The number of radial nodes and nodal planes in 4p orbitals are respectively

Options

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

Answer

To determine the number of radial nodes and nodal planes in the 4p orbitals, we can follow these steps:

### Step 1: Identify the Principal Quantum Number (n) and Azimuthal Quantum Number (l)
For the 4p orbital:
- The principal quantum number \( n = 4 \).
- The azimuthal quantum number \( l = 1 \) (since 'p' corresponds to \( l = 1 \)).

### Step 2: Calculate the Number of Radial Nodes
The formula for calculating the number of radial nodes is:
\[ \text{Number of radial nodes} = n - l - 1 \]
Substituting the values we have:
\[ \text{Number of radial nodes} = 4 - 1 - 1 = 2 \]

### Step 3: Calculate the Number of Nodal Planes
The number of nodal planes is equal to the value of the azimuthal quantum number \( l \):
\[ \text{Number of nodal planes} = l = 1 \]

### Step 4: Summarize the Results
Thus, for the 4p orbital:
- The number of radial nodes is 2.
- The number of nodal planes is 1.

### Final Answer
The number of radial nodes and nodal planes in 4p orbitals are respectively \( 2, 1 \).