A fictional element has two naturally occurring isotopes with the natural abundances shown here: ATOMIC MASS (AMU) ABUNDANCE1650.0%1850.0% Which statement is TRUE for this element?Group of answer choicesThe atomic mass would be 16.The atomic mass would be less than 16.The atomic mass would be 18.The atomic mass would be more than 18.The atomic mass would be 17.
Question
A fictional element has two naturally occurring isotopes with the natural abundances shown here: ATOMIC MASS (AMU) ABUNDANCE1650.0%1850.0% Which statement is TRUE for this element?Group of answer choicesThe atomic mass would be 16.The atomic mass would be less than 16.The atomic mass would be 18.The atomic mass would be more than 18.The atomic mass would be 17.
Solution
The atomic mass of an element is calculated by multiplying the atomic mass of each isotope by its abundance (in decimal form), and then adding these values together.
Here's how you can calculate it for this element:
- Convert the abundances to decimal form: 50.0% = 0.50
- Multiply the atomic mass of each isotope by its abundance:
- For the isotope with an atomic mass of 16: 16 * 0.50 = 8
- For the isotope with an atomic mass of 18: 18 * 0.50 = 9
- Add these values together: 8 + 9 = 17
So, the atomic mass of this element would be 17. Therefore, the correct statement is "The atomic mass would be 17."
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