Radioactive sulfur isotopes; Stable sulfur isotopes
Sulfur. A chemical element that is one of the constituents of living organisms and of the Earth.
Isotopes. Isotopes are different nuclear forms of the same element. For a given element, a constant number of protons but different numbers of neutrons in the nucleus correspond to different isotopes. Sulfur of standard atomic mass 32.065 u has 18 isotopes, most of which are not stable and undergo radioactive decay.
Stable sulfur isotopes. Stable isotopes are isotopes that do not decay within an experimentally observable time frame. Stable isotopes have essentially the same chemical characteristics and, therefore, their behavior is chemically almost identical. The different masses lead to isotope fractionation in chemical, physical, and especially biological reactions. Four stable isotopes occur in nature: 32S (95.02%), 33S (0.75%), 34S (4.21%), and 36S (0.02%) (Hoefs, 2008). Typically, the ratio of the two most...
KeywordsSulfate Reduction Hydrogen Sulfide Sulfur Isotope Iron Sulfide Sulfur Cycle
- Amend, J. P., Edwards, K. J., and Lyons, T. W. (eds.), 2004. Sulfur Biogeochemistry - Past and Present. Boulder: Geological Society of America.Google Scholar
- Böttcher, M. E., and Piel, C., 2008. Kinetic S-34/S-32 fractionation during degassing and hydroxylation of hydrogen sulfide, and protonation of bisulfide. Geophysical Research Abstracts, 10, 232.Google Scholar
- Canfield, D. E., 2001. Biogeochemistry of sulfur isotopes. In Valley, J. W., and Cole, D. R. (eds.), Reviews in Mineralogy and Geochemistry, The Mineralogical Society of America, 607.Google Scholar
- Clark, I. D., and Fritz, P., 1997. Environmental Isotopes in Hydrogeology. Boca Raton: Lewis.Google Scholar
- Hoefs, J., 2008. Stable Isotope Geochemistry, 6th edn. Berlin: Springer.Google Scholar