The pairs of species of oxygen and their magnetic behaviour are noted below. Which of the following presents the correct description ?

Options

A. `O_(2)^(+), O_(2)` - Both paramagnetic
B. `O_(2), O_(2)^(2)` - Both paramagnetic
C. `O_(2)^(-), O_(2)^(2-)` - Both diamagnetic
D. `O_(2)^(+), O_(2)^(2-) ` - Both paramagnetic

Answer

To solve the question regarding the magnetic behavior of different species of oxygen, we will analyze the electronic configurations and molecular orbital diagrams of the relevant species.

### Step-by-Step Solution:

1. **Identify the Species**: The species we are looking at are O2 (dioxygen), O2⁺ (superoxide ion), O2⁻ (peroxide ion), and O2²⁻ (dioxide ion).

2. **Electronic Configuration**:
- For O2: The electronic configuration is 1s² 2s² 2p⁴. When combined, the total number of electrons is 16 (8 from each O atom).
- For O2⁺: This species has one less electron than O2, so its configuration is similar to O2 but with one less electron in the molecular orbitals.
- For O2⁻: This species has one additional electron compared to O2, meaning it will have one more electron in the molecular orbitals.
- For O2²⁻: This species has two additional electrons compared to O2.

3. **Molecular Orbital Diagram**:
- Draw the molecular orbital diagram for O2. The molecular orbitals are filled in the following order:
- σ(1s)², σ*(1s)², σ(2s)², σ*(2s)², σ(2p)², π(2p)², π*(2p)².
- For O2, the filling results in two unpaired electrons in the π*(2p) orbitals, indicating that O2 is paramagnetic.

4. **Magnetic Behavior of Each Species**:
- **O2**: Contains 2 unpaired electrons → **Paramagnetic**.
- **O2⁺**: Contains 1 unpaired electron (after removing one from O2) → **Paramagnetic**.
- **O2⁻**: Contains 3 unpaired electrons (adding one to O2) → **Paramagnetic**.
- **O2²⁻**: Contains all paired electrons (adding two electrons to O2) → **Diamagnetic**.

5. **Evaluate Options**:
- The question provides options regarding the magnetic behavior of these species.
- From our analysis:
- O2 and O2⁺ are both paramagnetic.
- O2 and O2⁻ are not both paramagnetic (O2⁻ is paramagnetic).
- O2²⁻ is diamagnetic.
- O2⁻ and O2⁻ are not both paramagnetic (O2²⁻ is diamagnetic).

6. **Conclusion**: The correct option that represents the magnetic behavior of the pairs of species of oxygen is that O2 and O2⁺ are both paramagnetic.

### Final Answer:
The correct description is that O2 and O2⁺ are both paramagnetic.