Which of the following pairs have identical value of bond order?

Options

A. `N_(2) and O_(2)^(2-)`
B. `NO^(+) and N_(2)`
C. `CN^(-) and O_(2)^(-)`
D. `CO and O_(2)`

Explanation

To determine which pairs have identical bond orders, we will calculate the bond order for each species in the options provided. The bond order can be calculated using the formula:

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

We will analyze each option step by step.

### Step 1: Analyze Option A (N₂ and O₂⁻)
- **N₂**:
- Total electrons = 14 (7 from each nitrogen)
- Bonding electrons = 10, Antibonding electrons = 4
- Bond Order = (10 - 4) / 2 = 3

- **O₂⁻**:
- Total electrons = 18 (8 from each oxygen + 2 extra)
- Bonding electrons = 10, Antibonding electrons = 6
- Bond Order = (10 - 6) / 2 = 2

**Conclusion for A**: Bond orders are not identical.

### Step 2: Analyze Option B (NO⁺ and N₂)
- **NO⁺**:
- Total electrons = 14 (7 from nitrogen + 7 from oxygen - 1 for the positive charge)
- Bonding electrons = 10, Antibonding electrons = 4
- Bond Order = (10 - 4) / 2 = 3

- **N₂**:
- Already calculated as Bond Order = 3.

**Conclusion for B**: Bond orders are identical.

### Step 3: Analyze Option C (CN⁻ and O₂⁻)
- **CN⁻**:
- Total electrons = 14 (6 from carbon + 7 from nitrogen + 1 extra for the negative charge)
- Bonding electrons = 10, Antibonding electrons = 4
- Bond Order = (10 - 4) / 2 = 3

- **O₂⁻**:
- Already calculated as Bond Order = 2.

**Conclusion for C**: Bond orders are not identical.

### Step 4: Analyze Option D (CO and O₂)
- **CO**:
- Total electrons = 14 (6 from carbon + 8 from oxygen)
- Bonding electrons = 10, Antibonding electrons = 4
- Bond Order = (10 - 4) / 2 = 3

- **O₂**:
- Already calculated as Bond Order = 2.

**Conclusion for D**: Bond orders are not identical.

### Final Conclusion:
The only pair that has identical bond orders is **Option B (NO⁺ and N₂)**, both having a bond order of 3.

---