Two isotopes of gallium are naturally occurring, with ^6931...

Two isotopes of gallium are naturally occurring, with $^{69}_{31}$ Ga at $60.11 \%(68.93 \mathrm{amu})$ and $^{71}_{31} \mathrm{Ga}$ at $39.89 \%(70.92 \mathrm{amu})$ Calculate the atomic mass for gallium using the weighted average mass method.

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Key Concepts

Atomic Mass Calculation

Atomic mass calculation involves determining the average mass of an element by summing the products of each isotope's mass and its fractional abundance. This calculation provides a value that reflects the natural isotopic distribution of the element.

Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different mass numbers. They play a crucial role in determining the physical properties of the element.

Isotopic Abundance

Isotopic abundance refers to the relative amount or percentage of each isotope of an element present in a natural sample. This information is vital for calculating average atomic properties like atomic mass.

Weighted Average

A weighted average is an average that takes into account the relative importance or frequency of components. In the context of atomic mass, each isotope's mass is multiplied by its fractional abundance before summing to account for its contribution.

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