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Chemistry Help...does anyone know this?
Why is the difference between the atomic radii of Na and K relatively large compared to the difference between the atomic radii of Rb and Cs? I know that as you go down the periodic table, atomic radii increases because of the shielding effect, but how does this apply to the question I must answer?
I'm looking for why the difference between the atomic radii of Na and K is greater that the difference between that of Cs and Rb, not why Na is smaller than Cs.
1 Answer
- 1 decade agoFavorite Answer
The Shielding effect does occur on the periodic table, from left to right and from the bottom of the group to the top. But the main point of this question is the added octets or shells, to Rb and Cs. As you go down in the periodic table (in a group) you have added 8 electrons, which form a complete shell. These take up more volume and make the atomic radii larger.
Example: Li has 3 electons and protons, and Na has 11 electons and protons...I'm talking about their metal states, not ions.
Try thinking of it like rings around a planet..but the rings are part of the radii of the atom.
In reality, the motions of electrons are not points or rings, but wave equations...This is quite difficult to work with, so we simplify it for most chemistry fields.
Source(s): I'm a chemist
