Match the LIST-I with LIST-II

List-I Orbital		List-II Radial nodes and nodal plane
A.	2s	I.	1 Radial node + two nodal planes
B.	3s	II.	1 Radial node + one nodal plane
C.	3p	III.	2 Radial nodes + No nodal plane
D.	4d	IV.	1 Radial node + No nodal plane

Choose the correct answer from the options given below:

The number of angular (nodal) planes for an orbital is equal to the azimuthal quantum number (l), while the number of radial nodes is given by

$$\text{Radial nodes}=n-l-1.$$

For the (2s) orbital,

$$n=2,\qquad l=0,$$

so,

$$\text{Angular nodes}=0,$$

$$\text{Radial nodes}=2-0-1=1.$$

Hence,

$$A\rightarrow IV.$$

For the (3s) orbital,

$$n=3,\qquad l=0,$$

so,

$$\text{Angular nodes}=0,$$

$$\text{Radial nodes}=3-0-1=2.$$

Hence,

$$B\rightarrow III.$$

For the (3p) orbital,

$$n=3,\qquad l=1,$$

so,

$$\text{Angular nodes}=1,$$

$$\text{Radial nodes}=3-1-1=1.$$

Hence,

$$C\rightarrow II.$$

For the (4d) orbital,

$$n=4,\qquad l=2,$$

so,

$$\text{Angular nodes}=2,$$

$$\text{Radial nodes}=4-2-1=1.$$

Hence,

$$D\rightarrow I.$$

Therefore, the correct matching is

$$A\rightarrow IV,\qquad B\rightarrow III,\qquad C\rightarrow II,\qquad D\rightarrow I.$$

Hence, the correct answer is A-IV, B-III, C-II, D-I.