What Is A Daughter Isotope
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| Standard atomic weight A r°(O) |
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There are three known stable isotopes of oxygen (8O): 16
O
, 17
O
, and 18
O
.
Radioactive isotopes ranging from eleven
O
to 28
O
have besides been characterized, all short-lived. The longest-lived radioisotope is fifteen
O
with a half-life of 122.266(43) south, while the shortest-lived isotope is 11
O
with a half-life of 198(12) yoctoseconds (though the half-lives of the neutron-unbound 27
O
and 28
O
are still unknown).
Listing of isotopes [edit]
| Nuclide[three] [n 1] | Z | N | Isotopic mass (Da) [4] [n 2] | Half-life [resonance width] | Disuse way [n 3] | Girl isotope [n 4] | Spin and parity [n 5] [n vi] | Natural abundance (mole fraction) | |||||||||||
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| Excitation energy | Normal proportion | Range of variation | |||||||||||||||||
| 11 O [5] | 8 | 3 | eleven.051250(threescore) | 198(12) ys [ two.31(14) MeV] | 2p | 9 C | (3/2−) | ||||||||||||
| 12 O | 8 | 4 | 12.034368(13) | 8.nine(three.3) zs | 2p | ten C | 0+ | ||||||||||||
| thirteen O | 8 | 5 | 13.024815(10) | eight.58(5) ms | β+ ( 89.1(2)%) | thirteen N | (3/2−) | ||||||||||||
| β+p ( x.9(2)%) | 12 C | ||||||||||||||||||
| xiv O | eight | six | fourteen.008596 706(27) | 70.621(11) s | β+ | 14 N | 0+ | ||||||||||||
| 15 O | 8 | vii | 15.0030656(v) | 122.266(43) s | β+ | fifteen Due north | 1/2− | ||||||||||||
| 16 O [n vii] | 8 | eight | fifteen.994914 619 257(319) | Stable | 0+ | [ 0.99738 , 0.99776 ][6] | |||||||||||||
| 17 O [n 8] | 8 | nine | sixteen.999131 755 953(692) | Stable | 5/two+ | [ 0.000367 , 0.000400 ][6] | |||||||||||||
| 18 O [n seven] [due north 9] | 8 | 10 | 17.999159 612 136(690) | Stable | 0+ | [ 0.00187 , 0.00222 ][6] | |||||||||||||
| 19 O | viii | 11 | 19.0035780(28) | 26.470(six) s | β− | 19 F | 5/2+ | ||||||||||||
| 20 O | viii | 12 | twenty.0040754(9) | thirteen.51(five) s | β− | 20 F | 0+ | ||||||||||||
| 21 O | 8 | thirteen | 21.008655(xiii) | 3.42(10) due south | β− | 21 F | (five/2+) | ||||||||||||
| β−n ?[due north 10] | 20 F ? | ||||||||||||||||||
| 22 O | 8 | xiv | 22.009970(lx) | two.25(9) s | β− (> 78%) | 22 F | 0+ | ||||||||||||
| β−n (< 22%) | 21 F | ||||||||||||||||||
| 23 O | 8 | 15 | 23.015700(130) | 97(viii) ms | β− ( 93(two)%) | 23 F | 1/2+ | ||||||||||||
| β−n ( 7(two)%) | 22 F | ||||||||||||||||||
| 24 O | 8 | sixteen | 24.019860(180) | 77.4(4.5) ms | β− ( 57(4)%) | 24 F | 0+ | ||||||||||||
| β−n ( 43(four)%) | 23 F | ||||||||||||||||||
| 25 O | 8 | 17 | 25.029340(180) | 5.18(35) zs | due north | 24 O | 3/2+# | ||||||||||||
| 26 O | 8 | xviii | 26.037210(180) | 4.2(3.3) ps | 2n | 24 O | 0+ | ||||||||||||
| 27 O | eight | 19 | 27.047960(540) # | < 260 ns | north ?[n x] | 26 O ? | 3/two+# | ||||||||||||
| 2n ?[n 10] | 25 O ? | ||||||||||||||||||
| 28 O | 8 | 20 | 28.055910(750) # | < 100 ns | 2n ?[n 10] | 26 O ? | 0+ | ||||||||||||
| β− ( 0%) | 28 F | ||||||||||||||||||
| This table header & footer: | |||||||||||||||||||
- ^ mO – Excited nuclear isomer.
- ^ ( ) – Uncertainty (1σ) is given in concise form in parentheses after the corresponding last digits.
- ^ Modes of decay:
- ^ Bold symbol equally daughter – Daughter product is stable.
