Nitrogen forms `N_(2)` , but phosphorus does not form `P_(2)` , however , it forms `P_(4)` , reason is

Options

A. Triple bond present between phosphorus atom
B. `p pi - p pi` bonding is weak
C. `p pi - p pi ` bonding is strong
D. Multiple bonds form easily

Answer

To understand why nitrogen forms N₂ while phosphorus does not form P₂ but forms P₄, we need to analyze the bonding characteristics of these elements.

### Step-by-Step Solution:

1. **Bonding in Nitrogen (N₂)**:
- Nitrogen exists as a diatomic molecule (N₂) due to the formation of a strong triple bond between two nitrogen atoms.
- The electronic configuration of nitrogen is 1s² 2s² 2p³. In N₂, each nitrogen atom contributes three p electrons, allowing for effective overlap and the formation of one sigma (σ) bond and two pi (π) bonds.
- The strong p-pi (π) overlapping leads to a stable triple bond, making N₂ a stable molecule.

2. **Bonding in Phosphorus**:
- Phosphorus does not form P₂ because the ability to form strong multiple bonds (like triple bonds) is less than that of nitrogen.
- The electronic configuration of phosphorus is 1s² 2s² 2p⁶ 3s² 3p³. In phosphorus, the 3p orbitals are larger and more diffuse compared to the 2p orbitals in nitrogen, leading to weaker p-pi (π) bonding.
- As a result, phosphorus prefers to form P₄, which is a tetrahedral molecule. In P₄, each phosphorus atom forms single bonds with three other phosphorus atoms, resulting in a stable structure without the need for multiple bonding.

3. **Conclusion**:
- The reason phosphorus does not form P₂ is due to the weak p-pi (π) bonding compared to nitrogen. Instead, it forms P₄, where single bonds are sufficient to maintain stability.

### Final Answer:
Phosphorus does not form P₂ because the p-pi (π) bonding is weak, while nitrogen forms N₂ due to strong triple bonding.