An element has three isotopes: isotope A with a mass of 22.0...

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 determined by summing the products of each isotope's mass and its fractional abundance (natural abundance divided by 100).

Step-by-step Solution
1. Convert percent abundances to decimals:
Isotope A: 20% = 20 ÷ 100 = 0.20
Isotope B: 50% = 50 ÷ 100 = 0.50
Isotope C: 30% = 30 ÷ 100 = 0.30
2. Calculate each isotope’s contribution to the average atomic mass:
Isotope A: 22.0 amu × 0.20 = 4.40 amu
Isotope B: 24.0 amu × 0....

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