JEE Main 2022 · 26 June · evening · Single correct · +4 / −1

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

  1. (a) 1 and 2
  2. (b) 3 and 2
  3. (c) 1 and 0
  4. (d) 2 and 1
Answer and solution

Answer (a) 1 and 2

Solution

Chemistry ma’am · 4 steps

Read n and l off the label first: n gives the total nodes, l gives the angular ones, and radial is the rest.

  1. Quantum numbers. For a 4d orbital, n = 4. The letter d means l = 2.
  2. Count the nodes. An orbital has n - 1 nodes in total. The angular nodes number l, and the radial nodes make up the rest.

    radial = n - l - 1, angular = l

  3. Put in numbers. Radial nodes = 4 - 2 - 1 = 1. Angular nodes = l = 2. Check: 1 + 2 = 3 = n - 1, the total.
  4. So. A 4d orbital has 1 radial node and 2 angular nodes, which is option (a).

The idea to keep. Total nodes = n - 1, angular nodes = l, radial nodes = n - l - 1. Always split the total this way and check that the two parts add back up.

Answer from the NTA final answer key. Solution by PrepWiser.

Study Atomic Structure

Asked about 170 times in JEE Main since 2020. This question is from 2022.