Which of the following statement is incorrect?

Options

A. `O_(2)` is paramagnetic, `O_(3)` is also paramagnetic
B. `O_(2)` is paramagnetic, `O_(2)` is diamagnetic
C. `B_(2)` is paramagnetic, `C_(2)` is also paramagnetic
D. Different obervation is found in their bond length when `NO to NO^(+) and CO to CO^(+)`

Explanation

To solve the question of identifying the incorrect statement regarding the paramagnetism and diamagnetism of certain molecules, we will analyze each statement step-by-step.

### Step 1: Understand the Definitions
- **Paramagnetic Species**: These are species that have unpaired electrons and are attracted to a magnetic field.
- **Diamagnetic Species**: These are species that have all electrons paired and are not attracted to a magnetic field.

### Step 2: Analyze O2
- **Oxygen (O2)**:
- Atomic number of oxygen = 8, so O2 has 16 electrons.
- The molecular orbital configuration for O2 is:
- σ1s² σ*1s² σ2s² σ*2s² σ2p_z² (2 paired)
- π2p_x² π2p_y² (2 unpaired)
- O2 has 2 unpaired electrons, therefore it is **paramagnetic**.

### Step 3: Analyze Ozone (O3)
- **Ozone (O3)**:
- O3 has 24 electrons (8 from each oxygen).
- The molecular orbital configuration can be deduced similarly.
- Ozone has unpaired electrons, hence it is also **paramagnetic**.

### Step 4: Analyze B2
- **Boron (B2)**:
- Atomic number of boron = 5, so B2 has 10 electrons.
- The molecular orbital configuration for B2 is:
- σ1s² σ*1s² σ2s² σ*2s² σ2p_z² (2 paired)
- π2p_x¹ π2p_y¹ (2 unpaired)
- B2 has unpaired electrons, therefore it is **paramagnetic**.

### Step 5: Analyze C2
- **Carbon (C2)**:
- Atomic number of carbon = 6, so C2 has 12 electrons.
- The molecular orbital configuration for C2 is:
- σ1s² σ*1s² σ2s² σ*2s² σ2p_z² (2 paired)
- π2p_x² π2p_y² (2 paired)
- C2 has all paired electrons, therefore it is **diamagnetic**.

### Step 6: Conclusion on Statements
- The statements regarding O2 and O3 being paramagnetic are **correct**.
- The statement regarding B2 being paramagnetic is **correct**.
- The statement regarding C2 being paramagnetic is **incorrect**; C2 is actually **diamagnetic**.

### Final Answer
The incorrect statement is: **C2 is paramagnetic**.

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