Consider the following species:
`N^(3-),O^(2-),F^(-),Na^(+),Mg^(2+)` and `Al^(3+)`
What is common in them?

Explanation

To determine what is common among the species \( N^{3-}, O^{2-}, F^{-}, Na^{+}, Mg^{2+}, \) and \( Al^{3+} \), we can follow these steps:

### Step 1: Identify the number of electrons in each species
- **For \( N^{3-} \)**: Nitrogen has an atomic number of 7. With a \( 3- \) charge, it gains 3 electrons. Therefore, total electrons = \( 7 + 3 = 10 \).
- **For \( O^{2-} \)**: Oxygen has an atomic number of 8. With a \( 2- \) charge, it gains 2 electrons. Therefore, total electrons = \( 8 + 2 = 10 \).
- **For \( F^{-} \)**: Fluorine has an atomic number of 9. With a \( - \) charge, it gains 1 electron. Therefore, total electrons = \( 9 + 1 = 10 \).
- **For \( Na^{+} \)**: Sodium has an atomic number of 11. With a \( + \) charge, it loses 1 electron. Therefore, total electrons = \( 11 - 1 = 10 \).
- **For \( Mg^{2+} \)**: Magnesium has an atomic number of 12. With a \( 2+ \) charge, it loses 2 electrons. Therefore, total electrons = \( 12 - 2 = 10 \).
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