Diamangetic species are

Options

A. `N_(2)`
B. `O_(2)`
C. `B_(2)`
D. `O_(2)^(2-)`

Explanation

### Step-by-Step Solution

1. **Definition of Diamagnetic Species**:
- Diamagnetic species are defined as those species that have no unpaired electrons in their atomic or molecular orbitals. This results in a net magnetic moment of zero.

2. **Electron Configuration of N2**:
- Nitrogen (N) has an atomic number of 7, so N2 has a total of 14 electrons (7 from each nitrogen atom).
- The electron configuration for N2 can be filled as follows:
- σ1s² (2 electrons)
- σ*1s² (2 electrons)
- σ2s² (2 electrons)
- σ*2s² (2 electrons)
- π2px² = π2py² (4 electrons)
- σ2pz² (2 electrons)
- Total: 2 + 2 + 2 + 2 + 4 + 2 = 14 electrons.
- Since all electrons are paired, N2 is diamagnetic.

3. **Electron Configuration of O2**:
- Oxygen (O) has an atomic number of 8, so O2 has a total of 16 electrons (8 from each oxygen atom).
- The electron configuration for O2 is:
- σ1s² (2 electrons)
- σ*1s² (2 electrons)
- σ2s² (2 electrons)
- σ*2s² (2 electrons)
- σ2pz² (2 electrons)
- π2px² = π2py² (4 electrons)
- π*2px¹ = π*2py¹ (2 unpaired electrons)
- Total: 2 + 2 + 2 + 2 + 2 + 4 + 2 = 16 electrons.
- O2 has 2 unpaired electrons, making it paramagnetic.

4. **Electron Configuration of B2**:
- Boron (B) has an atomic number of 5, so B2 has a total of 10 electrons (5 from each boron atom).
- The electron configuration for B2 is:
- σ1s² (2 electrons)
- σ*1s² (2 electrons)
- σ2s² (2 electrons)
- σ*2s² (2 electrons)
- π2px¹ = π2py¹ (2 unpaired electrons)
- Total: 2 + 2 + 2 + 2 + 2 = 10 electrons.
- B2 also has 2 unpaired electrons, making it paramagnetic.

5. **Electron Configuration of O2²⁻**:
- O2²⁻ has 18 electrons (16 from O2 and 2 additional from the 2 negative charges).
- The electron configuration for O2²⁻ is:
- σ1s² (2 electrons)
- σ*1s² (2 electrons)
- σ2s² (2 electrons)
- σ*2s² (2 electrons)
- σ2pz² (2 electrons)
- π2px² = π2py² (4 electrons)
- π*2px² = π*2py² (2 electrons)
- Total: 2 + 2 + 2 + 2 + 2 + 4 + 2 = 18 electrons.
- Since all electrons are paired, O2²⁻ is diamagnetic.

6. **Conclusion**:
- From the analysis, N2 and O2²⁻ are diamagnetic species (no unpaired electrons), while O2 and B2 are paramagnetic species (with unpaired electrons).