- ^ ( ) spin value – Indicates spin with weak assignment arguments.
- ^ # – Values marked # are not purely derived from experimental information, but at least partly from trends of neighboring nuclides (TNN).
- ^ a b The ratio between 16
O
and 18
O
is used to deduce ancient temperatures. - ^ Can be used in NMR studies of metabolic pathways.
- ^ Can exist used in studying certain metabolic pathways.
- ^ a b c d Disuse mode shown is energetically allowed, simply has not been experimentally observed to occur in this nuclide.
Stable isotopes [edit]
Late in a massive star's life, sixteen
O
concentrates in the Due north-beat out, 17
O
in the H-beat out and 18
O
in the He-shell.
Natural oxygen is made of three stable isotopes, 16
O
, 17
O
, and xviii
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).
sixteen
O
has high relative and absolute affluence because it is a primary product of stellar evolution and considering it is a primary isotope, meaning it can exist fabricated by stars that were initially hydrogen only.[vii] Most 16
O
is synthesized at the terminate 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 boosted 16
O
.[7]
Both 17
O
and 18
O
are secondary isotopes, significant their synthesis requires seed nuclei. 17
O
is primarily made by called-for hydrogen into helium in the CNO wheel, making it a common isotope in the hydrogen called-for zones of stars.[seven] Most xviii
O
is produced when 14
N
(made abundant from CNO burning) captures a 4
He
nucleus, becoming eighteen
F
. This quickly (half life effectually 110 minutes) beta decays to eighteen
O
making that isotope common in the helium-rich zones of stars.[seven] Well-nigh ten9 kelvin is needed to fuse oxygen into sulfur.[8]
An atomic mass of xvi was assigned to oxygen prior to the definition of the unified atomic mass unit based on 12
C
.[9] Since physicists referred to 16
O
simply, while chemists meant the natural mix of isotopes, this led to slightly dissimilar mass scales.
Applications of various isotopes [edit]
Measurements of 18O/16O ratio are often used to interpret changes in paleoclimate. Oxygen in Earth's air is 99.759% sixteen
O
, 0.037% 17
O
and 0.204% 18
O
.[x] H2o molecules with a lighter isotope are slightly more probable to evaporate and less likely to fall as precipitation,[eleven] and so Earth'southward freshwater and polar ice have slightly less ( 0.1981%) eighteen
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 normally stored in silverish cups and measured with pyrolysis and mass spectrometry.[12] Researchers demand to avoid improper or prolonged storage of the samples for authentic measurements.[12]
Due to natural oxygen beingness mostly sixteen
O samples enriched with the other stable isotopes can be used for isotope labeling. For instance, it was proven, that the oxygen released in photosynthesis originates in HiiO, rather than in the also consumed CO2, past isotope tracing experiments. The oxygen contained in COii in turn is used to make up the sugars formed by photosynthesis.
In heavy water reactors the neutron moderator should preferably be depression in 17
O and 18
O due to their college neutron assimilation cross section compared to 16
O. While this effect tin also be observed in light water reactors, ordinary hydrogen (protium) has a higher absorption cantankerous section than whatever stable isotope of oxygen and its number density is twice equally high in water every bit that of oxygen so that the event is negligible. As some methods of isotope separation enrich non only heavier isotopes of hydrogen simply likewise heavier isotopes of oxygen when producing heavy water, the concentration of 17
O and xviii
O can be measurably higher. Furthermore the 17
O(n,α) xiv
C reaction is a farther 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 limerick and temperature which seafood is from.[xiii]
Radioisotopes [edit]
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 accept half-lives less than 27 s and virtually have half-lives less than 0.1 south. 24
O
has half-life 77.4(4.five) ms. The virtually common disuse way for isotopes lighter than the stable isotopes is β+ decay to nitrogen, and the about common way later is β− decay to fluorine.
Oxygen-13 [edit]
Oxygen-thirteen is an unstable isotope, with 8 protons and v neutrons. It has spin 3/2−, and half-life 8.58(5) ms. Its atomic mass is xiii.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-15 [edit]
Oxygen-xv is a radioisotope, often used in positron emission tomography (PET). It tin be used in, amongst other things, water for PET myocardial perfusion imaging and for brain imaging.[14] [xv] It has an atomic mass of fifteen.0030656(5), and a half-life of 122.266(43) due south. It is produced through deuteron bombardment of nitrogen-xiv using a cyclotron.[16]
Oxygen-15 and nitrogen-13 are produced in air when gamma rays (for instance from lightning) knock neutrons out of 16O and 14N:[17]
- sixteen
O
+ γ → 15
O
+ northward - 14
North
+ γ → xiii
N
+ n
xv
O
decays to fifteen
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 radiations dies down with half-life 2 min, but these low-energy gamma rays go on boilerplate just about 90 metres through the air. Together with rays produced from positrons from nitrogen-13 they may but exist detected for a infinitesimal or so as the "cloud" of 15
O
and 13
O
floats past, carried past the wind.[eighteen]
See likewise [edit]
- Dole effect
References [edit]
- ^ "Standard Atomic Weights: Oxygen". CIAAW. 2009.
