Out of the following bond order of oxygen species identify the correct answer

Options

A. `O_2^(-)gtO_2gtO_2^+`
B. `O_2^(-)ltO_2ltO_2^+`
C. `O_2^(-)gtO_2ltO_2^+`
D. `O_2^(-)ltO_2gtO_2^+`

Answer

To determine the bond order of the oxygen species (O2, O2+, O2-), we will follow these steps:

### Step 1: Understand Bond Order
Bond order is defined as the difference between the number of bonding electrons and the number of antibonding electrons, divided by two:
\[ \text{Bond Order} = \frac{(\text{Number of bonding electrons} - \text{Number of antibonding electrons})}{2} \]

### Step 2: Determine the Electron Configuration
1. **O2**:
- Total electrons = 16 (8 from each oxygen atom)
- Electron configuration:
- 1s² 2s² 2p⁴ (for each O atom)
- Total: 1s² 2s² (bonding) + 2p⁴ (bonding) + 2p² (antibonding) = 10 bonding electrons and 6 antibonding electrons.

2. **O2+**:
- Total electrons = 15 (one less due to positive charge)
- Electron configuration:
- 1s² 2s² 2p³ (for each O atom)
- Total: 1s² 2s² (bonding) + 2p³ (bonding) + 2p² (antibonding) = 10 bonding electrons and 5 antibonding electrons.

3. **O2-**:
- Total electrons = 17 (one more due to negative charge)
- Electron configuration:
- 1s² 2s² 2p⁵ (for each O atom)
- Total: 1s² 2s² (bonding) + 2p⁵ (bonding) + 2p² (antibonding) = 10 bonding electrons and 7 antibonding electrons.

### Step 3: Calculate Bond Order for Each Species
1. **For O2**:
\[ \text{Bond Order} = \frac{(10 - 6)}{2} = \frac{4}{2} = 2 \]

2. **For O2+**:
\[ \text{Bond Order} = \frac{(10 - 5)}{2} = \frac{5}{2} = 2.5 \]

3. **For O2-**:
\[ \text{Bond Order} = \frac{(10 - 7)}{2} = \frac{3}{2} = 1.5 \]

### Step 4: Compare the Bond Orders
- O2+: Bond Order = 2.5
- O2: Bond Order = 2
- O2-: Bond Order = 1.5

### Conclusion
The correct order of bond order from highest to lowest is:
1. O2+ (2.5)
2. O2 (2)
3. O2- (1.5)

Thus, the correct answer is **O2+ > O2 > O2-**.