Isotopes of oxygen

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Isotopes of oxygen  (8O)
Main isotopes Decay
abun­dance half-life (t1/2) mode pro­duct
15O trace 122.266 sβ+100%15N
16O 99.8% stable
17O 0.0380%stable
18O 0.205%stable
Standard atomic weight Ar°(O)

There are three known stable isotopes of oxygen (8O): 16
O
, 17
O
, and 18
O
.

Contents

Radioactive isotopes ranging from 11
O
 to 28
O
 have also been characterized, all short-lived. The longest-lived radioisotope is 15
O
 with a half-life of 122.266(43)  s , while the shortest-lived isotope is the unbound 11
O
 with a half-life of 198(12)  yoctoseconds , though half-lives have not been measured for the unbound heavy isotopes 27
O
 and 28
O
. [3]

List of isotopes

Nuclide
[n 1] 		Z N Isotopic mass (Da) [4]
[n 2] 		Half-life [5]

[resonance width]		 Decay
mode [5]
[n 3] 		Daughter
isotope
[n 4] 		Spin and
parity [5]
[n 5] [n 6] 		Natural abundance (mole fraction)
Excitation energyNormal proportion [5] Range of variation
11
O
 [6] 		8311.05125(6)198(12) ys
[2.31(14)  MeV ]		 2p 9
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 ? [n 11] 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 12] 		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
 [3] 		819≥ 2.5 zsn26
O
(3/2+, 7/2−)
28
O
 [3] 		820≥ 650 ys2n26
O
0+
This table header & footer:
  1. ↑ mO – Excited nuclear 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 of CNO-I in stellar nucleosynthesis as part of the process producing helium from hydrogen
  8. 1 2 The ratio between 16
    O
     and 18
    O
     is used to deduce ancient temperatures.
  9. ↑ Can be used in NMR studies of metabolic pathways.
  10. ↑ Can be used in studying certain metabolic pathways.
  11. ↑ Decay mode shown is energetically allowed, but has not been experimentally observed to occur in this nuclide.
  12. ↑ Heaviest particle-bound isotope of oxygen, see Nuclear drip line

Stable isotopes

Late in a massive star's life, O concentrates in the Ne-shell, O in the H-shell and O in the He-shell. Evolved star fusion shells.svg
Late in a massive star's life,
O
 concentrates in the Ne-shell,
O
 in the H-shell and
O
 in the He-shell.

Natural oxygen is made of three stable isotopes, 16
O
, 17
O
, and 18
O
, with 16
O
 being the most abundant (99.762% natural abundance). Depending on the terrestrial source, the standard atomic weight varies within the range of [15.99903, 15.99977] (the conventional value is 15.999).

16
O
 has high relative and absolute abundance because it is a principal product of stellar evolution and because it is a primary isotope, meaning it can be made by stars that were initially hydrogen only. [10] Most 16
O
 is synthesized at the end of the helium fusion process in stars; the triple-alpha process creates 12
C
, which captures an additional 4
He
 nucleus to produce 16
O
. The neon burning process creates additional 16
O
. [10]

Both 17
O
 and 18
O
 are secondary isotopes, meaning their synthesis requires seed nuclei. 17
O
 is primarily made by burning hydrogen into helium in the CNO cycle, making it a common isotope in the hydrogen burning zones of stars. [10] Most 18
O
 is produced when 14
N
 (made abundant from CNO burning) captures a 4
He
 nucleus, becoming 18
F
. This quickly (half-life around 110 minutes) beta decays to 18
O
 making that isotope common in the helium-rich zones of stars. [10] Temperatures on the order of 109  kelvins are needed to fuse oxygen into sulfur. [11]

An atomic mass of 16 was assigned to oxygen prior to the definition of the unified atomic mass unit based on 12
C
. [12] Since physicists referred to 16
O
 only, while chemists meant the natural mix of isotopes, this led to slightly different mass scales.

Applications of various isotopes

Measurements of 18O/16O ratio are often used to interpret changes in paleoclimate. Oxygen in Earth's air is 99.759%16
O
, 0.037%17
O
 and 0.204%18
O
. [13] Water molecules with a lighter isotope are slightly more likely to evaporate and less likely to fall as precipitation, [14] so Earth's freshwater and polar ice have slightly less (0.1981%) 18
O
 than air (0.204%) or seawater (0.1995%). This disparity allows analysis of temperature patterns via historic ice cores.

Solid samples (organic and inorganic) for oxygen isotopic ratios are usually stored in silver cups and measured with pyrolysis and mass spectrometry. [15] Researchers need to avoid improper or prolonged storage of the samples for accurate measurements. [15]

Due to natural oxygen being mostly 16
O, samples enriched with the other stable isotopes can be used for isotope labeling. For example, it was proven that the oxygen released in photosynthesis originates in H2O, rather than in the also consumed CO2, by isotope tracing experiments. The oxygen contained in CO2 in turn is used to make up the sugars formed by photosynthesis.

