3. Bromine atomic mass is 79.9 amu. It exists as two isotopes, one with a mass of 79 and one with a mass of 81. What does this tell you about the relative amount of each isotope? Use numerical ratios. 4 In a sample of 17 500 cilvor:
3. Bromine atomic mass is 79.9 amu. It exists as two isotopes, one with a mass of 79 and one with a mass of 81. What does this tell you about the relative amount of each isotope? Use numerical ratios. 4 In a sample of 17 500 cilvor:
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![**Question:**
3. Bromine atomic mass is 79.9 amu. It exists as two isotopes, one with a mass of 79 and one with a mass of 81. What does this tell you about the relative amount of each isotope? Use numerical ratios.
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**Explanation:**
This exercise involves understanding isotopes and average atomic mass. Bromine's atomic mass is given as 79.9 amu, which is a weighted average of the masses of its isotopes. Since it has isotopes with masses of 79 and 81, one can infer the relative abundances of these isotopes by balancing their contributions to the average mass.
- Let the abundance of the isotope with mass 79 be \( x \).
- Let the abundance of the isotope with mass 81 be \( y \).
Since these are the only two isotopes, \( x + y = 1 \).
The average atomic mass can be expressed as:
\[ 79x + 81y = 79.9 \]
Solving these equations provides the numerical ratio of the isotopes. The isotope with mass 79 must be more prevalent than the isotope with mass 81, as the average atomic mass (79.9) is closer to 79.
Graphs or diagrams related to this could involve:
- A pie chart showing the percentage of each isotope.
- A bar graph comparing the relative amounts.
This understanding of isotope abundance is essential for fields such as chemistry and environmental science, where isotopic composition is used to trace processes and origins.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F79d4d229-649f-4192-a00b-385a235528b8%2Fdf4651ac-5f70-4641-bb06-cc7857d3ce87%2F78yixv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
3. Bromine atomic mass is 79.9 amu. It exists as two isotopes, one with a mass of 79 and one with a mass of 81. What does this tell you about the relative amount of each isotope? Use numerical ratios.
---
**Explanation:**
This exercise involves understanding isotopes and average atomic mass. Bromine's atomic mass is given as 79.9 amu, which is a weighted average of the masses of its isotopes. Since it has isotopes with masses of 79 and 81, one can infer the relative abundances of these isotopes by balancing their contributions to the average mass.
- Let the abundance of the isotope with mass 79 be \( x \).
- Let the abundance of the isotope with mass 81 be \( y \).
Since these are the only two isotopes, \( x + y = 1 \).
The average atomic mass can be expressed as:
\[ 79x + 81y = 79.9 \]
Solving these equations provides the numerical ratio of the isotopes. The isotope with mass 79 must be more prevalent than the isotope with mass 81, as the average atomic mass (79.9) is closer to 79.
Graphs or diagrams related to this could involve:
- A pie chart showing the percentage of each isotope.
- A bar graph comparing the relative amounts.
This understanding of isotope abundance is essential for fields such as chemistry and environmental science, where isotopic composition is used to trace processes and origins.
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