What is no.of radial nodes of4f orbital?

Answer

To find the number of radial nodes in a 4f orbital, we can use the formula:

**Radial Nodes = n - l - 1**

Where:
- **n** is the principal quantum number.
- **l** is the azimuthal quantum number.

### Step-by-step Solution:

1. **Identify the Principal Quantum Number (n)**:
- For the 4f orbital, the principal quantum number \( n \) is 4.

2. **Identify the Azimuthal Quantum Number (l)**:
- For f orbitals, the azimuthal quantum number \( l \) is 3.

3. **Substitute the values into the formula**:
- Now, we can substitute the values of \( n \) and \( l \) into the formula for radial nodes:
\[ \text{Radial Nodes} = n - l - 1 \]
\[ \text{Radial Nodes} = 4 - 3 - 1 \]

4. **Calculate the number of radial nodes**:
- Performing the calculation:
\[ \text{Radial Nodes} = 4 - 3 - 1 = 0 \]

5. **Conclusion**:
- Therefore, the number of radial nodes in a 4f orbital is **0**.