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Match each set of quantum numbers in List-I with the maximum number of electrons it can describe from List-II. List-I: (P) n=4, l=2, m=-1 (Q) n=3, l=1 (R) n=5, l=0, s=-1/2 (S) n=2, l=2 List-II: (1) one electron (2) six electrons (3) two electrons (4) zero electrons Choose the CORRECT matching:

1. P -> 1; Q -> 2; R -> 3; S -> 4
2. P -> 2; Q -> 3; R -> 1; S -> 4
3. P -> 3; Q -> 2; R -> 1; S -> 4
4. P -> 3; Q -> 2; R -> 4; S -> 1

Correct answer: P -> 3; Q -> 2; R -> 1; S -> 4

Solution

P: n=4,l=2,m=-1 — three quantum numbers specified (no spin), so 2 electrons (spin +1/2 and -1/2) can be accommodated. Q: n=3,l=1 — only n and l given; l=1 means p-subshell with m = -1,0,+1, each with 2 spins = 6 electrons. R: n=5,l=0,s=-1/2 — three numbers including spin fixed; only m=0 is possible (l=0), so exactly 1 electron. S: n=2,l=2 — impossible since l must be less than n (max l=1 for n=2), so 0 electrons.

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