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Isotopes of oxygen

From Wikipedia, the free encyclopedia

Isotopes ofoxygen (8O)
Main isotopes[1]Decay
Isotopeabun­dancehalf-life(t1/2)modepro­duct
15Otrace122.27 sβ+15N
16O99.8%stable
17O0.0384%stable
18O0.205%stable
Standard atomic weightAr°(O)

There are three known stableisotopes ofoxygen (8O):16
O,17
O, and18
O. Radioisotopes are known from11O to28O (particle-bound from mass number 13 to 24), and the most stable are15
O withhalf-life 122.27 seconds and14
O with half-life 70.62 seconds. All remaining radioisotopes are even shorter in lifetime. The four heaviest known isotopes (up to28
O) decay byneutron emission to24
O, whose half-life is 77 milliseconds;24O, along with28Ne, have been used in the model of reactions in the crust of neutron stars.[4] The most commondecay mode for isotopes lighter than the stable isotopes isβ+ decay tonitrogen, and the most common mode after isβ− decay tofluorine.

List of isotopes

[edit]
Nuclide
[n 1]		ZNIsotopic mass(Da)[5]
[n 2]		Half-life[1]

[resonance width]		Decay
mode[1]
[n 3]		Daughter
isotope
[n 4]		Spin and
parity[1]
[n 5][n 6]		Natural abundance(mole fraction)
Excitation energyNormal proportion[1]Range of variation
11
O[6]		8311.05125(6)198(12) ys
[2.31(14) MeV]		2p9
C		(3/2−)
12
O		8412.034368(13)8.9(3.3) zs2p10
C		0+
13
O		8513.024815(10)8.58(5) msβ+ (89.1(2)%)13
N		(3/2−)
β+p (10.9(2)%)12
C
β+p,α (<0.1%)24
He[7]
14
O		8614.008596706(27)70.621(11) sβ+14
N		0+
15
O[n 7]		8715.0030656(5)122.266(43) sβ+15
N		1/2−Trace[8]
16
O[n 8]		8815.994914619257(319)Stable0+[0.99738,0.99776][9]
17
O[n 9]		8916.999131755953(692)Stable5/2+[0.000367,0.000400][9]
18
O[n 8][n 10]		81017.999159612136(690)Stable0+[0.00187,0.00222][9]
19
O		81119.0035780(28)26.470(6) sβ−19
F		5/2+
20
O		81220.0040754(9)13.51(5) sβ−20
F		0+
21
O		81321.008655(13)3.42(10) sβ−21
F		(5/2+)
β−n ?20
F ?
22
O		81422.00997(6)2.25(9) sβ− (>78%)22
F		0+
β−n (<22%)21
F
23
O		81523.01570(13)97(8) msβ− (93(2)%)23
F		1/2+
β−n (7(2)%)22
F
24
O[n 11]		81624.01986(18)77.4(4.5) msβ− (57(4)%)24
F		0+
β−n (43(4)%)23
F
25
O		81725.02934(18)5.18(35) zsn24
O		3/2+#
26
O		81826.03721(18)4.2(3.3) ps2n24
O		0+
27
O[10]		819≥2.5 zsn26
O		(3/2+, 7/2−)
28
O[10]		820≥650 ys2n26
O		0+
This table header & footer:
  1. ^mO – Excitednuclear isomer.
  2. ^( ) – Uncertainty (1σ) is given in concise form in parentheses after the corresponding last digits.
  3. ^Modes of decay:
    n:Neutron emission
    p:Proton emission
  4. ^Bold symbol as daughter – Daughter product is stable.
  5. ^( ) spin value – Indicates spin with weak assignment arguments.
  6. ^# – Values marked # are not purely derived from experimental data, but at least partly from trends of neighboring nuclides (TNN).
  7. ^Intermediate product ofCNO-I instellar nucleosynthesis as part of the process producing helium from hydrogen
  8. ^abThe ratio between16
    O     and18
    O     is used todeduce ancient temperatures.
  9. ^Can be used in NMR studies of metabolic pathways.
  10. ^Can be used in studying certain metabolic pathways.
  11. ^Heaviest particle-bound isotope of oxygen, seeNuclear drip line

Oxygen-14

[edit]

Oxygen-14 (half-life 70.62 seconds) is the second most stable radioisotope of oxygen, and decays bypositron emission tonitrogen-14.

Oxygen-14ion beams are of interest to researchers of proton-rich nuclei; for example, one early experiment at theFacility for Rare Isotope Beams inEast Lansing, Michigan, produced a14O beam by proton bombardment of14N,[11][12] using it to determine the absolute strength of the electron capture transition.

