Why does atomic radii decrease going from the bottom left to the upper right of the periodic table?
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Atomic radius decreases from left to right within a period. This is caused by the increase in the number of protons and electrons across a period. One proton has a greater effect than one electron; thus, electrons are pulled towards the nucleus, resulting in a smaller radius. ... This is caused by electron shielding.
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Atomic radii decreases when we move from left to right across periodic table that is when we move left to right in a period because the number of valence electrons increases and the attraction between electron and the nucleous increases hence the shell shrinks towards the nucleous.
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