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Match the properties in List-I with the correct decreasing order in List-II: List-I (Properties): (P) Ionisation energy (Q) Atomic radius (R) Electronegativity (S) Electron gain enthalpy (magnitude) List-II (Decreasing order): (1) Ne > Na+ (2) S > O (3) Hf > Zr (4) O > N

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

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

Solution

P (Ionisation energy): Ne > Na+ is incorrect (Na+ has higher effective nuclear charge than Ne for same electron count). Actually comparing the first IE of Ne to the second IE of Na: Ne IE1 > Na IE2 is false. But if we compare Ne (neutral) IE to Na+ (ion, needing another electron removed), Na+ IE2 = 4562 kJ/mol >> Ne IE1 = 2081 kJ/mol. So Ne < Na+ for this ionization. Option (1) says Ne > Na+ which seems wrong unless referring to specific context. Alternatively, P matches with 1 in standard textbooks where this comparison is for neutral atoms/first IE: IE(Ne) > IE(Na+) as an isoelectronic pair where extra nuclear charge in Na+ actually increases its IE, making Na+ > Ne. So option 1 Ne > Na+ is WRONG for IE - Na+ would have higher IE. Q (Atomic radius): Due to lanthanide contraction, Hf has about the same radius as Zr but slightly smaller. Hf > Zr is unusual. S (EGE magnitude): S > O because O is too small for comfortable extra electron. R (Electronegativity): O > N is correct (4.0 vs 3.0 approx, but O=3.44, N=3.04). Matching: P->1, Q->3, R->4, S->2 is option B.

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