Oxygen-17
| General | |
|---|---|
Excess energy | −809 keV |
| Binding energy | 131763 keV |
| Isotopes of oxygen Complete table of nuclides | |
Oxygen-17 (17O) is a low-abundance, natural, stable isotope of oxygen (0.0373% in seawater; approximately twice as abundant as deuterium).
As the only stable isotope of oxygen possessing a
Water used as nuclear reactor coolant is subjected to intense neutron flux. Natural water starts out with 373 ppm of 17O; heavy water starts out incidentally enriched to about 550 ppm of oxygen-17. 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.[4][5]
History
The isotope was first hypothesized and subsequently imaged by
Of the nature of the integrated nucleus little can be said without further data. It must however have a mass 17, and provided no other nuclear electrons are gained or lost in the process, an atomic number 8. It ought therefore to be an isotope of oxygen. If it is stable it should exist on the earth.
—Patrick Blackett
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.[7] Its natural abundance in Earth's atmosphere was later detected in 1929 by Giauque and Johnson in absorption spectra.[8]
References
- ISBN 978-3-540-40227-5.
- .
- PMID 2350339.
- ^ http://www.nrc.gov/docs/ML1016/ML101650129.pdf Estimation of Carbon-14 in Nuclear Power Plant Gaseous Effluents; EPRI; June 10, 2010
- ^ A Compact, Low Cost, Tritium Removal Plant for Candu-6 Reactors; S.K. Sood, C. Fong, and K.M. Kalyanam; Ontario Hydro
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