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Examkrackers says "Zeff also increases going from top to bottom down the periodic table. Though the energy level of the outermost electrons increases down a group, the attractive pull of the growing positively charged nucleus outweighs the additional shielding effects of higher electron shells". Is there a certain point going down a group that the attractive pull of the nucleus outweighs electron shielding? If this is the case, why would the atomic radii increase if there's more nuclear attractive forces going down a group?
Looking at group 1 for example, it seems that Zeff remains the same at 1 (i.e., the increase in number of shielding electrons is negated by the increase in protons), and consequently atomic radii increases.
Looking at group 1 for example, it seems that Zeff remains the same at 1 (i.e., the increase in number of shielding electrons is negated by the increase in protons), and consequently atomic radii increases.