Oxygen-15

[edit]

Oxygen-15 (half-life 122.27 seconds) is the most stable radioisotope of oxygen, decaying bypositron emission tonitrogen-15.

It is thus the isotope of oxygen used inpositron emission tomography (PET). It can be used in, among other things,water for PETmyocardial perfusion imaging and forbrain imaging.[13][14] It is produced for this application throughdeuteron bombardment ofnitrogen-14 using acyclotron.[15]

14
N +2
H →15
O + n

Oxygen-15 and nitrogen-13 are produced in air whengamma rays (for example fromlightning) knock neutrons[16] out of16O and14N:[17]

16
O + γ →15
O + n
14
N + γ →13
N + n

15
O decays to15
N, emitting apositron. 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" of15
O and13
N floats by, carried by the wind.[8]

Oxygen-16

[edit]

Oxygen-16 (symbol:16O or16
8O) is astable isotope of oxygen, with 8neutrons and 8protons in itsnucleus, making it adoubly 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 ofstellar evolution. It can be made by stars that wereinitially made exclusively of hydrogen.[18] Most oxygen-16 issynthesized at the end of the helium fusion process in stars. Thetriple-alpha process creates carbon-12, which captures an additional helium-4 to make oxygen-16. It is also created by theneon-burning process.

Prior to the definition of thedalton based on12
C, one atomic mass unit was defined as one sixteenth of the mass of an oxygen-16 atom.[19] Since physicists referred to16
O only, while chemists meant the natural mix of isotopes, this led to slightly different mass scales.

Oxygen-17

[edit]

Oxygen-17 (17O) is astable isotope of oxygen with a low isotopic abundance of about 0.038%.17
O is primarily made by burning hydrogen into helium in theCNO cycle, making it a common isotope in the hydrogen burning zones of stars.[18]

As the only stable isotope of oxygen possessing anuclear spin (+5⁄2) and a favorable characteristic of field-independentrelaxation in liquid water,17O enablesNMR studies of oxidativemetabolic pathways through compounds containing17O (i.e. metabolically produced H217O water byoxidative phosphorylation inmitochondria[20]) at high magnetic fields.

Water used asnuclear reactor coolant is subjected to intenseneutron flux. Natural water starts out with 0.038% of17O;heavy water starts out incidentally enriched to about 0.055% in that isotopes. Further, the neutron flux slowly converts16O in the cooling water to17O byneutron capture, increasing its concentration. The neutron flux slowly converts17O (with much greatercross section) in the cooling water tocarbon-14, an undesirable product that can escape to the environment:

17O (n,α) →14C

Sometritium removal facilities make a point of replacing the oxygen of the water with natural oxygen (mostly16O) to give the added benefit of reducing14C production.[21][22]

The isotope was first hypothesized and subsequently imaged byPatrick Blackett in Rutherford's lab in 1925:[23] It was a product out of the first man-madetransmutation of14N and4He2+ conducted byFrederick Soddy andErnest Rutherford in 1917–1919.[24] Its presence in Earth's atmosphere was later detected in 1929 byGiauque and Johnson in absorption spectra,[25] demonstrating its natural existece.

Oxygen-18

[edit]

Oxygen-18 (18
O, Ω[26]) is one of the stable isotopes ofoxygen, with roughly 0.20% abundance, and considered one of theenvironmental isotopes. Most18
O is produced when14
N (made abundant from CNO burning) captures a4
He nucleus, becoming18
F. This quickly (half-life around 110 minutes)beta decays to18
O making that isotope common in the helium-rich zones of stars.[18] Temperatures on the order of 109 kelvins are needed tofuse oxygen intosulfur.[27]

Fluorine-18 is usually produced by irradiation of18O-enriched water with high-energy (about 18MeV)protons prepared in acyclotron or alinear accelerator, yielding an aqueous solution containing18F as fluoride ion. This solution is then used for rapid synthesis of alabeled molecule, often with the fluorine atom replacing ahydroxy group. The labeled molecules orradiopharmaceuticals 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 inpositron emission tomography centers, for on-site production of18F-labeledfluorodeoxyglucose (FDG).[28]

Measurements of the18O/16O ratio (known asδ18
O) are often used inpaleoclimatology. Water molecules with a lighter isotope are slightly more likely toevaporate and less likely to fall asprecipitation, so Earth's freshwater and polar ice have slightly less (0.1981%)18
O than air (0.204%) orseawater (0.1995%).[29] This disparity allows the study of historical temperature patterns via the analysis ofice cores. Assuming that atmospheric circulation and elevation has not changed significantly over the poles, the temperature of ice formation can be calculated asequilibrium fractionation between phases of water that is known for different temperatures. Water molecules are also subject toRayleigh fractionation as atmospheric water moves from the equator poleward which results in progressive depletion of18
O, or lower δ18
O values.[30]

