What Is The Average Atomic Mass Of The Element In The Data Table?${ \begin{tabular}{|c|c|} \hline \text{Mass (amu)} & \text{Abundance (%)} \ \hline 63.00 & 69.17 \ \hline 65.00 & 30.83 \ \hline \end{tabular} }$A. 15.46 Amu B. 85.24 Amu
Understanding the Concept of Average Atomic Mass
In chemistry, the average atomic mass of an element is a weighted average of the masses of its naturally occurring isotopes. This value is essential in understanding the properties and behavior of elements in various chemical reactions and processes. In this article, we will explore how to calculate the average atomic mass of an element using a data table that provides the mass and abundance of its isotopes.
The Data Table
The following data table provides the mass and abundance of the isotopes of an element:
| Mass (amu) | Abundance (%) |
|---|---|
| 63.00 | 69.17 |
| 65.00 | 30.83 |
Calculating the Average Atomic Mass
To calculate the average atomic mass of the element, we need to multiply the mass of each isotope by its abundance and then sum up the results. The abundance is given as a percentage, so we need to convert it to a decimal by dividing by 100.
Step 1: Convert Abundance to Decimal
| Mass (amu) | Abundance (%) | Abundance (Decimal) |
|---|---|---|
| 63.00 | 69.17 | 0.6917 |
| 65.00 | 30.83 | 0.3083 |
Step 2: Multiply Mass by Abundance
| Mass (amu) | Abundance (Decimal) | Product |
|---|---|---|
| 63.00 | 0.6917 | 43.65 |
| 65.00 | 0.3083 | 20.04 |
Step 3: Sum Up the Products
The sum of the products is:
43.65 + 20.04 = 63.69
Calculating the Average Atomic Mass
The average atomic mass is calculated by dividing the sum of the products by the sum of the abundances. However, since the sum of the abundances is equal to 1 (100%), we can simply use the sum of the products as the average atomic mass.
Average Atomic Mass
The average atomic mass of the element is:
63.69 amu
Comparison with the Options
The calculated average atomic mass of 63.69 amu is closest to option B. 63.00 amu. However, since the calculated value is slightly higher than 63.00 amu, we can conclude that the correct answer is not option A or B, but rather a value that is close to 63.69 amu.
Conclusion
In conclusion, the average atomic mass of the element in the data table is 63.69 amu. This value is calculated by multiplying the mass of each isotope by its abundance and then summing up the results. The calculated value is closest to option B, but since the calculated value is slightly higher than 63.00 amu, we can conclude that the correct answer is not option A or B, but rather a value that is close to 63.69 amu.
Frequently Asked Questions
Q: What is the average atomic mass of an element?
A: The average atomic mass of an element is a average of the masses of its naturally occurring isotopes.
Q: How is the average atomic mass calculated?
A: The average atomic mass is calculated by multiplying the mass of each isotope by its abundance and then summing up the results.
Q: What is the significance of the average atomic mass?
A: The average atomic mass is essential in understanding the properties and behavior of elements in various chemical reactions and processes.
Q: How is the abundance of an isotope represented in the data table?
A: The abundance of an isotope is represented as a percentage in the data table.
Q: What is the sum of the products in the calculation of the average atomic mass?
A: The sum of the products is 63.69 amu.
Q: What is the average atomic mass of the element in the data table?
A: The average atomic mass of the element in the data table is 63.69 amu.
References
- [1] "Atomic Masses of the Elements 2016" by IUPAC
- [2] "The Elements" by John Emsley
- [3] "Chemistry: An Atoms First Approach" by Steven S. Zumdahl
Glossary
- Abundance: The percentage of an isotope in a naturally occurring sample of an element.
- Average Atomic Mass: A weighted average of the masses of the naturally occurring isotopes of an element.
- Isotope: A version of an element that has a different number of neutrons in its atomic nucleus.
- Mass: The amount of matter in an object or particle.
- Nucleus: The central part of an atom that contains the protons and neutrons.
Frequently Asked Questions: Average Atomic Mass =====================================================
Q: What is the average atomic mass of an element?
A: The average atomic mass of an element is a weighted average of the masses of its naturally occurring isotopes.
Q: How is the average atomic mass calculated?
A: The average atomic mass is calculated by multiplying the mass of each isotope by its abundance and then summing up the results.
Q: What is the significance of the average atomic mass?
A: The average atomic mass is essential in understanding the properties and behavior of elements in various chemical reactions and processes.
Q: How is the abundance of an isotope represented in the data table?
A: The abundance of an isotope is represented as a percentage in the data table.
Q: What is the sum of the products in the calculation of the average atomic mass?
A: The sum of the products is 63.69 amu.
Q: What is the average atomic mass of the element in the data table?
A: The average atomic mass of the element in the data table is 63.69 amu.
Q: How do I calculate the average atomic mass of an element with multiple isotopes?
A: To calculate the average atomic mass of an element with multiple isotopes, you need to multiply the mass of each isotope by its abundance and then sum up the results.
Q: What is the difference between atomic mass and average atomic mass?
A: Atomic mass refers to the mass of a single atom of an element, while average atomic mass refers to the weighted average of the masses of its naturally occurring isotopes.
Q: How do I determine the abundance of an isotope in a naturally occurring sample?
A: The abundance of an isotope in a naturally occurring sample can be determined using various methods, including mass spectrometry and nuclear reactions.
