Which of these is true regarding the 3d orbital ?

Options

A. It possesses two radial nodes
B. It possesses two conical nodes
C. It possesses zero angular nodes
D. All of the above are correct statements

Answer

To determine which statements are true regarding the 3d orbital, we need to analyze the properties of the 3d orbital, particularly focusing on the number of radial nodes and angular nodes.

### Step-by-Step Solution:

1. **Identify the Principal Quantum Number (n)**:
- For the 3d orbital, the principal quantum number \( n \) is 3.

2. **Determine the Azimuthal Quantum Number (l)**:
- The azimuthal quantum number \( l \) for a d orbital is 2.

3. **Calculate the Number of Radial Nodes**:
- The formula to calculate radial nodes is given by:
\[ \text{Radial Nodes} = n - l - 1 \]
- Plugging in the values:
\[ \text{Radial Nodes} = 3 - 2 - 1 = 0 \]
- Therefore, the 3d orbital has **0 radial nodes**.

4. **Calculate the Number of Angular Nodes**:
- The number of angular nodes is equal to the value of \( l \):
\[ \text{Angular Nodes} = l = 2 \]
- Thus, the 3d orbital has **2 angular nodes**.

5. **Identify Conical Nodes**:
- Conical nodes are similar to angular nodes. Since the 3d orbital has 2 angular nodes, it also possesses **2 conical nodes**.

6. **Evaluate the Options**:
- **Option 1**: "It possesses 2 radial nodes" - **Incorrect** (it has 0 radial nodes).
- **Option 2**: "It possesses 2 conical nodes" - **Correct** (it has 2 conical nodes).
- **Option 3**: "It possesses 0 angular nodes" - **Incorrect** (it has 2 angular nodes).
- **Option 4**: "All of the above are correct statements" - **Incorrect**.

### Conclusion:
The correct statement regarding the 3d orbital is that it possesses **2 conical nodes**.