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The image you've uploaded contains a table that focuses on isotopes of tellurium (\( \text{Te} \)) and requires completing the number of neutrons, protons, and electrons for different isotopes.

Here’s a breakdown:

1. **Isotopes**: The table compares isotopes \( ^{120}Te \) and \( ^{122}Te \).
   - **Protons**: The atomic number of tellurium (\( \text{Te} \)) is 52, so both isotopes have **52 protons**.
   - **Neutrons**:
     - \( ^{120}Te \) has 120 - 52 = **68 neutrons**.
     - \( ^{122}Te \) has 122 - 52 = **70 neutrons**.
   - **Electrons**: Since the isotopes are neutral, the number of electrons equals the number of protons, which is **52** for both.

### Completed Table:

| Isotope      | Number of Protons | Number of Neutrons | Number of Electrons |
|--------------|-------------------|--------------------|---------------------|
| \( ^{120}Te \) | 52                | 68                 | 52                  |
| \( ^{122}Te \) | 52                | 70                 | 52                  |

If you need further explanations or have any additional questions, feel free to ask!

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Here are 5 questions related to this topic:

1. What is the general relationship between isotopes and the number of neutrons?
2. How does the mass number of an isotope affect its physical and chemical properties?
3. Why do isotopes of the same element have the same number of protons but different numbers of neutrons?
4. How can the percentage abundance of isotopes be calculated?
5. How do stable and radioactive isotopes differ in terms of their neutron-to-proton ratio?

**Tip**: The number of neutrons in an isotope can be found by subtracting the atomic number from the mass number.

Complete the table to show the numbers of neutrons, protons, and electrons for the isotopes shown: ^{120}Te and ^{122}Te.

Learn how to calculate the number of protons, neutrons, and electrons in isotopes of tellurium, specifically ^{120}Te and ^{122}Te. This detailed explanation includes key concepts of atomic structure, the relationship between mass number and atomic number, and the formulas used. Suitable for high school students.

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