Which of the following is correct for `N_(2)` triple bond

Options

A. 3s
B. 1p,2s
C. 2p,1s
D. 3p

Answer

To determine the correct statement regarding the triple bond in nitrogen gas (N₂), we need to analyze the electronic configuration and bonding characteristics of nitrogen atoms.

### Step-by-Step Solution:

1. **Identify the Atomic Number of Nitrogen**:
- Nitrogen (N) has an atomic number of 7, which means it has 7 electrons.

2. **Write the Electronic Configuration**:
- The electronic configuration of nitrogen is:
\[ 1s^2 \, 2s^2 \, 2p^3 \]
- This indicates that nitrogen has 2 electrons in the 1s orbital, 2 electrons in the 2s orbital, and 3 electrons in the 2p orbital.

3. **Determine the Ground State Configuration**:
- In the ground state, the electrons are arranged as follows:
- 1s: 2 electrons (paired)
- 2s: 2 electrons (paired)
- 2p: 3 electrons (one pair and one unpaired electron in separate orbitals).

4. **Excited State Configuration**:
- When nitrogen forms a triple bond, one of the 2s electrons can be promoted to the 2p orbital, resulting in:
- 1s: 2 electrons (paired)
- 2s: 1 electron (unpaired)
- 2p: 4 electrons (two pairs and one unpaired electron).
- This allows for the formation of three bonds (one sigma bond and two pi bonds) between two nitrogen atoms.

5. **Bonding in N₂**:
- The N₂ molecule consists of a triple bond, which includes:
- 1 sigma bond formed by the overlap of 2s and 2p orbitals.
- 2 pi bonds formed by the side-to-side overlap of the remaining 2p orbitals.

6. **Conclusion**:
- Based on the electronic configuration and bonding characteristics, the correct option regarding the N₂ triple bond is:
- **Option 3: It involves 2p and 1s orbitals.**