[sd79812]

gp1/2 ionic radius sharper drop


With the exception of phosphide, the difference in ionic radius between successive anion forming non-metals is smaller than that between group I and group II's cations

What explains this slope ( atomic radius to atomic number) besides the Bohr radius trend for isoelectronic to hydrogen elements is applicable to just about all atoms in the main group?

Why is the Bohr radius (slope versus atomic number) trend in the figure below consistent for atoms non-isoelectronic to Hydrogen?


Why is the following true besides it is consistent with Slater's rules? "Lithium has but 3 protons in its nucleus. Adding a fourth, to make it beryllium, increases the nuclear charge by 33%. But if you add yet another proton, to make it boron, you are increasing the nuclear charge by 25%. And so on, down to the change from oxygen to fluorine, an increase in the nuclear charge (really, the proton count) of only 12.5%. This accounts for the decline in rate of change that you observ

[Corribus]

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