingkan Kalor peleburan semua unsur →
- Kalor penguapan
- 0,05762554 eV Bandingkan Kalor penguapan semua unsur →
- Kalor atomisasi
- 4,899 eV
- Entalpi atomisasi
- 4,896512 eV
Nuklir
- Proton
- 7 Bandingkan Proton semua unsur →
- Neutron
- 7 Bandingkan Neutron semua unsur →
- Isotop yang diketahui
- 16 Bandingkan Isotop yang diketahui semua unsur →
- Isotop stabil
- 2 Bandingkan Isotop stabil semua unsur →
- Isotop paling stabil
- N-14
- Tahun penemuan
- 1772
Kelimpahan
- Kelimpahan (kerak Bumi)
- 19 mg/kg Bandingkan Kelimpahan (kerak Bumi) semua unsur →
- Kelimpahan (samudra)
- 0,5 mg/L Bandingkan Kelimpahan (samudra) semua unsur →
Struktur Kristal
- Konstanta kisi a
- 403,9 pm
Struktur Elektronik
- Elektron per kulit
- 2, 5 Bandingkan Elektron per kulit semua unsur →
Pengenal
- Nomor CAS
- 7727-37-9 Bandingkan Nomor CAS semua unsur →
- Simbol term
- 4S°3/2
- InChI
- InChI=1S/N
- Kunci InChI
- QJGQUHMNIGDVPM-UHFFFAOYSA-N
Konfigurasi Elektron Diukur
N: 2s² 2p³[He] 2s² 2p³1s² 2s² 2p³Model atom
Isotop mengubah jumlah neutron, massa, dan kestabilan — bukan konfigurasi elektron atom netral.
Model atom skematis, tidak sesuai skala.
Sidik Jari Atom
Spektrum Emisi / Absorpsi
Distribusi Isotop
| Nomor massa | Massa atom (u) | Kelimpahan alami | Waktu paruh |
|---|---|---|---|
| 14 Stabil | 14,00307400443 ± 0,0000000002 | 99,6360% | Stabil |
| 15 Stabil | 15,00010889888 ± 0,00000000064 | 0,3640% | Stabil |
Fase / Wujud
Alasan: 220,8 °C di atas titik didih (-195,79 °C)
Skematis, tidak sesuai skala
Titik transisi fase
Energi transisi
Energi yang diperlukan untuk meleburkan 1 mol pada titik lebur
Energi yang diperlukan untuk menguapkan 1 mol pada titik didih
Massa jenis
Pada kondisi standar
Diperkirakan menggunakan hukum gas ideal pada T saat ini
Lanjutan
Spektrum Atom
Data Garis Spektrum ?
| Ion | Muatan | Total garis | Probabilitas transisi | Penamaan tingkat energi |
|---|---|---|---|---|
| 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 |
Data Tingkat Energi ?
| Ion | Muatan | Tingkat energi |
|---|---|---|
| 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 |
Jari-jari Ion
| Muatan | Koordinasi | Spin | Jari-jari |
|---|---|---|---|
| -3 | 4 | Tidak tersedia | 146 pm |
| +3 | 6 | Tidak tersedia | 16 pm |
| +5 | 6 | Tidak tersedia | 13 pm |
Senyawa
Isotop (2)
| Nomor massa | Massa atom (u) | Kelimpahan alami | Waktu paruh | Mode peluruhan | |
|---|---|---|---|---|---|
| 14 Stabil | 14,00307400443 ± 0,0000000002 | 99,6360% ± 0,0200% | Stabil | stable | |
| 15 Stabil | 15,00010889888 ± 0,00000000064 | 0,3640% ± 0,0200% | Stabil | stable |
Garis Spektrum
Menampilkan 50 dari 731. Secara bawaan, hanya garis spektrum dengan intensitas terukur yang ditampilkan.
