JEE Main 2026 — Jan 22, Shift 2 — Chemistry solution

JEE Main2026Jan 22, Shift 2Chemistry

Given below are two statements :

Statement-I : $C < O < N < F$ is the correct order in terms of first ionization enthalpy values.

Statement-II : $S > S e > T e > P o > O$ is the correct order in the magnitude of electron gain enthalpy values.

In the light of the above statements, choose the correct answer from the options given below :

A
Statement-I is false but Statement-II is true
B
Both Statement-I and Statement-II are true.
C
Both Statement-I and Statement-II are false.
D
Statement-I is true but Statement-II is false.

Solution

Statement-I: Along period 2 the trend is $C < O < N < F$ because N has the extra stability of a half-filled $2 p^{3}$ configuration, making $I E_{1} (N) > I E_{1} (O)$ . True.

Statement-II: For group 16 elements the magnitudes of $∣ Δ_{e g} H ∣$ are approximately $S > S e > T e > P o > O$ (kJ/mol: 200, 195, 190, 174, 141). Oxygen is the anomaly — its small size causes electron-electron repulsion that reduces its electron affinity. True.

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