The δ18
O ratio can also be used inpaleothermometry for certain types offossils. The fossil material used is generallycalcite oraragonite, however oxygen isotope paleothermometry has also been done ofphosphatic fossils usingSHRIMP.[31] For determination of ocean temperatures over geologic time, multiple fossils of the same species in differentstratigraphic layers would be measured, and the difference between them would indicate long term changes.[32]

18O has also been used to trace ocean composition and temperature whichseafood is from.[33]

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 by18
O
2 gives the unidirectional flux ofO
2 uptake, while there is a net photosynthetic16
O
2 evolution. It was demonstrated that, under preindustrial atmosphere, most plants reabsorb, by photorespiration, half of the oxygen produced byphotosynthesis. Then, the yield of photosynthesis was halved by the presence of oxygen in atmosphere.[34][35]

Oxygen-20

[edit]

Oxygen-20 has a half-life of13.51±0.05 s and decays by β− decay to20F. It is one of the knowncluster decay ejected particles, being emitted in the decay of228Th with a branching ratio of about(1.13±0.22)×10−13.[36]

See also

[edit]

Daughter products other than oxygen

References

[edit]
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  10. ^abKondo, Y.; Achouri, N. L.; Falou, H. Al; et al. (2023-08-30)."First observation of 28O".Nature.620 (7976). Springer Science and Business Media LLC:965–970.Bibcode:2023Natur.620..965K.doi:10.1038/s41586-023-06352-6.ISSN 0028-0836.PMC 10630140.PMID 37648757.
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  14. ^Kim, E. Edmund; Lee, Myung-Chul; Inoue, Tomio; Wong, Wai-Hoi (2012).Clinical PET and PET/CT: Principles and Applications. Springer. p. 182.ISBN 978-1-4419-0802-5.
  15. ^"Production of PET Radionuclides". Austin Hospital, Austin Health. Archived fromthe original on 15 January 2013. Retrieved6 December 2012.
  16. ^If protons were knocked out, the stable isotopes13C and15N would be formed.
  17. ^Timmer, John (25 November 2017)."Lightning strikes leave behind a radioactive cloud".Ars Technica.
  18. ^abcB. S. Meyer (September 19–21, 2005)."Nucleosynthesis and galactic chemical evolution of the isotopes of oxygen"(PDF).Proceedings of the NASA Cosmochemistry Program and the Lunar and Planetary Institute.Workgroup on Oxygen in the Earliest Solar System. Gatlinburg, Tennessee. 9022.
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  20. ^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.Bibcode:1990BBRC..169..153A.doi:10.1016/0006-291X(90)91447-Z.PMID 2350339.
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  26. ^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"(PDF).cedex.es. Valencia, Spain: Ninth Conference on Geostatistics for Environmental Applications. Archived fromthe original(PDF) on September 23, 2015. RetrievedMay 8, 2017.
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  28. ^"Enriched water-H218O purification to be used in routine18FDG production"(PDF).www.iaea.org. Retrieved2024-05-20.
  29. ^Dansgaard, W (1964)."Stable isotopes in precipitation"(PDF).Tellus.16 (4):436–468.Bibcode:1964Tell...16..436D.doi:10.3402/tellusa.v16i4.8993.
  30. ^Kendall, C.; Caldwell, E.A. (1998)."Chapter 2: Fundamentals in Isotope Geochemistry".Isotope Tracers in Catchment Hydrology. Elsevier Science B.V., Amsterdam.
  31. ^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.Bibcode:2008Sci...321..550T.doi:10.1126/science.1155814.PMID 18653889.S2CID 28224399.
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  33. ^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.23 (6).Phys.org:1455–1468.doi:10.1111/faf.12703.S2CID 252173914.Archived from the original on September 13, 2022. RetrievedSeptember 13, 2022.
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Group12 3456789101112131415161718
PeriodHydrogen and
alkali metals		Alkaline
earth metals		Pnicto­gensChal­co­gensHalo­gensNoble gases
①12
②345678910
③1112131415161718
④192021222324252627282930313233343536
⑤373839404142434445464748495051525354
⑥55561 asterisk71727374757677787980818283848586
⑦87881 asterisk103104105106107108109110111112113114115116117118
⑧119120
1 asterisk5758596061626364656667686970 
1 asterisk8990919293949596979899100101102
National
Other
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