In heavy-water nuclear reactors the neutron moderator should preferably be low in 17
O and 18
O due to their higher neutron absorption cross section compared to 16
O. While this effect can also be observed in light-water reactors, ordinary hydrogen (protium) has a higher absorption cross section than any stable isotope of oxygen and its number density is twice as high in water as that of oxygen, so that the effect is negligible. As some methods of isotope separation enrich not only heavier isotopes of hydrogen but also heavier isotopes of oxygen when producing heavy water, the concentration of 17
O and 18
O can be measurably higher. Furthermore, the 17
O(n,α) 14
C reaction is a further undesirable result of an elevated concentration of heavier isotopes of oxygen. Therefore, facilities which remove tritium from heavy water used in nuclear reactors often also remove or at least reduce the amount of heavier isotopes of oxygen.

Oxygen isotopes are also used to trace ocean composition and temperature which seafood is from. [16]

Radioisotopes

Thirteen radioisotopes have been characterized; the most stable are 15
O
 with half-life 122.266(43) s and 14
O
 with half-life 70.621(11) s. All remaining radioisotopes have half-lives less than 27 s and most have half-lives less than 0.1 s. The four heaviest known isotopes (up to 28
O
) decay by neutron emission to 24
O
, whose half-life is 77.4(4.5) ms. This isotope, along with 28Ne, have been used in the model of reactions in crust of neutron stars. [17] 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.

Oxygen-13

Oxygen-13 is an unstable isotope, with 8 protons and 5 neutrons. It has spin 3/2−, and half-life 8.58(5)  ms . Its atomic mass is 13.024815(10)  Da . It decays to nitrogen-13 by electron capture, with a decay energy of 17.770(10)  MeV . Its parent nuclide is fluorine-14.

Oxygen-14

Oxygen-14 is the second most stable radioisotope. 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, used a 14O beam to study the beta decay transition of this isotope to 14N. [18] [19]

Oxygen-15

Oxygen-15 is a radioisotope, often used in positron emission tomography (PET). It can be used in, among other things, water for PET myocardial perfusion imaging and for brain imaging. [20] [21] It has an atomic mass of 15.0030656(5), and a half-life of 122.266(43) s. It is produced through deuteron bombardment of nitrogen-14 using a cyclotron. [22]

14
N
 + 2
H
 → 15
O
 + n

Oxygen-15 and nitrogen-13 are produced in air when gamma rays (for example from lightning) knock neutrons out of 16O and 14N: [23]

16
O
 + γ → 15
O
 + n
14
N
 + γ → 13
N
 + n

15
O
 decays to 15
N
, 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 15
O
 and 13
N
 floats by, carried by the wind. [8]

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. [24]

See also

Related Research Articles

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A chemical element is a chemical substance whose atoms all have the same number of protons. The number of protons is called the atomic number of that element. For example, oxygen has an atomic number of 8, meaning each oxygen atom has 8 protons in its nucleus. Atoms of the same element can have different numbers of neutrons in their nuclei, known as isotopes of the element. Two or more atoms can combine to form molecules. Some elements are formed from molecules of identical atoms, e. g. atoms of hydrogen (H) form diatomic molecules (H2). Chemical compounds are substances made of atoms of different elements; they can have molecular or non-molecular structure. Mixtures are materials containing different chemical substances; that means (in case of molecular substances) that they contain different types of molecules. Atoms of one element can be transformed into atoms of a different element in nuclear reactions, which change an atom's atomic number.

<span class="mw-page-title-main">Nuclear physics</span> Field of physics that studies atomic nuclei

Nuclear physics is the field of physics that studies atomic nuclei and their constituents and interactions, in addition to the study of other forms of nuclear matter.

<span class="mw-page-title-main">Stable nuclide</span> Nuclide that does not undergo radioactive decay

Stable nuclides are isotopes of a chemical element whose nucleons are in a configuration that does not permit them the surplus energy required to produce a radioactive emission. The nuclei of such isotopes are not radioactive and unlike radionuclides do not spontaneously undergo radioactive decay. When these nuclides are referred to in relation to specific elements they are usually called that element's stable isotopes.

<span class="mw-page-title-main">Nucleosynthesis</span> Process that creates new atomic nuclei from pre-existing nucleons, primarily protons and neutrons

Nucleosynthesis is the process that creates new atomic nuclei from pre-existing nucleons and nuclei. According to current theories, the first nuclei were formed a few minutes after the Big Bang, through nuclear reactions in a process called Big Bang nucleosynthesis. After about 20 minutes, the universe had expanded and cooled to a point at which these high-energy collisions among nucleons ended, so only the fastest and simplest reactions occurred, leaving our universe containing hydrogen and helium. The rest is traces of other elements such as lithium and the hydrogen isotope deuterium. Nucleosynthesis in stars and their explosions later produced the variety of elements and isotopes that we have today, in a process called cosmic chemical evolution. The amounts of total mass in elements heavier than hydrogen and helium remains small, so that the universe still has approximately the same composition.

