Correct order of bond strength for the following molecule or
ions is :

Options

A. `O_(2)^(-)gtO_(2)^(+)gtO_(2)`
B. `O_(2)gtO_(2)^(+)gtO_(2)^(-)`
C. `O_(2)gtO_(2)^(-)gtO_(2)^(+)`
D. `O_(2)^(+)gtO_(2)gtO_(2)^(-)`

Explanation

To determine the correct order of bond strength for the molecules or ions O2, O2+, and O2-, we will use molecular orbital theory to calculate the bond order for each species. The bond strength is directly proportional to the bond order.

### Step-by-Step Solution:

1. **Determine the Electron Configuration of O2:**
- The molecular orbital configuration for O2 is:
\[ \sigma_{1s}^2 \sigma^*_{1s}^2 \sigma_{2s}^2 \sigma^*_{2s}^2 \sigma_{2p_z}^2 \pi_{2p_x}^2 \pi_{2p_y}^2 \pi^*_{2p_x}^1 \pi^*_{2p_y}^1 \]
- Count the bonding and antibonding electrons:
- Bonding electrons (nB) = 10
- Antibonding electrons (nA) = 2

2. **Calculate the Bond Order for O2:**
- Bond order is calculated using the formula:
\[ \text{Bond Order} = \frac{1}{2} (nB - nA) \]
- For O2:
\[ \text{Bond Order} = \frac{1}{2} (10 - 2) = \frac{1}{2} \times 8 = 4 \]

3. **Determine the Electron Configuration of O2+:**
- O2+ has one less electron than O2. The electron is removed from the antibonding orbital:
\[ \sigma_{1s}^2 \sigma^*_{1s}^2 \sigma_{2s}^2 \sigma^*_{2s}^2 \sigma_{2p_z}^2 \pi_{2p_x}^2 \pi_{2p_y}^2 \pi^*_{2p_x}^1 \]
- Count the bonding and antibonding electrons:
- Bonding electrons (nB) = 10
- Antibonding electrons (nA) = 1

4. **Calculate the Bond Order for O2+:**
- For O2+:
\[ \text{Bond Order} = \frac{1}{2} (10 - 1) = \frac{1}{2} \times 9 = 4.5 \]

5. **Determine the Electron Configuration of O2-:**
- O2- has one additional electron compared to O2. The electron is added to the antibonding orbital:
\[ \sigma_{1s}^2 \sigma^*_{1s}^2 \sigma_{2s}^2 \sigma^*_{2s}^2 \sigma_{2p_z}^2 \pi_{2p_x}^2 \pi_{2p_y}^2 \pi^*_{2p_x}^2 \pi^*_{2p_y}^0 \]
- Count the bonding and antibonding electrons:
- Bonding electrons (nB) = 10
- Antibonding electrons (nA) = 3

6. **Calculate the Bond Order for O2-:**
- For O2-:
\[ \text{Bond Order} = \frac{1}{2} (10 - 3) = \frac{1}{2} \times 7 = 3.5 \]

7. **Summarize the Bond Orders:**
- O2: Bond Order = 4
- O2+: Bond Order = 4.5
- O2-: Bond Order = 3.5

8. **Determine the Order of Bond Strength:**
- The order of bond strength based on bond order is:
\[ O2^+ > O2 > O2^- \]

### Final Answer:
The correct order of bond strength is:
**O2+ > O2 > O2-**