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

Options

A. 4
B. 0
C. 2
D. 3

Explanation

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

### Step-by-Step Solution:

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

2. **Calculate Total Nodes**:
- The total number of nodes in an orbital is given by the formula:
\[ \text{Total Nodes} = n - 1 \]
- Substituting the value of \( n \):
\[ \text{Total Nodes} = 4 - 1 = 3 \]

3. **Determine the Azimuthal Quantum Number (l)**:
- For the s orbital, the azimuthal quantum number \( l \) is 0. Therefore, for the 4s orbital:
\[ l = 0 \]

4. **Calculate Angular Nodes**:
- The number of angular nodes is equal to \( l \):
\[ \text{Angular Nodes} = l = 0 \]

5. **Calculate Spherical (Radial) Nodes**:
- The number of spherical (or radial) nodes can be calculated using the formula:
\[ \text{Spherical Nodes} = \text{Total Nodes} - \text{Angular Nodes} \]
- Substituting the values we have:
\[ \text{Spherical Nodes} = 3 - 0 = 3 \]

### Final Answer:
The number of spherical nodes in the 4s orbital is **3**.

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