The number of anti bonding electrons in `N_(2)` is

Options

A. 4
B. 10
C. 12
D. 14

Explanation

To determine the number of anti-bonding electrons in the nitrogen molecule (N₂), we can follow these steps:

### Step 1: Determine the total number of electrons in N₂
Each nitrogen atom has an atomic number of 7, which means it has 7 electrons. Since there are two nitrogen atoms in N₂, the total number of electrons is:
\[ \text{Total electrons} = 7 \times 2 = 14 \]

### Step 2: Write the molecular orbital configuration for N₂
The molecular orbital configuration for N₂ can be written by filling the molecular orbitals in order of increasing energy. The order of filling for N₂ is as follows:
- σ(1s)²
- σ*(1s)²
- σ(2s)²
- σ*(2s)²
- π(2p_x)² = π(2p_y)²
- σ(2p_z)²

So, the complete molecular orbital configuration for N₂ is:
\[ \sigma(1s)^2 \sigma^*(1s)^2 \sigma(2s)^2 \sigma^*(2s)^2 \pi(2p_x)^2 \pi(2p_y)^2 \sigma(2p_z)^2 \]

### Step 3: Identify bonding and anti-bonding orbitals
In the configuration:
- Bonding orbitals: σ(1s), σ(2s), π(2p_x), π(2p_y), σ(2p_z)
- Anti-bonding orbitals: σ*(1s), σ*(2s)

### Step 4: Count the number of electrons in the anti-bonding orbitals
From the configuration:
- σ*(1s) has 2 electrons
- σ*(2s) has 2 electrons

Adding these gives:
\[ \text{Total anti-bonding electrons} = 2 + 2 = 4 \]

### Conclusion
The number of anti-bonding electrons in N₂ is **4**.

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