Electron Affinity  [ENDORSED]

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Robert Estrada
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Joined: Fri Sep 29, 2017 7:05 am

Electron Affinity

Postby Robert Estrada » Sun Oct 29, 2017 8:32 pm

Besides the general pattern of electron affinities being highest towards the right of the periodic table, how do you determine which elements have the highest affinity such as Chlorine vs. Bromide?

Juno Suzuki 3B
Posts: 9
Joined: Fri Sep 29, 2017 7:06 am

Re: Electron Affinity

Postby Juno Suzuki 3B » Sun Oct 29, 2017 8:47 pm

I can't answer this, but I'm interested in knowing the answer as well.

Chris Pleman 3E
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Re: Electron Affinity

Postby Chris Pleman 3E » Sun Oct 29, 2017 10:07 pm

Usually specific values will be provided through experimental data, but for the Chlorine vs. Bromine example, Chlorine would have the greater eletron affinity, as it is above Bromine in the periodic table.

Curtis Wong 2D
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Joined: Sat Jul 22, 2017 3:00 am

Re: Electron Affinity  [ENDORSED]

Postby Curtis Wong 2D » Sun Oct 29, 2017 10:26 pm

I believe that if you take a look at the electron configuration you can also figure out whether or not the electron affinity will be greater than 0, less than 0, or if it becomes more negative. For instance, the EA becomes more negative moving down the Group 11 elements because n increases. Because n increases, the atom becomes a bigger size, and the orbital becomes bigger. Thus, it's easier to add an electron and more energy is released. And the EA for Group 12 elements are positive mainly because the orbitals are already filled, and by adding an electron, that electron will go to a new orbital 4P. Thus, that shielding given from the full orbitals and repulsion between electrons in the full orbitals make EA positive, meaning that it requires energy to keep that electron there.

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