An element consists of 4.35% of an isotope with mass 49.946 u, 83.79% of an isotope with mass 51.9405 u, 9.50% of an isotope with mass 52.9406 u, and 2.36% of an isotope with mass 53.9389 u. Calculate the average atomic mass, and identify the element.
An element consists of 4.35% of an isotope with mass 49.946 u, 83.79% of an isotope with mass 51.9405 u, 9.50% of an isotope with mass 52.9406 u, and 2.36% of an isotope with mass 53.9389 u. Calculate the average atomic mass, and identify the element.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter3: Stoichiometry
Section: Chapter Questions
Problem 136AE: Boron consists of two isotopes, 10B and 11B. Chlorine also has two isotopes, 35Cl and 37Cl. Consider...
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An element consists of 4.35% of an isotope with mass 49.946 u, 83.79% of an isotope with mass 51.9405 u, 9.50% of an isotope with mass 52.9406 u, and 2.36% of an isotope with mass 53.9389 u. Calculate the
Expert Solution
Step 1
Average atomic mass:
The average atomic mass of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance. The average atomic mass of an element can be calculated as follows:
- Change each percent abundance of the isotope into decimal form by dividing by 100.
- Multiply this value by the atomic mass of that isotope.
- And finally, add together for each isotope to get the average atomic mass.
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