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Chemistry Question 53 – JEE-MAIN 2026

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Match the LIST-I with LIST-II List-IList-IIOrbitalRadial nodes and nodal planeA. 2sI. 1 Radial node + two nodal planesB. 3sII. 1 Radial node + one nodal planeC. 3pIII. 2 Radial nodes + No nodal planeD. 4dIV. 1 Radial node + No nodal plane Choose the correct answer from the options given below:

Atomic orbitals are regions around the nucleus where the probability of finding an electron is high. They are characterized by quantum numbers.

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Ninja Strategy•Prioritize s-orbitals

Calculate nodes for s-orbitals (2s and 3s) first, as they have l=0 (zero angular nodes), which quickly eliminates options that assign them angular nodes.

● Video Walkthrough
Step 1: Recall Node Formulas and Quantum Numbers✦ Active

The number of radial nodes in an orbital is given by the formula n−l−1. The number of angular nodes (nodal planes) is given by l. The principal quantum number is n, and the azimuthal quantum number is l. For different subshells, the l values are: s-subshell (l=0), p-subshell (l=1), d-subshell (l=2), and f-subshell (l=3). The total number of nodes is n−1.

Step 2: Calculate Nodes for Each Orbital○ Expand

Let's calculate the radial and angular nodes for each orbital in List-I:

A. 2s orbital: n=2,l=0⟹Radial nodes=2−0−1=1;Angular nodes=0 (No nodal plane). Matches List-II, IV.
B. 3s orbital: n=3,l=0⟹Radial nodes=3−0−1=2;Angular nodes=0 (No nodal plane). Matches List-II, III.
C. 3p orbital: n=3,l=1⟹Radial nodes=3−1−1=1;Angular nodes=1 (one nodal plane). Matches List-II, II.
D. 4d orbital: n=4,l=2⟹Radial nodes=4−2−1=1;Angular nodes=2 (two nodal planes). Matches List-II, I.
Step 3: Match Orbitals to Descriptions and Select Correct Option○ Expand

Based on the calculations, the correct matches are: A-IV, B-III, C-II, D-I. Comparing this with the given options, option 4 is the correct answer.

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