Lead consists of four naturally occurring isotopes....

Lead consists of four naturally occurring isotopes. Calculate the atomic mass for lead using the weighted average mass method. $(4.5)$ $$ \begin{array}{lll} \text { Isotope } & \text { Mass (amu) } & \text { Abundance (\%) } \\ { }_{82}^{204} \mathrm{~Pb} & 204.0 & 1.40 \\ { }_{82}^{206} \mathrm{~Pb} & 206.0 & 24.10 \\ { }^{207} \mathrm{~Pb} & 207.0 & 22.10 \\ { }^{20} \mathrm{~Pb} & 208.0 & 52.40 \end{array} $$

Lead consists of four naturally occurring isotopes. Calculate the atomic mass for lead using the weighted average mass method. $(4.5)$
$$
\begin{array}{lll}
\text { Isotope } & \text { Mass (amu) } & \text { Abundance (\%) } \\
{ }_{82}^{204} \mathrm{~Pb} & 204.0 & 1.40 \\
{ }_{82}^{206} \mathrm{~Pb} & 206.0 & 24.10 \\
{ }^{207} \mathrm{~Pb} & 207.0 & 22.10 \\
{ }^{20} \mathrm{~Pb} & 208.0 & 52.40
\end{array}
$$

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Key Concepts

Weighted Average Method

The weighted average method is a calculation technique used to determine the average atomic mass of an element by multiplying the mass of each isotope by its fractional abundance and then summing these products. This method accurately reflects the contributions of all naturally occurring isotopes based on their prevalence.

Isotopic Abundance

Isotopic abundance indicates the relative proportion of each isotope present in a sample of an element, typically expressed as a percentage. This distribution is critical for calculating the average atomic mass, as each isotope’s mass is weighted by its abundance.

Atomic Mass

Atomic mass refers to the mass of an atom as measured in atomic mass units (amu), taking into account the masses of protons, neutrons, and electrons. It represents an average value for elements that have multiple isotopes, thereby reflecting the weighted contribution of each isotope's mass based on its natural occurrence.

Isotope

An isotope is a variant of a given chemical element that shares the same number of protons but has a different number of neutrons. While isotopes exhibit nearly identical chemical properties, their differing masses influence the overall atomic mass of the element.

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