Carbon-12 (12 C) is the most abundant of the two stable isotopes of carbon (carbon-13 being the other), amounting to 98.93% of element carbon on Earth; [1] its abundance is due to the triple-alpha process by which it is created in stars.

In 1961 the isotope carbon-12 was selected to replace oxygen as the standard relative to which the atomic weights of all the other elements are measured. Carbon-14, which is radioactive, is the isotope used in radiocarbon dating and radiolabeling.

The following table shows the atomic nuclei that are isotonic (same neutron number N = 6) and isobaric (same nucleon number A = 12) with Carbon-12. Naturally occurring isotopes are marked in green; light green = naturally occurring radionuclides.

2020年1月23日 · Carbon-12 and carbon-14 are two isotopes of the element carbon. The difference between carbon-12 and carbon-14 is the number of neutrons in each of their atoms.

Carbon-12 (also written 12 C) is an isotope of carbon. It is the most common isotope of carbon, as 98.89% of all carbon is this type of carbon. It is one of two stable (non-radioactive) isotopes of carbon. The other is carbon-13. Carbon-12 is important in chemistry as it is the benchmark from which all other relative atomic masses are worked ...

Carbon-12 is the most abundant isotope of the element carbon, with a nucleus containing 6 protons and 6 neutrons. It is the primary standard used to define the atomic mass scale and is a crucial component in understanding atomic structure and the mole concept in chemistry.

Carbon-12 and Carbon-14 differ in their atomic structure due to the number of neutrons present in their nuclei. Carbon-12, the most abundant carbon isotope, has 6 protons and 6 neutrons, giving it an atomic mass of 12 atomic mass units (amu). On the other hand, Carbon-14 has 6 protons and 8 neutrons, resulting in an atomic mass of 14 amu.