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Introduction
Copper is a chemical element with the symbol Cu and atomic number 29. It is a highly versatile metal that has been used by humans for thousands of years due to its excellent electrical conductivity, malleability, and resistance to corrosion. Copper is found in nature in two main isotopes, which have different atomic masses and relative abundances. In this article, we will explore the concept of average atomic mass and how it is calculated for copper.
What is Average Atomic Mass?
The average atomic mass of an element is the weighted average of the masses of its naturally occurring isotopes. It is a measure of the total mass of an element, taking into account the masses of all its isotopes and their relative abundances. The average atomic mass is usually expressed in units of atomic mass units (amu) or grams per mole (g/mol).
Calculating Average Atomic Mass
To calculate the average atomic mass of an element, we need to know the masses of its isotopes and their relative abundances. The relative abundance of an isotope is the percentage of that isotope present in a sample of the element. We can calculate the average atomic mass using the following formula:
Average atomic mass = (mass of isotope 1 x relative abundance of isotope 1) + (mass of isotope 2 x relative abundance of isotope 2) + ...
The Isotopes of Copper
Copper has two naturally occurring isotopes: copper-63 (63Cu) and copper-65 (65Cu). The masses of these isotopes are 62.9296 u and 64.9278 u, respectively. The relative abundances of these isotopes are 69.15% and 30.85%, respectively.
| Isotope | Mass (u) | Relative Abundance (%) |
|---|---|---|
| 63Cu | 62.9296 | 69.15 |
| 65Cu | 64.9278 | 30.85 |
Calculating the Average Atomic Mass of Copper
Now that we have the masses and relative abundances of the two isotopes of copper, we can calculate the average atomic mass of copper using the formula above.
Average atomic mass = (62.9296 u x 69.15%) + (64.9278 u x 30.85%)
First, we need to convert the relative abundances from percentages to decimal form.
69.15% = 0.6915 30.85% = 0.3085
Now we can plug in the values and calculate the average atomic mass.
Average atomic mass = (62.9296 u x 0.6915) + (64.9278 u x 0.3085) = 43.555 u + 20.035 u = 63.59 u
Conclusion
In conclusion, the average atomic mass of copper is 63.59 u. This value is a weighted average of the masses of the two naturally occurring isotopes of copper, taking into account their relative abundances. The average atomic mass of an element is an important concept in chemistry, as it allows us to understand the total mass of an element and its isotopic composition.
References
- IUPAC. (2019). Atomic Weights of the Elements 2019. Journal of Physical and Chemical Reference Data, 48(3), 041101.
- National Institute of Standards and Technology. (2020). Atomic Weights of the Elements. Retrieved from https://www.nist.gov/pml/weights-and-measures/atomic-weights-elements
Further Reading
- Chemistry: An Atoms First Approach. (2019). By Steven S. Zumdahl. Cengage Learning.
- General Chemistry: Principles and Modern Applications. (2019). By Linus Pauling. Pearson Education.
Q: What is the average atomic mass of copper?
A: The average atomic mass of copper is 63.59 u.
Q: Why is the average atomic mass of copper important?
A: The average atomic mass of copper is important because it allows us to understand the total mass of the element and its isotopic composition. This information is crucial in chemistry, as it helps us to predict the behavior of copper in different chemical reactions and processes.
Q: What are the two naturally occurring isotopes of copper?
A: The two naturally occurring isotopes of copper are copper-63 (63Cu) and copper-65 (65Cu).
Q: What are the masses of the two naturally occurring isotopes of copper?
A: The masses of the two naturally occurring isotopes of copper are 62.9296 u and 64.9278 u, respectively.
Q: What are the relative abundances of the two naturally occurring isotopes of copper?
A: The relative abundances of the two naturally occurring isotopes of copper are 69.15% and 30.85%, respectively.
Q: How is the average atomic mass of copper calculated?
A: The average atomic mass of copper is calculated using the formula:
Average atomic mass = (mass of isotope 1 x relative abundance of isotope 1) + (mass of isotope 2 x relative abundance of isotope 2) + ...
Q: What is the significance of the average atomic mass of copper in chemistry?
A: The average atomic mass of copper is significant in chemistry because it helps us to predict the behavior of copper in different chemical reactions and processes. It also allows us to understand the total mass of the element and its isotopic composition.
Q: Can the average atomic mass of copper be changed?
A: No, the average atomic mass of copper cannot be changed. It is a fixed value that is determined by the masses of the two naturally occurring isotopes of copper and their relative abundances.
Q: How is the average atomic mass of copper used in real-world applications?
A: The average atomic mass of copper is used in real-world applications such as:
- Calculating the density of copper
- Predicting the behavior of copper in different chemical reactions and processes
- Understanding the total mass of copper and its isotopic composition
Q: What are some common mistakes to avoid when calculating the average atomic mass of copper?
A: Some common mistakes to avoid when calculating the average atomic mass of copper include:
- Not using the correct masses of the two naturally occurring isotopes of copper
- Not using the correct relative abundances of the two naturally occurring isotopes of copper
- Not converting the relative abundances from percentages to decimal form
Q: Where can I find more information about the average atomic mass of copper?
A: You can find more information about the average atomic mass of copper in the following resources:
- IUPAC. (2019). Atomic Weights of the Elements 2019. Journal of Physical and Chemical Reference Data, 48(3), 041101.
- National Institute of Standards and Technology. (2020). Atomic Weights of the Elements. Retrieved from https://www.nist.gov/pml/weights-and-measures/atomic-weights-elements
- Chemistry: An Atoms First Approach. (2019). By Steven S. Zumdahl. Cengage Learning.
- General Chemistry: Principles and Modern Applications. (2019). By Linus Pauling. Pearson Education.
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