Atomic Radii - or screening effect. Effective nuclear...

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Atomic Radii Atomic radii describes the relative sizes of atoms. Atomic radii increase within a column going from the top to the bottom of the periodic table. Atomic radii decrease within a row going from left to right on the periodic table. This last fact seems contrary to intuition. How does nature make the elements smaller even though the electron number is increasing? The reason the atomic radii decrease across a period is due to shielding
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Unformatted text preview: or screening effect. Effective nuclear charge, Z eff , experienced by an electron is less than the actual nuclear charge, Z. The inner electrons block the nuclear charges effect on the outer electrons. Moving across a period, each element has an increased nuclear charge and the electrons are going into the same shell (2s and 2p or 3s and 3p, etc.). Consequently, the outer electrons feel a stronger effective nuclear charge....
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This note was uploaded on 10/14/2011 for the course CHEM 1211 taught by Professor Atwood during the Fall '07 term at University of Georgia Athens.

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