The number of radial and angular nodes in 4d orbital are, respectively:

🧠 The Nodal Map Nodes are the "dead zones" of an orbital.

• Angular Nodes ($l$): These are planes or cones where electron probability is zero.
• Radial Nodes ($n-l-1$): These are spherical shells within the orbital.

🗺️ The Value Check for 4d

1. Identify Quantum Numbers: For 4d, $n=4$ and $l=2$.
2. Angular Nodes: $\text{Angular Nodes} = l = 2$
3. Radial Nodes: $\text{Radial Nodes} = n - l - 1$ $\text{Radial Nodes} = 4 - 2 - 1 = 1$

⚡ The "Total Nodes" Anchor Total Nodes $= n - 1 = 3$. Since angular nodes take up $l=2$, the remaining $1$ must be radial!

⚠️ Common Traps Be careful not to mix the two. d-orbitals always have exactly 2 angular nodes ($l=2$).

$\boxed{\text{Answer: (a)}}$