Average Atomic Mass

The weighted average mass of an element's isotopes, measured in atomic mass units (amu).

Average atomic mass = (mass of isotope 1 × abundance of isotope 1) + (mass of isotope 2 × abundance of isotope 2) + ...

Atoms of the same element that have the same number of protons but different numbers of neutrons.

The relative percentage of a particular isotope in a naturally occurring sample of an element.

Average atomic mass = (10 amu × 0.5) + (12 amu × 0.5) = 11 amu.

Atomic mass units provide a standard unit of mass for atoms and molecules, allowing for easier comparison.

Two atoms are isotopes if they have the same number of protons but different numbers of neutrons.

Average atomic mass = (35 amu × 0.75) + (37 amu × 0.25) = 35.5 amu.

Isotopes of an element are represented by the same element symbol but may have different atomic masses.

Average atomic mass = (mass1 × abundance1) + (mass2 × abundance2) + (mass3 × abundance3).