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9. Element X has two naturally occurring isotopes; 10x with a percent abundance of 85% and 12x with a percent of 15% abundance Which is the most likely average atomic mass for element X? A. 10.1 amu B. 11.9 amu C. 12.3 amu D. 22.0 amu 2

9. Element X has two naturally occurring isotopes; 10x with a percent abundance of 85% and 12x with a percent of 15% abundance Which is the most likely average atomic mass for element X? A. 10.1 amu B. 11.9 amu C. 12.3 amu D. 22.0 amu 2

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question 9:** Element X has two naturally occurring isotopes, \(^{10}\text{X}\) with a percent abundance of 85% and \(^{12}\text{X}\) with a percent abundance of 15%. Which is the most likely average atomic mass for element X? - A. 10.1 amu - B. 11.9 amu - C. 12.3 amu - D. 22.0 amu *Explanation:* To determine the most likely average atomic mass, use the formula: \[ \text{Average atomic mass} = (\text{mass of } ^{10}\text{X} \times \text{abundance of } ^{10}\text{X}) + (\text{mass of } ^{12}\text{X} \times \text{abundance of } ^{12}\text{X}) \] Convert the percentage abundances into decimal form before calculating.
Transcribed Image Text:**Question 9:** Element X has two naturally occurring isotopes, \(^{10}\text{X}\) with a percent abundance of 85% and \(^{12}\text{X}\) with a percent abundance of 15%. Which is the most likely average atomic mass for element X? - A. 10.1 amu - B. 11.9 amu - C. 12.3 amu - D. 22.0 amu *Explanation:* To determine the most likely average atomic mass, use the formula: \[ \text{Average atomic mass} = (\text{mass of } ^{10}\text{X} \times \text{abundance of } ^{10}\text{X}) + (\text{mass of } ^{12}\text{X} \times \text{abundance of } ^{12}\text{X}) \] Convert the percentage abundances into decimal form before calculating.
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