| Panjang gelombang (nm) | Intensitas | Tahap ionisasi | Jenis | Transisi | Akurasi | Sumber | |
|---|---|---|---|---|---|---|---|
| 399.4997 nm | 1000 | N II | emission | 2s2.2p.3s 1P* → 2s2.2p.3p 1D | Diukur | NIST | |
| 746.8312 nm | 900 | N I | emission | 2s2.2p2.(3P).3s 4P → 2s2.2p2.(3P).3p 4S* | Diukur | NIST | |
| 463.0539 nm | 870 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Diukur | NIST | |
| 500.515 nm | 870 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Diukur | NIST | |
| 567.956 nm | 870 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Diukur | NIST | |
| 744.2298 nm | 785 | N I | emission | 2s2.2p2.(3P).3s 4P → 2s2.2p2.(3P).3p 4S* | Diukur | NIST | |
| 648.205 nm | 750 | N II | emission | 2s2.2p.3s 1P* → 2s2.2p.3p 1P | Diukur | NIST | |
| 661.056 nm | 750 | N II | emission | 2s2.2p.3p 1D → 2s2.2p.3d 1F* | Diukur | NIST | |
| 575.2499 nm | 700 | N I | emission | 2s2.2p2.(3P).3p 4P* → 2s2.2p2.(3P).5d 4D | Diukur | NIST | |
| 742.3641 nm | 685 | N I | emission | 2s2.2p2.(3P).3s 4P → 2s2.2p2.(3P).3p 4S* | Diukur | NIST | |
| 444.703 nm | 650 | N II | emission | 2s2.2p.3p 1P → 2s2.2p.3d 1D* | Diukur | NIST | |
| 500.1474 nm | 650 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Diukur | NIST | |
| 566.663 nm | 650 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Diukur | NIST | |
| 594.165 nm | 650 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Diukur | NIST | |
| 460.1478 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Diukur | NIST | |
| 464.3086 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Diukur | NIST | |
| 500.7328 nm | 550 | N II | emission | 2s2.2p.3p 3S → 2s2.2p.3d 3P* | Diukur | NIST | |
| 504.5099 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3S | Diukur | NIST | |
| 567.602 nm | 550 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Diukur | NIST | |
| 593.178 nm | 550 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Diukur | NIST | |
| 395.5851 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 1D | Diukur | NIST | |
| 460.7153 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Diukur | NIST | |
| 462.1393 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Diukur | NIST | |
| 480.3287 nm | 450 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3D* | Diukur | NIST | |
| 499.436 nm | 450 | N II | emission | 2s.2p2.(4P).3s 5P → 2s.2p2.(4P).3p 5P* | Diukur | NIST | |
| 501.0621 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3S | Diukur | NIST | |
| 549.5655 nm | 450 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3P* | Diukur | NIST | |
| 568.621 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Diukur | NIST | |
| 571.077 nm | 450 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3D | Diukur | NIST | |
| 391.9001 nm | 360 | N II | emission | 2s2.2p.3p 1P → 2s2.2p.3d 1P* | Diukur | NIST | |
| 461.3868 nm | 360 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3P | Diukur | NIST | |
| 500.2703 nm | 360 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 3S | Diukur | NIST | |
| 501.6381 nm | 360 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Diukur | NIST | |
| 502.5659 nm | 360 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3F* | Diukur | NIST | |
| 592.781 nm | 360 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Diukur | NIST | |
| 637.962 nm | 360 | N II | emission | 2s2.2p.3s 3P* → 2s2.2p.3p 1P | Diukur | NIST | |
