Chlorine has two naturally occurring isotopes: chlorine-35 w...

Question Analysis
This question tests the student's ability to calculate the average atomic mass of an element with multiple isotopes, using their masses and natural abundances.

Key Concept Explanation
The average atomic mass is the sum of the products of each isotope's mass and its fractional abundance.

Step-by-step Solution
1. Convert the natural abundances to fractional abundances: 75.77% = 0.7577, 24.23% = 0.2423.
2. Calculate the contribution of each isotope: (34.97 amu * 0.7577) + (36.97 amu * 0.2423).
3. Perform ...

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