For electron gain enthalpies of the elements denoted as egH, the incorrect option is:

🧠 $\Delta_{eg}H$ is a signed value — "$<$" here means the actual number is smaller (more negative). Check each statement against the data The trick is to remember this is number-line "less than", not magnitude-less-than. So $-349 < -328$ is true ($-349$ sits to the left of $-328$). Now scan options.

🗺️ Standard $\Delta_{eg}H$ values (kJ/mol) $\ce{Cl} = -349$, $\ce{F} = -328$, $\ce{Br} = -325$, $\ce{I} = -295$, $\ce{At} = -270$, $\ce{S} = -200$, $\ce{Se} = -195$, $\ce{Te} = -190$, $\ce{Po} = -174$.

Check each: (a) $-349 < -328$? Yes — Cl is more negative than F. True statement. (b) $-195 < -200$? No — $-195$ is greater than $-200$ on the number line. False statement — this is the incorrect option. (c) $-295 < -270$? Yes. True statement. (d) $-190 < -174$? Yes. True statement.

So the incorrect option is (b).

⚠️ The trap Students mix up "more negative magnitude" with "less than". The "$<$" symbol is strict number-line comparison. Negative numbers further from zero are smaller, not bigger. $-200 < -195$ because $-200$ is to the left of $-195$. So the claim "Se < S" means "$-195 < -200$" which is false; the truth is "Se > S" in the signed-value sense, even though S is more exothermic in magnitude.

$\boxed{\text{Answer: (b)}}$