Average Atomic Mass

The weighted average of the masses of an element's isotopes, taking into account their relative abundances.

Multiply the mass of each isotope by its relative abundance (as a decimal), then sum these values.

0.30 * 4 amu = 1.2 amu.

10.812 amu.

Isotopes have different masses and abundances, which affect the overall average atomic mass of an element.

Isotopes are variants of the same element that have the same number of protons but different numbers of neutrons.

Isotopes of the same element have the same atomic number but different mass numbers.

The total number of protons and neutrons in the nucleus of an atom.

The isotopes contribute to this average based on their masses and relative abundances.

Contribution = (mass of isotope) * (relative abundance).