Question

Match the LIST-I with LIST-II

Choose the correct answer from the options given below:

• A. A-IV, B-I, C-III, D-II
• B. A-IV, B-II, C-III, D-I
• C. A-III, B-I, C-IV, D-II
• D. A-IV, B-III, C-II, D-I

Hint:

Remember that Radial nodes = n - l - 1 and Nodal planes = l. Calculate these values for each given orbital and match them with the statements in List-II.

Answer 1

The Correct Option is D

To match the orbitals with their respective nodes, we use the standard formulas for quantum numbers:
1. The number of radial nodes in an orbital is given by: $n - l - 1$.
2. The number of nodal planes (also known as angular nodes) is given by: $l$.
where $n$ is the principal quantum number and $l$ is the azimuthal quantum number (for s, $l=0$; for p, $l=1$; for d, $l=2$).

Analysis for each orbital in List-I:

A. 2s orbital: $n = 2$, $l = 0$.
Radial nodes = $2 - 0 - 1 = 1$.
Nodal planes = $0$.
This matches with IV (1 Radial node + No nodal plane).

B. 3s orbital: $n = 3$, $l = 0$.
Radial nodes = $3 - 0 - 1 = 2$.
Nodal planes = $0$.
This matches with III (2 Radial nodes + No nodal plane).

C. 3p orbital: $n = 3$, $l = 1$.
Radial nodes = $3 - 1 - 1 = 1$.
Nodal planes = $1$.
This matches with II (1 Radial node + one nodal plane).

D. 4d orbital: $n = 4$, $l = 2$.
Radial nodes = $4 - 2 - 1 = 1$.
Nodal planes = $2$.
This matches with I (1 Radial node + two nodal planes).

Comparing our findings with the provided options, the correct matching is A-IV, B-III, C-II, D-I.