Question

Lead consists of four naturally occurring isotopes. Calculate the atomic mass for lead using the weighted average mass method. (4.5) $$ \begin{array}{|l|l|l|} \hline \text { Isotope } & \text { Mass (amu) } & \text { Abundance (\%) } \\ \hline{ }_{82}^{204} \mathrm{~Pb} & 204.0 & 1.40 \\ \hline{ }_{82}^{206} \mathrm{~Pb} & 206.0 & 24.10 \\ \hline{ }_{82}^{207} \mathrm{~Pb} & 207.0 & 22.10 \\ \hline{ }_{82}^{208} \mathrm{~Pb} & 208.0 & 52.40 \\ \hline \end{array} $$

Name: Problem 81, Chapter 4: Basic Chemistry
Uploaded: 2022-03-18T23:59:11-08:00
Duration: 3 min 31 s
Channel: Asami Ehlert
Description: Lead consists of four naturally occurring isotopes. Calculate the atomic mass for lead using the weighted average mass method. (4.5) Isotope Mass (amu) Abundance (%) 82^204 Pb 204.0 1.40 82^206 Pb 206.0 24.10 82^207 Pb 207.0 22.10 82^208 Pb 208.0 52.40

   Lead consists of four naturally occurring isotopes. Calculate the atomic mass for lead using the weighted average mass method. (4.5)
$$
\begin{array}{|l|l|l|}
\hline \text { Isotope } & \text { Mass (amu) } & \text { Abundance (\%) } \\
\hline{ }_{82}^{204} \mathrm{~Pb} & 204.0 & 1.40 \\
\hline{ }_{82}^{206} \mathrm{~Pb} & 206.0 & 24.10 \\
\hline{ }_{82}^{207} \mathrm{~Pb} & 207.0 & 22.10 \\
\hline{ }_{82}^{208} \mathrm{~Pb} & 208.0 & 52.40 \\
\hline
\end{array}
$$

Basic Chemistry

Karen C. Timberlake,… 6th Edition

Chapter 4, Problem 81

Instant Answer

Solved by Expert Asami Ehlert

03/18/2022

Step 1

1.40% = 0.0140 24.10% = 0.2410 22.10% = 0.2210 52.40% = 0.5240 Show more…

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Lead consists of four naturally occurring isotopes. Calculate the atomic mass for lead using the weighted average mass method. (4.5) $$ \begin{array}{|l|l|l|} \hline \text { Isotope } & \text { Mass (amu) } & \text { Abundance (\%) } \\ \hline{ }_{82}^{204} \mathrm{~Pb} & 204.0 & 1.40 \\ \hline{ }_{82}^{206} \mathrm{~Pb} & 206.0 & 24.10 \\ \hline{ }_{82}^{207} \mathrm{~Pb} & 207.0 & 22.10 \\ \hline{ }_{82}^{208} \mathrm{~Pb} & 208.0 & 52.40 \\ \hline \end{array} $$

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Key Concepts

Weighted Average Atomic Mass Calculation

The weighted average atomic mass calculation is a method used to determine the average mass of an element by multiplying the mass of each isotope by its fractional abundance, and then summing these products. This process accurately reflects the contribution of each isotope according to how commonly it occurs in nature.

Isotopes

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. They are naturally occurring variations in an element and play a crucial role in determining the element's average atomic mass.

Isotopic Abundance

Isotopic abundance refers to the relative proportion of each isotope of an element found in nature. It is usually expressed as a percentage and is essential for calculating the weighted average atomic mass since it indicates how much each isotope contributes to the overall atomic mass.

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