Which among the following has the lowest electron affinity?
- A.Fluorine
- B.Chlorine
- C.Bromine
- D.Argon
Show answer
Correct answer: D. Argon
Explanation
The correct answer is D, Argon. Argon is a noble gas whose outer shell already holds eight electrons, so it has no room to take another one easily; adding an electron would mean starting a new shell, and energy has to be supplied rather than released. Its electron affinity is therefore effectively zero, the lowest of the four. Electron affinity is the energy change when a neutral gaseous atom gains an electron, and it generally rises across a period and falls down a group. The other three are halogens, one electron short of a stable octet, so they release a lot of energy on gaining an electron. Option A is wrong because fluorine has a very high electron affinity, though its small size and crowded electrons push it just below chlorine. Option B is wrong because chlorine has the highest electron affinity of all elements. Option C is wrong because bromine's affinity, while lower than chlorine's, is still far above argon's. Exam tip: order is Cl greater than F greater than Br greater than I, and noble gases sit at the bottom.