To answer the question "Nitrogen differs from other elements among the VA group, due to," we will analyze the properties of nitrogen in comparison to other elements in Group 15 (VA group) of the periodic table.
### Step-by-Step Solution:
1. **Identify the Elements in Group 15:**
- The elements in Group 15 are Nitrogen (N), Phosphorus (P), Arsenic (As), Antimony (Sb), and Bismuth (Bi).
2. **Compare Atomic Size:**
- Atomic size increases as you move down the group. Nitrogen, being the first element in this group, has the smallest atomic size compared to phosphorus, arsenic, antimony, and bismuth. This is due to the increasing number of electron shells.
3. **Evaluate Electronegativity:**
- Electronegativity tends to decrease down the group. Nitrogen has the highest electronegativity among the Group 15 elements. This means nitrogen has a stronger tendency to attract electrons in a chemical bond compared to the other elements in the group.
4. **Consider the Presence of d Orbitals:**
- Nitrogen does not have d orbitals available for bonding, as it is in the second period of the periodic table. In contrast, the heavier elements in Group 15 (like phosphorus, arsenic, etc.) have d orbitals that can participate in bonding. This absence of d orbitals in nitrogen limits its ability to expand its valency beyond three.
5. **Conclusion:**
- Based on the analysis, nitrogen differs from other elements in Group 15 due to:
- Its small atomic size.
- Its high electronegativity.
- The absence of d orbitals.
- Therefore, the correct answer is that nitrogen differs from other elements in the VA group due to all of the above factors.
### Final Answer:
Nitrogen differs from other elements among the VA group due to its small atomic size, high electronegativity, and absence of d orbitals. Thus, the answer is "all of this."
