Calculate the average atomic mass of chlorine 35 (% abundance = 75.77%) and chlorine 37 (% abundance = 24.23%).

To calculate the average atomic mass of chlorine, you can use the formula:

\[
\text{Average Atomic Mass} = (\text{mass of isotope 1} \times \text{fractional abundance of isotope 1}) + (\text{mass of isotope 2} \times \text{fractional abundance of isotope 2})
\]

Here, you are given:
- Mass of Chlorine-35 (\(^{35}\text{Cl}\)) = 35 amu
- Abundance of \(^{35}\text{Cl}\) = 75.77% = 0.7577 (as a decimal)
- Mass of Chlorine-37 (\(^{37}\text{Cl}\)) = 37 amu
- Abundance of \(^{37}\text{Cl}\) = 24.23% = 0.2423 (as a decimal)

Now, substituting these values into the formula:

\[
\text{Average Atomic Mass} = (35 \times 0.7577) + (37 \times 0.2423)
\]

Let's calculate it.

\[
\text{Average Atomic Mass} = (35 \times 0.7577) + (37 \times 0.2423) = 26.5195 + 8.9651 = 35.4846 \, \text{amu}
\]

So, the average atomic mass of chlorine is **35.48 amu**.

Would you like more details on how the calculation works or have any further questions?

Here are some related questions you might find interesting:
1. What is the importance of isotopic abundance in calculating average atomic mass?
2. How does the average atomic mass relate to the periodic table value for chlorine?
3. What are some examples of other elements with multiple isotopes?
4. Can the average atomic mass change over time for an element?
5. How is the average atomic mass used in chemical reactions?

**Tip:** When working with percentages, always convert them to decimals before using them in calculations!

Learn how to calculate the average atomic mass of chlorine using the mass and abundance of isotopes chlorine-35 and chlorine-37. Detailed step-by-step solution with decimal conversion and formula application.

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