Compara the relative stablilties of `O_(2)^(-) and N_(2)^(-)` and comment on their magnetic (paramagetic or diamagnetic ) behaviour.

Explanation

To compare the relative stabilities of \( O_2^{-} \) and \( N_2^{-} \) and comment on their magnetic behavior, we will follow these steps:

### Step 1: Determine the number of electrons in each ion
- **For \( O_2^{-} \)**: Oxygen has 8 electrons, so \( O_2 \) has \( 8 + 8 = 16 \) electrons. The negative charge adds 1 more electron, giving us a total of 17 electrons.
- **For \( N_2^{-} \)**: Nitrogen has 7 electrons, so \( N_2 \) has \( 7 + 7 = 14 \) electrons. The negative charge adds 1 more electron, giving us a total of 15 electrons.

### Step 2: Write the molecular orbital (MO) configurations
- **For \( O_2^{-} \)**:
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