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Across a period, the atomic radius decreases from left to right.
Because the outer electrons are present in the same valence shell during a
period and the atomic number increases from left to right across a period, the
effective nuclear charge increases. As a result, electrons become more
attracted to the nucleus.
The atomic radius, on the other hand, tends to rise as you
progress through the groups. This is due to the fact that as the primary
quantum number (n) decreases, the distance between the nucleus and valence
electrons rises.
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