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NEET Chemistry QUESTION #7406
Question 1
Which of the following correctly represents the order of increasing electron gain enthalpy (with negative sign) for O, S, F, and Cl?
  • \(\text{S} < \text{O} < \text{Cl} < \text{F}\)
  • \(\text{Cl} < \text{F} < \text{O} < \text{S}\)
  • \(\text{O} < \text{S} < \text{F} < \text{Cl}\)✔️
  • \(\text{F} < \text{S} < \text{O} < \text{Cl}\)
Correct Answer Explanation
Electron gain enthalpy (EGE) trend:
F and O are anomalously low due to their small atomic size causing high electron–electron repulsion when an extra electron is added.

Correct increasing order: \(\text{O} < \text{S} < \text{F} < \text{Cl}\)

Cl has the most negative EGE (releases most energy) among these four elements.