Which of the following orbitals does not have angular node?

Options

A. 2s
B. 2p
C. 3p
D. 3d

Answer

To determine which of the given orbitals does not have an angular node, we need to understand the concept of angular nodes and how they relate to the azimuthal quantum number (L).

### Step-by-Step Solution:

1. **Understand Angular Nodes**: Angular nodes are regions in an atomic orbital where the probability of finding an electron is zero. The number of angular nodes in an orbital is determined by the azimuthal quantum number (L).

2. **Identify the Azimuthal Quantum Number (L)**:
- For an s orbital (e.g., 2s), L = 0.
- For a p orbital (e.g., 2p, 3p), L = 1.
- For a d orbital (e.g., 3d), L = 2.

3. **Analyze the Given Orbitals**:
- **2s**: L = 0 (no angular nodes)
- **2p**: L = 1 (has 1 angular node)
- **3p**: L = 1 (has 1 angular node)
- **3d**: L = 2 (has 2 angular nodes)

4. **Conclusion**: The only orbital among the options that does not have any angular nodes is the **2s orbital**.

### Final Answer:
The orbital that does not have angular nodes is **2s**.

---