An element has two isotopes: isotope A with a mass of 18.0 amu and a natural abundance of 35%, and isotope B with a mass of 20.0 amu and a natural abundance of 65%. The average atomic mass of the element is _________ amu.
Answer & Analysis
Analysis
Question Analysis
This question evaluates the student's ability to calculate the average atomic mass of an element using the given isotopic masses and their natural abundances.
Key Concept Explanation
The average atomic mass is the weighted average of the masses of all naturally occurring isotopes, where the weights are given by their fractional abundances.
Step-by-step Solution
1. Convert the natural abundances to fractional abundances: 35% = 0.35, 65% = 0.65.
2. Use the formula for average atomic mass:
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