Q: What is the significance of the average atomic mass in chemistry?
A: The average atomic mass is essential in understanding the properties and behavior of elements in various chemical reactions and processes, such as nuclear reactions, chemical bonding, and phase changes.
Q: How do I calculate the average atomic mass of an element with a non-integer abundance?
A: To calculate the average atomic mass of an element with a non-integer abundance, you need to convert the abundance to a decimal by dividing by 100 and then multiply the mass of the isotope by the decimal abundance.
Q: What is the average atomic mass of an element with two isotopes, one with a mass of 12 amu and an abundance of 99.9% and the other with a mass of 13 amu and an abundance of 0.1%?
A: To calculate the average atomic mass of this element, you need to multiply the mass of each isotope by its abundance and then sum up the results.
| Mass (amu) | Abundance (%) | Abundance (Decimal) | Product |
|---|---|---|---|
| 12.00 99.9 | 0.999 | 11.988 | |
| 13.00 | 0.1 | 0.001 | 0.013 |
The sum of the products is 11.988 + 0.013 = 12.001 amu.
Q: What is the average atomic mass of an element with three isotopes, one with a mass of 12 amu and an abundance of 99.9%, one with a mass of 13 amu and an abundance of 0.1%, and one with a mass of 14 amu and an abundance of 0.01%?
A: To calculate the average atomic mass of this element, you need to multiply the mass of each isotope by its abundance and then sum up the results.
| Mass (amu) | Abundance (%) | Abundance (Decimal) | Product |
|---|---|---|---|
| 12.00 | 99.9 | 0.999 | 11.988 |
| 13.00 | 0.1 | 0.001 | 0.013 |
| 14.00 | 0.01 | 0.0001 | 0.0014 |
The sum of the products is 11.988 + 0.013 + 0.0014 = 12.003 amu.
Q: What is the average atomic mass of an element with four isotopes, one with a mass of 12 amu and an abundance of 99.9%, one with a mass of 13 amu and an abundance of 0.1%, one with a mass of 14 amu and an abundance of 0.01%, and one with a mass of 15 amu and an abundance of 0.001%?
A: To calculate the average atomic mass of this element, you need to multiply the mass of each isotope by its abundance and then sum up the results.
| Mass (amu) | Abundance (%) | Abundance (Decimal) | Product |
|---|---|---|---|
| 12.00 | 99.9 | 0.999 | 11.988 |
| 13.00 | 0.1 | 0.001 | 0.013 |
| 14.00 | 0.01 | 0.0001 | 0.0014 |
| 15.00 | 0.001 | 0.00001 | 0.00015 |
The sum of the products is 11.988 + 0.013 + 0.0014 + 0.00015 = 12.00315 amu.
Q: What is the average atomic mass of an element with five isotopes, one with a mass of 12 amu and an abundance of 99.9%, one with a mass of 13 amu and an abundance of 0.1%, one with a mass of 14 amu and an abundance of 0.01%, one with a mass of 15 amu and an abundance of 0.001%, and one with a mass of 16 amu and an abundance of 0.0001%?
A: To calculate the average atomic mass of this element, you need to multiply the mass of each isotope by its abundance and then sum up the results.
| Mass (amu) | Abundance | Abundance (Decimal) | Product |
|---|---|---|---|
| 12.00 | 99.9 | 0.999 | 11.988 |
| 13.00 | 0.1 | 0.001 | 0.013 |
| 14.00 | 0.01 | 0.0001 | 0.0014 |
| 15.00 | 0.001 | 0.00001 | 0.00015 |
| 16.00 | 0.0001 | 0.000001 | 0.000016 |
The sum of the products is 11.988 + 0.013 + 0.0014 + 0.00015 + 0.000016 = 12.003156 amu.
Q: What is the average atomic mass of an element with six isotopes, one with a mass of 12 amu and an abundance of 99.9%, one with a mass of 13 amu and an abundance of 0.1%, one with a mass of 14 amu and an abundance of 0.01%, one with a mass of 15 amu and an abundance of 0.001%, one with a mass of 16 amu and an abundance of 0.0001%, and one with a mass of 17 amu and an abundance of 0.00001%?
A: To calculate the average atomic mass of this element, you need to multiply the mass of each isotope by its abundance and then sum up the results.
| Mass (amu) | Abundance (%) | Abundance (Decimal) | Product |
|---|---|---|---|
| 12.00 | 99.9 | 0.999 | 11.988 |
| 13.00 | 0.1 | 0.001 | 0.013 |
| 14.00 | 0.01 | 0.0001 | 0.0014 |
| 15.00 | 0.001 | 0.00001 | 0.00015 |
| 16.00 | 0.0001 | 0.000001 | 0.000016 |
| 17.00 | 0.00001 | 0.0000001 | 0.0000017 |
The sum of the products is 11.988 + 0.013 + 0.0014 + 0.00015 + 0.000016 + 0.0000017 = 12.00315617 amu.
**Q: What is the average atomic mass of an element with seven isotopes, one with a mass of 12 amu and an abundance of 99.9%, one with a mass of 13 amu and an abundance of 0.1%, one with a mass of 14 amu and an abundance of 0.01%, one with a mass of 15 amu and an abundance of 0.001%, one with a mass of 16 amu and an abundance of 0.0001%, one with a