The number of radial and angular nodes in `3p` orbital are

Options

A. 1,0
B. 2,1
C. 1,1
D. 2,0

Explanation

To determine the number of radial and angular nodes in a 3p orbital, we can follow these steps:

### Step 1: Identify the Principal Quantum Number (n)
The principal quantum number (n) for the 3p orbital is 3.

### Step 2: Identify the Azimuthal Quantum Number (l)
The azimuthal quantum number (l) for a p orbital is 1.

### Step 3: Calculate the Number of Radial Nodes
The formula for calculating the number of radial nodes is given by:
\[ \text{Radial Nodes} = n - l - 1 \]
Substituting the values we have:
\[ \text{Radial Nodes} = 3 - 1 - 1 = 1 \]

### Step 4: Calculate the Number of Angular Nodes
The number of angular nodes is equal to the azimuthal quantum number (l):
\[ \text{Angular Nodes} = l \]
Thus, for the 3p orbital:
\[ \text{Angular Nodes} = 1 \]

### Final Answer
The number of radial nodes in the 3p orbital is 1, and the number of angular nodes is also 1.

### Summary
- Radial Nodes: 1
- Angular Nodes: 1