Which orbital notation does not have spherical node?

Options

A. n = 2, l = 0
B. n = 2, l = 1
C. n = 3, l = 0
D. n = 1, l = 0

Explanation

To determine which orbital notation does not have spherical nodes, we will use the formula for calculating radial nodes (spherical nodes):

**Formula for Radial Nodes:**
\[ \text{Radial Nodes} = n - l - 1 \]
where:
- \( n \) = principal quantum number
- \( l \) = azimuthal quantum number (angular momentum quantum number)

### Step-by-Step Solution:

1. **Identify the Options:**
We need to evaluate the options given in the question. Let's assume the options are:
- Option A: 2s
- Option B: 2p
- Option C: 3s
- Option D: 1s

2. **Calculate Radial Nodes for Each Option:**
- **Option A: 2s**
- \( n = 2 \), \( l = 0 \) (for s orbital)
- Radial Nodes = \( 2 - 0 - 1 = 1 \)
- **Conclusion:** 2s has 1 spherical node.

- **Option B: 2p**
- \( n = 2 \), \( l = 1 \) (for p orbital)
- Radial Nodes = \( 2 - 1 - 1 = 0 \)
- **Conclusion:** 2p has 0 spherical nodes.

- **Option C: 3s**
- \( n = 3 \), \( l = 0 \) (for s orbital)
- Radial Nodes = \( 3 - 0 - 1 = 2 \)
- **Conclusion:** 3s has 2 spherical nodes.

- **Option D: 1s**
- \( n = 1 \), \( l = 0 \) (for s orbital)
- Radial Nodes = \( 1 - 0 - 1 = 0 \)
- **Conclusion:** 1s has 0 spherical nodes.

3. **Identify the Correct Options:**
From our calculations:
- 2p (Option B) has 0 spherical nodes.
- 1s (Option D) has 0 spherical nodes.

### Final Answer:
The orbital notations that do not have spherical nodes are **2p** and **1s**.