- ^ Meija, Juris; et al. (2016). "Atomic weights of the elements 2013 (IUPAC Technical Study)". Pure and Applied Chemical science. 88 (3): 265–91. doi:10.1515/pac-2015-0305.
- ^ Half-life, decay style, nuclear spin, and isotopic composition is sourced in:
Kondev, F. Thousand.; Wang, One thousand.; Huang, Due west. J.; Naimi, S.; Audi, Chiliad. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:ten.1088/1674-1137/abddae. - ^ Wang, Meng; Huang, Due west.J.; Kondev, F.Thousand.; Audi, G.; Naimi, S. (2021). "The AME 2020 atomic mass evaluation (Two). Tables, graphs and references*". Chinese Physics C. 45 (3): 030003. doi:10.1088/1674-1137/abddaf.
- ^ Webb, T. B.; et al. (2019). "First Observation of Unbound elevenO, the Mirror of the Halo Nucleus xiLi". Physical Review Messages. 122 (12): 122501–1–122501–vii. arXiv:1812.08880. Bibcode:2019PhRvL.122l2501W. doi:10.1103/PhysRevLett.122.122501. PMID 30978039. S2CID 84841752.
- ^ a b c "Atomic Weight of Oxygen | Commission on Isotopic Abundances and Diminutive Weights". ciaaw.org . Retrieved 2022-03-15 .
- ^ a b c d B. South. 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.
- ^ Emsley 2001, p. 297.
- ^ Parks & Mellor 1939, Affiliate Half dozen, Department 7.
- ^ Melt & Lauer 1968, p. 500.
- ^ Dansgaard, W (1964). "Stable isotopes in precipitation" (PDF). Tellus. sixteen (4): 436–468. Bibcode:1964Tell...sixteen..436D. doi:10.1111/j.2153-3490.1964.tb00181.x.
- ^ a b Tsang, Homo-Yin; Yao, Weiqi; Tse, Kevin (2020). Kim, Il-Nam (ed.). "Oxidized silver cups can skew oxygen isotope results of small samples". Experimental Results. i: e12. doi:x.1017/exp.2020.xv. ISSN 2516-712X.
- ^ "Using 'chemical fingerprinting' to fight seafood fraud and illegal line-fishing". Phys.org. September 12, 2022. doi:10.1111/faf.12703. Retrieved September thirteen, 2022.
- ^ Rischpler, Christoph; Higuchi, Takahiro; Nekolla, Stephan G. (22 November 2014). "Current and Future Condition of PET Myocardial Perfusion Tracers". Electric current Cardiovascular Imaging Reports. 8 (1): 333–343. doi:x.1007/s12410-014-9303-z. S2CID 72703962.
- ^ Kim, E. Edmund; Lee, Myung-Chul; Inoue, Tomio; Wong, Wai-Hoi (2012). Clinical PET and PET/CT: Principles and Applications. Springer. p. 182. ISBN9781441908025.
- ^ "Production of PET Radionuclides". Austin Hospital, Austin Health. Archived from the original on 15 January 2013. Retrieved 6 Dec 2012.
- ^ Timmer, John (25 November 2017). "Lightning strikes leave behind a radioactive cloud". Ars Technica.
- ^ 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:x.1038/nature24630. PMID 29168803. S2CID 4388159.
- Cook, Gerhard A.; Lauer, Ballad M. (1968). "Oxygen". In Clifford A. Hampel (ed.). The Encyclopedia of the Chemic Elements . New York: Reinhold Book Corporation. pp. 499–512. LCCN 68-29938.
- Emsley, John (2001). "Oxygen". Nature's Edifice Blocks: An A–Z Guide to the Elements. Oxford, England, Great britain: Oxford University Printing. pp. 297–304. ISBN978-0-19-850340-viii.
- Parks, Thousand. D.; Mellor, J. W. (1939). Mellor's Modern Inorganic Chemical science (6th ed.). London: Longmans, Green and Co.
What Is A Daughter Isotope,
Source: https://en.wikipedia.org/wiki/Isotopes_of_oxygen
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