Nitrogen is relatively inactive element because

Options

A. its atoms has a stable electronic configuration
B. it has low atomic radius
C. its electronegativity is fairly high
D. dissociation energy of its molecule is fairly high.

Explanation

### Step-by-Step Solution:

1. **Understanding Nitrogen's Atomic Structure**:
- Nitrogen has an atomic number of 7, which means it has 7 electrons. The electronic configuration of nitrogen is \(1s^2 2s^2 2p^3\).

2. **Identifying Valence Electrons**:
- The valence shell of nitrogen is the second shell, which contains \(2s^2 2p^3\). This means nitrogen has 5 valence electrons (2 from the \(2s\) and 3 from the \(2p\)).

3. **Octet Rule**:
- To achieve a stable electronic configuration (octet), nitrogen needs 3 more electrons. This is why nitrogen often forms bonds to complete its octet.

4. **Formation of Nitrogen Molecule (N₂)**:
- Nitrogen exists as a diatomic molecule (N₂). In this molecule, two nitrogen atoms share three pairs of electrons, forming a triple bond (one sigma bond and two pi bonds).

5. **Bond Dissociation Energy**:
- The triple bond in N₂ is very strong, requiring a high amount of energy to break. The bond dissociation energy for N₂ is approximately 946 kJ/mol, which is significantly high.

6. **Conclusion**:
- The high bond dissociation energy of the nitrogen molecule (N₂) is the primary reason nitrogen is relatively inactive. It makes it difficult for nitrogen to react with other elements or compounds under normal conditions.

### Final Answer:
Nitrogen is relatively inactive because the dissociation energy of its molecule (N₂) is fairly high.

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