The bond order in the species `O_2, O_(2)^(+) and O_(2)^(-)`follows the order

Options

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

Explanation

To determine the bond order of the species \( O_2 \), \( O_2^+ \), and \( O_2^- \), we will follow these steps:

### Step 1: Determine the number of electrons in each species
- **For \( O_2 \)**: Each oxygen atom has 8 electrons, so for two oxygen atoms, the total number of electrons is \( 8 + 8 = 16 \).
- **For \( O_2^+ \)**: This species has one less electron than \( O_2 \), so the total number of electrons is \( 16 - 1 = 15 \).
- **For \( O_2^- \)**: This species has one extra electron compared to \( O_2 \), so the total number of electrons is \( 16 + 1 = 17 \).

### Step 2: Calculate the bond order for each species
The bond order can be estimated based on the total number of electrons:
- **For \( O_2 \)** (16 electrons): The bond order is 2.
- **For \( O_2^+ \)** (15 electrons): The bond order is 2.5.
- **For \( O_2^- \)** (17 electrons): The bond order is 1.5.

### Step 3: Arrange the bond orders in decreasing order
Now, we can arrange the bond orders:
1. \( O_2^+ \) (bond order = 2.5)
2. \( O_2 \) (bond order = 2)
3. \( O_2^- \) (bond order = 1.5)

### Final Answer
The order of bond order in the species \( O_2 \), \( O_2^+ \), and \( O_2^- \) follows:
\[ O_2^+ > O_2 > O_2^- \]