Use the following table of data to calculate the average atomic mass of an unknown element, X: #protons #neutrons % abundance atomic mass (amu) 27.9769 92.2297% 4.6832% 28.9765 3.0872% 29.9738 14 14 14 14 15 16 mass number 28 29 30 Your prediction: A. The calculated value will be closest to 28. B. The calculated value will be closest to 29. C. The calculated value will be closest to 30.

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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**Review & Preview: Calculating Average Atomic Mass**

To calculate the average atomic mass of an unknown element, X, refer to the data table below. The table lists isotopes of element X, characterized by their number of protons, number of neutrons, mass number, percentage abundance, and atomic mass (in amu).

| # protons | # neutrons | mass number | % abundance | atomic mass (amu) |
|-----------|------------|-------------|-------------|-------------------|
| 14        | 14         | 28          | 92.2297%    | 27.9769           |
| 14        | 15         | 29          | 4.6832%     | 28.9765           |
| 14        | 16         | 30          | 3.0872%     | 29.9738           |

**Your Prediction:**

A. The calculated value will be closest to 28.  
B. The calculated value will be closest to 29.  
C. The calculated value will be closest to 30.

**Question:**  
What evidence does the data contain to support your response?  

---

To solve for the average atomic mass, consider the weighted contribution of each isotope based on its abundance.
Transcribed Image Text:**Review & Preview: Calculating Average Atomic Mass** To calculate the average atomic mass of an unknown element, X, refer to the data table below. The table lists isotopes of element X, characterized by their number of protons, number of neutrons, mass number, percentage abundance, and atomic mass (in amu). | # protons | # neutrons | mass number | % abundance | atomic mass (amu) | |-----------|------------|-------------|-------------|-------------------| | 14 | 14 | 28 | 92.2297% | 27.9769 | | 14 | 15 | 29 | 4.6832% | 28.9765 | | 14 | 16 | 30 | 3.0872% | 29.9738 | **Your Prediction:** A. The calculated value will be closest to 28. B. The calculated value will be closest to 29. C. The calculated value will be closest to 30. **Question:** What evidence does the data contain to support your response? --- To solve for the average atomic mass, consider the weighted contribution of each isotope based on its abundance.
Expert Solution
Step 1

Given data: 

For isotope X-14 : 

% Abundance = 92.2297 ÷ 100 = 0.922297 

Atomic mass = 27.9769

For isotope X-15 : 

% abundance = 4.6832 ÷ 100 = 0.046832

Atomic mass = 28.9765

For isotope X-16 : 

% abundance = 3.0872 ÷100 = 0.030872 

Atomic mass = 29.9738 

Using the formula for average atomic mass : 

Average atomic mass of X = 

Sum of [Atomic mass × abundance ] of all isotopes 

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