The number of sperical nodes in `4s` orbital is

Options

A. 4
B. `oo`
C. 2
D. 3

Explanation

To determine the number of spherical (or radial) nodes in the 4s orbital, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Principal Quantum Number (n)**:
- The given orbital is 4s. Here, the principal quantum number \( n \) is 4.

2. **Identify the Azimuthal Quantum Number (l)**:
- The 's' in 4s indicates that this is an s orbital. For s orbitals, the azimuthal quantum number \( l \) is 0.

3. **Use the Formula for Radial Nodes**:
- The formula to calculate the number of radial nodes is:
\[ \text{Number of radial nodes} = n - l - 1 \]

4. **Substitute the Values into the Formula**:
- Now, substitute \( n = 4 \) and \( l = 0 \) into the formula:
\[ \text{Number of radial nodes} = 4 - 0 - 1 \]

5. **Calculate the Result**:
- Performing the calculation:
\[ \text{Number of radial nodes} = 4 - 0 - 1 = 3 \]

6. **Conclusion**:
- Therefore, the number of spherical nodes in the 4s orbital is **3**.