What is the Difference Between Carbon 12 and Carbon 14?

Carbon-12 and Carbon-14 are both isotopes of the element carbon, which means they have the same number of protons but different numbers of neutrons. The main differences between them are:

1. Neutrons: Carbon-12 has 6 neutrons, while Carbon-14 has 8 neutrons.
2. Stability: Carbon-12 is a stable isotope, meaning it does not undergo radioactive decay. In contrast, Carbon-14 is unstable and does undergo radioactive decay with a half-life of about 5,730 years.
3. Relative Atomic Mass: Carbon-12 has a relative atomic mass of approximately 12.00 atomic mass units (amu), while Carbon-14 has a relative atomic mass of approximately 14.00 amu.
4. Natural Abundance: Carbon-12 is the most abundant isotope of carbon, accounting for almost 99% of all carbon on Earth. Carbon-14 is much rarer, with only one out of every trillion carbon atoms being Carbon-14.

Carbon-14 is used in radiometric dating to determine the ages of old artifacts and fossils, as its radioactive decay can be used as a "clock" to measure the age of an object.

Comparative Table: Carbon 12 vs Carbon 14

Carbon-12 and carbon-14 are two isotopes of the element carbon. The main differences between them are the number of neutrons in each atom, their stability, and their natural abundance. Here is a comparison table highlighting the differences:

Carbon-12 is more abundant and has a stable nucleus due to its 1:1 ratio of protons and neutrons. On the other hand, carbon-14 has an unstable nucleus and undergoes alpha decay, producing atoms of nitrogen-14. Carbon-14 dating is a method used to determine the age of artifacts that are not more than 50,000 years old.