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It looks like the table you've provided is related to counting subatomic particles for nuclides, such as protons, neutrons, and electrons. Here's how we can fill in the missing information for each row in the table:

### Row 1:
- **Nuclide**: Given that the atomic number is 34 and the mass number is 78, this nuclide is **Selenium (Se)**.
  - **Atomic number (Z)** = 34 (this is the number of protons).
  - **Protons (p⁺)** = 34 (same as the atomic number).
  - **Electrons (e⁻)** = 34 (for a neutral atom, the number of electrons equals the number of protons).
  - **Neutrons (n⁰)** = Mass number - Atomic number = 78 - 34 = 44.
  - **Mass number** = 78.
  - **Nuclear symbol** = \( \ce{^{78}_{34}Se} \).

### Row 2:
- **Nuclide**: We are given that the number of protons (p⁺) is 91 and neutrons (n⁰) is 140.
  - **Atomic number (Z)** = 91 (this corresponds to the element **Protactinium (Pa)**).
  - **Protons (p⁺)** = 91.
  - **Electrons (e⁻)** = 91 (since it is a neutral atom).
  - **Neutrons (n⁰)** = 140.
  - **Mass number** = Protons + Neutrons = 91 + 140 = 231.
  - **Nuclear symbol** = \( \ce{^{231}_{91}Pa} \).

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### Related Questions:
1. What is the relationship between atomic number and element identity?
2. How do you calculate the number of neutrons in a nuclide?
3. What is the significance of the mass number in nuclear chemistry?
4. How does the number of electrons relate to the charge of an atom?
5. Can an atom have a different number of protons and still be the same element?

**Tip**: Remember, the atomic number (Z) defines the element, while the mass number (A) tells us the total number of protons and neutrons in the nucleus.

Counting subatomic particles for different nuclides based on atomic number, mass number, and other particle counts.

Learn how to count subatomic particles, including protons, neutrons, and electrons, for different nuclides based on atomic and mass numbers. This activity is suitable for high school students learning about atomic structure and nuclear symbols.

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