Anomalous behaviour of nitrogen is due to.

Options

A. Small size and high `EN`
B. Non-ability of d-orbitals in valence shell
C. Ease of multiple bond formation
D. All

Answer

To understand the anomalous behavior of nitrogen, we can break down the reasons into clear steps:

### Step 1: Small Size of Nitrogen
- Nitrogen has a smaller atomic size compared to other elements in Group 15 (the nitrogen family). This small size leads to stronger nuclear attraction for its electrons, which influences its chemical behavior.

### Step 2: High Electronegativity
- Nitrogen has a high electronegativity value, which means it has a strong tendency to attract electrons. This property differentiates nitrogen from its heavier group members, which have lower electronegativities.

### Step 3: Non-availability of d-orbitals
- Unlike heavier elements in the nitrogen family, nitrogen does not have vacant d-orbitals available for bonding. This limits its ability to expand its valence shell and affects its bonding characteristics.

### Step 4: Tendency for Multiple Bond Formation
- Due to its small size and high electronegativity, nitrogen has a strong tendency to form multiple bonds (like triple bonds) with itself and other elements. For example, nitrogen can form a strong N≡N triple bond, which is not commonly found in heavier group members.

### Conclusion
- The anomalous behavior of nitrogen is primarily due to its small size, high electronegativity, the non-availability of d-orbitals, and its ability to form multiple bonds. These factors collectively contribute to its unique chemical properties compared to other elements in the same group.