When the azimuthal quantum number has the value `2`, the number of orbitals possible is

Options

A. 3
B. 0
C. 7
D. 5

Explanation

To determine the number of orbitals possible when the azimuthal quantum number (l) has the value of 2, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Azimuthal Quantum Number (l)**:
- The azimuthal quantum number (l) determines the shape of the orbital and is associated with the subshells. The value of l can be 0, 1, 2, 3, etc., corresponding to s, p, d, f, and so on.

2. **Identify the Value of l**:
- In this case, the azimuthal quantum number is given as 2. This corresponds to the d subshell.

3. **Determine the Number of Orbitals**:
- The number of orbitals in a subshell is given by the formula:
\[ \text{Number of orbitals} = 2l + 1 \]
- Substituting the value of l:
\[ \text{Number of orbitals} = 2(2) + 1 = 4 + 1 = 5 \]

4. **Conclusion**:
- Therefore, when the azimuthal quantum number has the value of 2, the number of orbitals possible is 5.

### Final Answer:
The number of orbitals possible when the azimuthal quantum number has the value 2 is **5**.