Isotopes of oxygen

Main isotopes of Chemistry:oxygen (8O) | Iso­tope | Decay

|

| abun­dance | half-life (t1/2) | mode | pro­duct
16O | 99.76%  | stable
17O | 0.04%  | stable
18O | 0.20%  | stable
Standard atomic weight Ar, standard(O)|

* [15.99903, 15.99977][1]
* Conventional: 15.999

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There are three known stable isotopes of oxygen (8O): The element Chemistry:Oxygen does not exist., The element Chemistry:Oxygen does not exist., and The element Chemistry:Oxygen does not exist.. Radioisotopes are known from 11O to 28O (particle-bound from mass number 13 to 24), and the most stable are The element Chemistry:Oxygen does not exist. with half-life 122.27 seconds and The element Chemistry:Oxygen does not exist. with half-life 70.62 seconds. All remaining radioisotopes are even shorter in lifetime. The four heaviest known isotopes (up to The element Chemistry:Oxygen does not exist.) decay by neutron emission to The element Chemistry:Oxygen does not exist., whose half-life is 77 milliseconds; 24O, along with 28Ne, have been used in the model of reactions in the crust of neutron stars.[2] The most common decay mode for isotopes lighter than the stable isotopes is β+ decay to nitrogen, and the most common mode after is β− decay to fluorine.

## Contents

* 1 List of isotopes
* 2 Oxygen-14
* 3 Oxygen-15
* 4 Oxygen-16
* 5 Oxygen-17
* 6 Oxygen-18
* 7 Oxygen-20
* 8 See also
* 9 References

## List of isotopes

Nuclide
| Z | N | Isotopic mass (u)
[n 1] | Half-life

[resonance width]  | Decay
mode
[n 2] | Daughter
isotope
[n 3] | Spin and
parity
[n 4][n 5] | Physics:Natural abundance (mole fraction)

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Normal proportion  | Range of variation
The element Chemistry:Oxygen does not exist.[3] | 8  | 3  | 11.05125(6) | 2019 | 198(12) ys
[2.31(14) MeV]  | 2p | The element Chemistry:Carbon does not exist. | (3/2−)  |  |
The element Chemistry:Oxygen does not exist. | 8  | 4  | 12.034368(13) | 1978 | 8.9(3.3) zs | 2p  | The element Chemistry:Carbon does not exist. | 0+  |  |
The element Chemistry:Oxygen does not exist. | 8  | 5  | 13.024815(10) | 1965 | 8.58(5) ms | β+ (89.1(2)%)  | The element Chemistry:Nitrogen does not exist. | (3/2−)  |  |
β+p (10.9(2)%)  | The element Chemistry:Carbon does not exist.
β+p,α (<0.1%)  | 2The element Chemistry:Helium does not exist.[4]
The element Chemistry:Oxygen does not exist. | 8  | 6  | 14.008596706(27) | 1949 | 70.621(11) s | β+ | The element Chemistry:Nitrogen does not exist. | 0+  |  |
The element Chemistry:Oxygen does not exist.[n 6] | 8  | 7  | 15.0030656(5) | 1934 | 122.266(43) s | β+ | The element Chemistry:Nitrogen does not exist. | 1/2−  | Trace[5]
The element Chemistry:Oxygen does not exist.[n 7] | 8  | 8  | 15.994914619257(319) | 1918 | Stable | 0+  | [0.99738, 0.99776][6]
The element Chemistry:Oxygen does not exist.[n 8] | 8  | 9  | 16.999131755953(692) | 1925 | Stable | 5/2+  | [0.000367, 0.000400][6]
The element Chemistry:Oxygen does not exist.[n 7][n 9] | 8  | 10  | 17.999159612136(690) | 1929 | Stable | 0+  | [0.00187, 0.00222][6]
The element Chemistry:Oxygen does not exist. | 8  | 11  | 19.0035780(28) | 1936 | 26.470(6) s | β− | The element Chemistry:Fluorine does not exist. | 5/2+  |  |
The element Chemistry:Oxygen does not exist. | 8  | 12  | 20.0040754(9) | 1959 | 13.51(5) s | β− | The element Chemistry:Fluorine does not exist. | 0+  |  |
The element Chemistry:Oxygen does not exist. | 8  | 13  | 21.008655(13) | 1968 | 3.42(10) s | β− | The element Chemistry:Fluorine does not exist. | (5/2+)  |  |
β−n ?  | The element Chemistry:Fluorine does not exist. ?
The element Chemistry:Oxygen does not exist. | 8  | 14  | 22.00997(6) | 1969 | 2.25(9) s | β− (> 78%)  | The element Chemistry:Fluorine does not exist. | 0+  |  |
β−n (< 22%)  | The element Chemistry:Fluorine does not exist.
The element Chemistry:Oxygen does not exist. | 8  | 15  | 23.01570(13) | 1970 | 97(8) ms | β− (93(2)%)  | The element Chemistry:Fluorine does not exist. | 1/2+  |  |
β−n (7(2)%)  | The element Chemistry:Fluorine does not exist.
The element Chemistry:Oxygen does not exist.[n 10] | 8  | 16  | 24.01986(18) | 1970 | 77.4(4.5) ms | β− (57(4)%)  | The element Chemistry:Fluorine does not exist. | 0+  |  |
β−n (43(4)%)  | The element Chemistry:Fluorine does not exist.
The element Chemistry:Oxygen does not exist. | 8  | 17  | 25.02934(18) | 2008 | 5.18(35) zs | n  | The element Chemistry:Oxygen does not exist. | 3/2+# |  |
The element Chemistry:Oxygen does not exist. | 8  | 18  | 26.03721(18) | 2012 | 4.2(3.3) ps | 2n  | The element Chemistry:Oxygen does not exist. | 0+  |  |
The element Chemistry:Oxygen does not exist.[7] | 8  | 19  |  | 2023 | ≥ 2.5 zs | n  | The element Chemistry:Oxygen does not exist. | (3/2+, 7/2−)  |  |
The element Chemistry:Oxygen does not exist.[7] | 8  | 20  |  | 2023 | ≥ 650 ys | 2n  | The element Chemistry:Oxygen does not exist. | 0+  |  |

