Number of angular nodes for 4d orbital is.........

Options

A. 4
B. 3
C. 2
D. 1

Explanation

To determine the number of angular nodes for a 4d orbital, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Principal Quantum Number (n)**:
- The principal quantum number (n) for the 4d orbital is 4.

2. **Identify the Azimuthal Quantum Number (l)**:
- For d orbitals, the azimuthal quantum number (l) is always equal to 2.

3. **Determine the Number of Angular Nodes**:
- The number of angular nodes in an orbital is given by the formula:
\[ \text{Number of angular nodes} = l \]
- Since we have identified that \( l = 2 \) for the 4d orbital, we can conclude that:
\[ \text{Number of angular nodes} = 2 \]

4. **Final Answer**:
- Therefore, the number of angular nodes for the 4d orbital is **2**.