A 3p-orbital has

Options

A. Only one nodal plane and no spherical node
B. Only one spherical node and no nodal plane
C. One nodal plane and one spherical node
D. One nodal plane and two spherical nodes.

Explanation

To solve the question regarding the 3p-orbital, we need to determine the number of nodal planes and spherical nodes associated with it. Let's break this down step by step.

### Step 1: Identify the Quantum Numbers
For a 3p orbital:
- The principal quantum number (n) is 3.
- The azimuthal quantum number (l) for a p-orbital is 1.

### Step 2: Calculate the Number of Nodal Planes
Nodal planes (or angular nodes) can be calculated using the azimuthal quantum number (l). The formula for the number of nodal planes is:
\[ \text{Number of nodal planes} = l \]

Since for a p-orbital, \( l = 1 \):
\[ \text{Number of nodal planes} = 1 \]

### Step 3: Calculate the Number of Spherical Nodes
Spherical nodes (or radial nodes) can be calculated using the formula:
\[ \text{Number of spherical nodes} = n - l - 1 \]

Substituting the known values:
- \( n = 3 \)
- \( l = 1 \)

So,
\[ \text{Number of spherical nodes} = 3 - 1 - 1 = 1 \]

### Conclusion
For the 3p orbital:
- Number of nodal planes = 1
- Number of spherical nodes = 1

Thus, the answer is:
- **1 nodal plane and 1 spherical node.**

### Final Answer
The 3p-orbital has 1 nodal plane and 1 spherical node.

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