An isotope that is not decaying over time in contrast with radioactive isotopes.
An isotope of an element that is not radioactive.
Isotopes are atoms of the same element that differ in the number of neutrons contained in the atoms' nuclei. Unstable ‘radioisotopes’ will emit neutrons, protons, or electrons, decaying quickly to stable products. Stable isotopes such as 12C and 13C decay very slowly because their particular combinations of neutrons and protons are stable.
Isotopes of an element have the same atomic number, but different atomic mass. Stable isotopes do not undergo radioactive decay as radio-isotopes do. Elements can exist in both stable and unstable (radioactive) forms. Most elements of biological interest (including C, H, O, N, and S) have two or more stable isotopes, with the lightest of these present in much greater abundance than the others. Among stable isotopes the most useful as biological tracers are the heavy isotopes of hydrogen, carbon and nitrogen. These elements are found in the earth, the atmosphere, and all organisms.
a nonradioactive form of a chemical element
isotopes of an element have the same atomic number, but different atomic mass. Some isotopes undergo spontaneous radioactive decay; stable isotopes do not decay.
Different species of an element that have the same atomic number, but different atomic mass, that are not affected by radioactive decay.
An isotope that does not undergo radioactive decay.
Any naturally occurring, nondecaying isotope (see above) of an element. Many elements have several stable isotopes. For example, carbon (C) has carbon 12 (12C) and carbon 13 (13C).
Stable isotopes are chemical isotopes that are not radioactive. Stable isotopes of the same element have the same chemical characteristics and therefore behave almost identically. The mass differences, due to a difference in the number of neutrons, result in partial separation of the light from heavy isotopes during chemical reactions (isotope fractionation).