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?

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### 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) + (
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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