Asked by kayla
What are the trends and exceptions to the trends in electron affinity? Check all that apply.
The electron affinities of the elements in Group 17 are larger (more negative) than the elements in Group 1.
Electron affinities increase (become more negative) down a group.
Elements in Group 14 have larger (more negative) electron affinities than elements in Group 15.
Elements in Group 2 have very large electron affinities.
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Correct choices: 1 and 3.
- The electron affinities of the elements in Group 17 are larger (more negative) than the elements in Group 1. — True. Halogens gain an electron to reach a noble‑gas configuration, so they release a lot of energy compared with alkali metals.
- Electron affinities increase (become more negative) down a group. — False. EA generally becomes less negative down a group (adding an electron is less exothermic as atomic size and shielding increase).
- Elements in Group 14 have larger (more negative) electron affinities than elements in Group 15. — True. Group‑15 atoms have a half‑filled p subshell, so adding an electron is relatively less favorable; group‑14 members therefore often have more negative EAs than the group‑15 neighbors.
- Elements in Group 2 have very large electron affinities. — False. Alkaline earths have filled s subshells; adding an electron is not favorable (EAs are small or even endothermic).
Minor common exceptions to overall periodic trends: fluorine is slightly less exothermic than chlorine because of strong electron–electron repulsion in the very small 2p orbitals; oxygen is less exothermic than sulfur for a similar reason; Be and N are notable low‑EA exceptions in their periods due to filled or half‑filled subshells.
- The electron affinities of the elements in Group 17 are larger (more negative) than the elements in Group 1. — True. Halogens gain an electron to reach a noble‑gas configuration, so they release a lot of energy compared with alkali metals.
- Electron affinities increase (become more negative) down a group. — False. EA generally becomes less negative down a group (adding an electron is less exothermic as atomic size and shielding increase).
- Elements in Group 14 have larger (more negative) electron affinities than elements in Group 15. — True. Group‑15 atoms have a half‑filled p subshell, so adding an electron is relatively less favorable; group‑14 members therefore often have more negative EAs than the group‑15 neighbors.
- Elements in Group 2 have very large electron affinities. — False. Alkaline earths have filled s subshells; adding an electron is not favorable (EAs are small or even endothermic).
Minor common exceptions to overall periodic trends: fluorine is slightly less exothermic than chlorine because of strong electron–electron repulsion in the very small 2p orbitals; oxygen is less exothermic than sulfur for a similar reason; Be and N are notable low‑EA exceptions in their periods due to filled or half‑filled subshells.
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