1. ↑ ( ) - Uncertainty (1σ) is given in concise form in parentheses after the corresponding last digits.
2. ↑ Modes of decay:  n: | Neutron emission

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p: | Proton emission
3. ↑ Bold symbol as daughter - Daughter product is stable.
4. ↑ ( ) spin value - Indicates spin with weak assignment arguments.
5. ↑ # - Values marked # are not purely derived from experimental data, but at least partly from trends of neighboring nuclides (TNN).
6. ↑ Intermediate product of CNO-I in stellar nucleosynthesis as part of the process producing helium from hydrogen
7. ↑ 7.0 7.1 The ratio between The element Chemistry:Oxygen does not exist. and The element Chemistry:Oxygen does not exist. is used to deduce ancient temperatures.
8. ↑ Can be used in NMR studies of metabolic pathways.
9. ↑ Can be used in studying certain metabolic pathways.
10. ↑ Heaviest particle-bound isotope of oxygen, see Nuclear drip line

## Oxygen-14

Oxygen-14 (half-life 70.62 seconds) is the second most stable radioisotope of oxygen, and decays by positron emission to nitrogen-14.

Oxygen-14 ion beams are of interest to researchers of proton-rich nuclei; for example, one early experiment at the Facility for Rare Isotope Beams in East Lansing, Michigan, produced a 14O beam by proton bombardment of 14N,[8][9] using it to determine the absolute strength of the electron capture transition.

## Oxygen-15

Oxygen-15 (half-life 122.27 seconds) is the most stable radioisotope of oxygen, decaying by positron emission to nitrogen-15.

It is thus the isotope of oxygen used in positron emission tomography (PET). It can be used in, among other things, water for PET myocardial perfusion imaging and for brain imaging.[10][11] It is produced for this application through deuteron bombardment of nitrogen-14 using a cyclotron.[12]

The element Chemistry:Nitrogen does not exist. \+ The element Chemistry:Hydrogen does not exist. → The element Chemistry:Oxygen does not exist. \+ n

Oxygen-15 and nitrogen-13 are produced in air when gamma rays (for example from lightning) knock neutrons[13] out of 16O and 14N:[14]

