I understand the concept of electron affinity being the energy released when an atom receives an electron and that the trend is
that electron affinity generally increases across a period and decreases down a group. However, I was wondering why more energy
is released from atoms in the top right of the periodic table (Fluorine, Chlorine) when they want the electron more than other atoms.
Also, in the sixth edition textbook problem 2.67b, carbon is shown to have a higher electron affinity than nitrogen. Why is that?
Electron Affinity
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Re: Electron Affinity
The more negative the electron affinity value, the higher an atom's affinity for electrons. So the elements in the top corner (chlorine, fluorine) have a more negative value than lower down the column or left. It is more negative because the they give off energy to form an anion exothermic process.
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Re: Electron Affinity
The overall trend for electron affinity is that it increases across a period and decreases down a group
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Re: Electron Affinity
Flourine and Chlorine have gretaer electron affinities because of their need to fufill their octet and become more stable atoms. If CL and F were to recieve an electron they would reach the goal of having a noble gas configuration of Argon and Neon.
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Re: Electron Affinity
Can someone explain why C has a higher electron affinity than N in more detail plz? It’s confusing having said that N is closer to the right of the periodic table...
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Re: Electron Affinity
Daniela Alvarado 3B wrote:Can someone explain why C has a higher electron affinity than N in more detail plz? It’s confusing having said that N is closer to the right of the periodic table...
Carbon has a higher electron affinity because a half-filled p sub-shell is more stable, giving Carbon a higher electron affinity than N, which already has the stable half-filled p sub-shell.
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