Maximum number of covalent bonds formed by N and P are

Options

A. 3,5
B. 3,6
C. 3,4,5
D. 3, 4, 6

Explanation

To determine the maximum number of covalent bonds that nitrogen (N) and phosphorus (P) can form, we need to analyze their electronic configurations and valence electrons.

### Step-by-Step Solution:

1. **Identify the Atomic Number and Electronic Configuration**:
- **Nitrogen (N)** has an atomic number of 7. Its electronic configuration is \(1s^2 2s^2 2p^3\).
- **Phosphorus (P)** has an atomic number of 15. Its electronic configuration is \(1s^2 2s^2 2p^6 3s^2 3p^3\).

2. **Determine the Valence Electrons**:
- For nitrogen, the valence shell is the second shell (2s and 2p), which contains a total of 5 electrons (2 in 2s and 3 in 2p).
- For phosphorus, the valence shell is the third shell (3s and 3p), which also contains a total of 5 electrons (2 in 3s and 3 in 3p).

3. **Calculate the Maximum Number of Covalent Bonds**:
- **Nitrogen**: To achieve a stable octet, nitrogen needs to gain 3 more electrons. Therefore, it can form a maximum of **3 covalent bonds**.
- **Phosphorus**: Phosphorus can utilize its 3p and 3s electrons to form bonds. Additionally, it has empty 3d orbitals that can participate in bonding. Thus, phosphorus can form a maximum of **5 covalent bonds** (for example, in phosphorus pentachloride, PCl5).

4. **Conclusion**:
- The maximum number of covalent bonds formed by nitrogen (N) is **3**.
- The maximum number of covalent bonds formed by phosphorus (P) is **5**.

### Final Answer:
- Maximum number of covalent bonds formed by N = 3
- Maximum number of covalent bonds formed by P = 5