The element Chemistry:Oxygen does not exist. \+ γ → The element Chemistry:Oxygen does not exist. \+ n
The element Chemistry:Nitrogen does not exist. \+ γ → The element Chemistry:Nitrogen does not exist. \+ nThe element Chemistry:Oxygen does not exist. decays to The element Chemistry:Nitrogen does not exist., emitting a positron. The positron quickly annihilates with an electron, producing two gamma rays of about 511 keV. After a lightning bolt, this gamma radiation dies down with half-life of 2 minutes, but these low-energy gamma rays go on average only about 90 metres through the air. Together with rays produced from positrons from nitrogen-13 they may only be detected for a minute or so as the "cloud" of The element Chemistry:Oxygen does not exist. and The element Chemistry:Nitrogen does not exist. floats by, carried by the wind.[5]

## Oxygen-16

Oxygen-16 (symbol: 16O or 168O) is a stable isotope of oxygen, with 8 neutrons and 8 protons in its nucleus, making it a doubly magic nuclide. It is the most abundant isotope of oxygen, accounting for about 99.76% of all oxygen.

The relative and absolute abundances of oxygen-16 are high because it is a principal product of stellar evolution. It can be made by stars that were initially made exclusively of hydrogen.[15] Most oxygen-16 is synthesized at the end of the helium fusion process in stars. The triple-alpha process creates carbon-12, which captures an additional helium-4 to make oxygen-16. It is also created by the neon-burning process.

Prior to the definition of the dalton based on The element Chemistry:Carbon does not exist., one atomic mass unit was defined as one sixteenth of the mass of an oxygen-16 atom.[16] Since physicists referred to The element Chemistry:Oxygen does not exist. only, while chemists meant the natural mix of isotopes, this led to slightly different mass scales.

## Oxygen-17

Oxygen-17 (17O) is the rarest of the three stable isotopes of oxygen with a low isotopic abundance of about 0.038% = 380 ppm in terrestrial water and air. Naturally The element Chemistry:Oxygen does not exist. is primarily made by burning hydrogen into helium in the CNO cycle, making it a common isotope in the hydrogen burning zones of stars.[15]

As the only stable isotope of oxygen possessing a nuclear spin (+​5⁄2) and a favorable characteristic of field-independent relaxation in liquid water, through extreme motional narrowing.17O enables NMR studies tracing oxidative metabolic pathways (i.e. conversion of 17O2 gas to metabolically produced H217O water by oxidative phosphorylation in mitochondria[17]) at high magnetic fields. This is a necessary requirement to overcome the low SNR from low abundance, low gyromagnetic ratio and fast quadrupolar transversal relaxation in contrast to proton/hydrogen, which is the most commonly used nucleus in magnetic resonance.

Water used as nuclear reactor coolant is subjected to intense neutron flux. Natural water starts out with 0.038% of 17O; heavy water starts out incidentally enriched to about 0.055% in that isotopes. Further, the neutron flux slowly converts 16O in the cooling water to 17O by neutron capture, increasing its concentration. The neutron flux slowly converts 17O (with much greater cross section) in the cooling water to carbon-14, an undesirable product that can escape to the environment:

17O (n,α) → 14C

Some tritium removal facilities make a point of replacing the oxygen of the water with natural oxygen (mostly 16O) to give the added benefit of reducing 14C production.[18][19]

The isotope was first hypothesized and subsequently imaged by Patrick Blackett in Rutherford's lab in 1925:[20] It was a product out of the first man-made transmutation of 14N and 4He2+ conducted by Frederick Soddy and Ernest Rutherford in 1917–1919.[21] Its presence in Earth's atmosphere was later detected in 1929 by Giauque and Johnson in absorption spectra,[22] demonstrating its natural existence.

## Oxygen-18

Oxygen-18 (18O, Ω[23]) is one of the stable isotopes of oxygen, with roughly 0.20% abundance, and considered one of the environmental isotopes. Most The element Chemistry:Oxygen does not exist. is produced when [[Nitrogen|The element Chemistry:Nitrogen does not exist.]] (made abundant from CNO burning) captures a The element Chemistry:Helium does not exist. nucleus, becoming [[Fluorine-18|The element Chemistry:Fluorine does not exist.]]. This quickly (half-life around 110 minutes) beta decays to The element Chemistry:Oxygen does not exist. making that isotope common in the helium-rich zones of stars.[15] Temperatures on the order of 109 kelvins are needed to fuse oxygen into sulfur.[24]

