Isotopes Isotopes (Caesium-137) Caesium-137 is a radioactive isotope which is formed mainly by nuclear fission. It has a half-life of 30 years, and decays by pure beta decay to a metastable state of barium-137 ( Ba-137m). Barium-137m has a half-life of minutes and is responsible for all the of gamma ray emission. The ground state of barium-137 is stable. ...more on Wikipedia about "Caesium-137"
Calcium 48 is a rare isotope of calcium. 0.187% of natural calcium is calcium 48. Its half life is very long, so it is usually considered stable. It has been used to make ununquadium by bombarding targets of plutonium 244 by beams of calcium 48, accelerated in a particle accelerator. It is used for this purpose because it is a very stable and very neutron rich nucleus, and one problem in making superheavy nuclei like ununquadium is putting enough neutrons in their nucleus. ...more on Wikipedia about "Calcium 48"
Cobalt-60 is a radioactive isotope of cobalt, with a half life of 5.27 years. Cobalt-60 decays by beta decay to the stable isotope nickel-60. In the process of decay, cobalt-60 emits two gamma rays with energies of 1.73 and 1.33 MeV, and one electron with an energy of up to 315 keV. ...more on Wikipedia about "Cobalt-60"
Caesium-137 is a radioactive isotope which is formed mainly by nuclear fission. It has a half-life of 30 years, and decays by pure beta decay to a metastable state of barium-137 ( Ba-137m). Barium-137m has a half-life of minutes and is responsible for all of the gamma ray emission. The ground state of barium-137 is stable. ...more on Wikipedia about "Commonly used gamma emitting isotopes"
Cosmogenic isotopes are rare radioactive isotopes created when cosmic radiation interacts with an atomic nucleus. These isotopes are produced on Earth, in Earth's atmosphere, and in extraterrestrial items such as meteorites. ...more on Wikipedia about "Cosmogenic isotope"
Helium-3 is a light, non- radioactive isotope of helium. The helion, the nucleus of a helium-3 atom, consists of two protons but only one neutron, in contrast to two neutrons in ordinary helium. Helium-3 is rare on Earth and sought-after for use in nuclear fusion. More abundant helium-3 is thought to exist on the Moon (embedded in the upper layer of regolith by the solar wind over billions of years) and the solar system's gas giants (left over from the original solar nebula). As it is a primordial substance in the Earth's mantle, it is used in isotope geochemistry studies. ...more on Wikipedia about "Helium-3"
Helium-4 is a non- radioactive and light isotope of helium. It is by far the most abundant of the two naturally-occurring isotopes of helium, making up about 99.99986% of the helium on earth. Its nucleus is an alpha particle, having two protons and two neutrons. Since the alpha decay is a common decay mode for many radioactive isotopes, this probably explains its abundance. In fact, alpha decay of heavy elements is the source of most naturally occurring helium-4 on earth. ...more on Wikipedia about "Helium-4"
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Isotopes are forms of an element whose nuclei have the same atomic number–-the number of protons in the nucleus--but different atomic masses because they contain different numbers of neutrons. ...more on Wikipedia about "Isotope"
Isotope analysis is the identification of isotopic signature, the distribution of certain stable isotopes and chemical elements within chemical compounds. This can be applied to a food web to make it possible to draw direct inferences regarding diet, trophic level, and subsistence. ...more on Wikipedia about "Isotope analysis"
(Isotope map (0-55)) This isotope table shows all of the known isotopes of the chemical elements, arranged with increasing atomic numbers ( proton numbers) from left to right and increasing neutron numbers from top to bottom. ...more on Wikipedia about "Isotope table (complete)"
These isotope tables show all of the known isotopes of the chemical elements, arranged with increasing atomic number from left to right and increasing neutron number from top to bottom. ...more on Wikipedia about "Isotope table (divided)"
Actinium (Ac) has no stable isotopes. A standard atomic mass cannot be given. ...more on Wikipedia about "Isotopes of actinium"
Aluminium (Al) ...more on Wikipedia about "Isotopes of aluminium"
Americium (Am) has no stable isotopes. A standard atomic mass cannot be given. ...more on Wikipedia about "Isotopes of americium"
Antimony (Sb) ...more on Wikipedia about "Isotopes of antimony"
Argon (Ar) ...more on Wikipedia about "Isotopes of argon"
Arsenic (As) ...more on Wikipedia about "Isotopes of arsenic"
Astatine (At) has no stable isotopes. A standard atomic mass cannot be given. ...more on Wikipedia about "Isotopes of astatine"
Barium (Ba) ...more on Wikipedia about "Isotopes of barium"
Berkelium (Bk) has no stable isotopes. A standard atomic mass cannot be given. ...more on Wikipedia about "Isotopes of berkelium"
Beryllium (Be) ...more on Wikipedia about "Isotopes of beryllium"
Bismuth (Bi) ...more on Wikipedia about "Isotopes of bismuth"
Bohrium (Bh) has no stable isotopes. A standard atomic mass cannot be given. ...more on Wikipedia about "Isotopes of bohrium"
Boron (B) ...more on Wikipedia about "Isotopes of boron"
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