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In the review session, the UAs mentioned three ions that were isoelectronic, meaning they were equal in valence electrons, however, in this case they explained that ionic radius still increases as you move down a group and increases as you go down a period. I’m just confused as to why this is the case if all of the elements have the same amount of electrons in their shells. Does it have to do with the amount of protons in an element?
Yes, as elements move to the right in a period, they have more protons, resulting in a high effective nuclear charge (in other words, a stronger pull) on each electron from the nucleus. This stronger pull leads to a smaller radius.
Yes, because even though isoelectronic ions have the same number of electrons, they still have differing numbers of protons. When there are more protons in the nucleus, there is a stronger pull. Therefore, isoelectronic ions have the same electron-electron repulsion but different pulls from the nucleus.
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