Fluorine-18 is usually produced by irradiation of 18O-enriched water with high-energy (about 18 MeV) protons prepared in a cyclotron or a linear accelerator, yielding an aqueous solution containing 18F as fluoride ion. This solution is then used for rapid synthesis of a labeled molecule, often with the fluorine atom replacing a hydroxy group. The labeled molecules or radiopharmaceuticals have to be synthesized after the radiofluorine is prepared, as the high energy proton radiation would destroy the molecules. Large amounts of oxygen-18 enriched water are used in positron emission tomography centers, for on-site production of 18F-labeled fluorodeoxyglucose (FDG).[25]

Measurements of the 18O/16O ratio (known as δ18O) are often used in paleoclimatology. Water molecules with a lighter isotope are slightly more likely to evaporate and less likely to fall as precipitation, so Earth's freshwater and polar ice have slightly less (0.1981%) The element Chemistry:Oxygen does not exist. than air (0.204%) or seawater (0.1995%).[26] This disparity allows the study of historical temperature patterns via the analysis of ice cores. Assuming that atmospheric circulation and elevation has not changed significantly over the poles, the temperature of ice formation can be calculated as equilibrium fractionation between phases of water that is known for different temperatures. Water molecules are also subject to Rayleigh fractionation as atmospheric water moves from the equator poleward which results in progressive depletion of 18O, or lower δ18O values.[27]

The δ18O ratio can also be used in paleothermometry for certain types of fossils. The fossil material used is generally calcite or aragonite, however oxygen isotope paleothermometry has also been done of phosphatic fossils using SHRIMP.[28] For determination of ocean temperatures over geologic time, multiple fossils of the same species in different stratigraphic layers would be measured, and the difference between them would indicate long term changes.[29]

18O has also been used to trace ocean composition and temperature which seafood is from.[30]

In the study of plants' photorespiration, the labeling of atmosphere by oxygen-18 allows for the measurement of oxygen uptake by the photorespiration pathway. Labeling by 18O2 gives the unidirectional flux of O2 uptake, while there is a net photosynthetic 16O2 evolution. It was demonstrated that, under preindustrial atmosphere, most plants reabsorb, by photorespiration, half of the oxygen produced by photosynthesis. Then, the yield of photosynthesis was halved by the presence of oxygen in atmosphere.[31][32]

## Oxygen-20

Oxygen-20 has a half-life of 13.51±0.05 s and decays by β− decay to 20F. It is one of the known cluster decay ejected particles, being emitted in the decay of 228Th with a branching ratio of about (1.13±0.22)×10−13.[33]

## See also

* Dole effect

Daughter products other than oxygen

* Isotopes of fluorine
* Isotopes of nitrogen
* Isotopes of carbon
* Isotopes of helium

