Question

Is effective nuclear charge of isoelectronic ions equal?

Answer 1

Answer:

Explanation:

For the isoelectronic ions Na+, F-, and Mg2+, why is it that Mg2+ has the largest nuclear charge of the 3 (it has the strongest attrition for the electrons and therefore the smallest radius of the 3)?? I thought that as we go down a group, there is shielding which causes electrons to be further from the nucleus, increasing the radius,

Likewise, why does F- ion have the lowest nuclear charge of the 3 (it has the largest radius of the 3)? When we go down a period, doesn't the effective nuclear charge increase, causing the atomic radius to be smaller?

Im really confused.