Question

The number of radial nodes present in 4f orbital is:

• A. 0
• B. 1
• C. 2
• D. 3

Hint:

For \( n \)th shell and \( l \)th orbital, the number of radial nodes can be calculated as \( n - l - 1 \).

Answer 1

The Correct Option is C

Step 1: Number of Nodes in Orbitals.
The number of radial nodes in an orbital is given by the formula: \[ \text{Radial Nodes} = n - l - 1 \] where: - \( n \) is the principal quantum number - \( l \) is the azimuthal quantum number For the 4f orbital: - \( n = 4 \) (because it is the 4th shell) - \( l = 3 \) (for f-orbitals, \( l = 3 \)) Thus, the number of radial nodes is: \[ \text{Radial Nodes} = 4 - 3 - 1 = 0 \]

Step 2: Conclusion.
Hence, the correct number of radial nodes in the 4f orbital is \( 2 \), which corresponds to option (3).