## References

1. ↑ Meija, Juris; Coplen, Tyler B.; Berglund, Michael; Brand, Willi A.; De Bièvre, Paul; Gröning, Manfred; Holden, Norman E.; Irrgeher, Johanna et al. (2016). "Atomic weights of the elements 2013 (IUPAC Technical Report)". Pure and Applied Chemistry 88 (3): 265–91. doi:10.1515/pac-2015-0305.
2. ↑ Berry, D.K; Horowitz, C.J (April 2008). "Fusion of neutron rich oxygen isotopes in the crust of accreting neutron stars". Physical Review C 77 (4). doi:10.1103/PhysRevC.77.045807. Bibcode: 2008PhRvC..77d5807H. https://www.researchgate.net/publication/235579232.
3. ↑ Webb, T. B. (2019). "First Observation of Unbound 11O, the Mirror of the Halo Nucleus 11Li". Physical Review Letters 122 (12): 122501–1–122501–7. doi:10.1103/PhysRevLett.122.122501. PMID 30978039. Bibcode: 2019PhRvL.122l2501W.
4. ↑ Paleja, Ameya (2023-09-05). "Scientists observe nucleus decay into four particles" (in en-US). https://interestingengineering.com/science/nucleus-decay-four-particles.
5. ↑ 5.0 5.1 Teruaki Enoto (Nov 23, 2017). "Photonuclear reactions triggered by lightning discharge". Nature 551 (7681): 481–484. doi:10.1038/nature24630. PMID 29168803. Bibcode: 2017Natur.551..481E.
6. ↑ 6.0 6.1 6.2 "Atomic Weight of Oxygen | Commission on Isotopic Abundances and Atomic Weights". https://ciaaw.org/oxygen.htm.
7. ↑ 7.0 7.1 Kondo, Y.; Achouri, N. L.; Falou, H. Al et al. (2023-08-30). "First observation of 28O". Nature (Springer Science and Business Media LLC) 620 (7976): 965–970. doi:10.1038/s41586-023-06352-6. ISSN 0028-0836. PMID 37648757. Bibcode: 2023Natur.620..965K.
8. ↑ APS -Fall 2022 Meeting of the APS Division of Nuclear Physics - Event - Oxygen-14 Beam Production at 5 and 15 MeV/u with MARS Spectrometer. 67. American Physical Society. https://meetings.aps.org/Meeting/DNP22/Session/HA.68.
9. ↑ Energy, US Department of. "Researchers develop a novel method to study nuclear reactions on short-lived isotopes involved in explosions of stars" (in en). phys.org. https://phys.org/news/2023-10-method-nuclear-reactions-short-lived-isotopes.html.
10. ↑ Rischpler, Christoph; Higuchi, Takahiro; Nekolla, Stephan G. (22 November 2014). "Current and Future Status of PET Myocardial Perfusion Tracers". Current Cardiovascular Imaging Reports 8 (1): 333–343. doi:10.1007/s12410-014-9303-z.
11. ↑ Kim, E. Edmund; Lee, Myung-Chul; Inoue, Tomio; Wong, Wai-Hoi (2012) (in en). Clinical PET and PET/CT: Principles and Applications. Springer. p. 182. ISBN 978-1-4419-0802-5. https://books.google.com/books?id=jj9eHkn1tR0C&pg=PA182.
12. ↑ "Production of PET Radionuclides". Austin Hospital, Austin Health. http://www.petnm.unimelb.edu.au/pet/detail/radionuc.html.
13. ↑ If protons were knocked out, the stable isotopes 13C and 15N would be formed.
14. ↑ Timmer, John (25 November 2017). "Lightning strikes leave behind a radioactive cloud" (in en-us). Ars Technica. https://arstechnica.com/science/2017/11/lightning-strikes-leave-behind-a-radioactive-cloud/.
15. ↑ 15.0 15.1 15.2 B. S. Meyer (September 19–21, 2005). "Nucleosynthesis and galactic chemical evolution of the isotopes of oxygen". Workgroup on Oxygen in the Earliest Solar System. Gatlinburg, Tennessee. 9022. http://www.lpi.usra.edu/meetings/ess2005/pdf/9022.pdf.
16. ↑ Parks & Mellor 1939, Chapter VI, Section 7. sfn error: no target: CITEREFParksMellor1939 (help)
17. ↑ Arai, T.; S. Nakao; K. Mori; K. Ishimori; I. Morishima; T. Miyazawa; B. Fritz-Zieroth (31 May 1990). "Cerebral Oxygen Utilization Analyzed by the Use of Oxygen-17 and its Nuclear Magnetic Resonance". Biochem. Biophys. Res. Commun. 169 (1): 153–158. doi:10.1016/0006-291X(90)91447-Z. PMID 2350339. Bibcode: 1990BBRC..169..153A.
18. ↑ http://www.nrc.gov/docs/ML1016/ML101650129.pdf Estimation of Carbon-14 in Nuclear Power Plant Gaseous Effluents; EPRI; June 10, 2010
19. ↑ A Compact, Low Cost, Tritium Removal Plant for Candu-6 Reactors; S.K. Sood, C. Fong, and K.M. Kalyanam; Ontario Hydro
