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
1849
views
4
rank
9. Electrons in Atoms and the Periodic Table
Periodic Trend: Electron Affinity (Simplified)
Multiple Choice
Which element has the largest (most exothermic) electron affinity?
A
B
C
D
Verified step by step guidance1
Understand that electron affinity refers to the energy change when an atom gains an electron, typically releasing energy (exothermic). The more negative the electron affinity value, the more energy is released, indicating a stronger attraction for the added electron.
Recall the general trend of electron affinity in the periodic table: it tends to increase (become more exothermic) across a period from left to right and generally decreases down a group.
Analyze the given elements: Sodium (Na) is in Group 1, Fluorine (F) and Chlorine (Cl) are halogens in Group 17, and Argon (Ar) is a noble gas in Group 18. Halogens typically have high (more exothermic) electron affinities because they need only one electron to complete their valence shell.
Compare the electron affinities of Fluorine and Chlorine, noting that although Fluorine is more electronegative, Chlorine has a larger atomic size which reduces electron-electron repulsion when gaining an electron, often resulting in a more exothermic electron affinity.
Conclude that among the options, Chlorine (Cl) has the largest (most exothermic) electron affinity based on periodic trends and atomic structure considerations.
Related Videos
Related Practice
