Why the atomic mass on your periodic table is rarely a whole number
In short: This video explains average atomic mass, detailing how scientists calculate the weighted average mass of atoms found in a naturally occurring sample of an element. It is essential for understanding why these values are not simple integers.
Average atomic mass, occasionally referred to as atomic weight, represents the weighted average of all atoms within a natural sample of a specific element. Because elements exist as mixtures of different isotopes, these values reflect the distribution of those isotopes in nature.
These masses are measured in unified atomic mass units, denoted as u. By definition, 1 u is exactly one-twelfth the mass of a single neutral carbon-12 atom.
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Sources
- Summary by Intellect · source: Average atomic mass | AP Chemistry | Khan Academy
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