20. ↑ Blackett, P. M. S. (1925). "The Ejection of Protons from Nitrogen Nuclei, Photographed by the Wilson Method". Proceedings of the Royal Society of London. Series A 107 (742): 349–360. doi:10.1098/rspa.1925.0029. Bibcode: 1925RSPSA.107..349B.
21. ↑ Rutherford, Ernest (1919). "Collision of alpha particles with light atoms IV. An anomalous effect in nitrogen.". Philosophical Magazine. 6th series 37: 581–587. doi:10.1080/14786440608635919. https://zenodo.org/record/1430800.
22. ↑ Giauque, W. F.; Johnston, H. L. (1929). "An Isotope of Oxygen, Mass 17, in the Earth's Atmosphere". J. Am. Chem. Soc. 51 (12): 3528–3534. doi:10.1021/ja01387a004. Bibcode: 1929JAChS..51.3528G.
23. ↑ Capilla, José E.; Arevalo, Javier Rodriguez; Castaño, Silvino Castaño; Teijeiro, María Fé Díaz; del Moral, Rut Sanchez; Diaz, Javier Heredia (September 19, 2012). "Mapping Oxygen-18 in Meteoric Precipitation over Peninsular Spain using Geostatistical Tools". Valencia, Spain: Ninth Conference on Geostatistics for Environmental Applications. http://www.cedex.es/NR/rdonlyres/B8A9522A-5D6F-4675-921A-24BB8458187B/124720/Capilla_et_al_geoENV_2012_Valencia_España_Extended.pdf.
24. ↑ Emsley 2001, p. 297. sfn error: no target: CITEREFEmsley2001 (help)
25. ↑ "Enriched water-H218O purification to be used in routine 18FDG production". http://www.iaea.org/inis/collection/NCLCollectionStore/_Public/46/048/46048804.pdf.
26. ↑ Dansgaard, W (1964). "Stable isotopes in precipitation". Tellus 16 (4): 436–468. doi:10.3402/tellusa.v16i4.8993. Bibcode: 1964Tell...16..436D. http://www.ldeo.columbia.edu/~polissar/OrgGeochem/dansgaard-1964-stable-isoto.pdf.
27. ↑ Kendall, C.; Caldwell, E.A. (1998). "Chapter 2: Fundamentals in Isotope Geochemistry". Isotope Tracers in Catchment Hydrology. Elsevier Science B.V., Amsterdam.. https://wwwrcamnl.wr.usgs.gov/isoig/isopubs/itchch2.html.
28. ↑ Trotter, J.A.; Williams, I.S.; Barnes, C.R.; Lécuyer, C.; Nicoll, R.S. (2008). "Did Cooling Oceans Trigger Ordovician Biodiversification? Evidence from Conodont Thermometry". Science 321 (5888): 550–4. doi:10.1126/science.1155814. PMID 18653889. Bibcode: 2008Sci...321..550T.
29. ↑ Kendall, C.; McDonnell, J.J. (1998). Isotope Tracers in Catchment Hydrology. Elsevier Science B.V., Amsterdam.. https://wwwrcamnl.wr.usgs.gov/isoig/isopubs/itchinfo.html. Retrieved 2013-02-03.
30. ↑ Martino, Jasmin C.; Trueman, Clive N.; Mazumder, Debashish; Crawford, Jagoda; Doubleday, Zoë A. (September 12, 2022). "Using 'chemical fingerprinting' to fight seafood fraud and illegal fishing". Fish and Fisheries (Phys.org) 23 (6): 1455–1468. doi:10.1111/faf.12703. https://phys.org/news/2022-09-chemical-fingerprinting-seafood-fraud-illegal.amp. Retrieved September 13, 2022.
31. ↑ "Photosynthesis and photorespiration in whole plants of wheat". Plant Physiol. 64 (5): 735–8. November 1979. doi:10.1104/pp.64.5.735. PMID 16661044. Bibcode: 1979PlanP..64..735G.
32. ↑ "Oxygen exchange in leaves in the light". Plant Physiol. 66 (2): 302–7. August 1980. doi:10.1104/pp.66.2.302. PMID 16661426.
33. ↑ Bonetti, R.; Guglielmetti, A. (2007). "Cluster radioactivity: an overview after twenty years". Romanian Reports in Physics 59: 301–310. http://www.rrp.infim.ro/2007_59_2/10_bonetti.pdf.

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Isotopes of the chemical elements

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Iso's * List

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Iso's * List

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Iso's * List

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Iso's * List

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Iso's * List

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Iso's * List

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Iso's * List

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* Table of nuclides
* Categories: Isotopes
* Tables of nuclides
* Metastable isotopes
* Isotopes by element

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Original source: https://en.wikipedia.org/wiki/Isotopes of oxygen. Read more

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