In chemistry, natural abundance (NA) refers to the prevalence of isotopes of a chemical element as naturally found on a planet. Chemistry (from Egyptian kēme (chem meaning "earth") is the Science concerned with the composition structure and properties Isotopes (Greek isos = "equal" tópos = "site place" are any of the different types of atoms ( Nuclides A chemical element is a type of Atom that is distinguished by its Atomic number; that is by the number of Protons in its nucleus. The relative atomic mass (a weighted average) of these isotopes is the atomic weight listed for the element in the periodic table. The atomic mass (ma is the Mass of an atom most often expressed in unified atomic mass units The atomic mass may be considered to be the total mass The periodic table of the chemical elements is a tabular method of displaying the Chemical elements Although precursors to this table exist its invention is The abundance of an isotope varies from planet to planet but remains relatively constant in time.
As an example, uranium has three naturally occurring isotopes: U-238, U-235 and U-234. Uranium (jʊˈreɪniəm is a silvery-gray Metallic Chemical element in the Their respective NA is 99. 2745%, 0. 72% and 0. 0055%. For example, if 100,000 uranium atoms were analyzed, one would expect to find approximately 99,275 U-238 atoms, 720 U-235 atoms, and no more than 5 or 6 U-234 atoms. This is because U-238 is much more stable than U-235 or U-234, as the half-life of each isotope reveals: 4. Half-Life (computer-game page here It's already listed in the disambiguation page 468×109 years for U-238 compared to 7. 038×108 years for U-235 and 245,500 years for U-234.
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Deviations from natural abundance
We now know from study of the sun and primitive meteorites that our solar system was initially almost homogeneous in isotopic composition. Deviations from the (evolving) galactic average, locally-sampled around the time that the sun's nuclear burning began, can generally be accounted for by mass fractionation plus a limited number of nuclear decay and transmutation processes[1]. There is also evidence for injection of short-lived (now extinct) isotopes from a nearby supernova explosion that may have triggered solar nebula collapse[2]. Hence deviations from natural abundance on earth are often measured in parts per thousand (per mil or ‰) because they are less than one percent (%).
The single exception to this lies with the presolar grains found in primitive meteorites. Presolar grains are isotopically-distinct clusters of material found in the fine-grained matrix of primitive Meteorites, whose differences from the surrounding meteorite These bypassed the homogenization, and often carry the nuclear signature of specific nucleosynthesis processes in which their elements were made[3]. In these materials, deviations from "natural abundance" are sometimes measured in factors of 100.
See also
Footnotes and References
- ^ Robert N. See also Abundances of the elements (data page The abundance of a Chemical element measures how relatively common the element is or how much of the element Clayton (1978) Isotopic anomalies in the early solar system, Annual Review of Nuclear and Particle Science 28:501-522.
- ^ Ernst Zinner (2003) An isotopic view of the early solar system, Science 300:5617, 265-267.
- ^ Ernst Zinner (1998) Stellar nucleosynthesis and the isotopic composition of presolar grains from primitive meteorites, Annual Review of Earth and Planetary Sciences 26:147-188.
External links
- Stable element isotopic abundance list from the NanoSIMS group at Washington University
- Berkeley Isotopes Project Interactive Table
- Scientific Instrument Services List
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