/sci/ - Science & Math » Thread #14256660

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Anonymous Tue 22 Feb 20:06:46 2022 No.14256660 View Reply Original Report

Quoted By:

If sulfur has less ionization energy than phosphorus due to greater electrostatic repulsion, why doesn't this pattern follow from sulfur to chlorine?

Anonymous

Anonymous Wed 23 Feb 2022 11:43:39 No.14258285 Report

Quoted By: >>14258288

Bump?

Anonymous

Anonymous Wed 23 Feb 2022 11:45:12 No.14258288 Report

Quoted By:

>>14258285
do your own homework

Anonymous

Anonymous Wed 23 Feb 2022 11:58:17 No.14258300 Report

Quoted By: >>14261222

Sulfur probably has a smaller ionization energy than phosphorus because if you take one electron from Sulfur it reaches a really stable configuration where this p-Orbital is exactly half full. You can't say the same thing about Chlorine.

Anonymous

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Anonymous Thu 24 Feb 2022 16:36:37 No.14261222 Report

Quoted By:

>>14258300
This, the first ionization energy of group V is slightly higher than that of group VI because the half filled shells are more stable. Look up spin-pairing energy.
Further confirmation of this is that the second ionization energy shows the same effect, but one group shifted right.

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