Oxyegn molecule is diamagnetic.

Explanation

To determine whether the statement "Oxygen molecule is diamagnetic" is correct or false, we can analyze the electronic configuration and magnetic properties of the oxygen molecule (O₂) step by step.

### Step-by-Step Solution:

1. **Understanding the Electronic Configuration of Oxygen:**
- The atomic number of oxygen (O) is 8. Therefore, the electronic configuration of a single oxygen atom is:
\[ 1s^2 2s^2 2p^4 \]
- When two oxygen atoms combine to form an O₂ molecule, we need to consider the total number of electrons:
\[ 2 \times (1s^2 2s^2 2p^4) = 1s^2 2s^2 2p^4 \, (from \, one \, O) + 1s^2 2s^2 2p^4 \, (from \, another \, O) = 1s^2 2s^2 2p^4 \, (total \, for \, O_2) \]
- Therefore, O₂ has a total of 16 electrons.

2. **Molecular Orbital Theory (MOT) Diagram:**
- According to MOT, the molecular orbitals for O₂ are filled in the following order:
- \(\sigma_{2s}\), \(\sigma^*_{2s}\), \(\sigma_{2p_z}\), \(\pi_{2p_x}\), \(\pi_{2p_y}\), \(\pi^*_{2p_x}\), \(\pi^*_{2p_y}\), \(\sigma^*_{2p_z}\)
- The filling of the molecular orbitals for O₂ is as follows:
- \(\sigma_{2s}^2\)
- \(\sigma^*_{2s}^2\)
- \(\sigma_{2p_z}^2\)
- \(\pi_{2p_x}^2\)
- \(\pi_{2p_y}^2\)
- \(\pi^*_{2p_x}^1\)
- \(\pi^*_{2p_y}^1\)

3. **Identifying Unpaired Electrons:**
- In the molecular orbital configuration for O₂, we can see that there are two unpaired electrons in the \(\pi^*_{2p_x}\) and \(\pi^*_{2p_y}\) orbitals.
- The presence of unpaired electrons indicates that O₂ is **paramagnetic**.

4. **Conclusion:**
- Since the statement claims that the oxygen molecule is diamagnetic, which means it has no unpaired electrons, this statement is **false**.
- The correct statement is: "Oxygen molecule (O₂) is paramagnetic due to the presence of unpaired electrons."

### Final Answer:
The statement "Oxygen molecule is diamagnetic" is **false**. The correct statement is "Oxygen molecule is paramagnetic."

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