Oxygen molecule shows the property of :

Options

A. diamagnetism
B. ferromagnetism
C. paramagnetism
D. none of these

Explanation

To determine the magnetic property of the oxygen molecule (O₂), we will analyze its molecular orbital (MOT) configuration step by step.

### Step 1: Write the Electron Configuration of Oxygen Atoms
Oxygen has an atomic number of 8, which means each oxygen atom has 8 electrons. The electron configuration for a single oxygen atom is:
- 1s² 2s² 2p⁴

### Step 2: Combine the Electron Configurations of Two Oxygen Atoms
When two oxygen atoms combine to form an O₂ molecule, we combine their electron configurations:
- Total configuration: 1s² 2s² 2p⁴ (from one O) + 1s² 2s² 2p⁴ (from another O) = 1s² 2s² 2p⁴ 1s² 2s² 2p⁴

### Step 3: Construct the Molecular Orbital Diagram
In the molecular orbital theory, we fill the molecular orbitals based on the energy levels. The order of filling for O₂ is:
- σ(1s)², σ*(1s)², σ(2s)², σ*(2s)², σ(2p_z)², π(2p_x)², π(2p_y)², π*(2p_x)¹, π*(2p_y)¹

### Step 4: Fill the Molecular Orbitals
1. Fill the bonding orbitals first:
- σ(1s)²
- σ*(1s)²
- σ(2s)²
- σ*(2s)²
- σ(2p_z)²
- π(2p_x)²
- π(2p_y)²

2. The 2p orbitals are filled as follows:
- π(2p_x) and π(2p_y) each get 2 electrons (bonding).
- The remaining two electrons will occupy the π* (anti-bonding) orbitals, resulting in:
- π*(2p_x)¹ and π*(2p_y)¹ (each has one unpaired electron).

### Step 5: Analyze the Number of Unpaired Electrons
In the molecular orbital configuration of O₂, we find that there are two unpaired electrons in the π* orbitals.

### Conclusion: Determine the Magnetic Property
Since O₂ has unpaired electrons, it exhibits **paramagnetism**. Paramagnetic substances are attracted to magnetic fields due to the presence of unpaired electrons.

### Final Answer
The oxygen molecule shows the property of **paramagnetism**.

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