The majority of elements are found in mixtures of two or more isotopes in nature. Every element's isotope has a set mass and a natural percent abundance. These isotopes' masses in their respective abundances must be reflected in the element's mass.
- Every isotope contributes to the average atomic mass of an element, which is displayed in the element's box on most periodic tables (at least, the isotopes that exist naturally). However, the average is a weighted average.
- A weighted average mass is an average that considers the frequency of each mass in the sample.
- Atoms with the same atomic number that have varied masses because of differing neutron counts are known as isotopes. The weighted average of an element's isotopes' masses determines its atomic mass. Each isotope's mass and relative abundance as they exist in nature are considered in the weighted average.
These are the reasons for different values of weighted average atomic mass.
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