Abstract
Many of the elements in the periodic table consist of more than one isotope, i.e., chemically identical species with differing atomic masses. Most of these isotopes are not radioactive in their natural state and are referred to as stable isotopes. The element copper, for example, has an atomic number of 29 and an atomic weight of 63.5, and consists of two stable isotopes: 63Cu and 65Cu. The atomic nucleus of each contains 29 protons, but 65Cu contains 2 more neutrons than 63Cu in its nucleus. The 2 stable isotopes of copper have “atomic weights” of 63 and 65 and thus differ in mass while being chemically identical. Naturally occurring copper is about 69% 63Cu and about 31% 65Cu, resulting in the overall elemental atomic weight of 63.5.
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References
Veillon, C. and R. Alvarez. 1983. Determination of trace metals in biological materials by stable isotope dilution. Chapter 5 in “Metal Ions in Biological Systems”, H. Sigel, ed. Marcel Dekker, Inc. New York, pp. 103–122.
Swanson, C.A., D.C. Reamer, C. Veillon, J.C. King and O.A. Levander. 1983. Quantitative and qualitative aspects of selenium utilization in pregnant and nonpregnant women: an application of stable isotope methodology. Am. J. Clin. Nutr. 38: 169–180.
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© 1988 Martinus Nijhoff Publishers, Dordrecht
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Veillon, C. (1988). Application of stable isotopes in analysis and metabolism. In: Beecher, G.R. (eds) Research Instrumentation for the 21st Century. Beltsville Symposia in Agricultural Research, vol 11. Springer, Dordrecht. https://doi.org/10.1007/978-94-009-2748-3_3
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DOI: https://doi.org/10.1007/978-94-009-2748-3_3
Publisher Name: Springer, Dordrecht
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