Write which one out of `O_(2)^(+) and O_(2)^(2-) ` is more stable on the basis of bond order calculations .

Explanation

To determine which ion, \( O_2^+ \) or \( O_2^{2-} \), is more stable based on bond order calculations, we need to follow these steps:

### Step 1: Determine the number of electrons in each ion
- For \( O_2^+ \): Oxygen (O) has 8 electrons, so \( O_2 \) has \( 8 + 8 = 16 \) electrons. Since \( O_2^+ \) has lost one electron, it has \( 16 - 1 = 15 \) electrons.
- For \( O_2^{2-} \): \( O_2 \) has 16 electrons, and since it has gained two electrons, it has \( 16 + 2 = 18 \) electrons.

### Step 2: Write the electron configuration for each ion
- For \( O_2^+ \) (15 electrons):
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