The following are selected properties of the most abun- dant isotope of a particular element. Which of these properties would also be the same for the second-most- abundant isotope of the clement?
The following are selected properties of the most abun- dant isotope of a particular element. Which of these properties would also be the same for the second-most- abundant isotope of the clement?
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
![### Atomic Structure and the Periodic Table
#### Question 1:
The following are selected properties of the most abundant isotope of a particular element. Which of these properties would also be the same for the second-most-abundant isotope of the element?
1. Mass number is 70
2. 31 electrons are present
3. Isotopic mass is 69.92 amu
4. Isotope reacts with chlorine to give a green compound
#### Answer:
**Explanation:**
- The number of electrons (option 2) would remain the same for the second-most-abundant isotope if it's the same element but with a different number of neutrons.
#### Question 2:
The following are selected properties of the most abundant isotope of a particular element. Which of these properties would also be the same for the second-most-abundant isotope of the element?
1. Atomic number is 31
2. Does not react with the element gold
3. 40 neutrons are present
4. Density is 1.03 g/mL
#### Answer:
**Explanation:**
- The atomic number (option 1) is characteristic of the element itself and does not change with isotopes.
#### Calculation Problem:
Calculate the atomic mass of each of the following elements using the given data for the percentage abundance and mass of each isotope.
1. **Lithium:**
- 7.42% of \( ^6 \text{Li} \) (6.01 amu) and 92.58% of \( ^7 \text{Li} \) (7.03 amu)
2. **Magnesium:**
- 78.99% of \( ^{24} \text{Mg} \) (23.99 amu), 10.00% of \( ^{25} \text{Mg} \) (24.99 amu), and 11.01% of \( ^{26} \text{Mg} \) (25.98 amu)
#### Explanation:
To calculate the atomic mass, you use the formula:
\[ \text{Atomic Mass} = \sum (\text{Fractional Abundance} \times \text{Isotope Mass}) \]
This can be broken down step-by-step for each element:
- **Example for Lithium:**
- \( \text{Atomic Mass of Li} = (0.0742 \times 6.01) + (](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff61ca72c-0d07-4731-84aa-6e37b38bdca8%2F3e3bdf73-6cc4-4570-a0ee-bf6f0758f386%2Fm29olj.jpeg&w=3840&q=75)
Transcribed Image Text:### Atomic Structure and the Periodic Table
#### Question 1:
The following are selected properties of the most abundant isotope of a particular element. Which of these properties would also be the same for the second-most-abundant isotope of the element?
1. Mass number is 70
2. 31 electrons are present
3. Isotopic mass is 69.92 amu
4. Isotope reacts with chlorine to give a green compound
#### Answer:
**Explanation:**
- The number of electrons (option 2) would remain the same for the second-most-abundant isotope if it's the same element but with a different number of neutrons.
#### Question 2:
The following are selected properties of the most abundant isotope of a particular element. Which of these properties would also be the same for the second-most-abundant isotope of the element?
1. Atomic number is 31
2. Does not react with the element gold
3. 40 neutrons are present
4. Density is 1.03 g/mL
#### Answer:
**Explanation:**
- The atomic number (option 1) is characteristic of the element itself and does not change with isotopes.
#### Calculation Problem:
Calculate the atomic mass of each of the following elements using the given data for the percentage abundance and mass of each isotope.
1. **Lithium:**
- 7.42% of \( ^6 \text{Li} \) (6.01 amu) and 92.58% of \( ^7 \text{Li} \) (7.03 amu)
2. **Magnesium:**
- 78.99% of \( ^{24} \text{Mg} \) (23.99 amu), 10.00% of \( ^{25} \text{Mg} \) (24.99 amu), and 11.01% of \( ^{26} \text{Mg} \) (25.98 amu)
#### Explanation:
To calculate the atomic mass, you use the formula:
\[ \text{Atomic Mass} = \sum (\text{Fractional Abundance} \times \text{Isotope Mass}) \]
This can be broken down step-by-step for each element:
- **Example for Lithium:**
- \( \text{Atomic Mass of Li} = (0.0742 \times 6.01) + (
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