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As a result it is always undergoing natural radioactive decay while the abundances of the other isotopes are unchanged.
When isotopes are to be designated specifically, the chemical symbol is expanded to identify the mass (for example, C is not stable.They have masses of 13 and 14 respectively and are referred to as "carbon-13" and "carbon-14." If two atoms have equal numbers of protons but differing numbers of neutrons, one is said to be an "isotope" of the other.Carbon-13 and carbon-14 are thus isotopes of carbon-12.Rachel Wood does not work for, consult, own shares in or receive funding from any company or organisation that would benefit from this article, and has disclosed no relevant affiliations beyond the academic appointment above.Australian National University provides funding as a member of The Conversation AU.
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The total mass of the isotope is indicated by the numerical superscript.