<span class="mw-page-title-main">Nuclide</span> Atomic species

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<span class="mw-page-title-main">Decay chain</span> Series of radioactive decays

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F
 to 31
F
 and two isomers. Only fluorine-19 is stable and naturally occurring in more than trace quantities; therefore, fluorine is a monoisotopic and mononuclidic element.

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Naturally occurring nickel (28Ni) is composed of five stable isotopes; 58
Ni
, 60
Ni
, 61
Ni
, 62
Ni
 and 64
Ni
, with 58
Ni
 being the most abundant. 26 radioisotopes have been characterised with the most stable being 59
Ni
 with a half-life of 76,000 years, 63
Ni
 with a half-life of 100.1 years, and 56
Ni
 with a half-life of 6.077 days. All of the remaining radioactive isotopes have half-lives that are less than 60 hours and the majority of these have half-lives that are less than 30 seconds. This element also has 8 meta states.

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References

  1. ↑ "Standard Atomic Weights: Oxygen". CIAAW. 2009.
  2. ↑ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN   1365-3075.
  3. 1 2 3 Kondo, 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.
  4. ↑ Wang, Meng; Huang, W.J.; Kondev, F.G.; Audi, G.; Naimi, S. (2021). "The AME 2020 atomic mass evaluation (II). Tables, graphs and references*". Chinese Physics C. 45 (3): 030003. doi:10.1088/1674-1137/abddaf.
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  6. ↑ Webb, T. B.; et al. (2019). "First Observation of Unbound 11O, the Mirror of the Halo Nucleus 11Li". Physical Review Letters. 122 (12): 122501–1–122501–7. arXiv: 1812.08880 . Bibcode:2019PhRvL.122l2501W. doi:10.1103/PhysRevLett.122.122501. PMID   30978039. S2CID   84841752.
  7. ↑ Paleja, Ameya (2023-09-05). "Scientists observe nucleus decay into four particles". interestingengineering.com. Retrieved 2023-09-29.
  8. 1 2 Teruaki Enoto; et al. (Nov 23, 2017). "Photonuclear reactions triggered by lightning discharge". Nature. 551 (7681): 481–484. arXiv: 1711.08044 . Bibcode:2017Natur.551..481E. doi:10.1038/nature24630. PMID   29168803. S2CID   4388159.
  9. 1 2 3 "Atomic Weight of Oxygen | Commission on Isotopic Abundances and Atomic Weights". ciaaw.org. Retrieved 2022-03-15.
  10. 1 2 3 4 B. 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.
  11. ↑ Emsley 2001, p. 297.
  12. ↑ Parks & Mellor 1939, Chapter VI, Section 7.
  13. ↑ Cook & Lauer 1968, p. 500.
  14. ↑ Dansgaard, W (1964). "Stable isotopes in precipitation" (PDF). Tellus. 16 (4): 436–468. Bibcode:1964Tell...16..436D. doi:10.1111/j.2153-3490.1964.tb00181.x.
  15. 1 2 Tsang, Man-Yin; Yao, Weiqi; Tse, Kevin (2020). Kim, Il-Nam (ed.). "Oxidized silver cups can skew oxygen isotope results of small samples". Experimental Results. 1: e12. doi: 10.1017/exp.2020.15 . ISSN   2516-712X.
  16. ↑ 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. Retrieved September 13, 2022.
  17. ↑ 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): 045807. arXiv: 0710.5714 . Bibcode:2008PhRvC..77d5807H. doi:10.1103/PhysRevC.77.045807. S2CID   118639621.
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  19. ↑ Energy, US Department of. "Researchers develop a novel method to study nuclear reactions on short-lived isotopes involved in explosions of stars". phys.org. Retrieved 16 December 2023.
  20. ↑ 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. S2CID   72703962.
  21. ↑ Kim, E. Edmund; Lee, Myung-Chul; Inoue, Tomio; Wong, Wai-Hoi (2012). Clinical PET and PET/CT: Principles and Applications. Springer. p. 182. ISBN   9781441908025.
  22. ↑ "Production of PET Radionuclides". Austin Hospital, Austin Health. Archived from the original on 15 January 2013. Retrieved 6 December 2012.
  23. ↑ Timmer, John (25 November 2017). "Lightning strikes leave behind a radioactive cloud". Ars Technica.
  24. ↑ Bonetti, R.; Guglielmetti, A. (2007). "Cluster radioactivity: an overview after twenty years" (PDF). Romanian Reports in Physics. 59: 301–310. Archived from the original (PDF) on 19 September 2016.
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