Antimony (Sb) has two naturally occurring isotopes: Sb-121...

Antimony (Sb) has two naturally occurring isotopes: Sb-121 that has a percentage abundance of $57.21 \%$ and a mass of $120.90 \mathrm{amu}$, and $\mathrm{Sb}-123$ that has a percentage abundance of $42.79 \%$ and a mass of $122.90$ amu. Calculate the atomic mass for antimony using the weighted average mass method. (4.5)

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Key Concepts

Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons. They result in different atomic masses for the same element, and their natural occurrence in various proportions affects the overall atomic mass of the element.

Percent Abundance

Percent abundance refers to the relative amount of each isotope present in a naturally occurring sample of an element. These percentages represent how common each isotope is and are used as weights in calculating the atomic mass.

Weighted Average Calculation

The weighted average calculation is a method for determining a representative average value by multiplying each value by its corresponding weight (or percent abundance) and then summing the results. This method ensures that the more abundant isotopes have a proportionally larger effect on the overall average.

Atomic Mass Computation

Atomic mass computation for an element involves summing the products of each isotope's mass and its corresponding fractional abundance (percent abundance divided by 100). The result gives the weighted atomic mass, providing a more accurate representation of the element's mass as found in nature.

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