Assertion `O_(2)` and `N_(2)^(2-)` have same number of electrons and same molecular orbital configuration
Reasoning `O_(2)` and `N_(2)^(2-)` have the same bond order .

Options

A. If both `(A)` and `(R )` are correct and `(R )` is the correct
explanation of `(A)`
B. If both `(A)` and `(R )` are correct and `(R )` is the correct
explanation of `(A)`
C. If `(A)` is correct but `(R )` is incorrect
D. If `(A)` is incorrect but `(R )` is correct

Explanation

To solve the question, we need to analyze the assertion and reasoning provided:

**Assertion**: O₂ and N₂²⁻ have the same number of electrons and the same molecular orbital configuration.
**Reasoning**: O₂ and N₂²⁻ have the same bond order.

### Step-by-Step Solution:

1. **Determine the Number of Electrons**:
- O₂ has 8 electrons (4 from each oxygen atom).
- N₂²⁻ has 7 electrons from each nitrogen atom (total 14) plus 2 additional electrons due to the -2 charge, giving a total of 16 electrons.
- Therefore, both O₂ and N₂²⁻ have 16 electrons.

2. **Molecular Orbital Configuration**:
- For O₂, the molecular orbital configuration is:
- σ1s², σ*1s², σ2s², σ*2s², σ2p_z², π2p_x², π2p_y², π*2p_x¹, π*2p_y¹.
- For N₂²⁻, the molecular orbital configuration is:
- σ1s², σ*1s², σ2s², σ*2s², π2p_x², π2p_y², σ2p_z², π*2p_x¹, π*2p_y¹.
- Comparing the configurations, we see that they are not the same. The order of filling is different, especially in the 2p orbitals.

3. **Bond Order Calculation**:
- Bond order is calculated using the formula:
\[ \text{Bond Order} = \frac{1}{2} (N_B - N_A) \]
where \( N_B \) is the number of bonding electrons and \( N_A \) is the number of antibonding electrons.
- For O₂:
- Bonding electrons: 10 (σ1s² + σ2s² + σ2p_z² + π2p_x² + π2p_y²)
- Antibonding electrons: 6 (σ*1s² + σ*2s² + π*2p_x¹ + π*2p_y¹)
- Bond order = \( \frac{1}{2} (10 - 6) = 2 \).
- For N₂²⁻:
- Bonding electrons: 10 (same as O₂)
- Antibonding electrons: 4 (σ*1s² + σ*2s²)
- Bond order = \( \frac{1}{2} (10 - 4) = 3 \).

4. **Conclusion**:
- The assertion is **incorrect** because O₂ and N₂²⁻ do not have the same molecular orbital configuration.
- The reasoning is **incorrect** because O₂ has a bond order of 2, while N₂²⁻ has a bond order of 3.
- Therefore, both the assertion and reasoning are incorrect.

### Final Answer:
Both the assertion and reasoning are incorrect.