Question

Column-I and Column-II are given below. Match the correct list:

• A. P-(iv), Q-(iii), R-(ii), S-(i)
• B. P-(iii), Q-(i), R-(ii), S-(ii)
• C. P-(i), Q-(ii), R-(iii), S-(i)
• D. P-(ii), Q-(i), R-(iv), S-(iii)

Answer 1

The Correct Option is B

Step 1: Understanding the number of radial and angular nodes for each orbital.
In an atomic orbital, the number of radial and angular nodes can be determined using the quantum numbers \( n \), \( l \), and \( m_l \). 1. For s-orbitals (P: 2s, Q: 3s): - For any \( s \)-orbital, \( l = 0 \) (angular node = 0).
- The number of radial nodes is given by \( n - l - 1 \). For 2s, \( n = 2 \), so the number of radial nodes is \( 2 - 0 - 1 = 1 \). For 3s, \( n = 3 \), so the number of radial nodes is \( 3 - 0 - 1 = 2 \). 2. For p-orbitals (R: 4p): - For a \( p \)-orbital, \( l = 1 \) (angular node = 1).
- The number of radial nodes is \( n - l - 1 \). For 4p, \( n = 4 \), so the number of radial nodes is \( 4 - 1 - 1 = 2 \). 3. For d-orbitals (S: 3d): - For a \( d \)-orbital, \( l = 2 \) (angular node = 2).
- The number of radial nodes is \( n - l - 1 \). For 3d, \( n = 3 \), so the number of radial nodes is \( 3 - 2 - 1 = 0 \).
Step 2: Matching the options.
- \( P \) is 2s: Radial nodes = 1, Angular nodes = 0. So, it matches with (iii) Radial node = 1.
- \( Q \) is 3s: Radial nodes = 2, Angular nodes = 0. So, it matches with (i) Radial node = 2.
- \( R \) is 4p: Radial nodes = 2, Angular nodes = 1. So, it matches with (ii) Radial node = 2.
- \( S \) is 3d: Radial nodes = 0, Angular nodes = 2. So, it matches with (ii) Radial node = 0.

Step 3: Final Answer.
Therefore, the correct matching is: \[ \text{P-(iii), Q-(i), R-(ii), S-(ii)} \] Thus, the correct option is (B).

Final Answer: P-(iii), Q-(i), R-(ii), S-(ii).