No. of radial nodes = n-l-1 no. of angular nodes = l here n=principal quantum no. l=azimuthal quantum no.

Angular Nodes in 4s- Suborbit is Equal to Radial Nodes in (A) 3d and (B) 2p Orbitals

Angular Nodes and Radial Nodes:
Before we proceed to explain the answer, let's understand the concepts of angular nodes and radial nodes in atomic orbitals.

- Angular Nodes: Angular nodes are regions in an atomic orbital where the probability of finding an electron is zero. These nodes are characterized by the angular momentum quantum number (l) and determine the shape of the orbital. The number of angular nodes is given by (l - 1).

- Radial Nodes: Radial nodes are regions in an atomic orbital where the probability of finding an electron is zero along the radial direction. These nodes are determined by the principal quantum number (n) and determine the size of the orbital. The number of radial nodes is given by (n - l - 1).

Explanation of the Answer:
In the given question, we are comparing the angular nodes in the 4s-suborbit with the radial nodes in the 3d and 2p orbitals. Let's analyze each option:

a) Angular Nodes in 4s- Suborbit = 4 - 1 = 3
Radial Nodes in 3d Orbital = 3 - 2 - 1 = 0

b) Angular Nodes in 4s- Suborbit = 4 - 1 = 3
Radial Nodes in 2p Orbital = 2 - 1 - 1 = 0

From the above calculations, it is evident that both options (A) and (B) have zero radial nodes. Therefore, the correct answer is option (C) - Both (A) and (B).

Conclusion:
Angular nodes and radial nodes are important concepts in atomic orbitals. Angular nodes determine the shape of the orbital, while radial nodes determine the size. In the case of the 4s-suborbit, it has three angular nodes, which are equivalent to the zero radial nodes in both the 3d and 2p orbitals.