An element has two isotopes: Isotope 1 with a mass of 13.0 a...

Question Analysis
This question tests the student's ability to calculate the average atomic mass of an element given the masses and natural abundances of its isotopes.

Key Concept Explanation
The average atomic mass is calculated by taking 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: 45% = 0.45 and 55% = 0.55.
2. Use the formula for average atomic mass:
3. Perform the multiplication:

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