Molecular orbitals are formed by the overlap of atomic orbitals. Two atomic orbitals combine to form two molecular orbitals called bonding and antibonding `MO s`. The molecular orbitals are filled with electrons following the same rules as followed for filling of atomic orbitals. The molecular orbitals electronic configurations help us to calculate bond order when which give important information about bond strength and bond length.
Which out oof `O_(2)^(+)` and `O_(2)^(-)` is more stable?

Explanation

To determine which of the two species, \( O_2^+ \) or \( O_2^- \), is more stable, we will calculate the bond order for each species. The bond order can be calculated using the formula:

\[ \text{Bond Order} = \frac{(\text{Number of bonding electrons} - \text{Number of antibonding electrons})}{2} \]

### Step 1: Determine the electron configuration of \( O_2 \)

...