Multiple Choice
Determine which atom in the following set has the largest electron affinity:N, O, C, B, Ne
a) N b) O c) C d) B e) Ne
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9. Electrons in Atoms and the Periodic Table
Periodic Trend: Electron Affinity (Simplified)
Multiple Choice
Which element has the lowest (least exothermic) electron affinity among the following?
A
Oxygen (O)
B
Chlorine (Cl)
C
Neon (Ne)
D
Fluorine (F)
Verified step by step guidance1
Understand that electron affinity is the energy change that occurs when an atom gains an electron. A more negative value means the atom releases more energy (more exothermic) when gaining an electron.
Recall that noble gases like Neon (Ne) have a full valence shell, making them very stable and generally unwilling to gain electrons, resulting in a low or even positive electron affinity (less exothermic or endothermic).
Compare the elements given: Oxygen (O), Chlorine (Cl), Fluorine (F), and Neon (Ne). Oxygen, Chlorine, and Fluorine are all nonmetals that tend to gain electrons and have relatively high (more negative) electron affinities.
Recognize that among these, Neon (Ne) is a noble gas with a complete octet, so it has the lowest (least exothermic) electron affinity because it does not easily accept an extra electron.
Therefore, the element with the lowest electron affinity among the options is Neon (Ne) due to its stable electron configuration and reluctance to gain electrons.
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