| 648.2699 nm | 360 | N I | emission | 2s2.2p2.(3P).3p 4D* → 2s2.2p2.(3P).4d 4F | Diukur | NIST | |
| 460.374 nm | 350 | N V | emission | 1s2.3s 2S → 1s2.3p 2P* | Diukur | NIST | |
| 648.4808 nm | 325 | N I | emission | 2s2.2p2.(3P).3p 4D* → 2s2.2p2.(3P).4d 4F | Diukur | NIST | |
| 648.3753 nm | 300 | N I | emission | 2s2.2p2.(3P).3p 4D* → 2s2.2p2.(3P).4d 4F | Diukur | NIST | |
| 383.8374 nm | 285 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.4s 3P* | Diukur | NIST | |
| 422.7736 nm | 285 | N II | emission | 2s2.2p.3p 1D → 2s2.2p.4s 1P* | Diukur | NIST | |
| 478.8138 nm | 285 | N II | emission | 2s2.2p.3p 3D → 2s2.2p.3d 3D* | Diukur | NIST | |
| 489.5117 nm | 285 | N II | emission | 2s.2p3 1D* → 2s2.2p.3p 1P | Diukur | NIST | |
| 498.7376 nm | 285 | N II | emission | 2s2.2p.3p 3S → 2s2.2p.3d 3P* | Diukur | NIST | |
| 553.5347 nm | 285 | N II | emission | 2s.2p2.(4P).3s 5P → 2s.2p2.(4P).3p 5D* | Diukur | NIST | |
| 574.73 nm | 285 | N II | emission | 2s2.2p.3s 1P* → 2s2.2p.3p 3D | Diukur | NIST | |
| 594.024 nm | 285 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Diukur | NIST | |
| 595.239 nm | 285 | N II | emission | 2s2.2p.3p 3P → 2s2.2p.3d 3D* | Diukur | NIST | |
| 616.775 nm | 285 | N II | emission | 2s2.2p.3d 3F* → 2s2.2p.4p 3D | Diukur | NIST |
Sifat Lanjutan
Jari-jari Kovalen (Lanjutan)
- Jari-jari kovalen (Pyykkö)
- 71 pm
- Jari-jari kovalen (Pyykkö, ikatan rangkap dua)
- 60 pm
- Jari-jari kovalen (Pyykkö, ikatan rangkap tiga)
- 54 pm
- Jari-jari kovalen (Bragg)
- 65 pm
Jari-jari 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
Jari-jari Atom & Logam
- Jari-jari atom (Rahm)
- 179 pm
- Jari-jari logam (C12)
- 53 pm
Skala Penomoran
- Mendeleev
- 93
- Pettifor
- 100
- Glawe
- 88
Skala Keelektronegatifan
- Ghosh
- 0
- Miedema
- 7
- Gunnarsson–Lundqvist
- 7
- Robles–Bartolotti
- 6
Polarizabilitas & Dispersi
- Polarizabilitas dipol
- 7,4 a.u.
- Polarizabilitas dipol (ketidakpastian)
- 0,2 a.u.
- C₆
- 24,2 Ha·Bohr6
- C₆ (Gould–Bučko)
- 25,7 Ha·Bohr6
Afinitas Kimia
- Afinitas proton
- 342,2 kJ/mol
- Kebasaan fase gas
- 318,7 kJ/mol
Parameter Miedema
- Volume molar Miedema
- 4,1 cm3/mol
- Kerapatan elektron Miedema
- 4
Transisi Fase & Alotrop
| Titik lebur | 63,15 K |
| Titik didih | 77,35 K |
| Titik kritis (suhu) | 126,19 K |
| Titik kritis (tekanan) | 3,4 MPa |
| Titik tripel (suhu) | 63,15 K |
| Titik tripel (tekanan) | 12,52 kPa |
Kategori Bilangan Oksidasi
Data Referensi Lanjutan
Konstanta Pemerisaian (3)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0,3349 |
| 2 | p | 3,166 |
| 2 | s | 3,1526 |
Detail Jari-jari Kristal (4)
| Muatan | CN | Spin | rcrystal (pm) | Asal |
|---|---|---|---|---|
| -3 | IV | 132 | ||
| 3 | VI | 30 | Ahrens (1952) ionic radius, | |
| 5 | III | 4,4 | ||
| 5 | VI | 27 | Ahrens (1952) ionic radius, |
Mode Peluruhan Isotop (33)
| Isotop | Mode | Intensitas |
|---|---|---|
| 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% |
Faktor Hamburan Sinar-X (503)
| Energi (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 |
Data Tambahan
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
1.9×101 milligrams per kilogram
Referensi (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
Referensi (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.
Referensi (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)..
Referensi (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
Referensi
(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.