An element Q has three isotopes: Q-16 (mass = 15.99 amu, abu...

Question Analysis
This question evaluates the student's ability to calculate the average atomic mass of an element using the given 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 abundances to decimals:
Q-16: 50% = 0.50; Q-17: 25% = 0.25; Q-18: 25% = 0.25
2. Calculate contributions:
Q-16: 15.99 × 0.50 = 7.995 amu
Q-17: 16.99 × 0.25 = 4.2475 amu
Q-18: 17.99 ×...

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