There are two naturally occurring isotopes of Copper (Cu). The table shows the two isotopes, their abundance, and their mass in amu. Calculate the average atomic mass of copper.
There are two naturally occurring isotopes of Copper (Cu). The table shows the two isotopes, their abundance, and their mass in amu. Calculate the average atomic mass of copper.
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
Chapter1: Chemical Foundations
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There are two naturally occurring isotopes of Copper (Cu). The table shows the two isotopes, their abundance, and their mass in amu. Calculate the average atomic mass of copper.
![The image provides two formulas for calculating the average atomic mass of an element based on its isotopes:
1. **Using Percentage Abundances:**
\[
\text{Avg Atomic Mass} = \frac{(M_1 \times A_1) + (M_2 \times A_2) + (M_3 \times A_3)}{100}
\]
- \( M_1, M_2, M_3 \) are the masses of the isotopes.
- \( A_1, A_2, A_3 \) are the percentage abundances of these isotopes.
2. **Using Decimal Abundances:**
\[
\text{Avg Atomic Mass} = (M_1 \times a_1) + (M_2 \times a_2) + (M_3 \times a_3)
\]
- Here, \( a_1, a_2, a_3 \) represent the decimal abundances of the isotopes instead of percentages.
These equations are used in chemistry to determine the weighted average mass of an element's atoms as they occur in nature.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1b25ade9-dba1-417e-936c-f60e5fc2acc1%2F6202c05b-64ab-4632-8e67-bf0d2c1b9c88%2Fnb6t9y_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The image provides two formulas for calculating the average atomic mass of an element based on its isotopes:
1. **Using Percentage Abundances:**
\[
\text{Avg Atomic Mass} = \frac{(M_1 \times A_1) + (M_2 \times A_2) + (M_3 \times A_3)}{100}
\]
- \( M_1, M_2, M_3 \) are the masses of the isotopes.
- \( A_1, A_2, A_3 \) are the percentage abundances of these isotopes.
2. **Using Decimal Abundances:**
\[
\text{Avg Atomic Mass} = (M_1 \times a_1) + (M_2 \times a_2) + (M_3 \times a_3)
\]
- Here, \( a_1, a_2, a_3 \) represent the decimal abundances of the isotopes instead of percentages.
These equations are used in chemistry to determine the weighted average mass of an element's atoms as they occur in nature.
Transcribed Image Text:**Naturally Occurring Isotopes of Copper**
| Isotope | Atomic Mass (atomic mass units, u) | Percent Natural Abundance (%) |
|---------|-----------------------------------|-------------------------------|
| Cu-63 | 62.93 | 69.17 |
| Cu-65 | 64.93 | 30.83 |
This table provides information about the two naturally occurring isotopes of copper. It includes their atomic masses in atomic mass units (u) and their percent natural abundances. Cu-63 has an atomic mass of 62.93 u and a natural abundance of 69.17%, while Cu-65 has an atomic mass of 64.93 u and a natural abundance of 30.83%.
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