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The nucleus of each atom consists of protons and neutrons. The number of protons defines the element and the sum of protons and neutrons gives the atomic mass, while the number of neutron defines the isotopes of that element. For example, most carbon has 6 protons and 6 neutrons, and it is written as 12C, which represents its atomic mass. However, about 1% of the earth's carbon has 6 protons and 7 neutrons (13C), forming a stable isotope of this important element. Stable isotopes do not decay into other elements. On the contrary, radioisotopes (such as 14C) are unstable and easily decay into other elements. In general, the less abundant stable isotopes have one or two additional neutrons than protons. Both heavy and light stable isotopes are free to participate in chemical reactions and biological and geochemical processes, but the rates during the reactions are different. The light stable isotopes react faster than the heavy ones.
