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Shielding Effect in the Periodic Table

Understanding how shielding affects elements in the periodic table. Learn about effective nuclear charge, electronegativity, ionization energy, and atomic radius variations.

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Shielding Effect in the Periodic Table

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  1. PERIODIC TABLE REVIEW 10/23/12 CAIAFA

  2. SHIELDING DOWN A GROUP READING DOWN A GROUP NUMBER OF KERNEL SHELLS INCREASES, (SHIELDS VALENCE FROM NUCLEAR CHARGE) DISTANCE FROM NUC TO VELENCE INCREASES NUCLEAR CHARGE (# OF PROTONS, ATOMIC #) INCREASES INCREASE EFFECTIVE NUCLEAR CHARGE TO VALENCE ELECTRON(S) DECREASES EFFECTIVE NUCLEAR CHARGE TO VALENCE ELECTRON(S) DECREASES EFFECTIVE NUCLEAR CHARGE TO VALENCE ELECTRON(S) DECREASES ELECTRONEGATIVITY AND IONIZATION ENERGY INCREASES ATOMIC RADIUS

  3. SHIELDING L TO R IN A PERIOD READING LEFT TO RIGHT ACROSS A PERIOD NUCLEAR CHARGE (# OF PROTONS, ATOMIC #) INCREASES NUMBER OF KERNEL SHELLS UNCHANGED, (SHIELDS VALENCE FROM NUCLEAR CHARGE) INCREASE EFFECTIVE NUCLEAR CHARGE TO VALENCE ELECTRON(S) NO EFFECT ONEFFECTIVE NUCLEAR CHARGE TO VALENCE ELECTRON(S) INCREASESEFFECTIVE NUCLEAR CHARGE TO VALENCE ELECTRON(S) INCREASESELECTRONEGATIVITY AND IONIZATION ENERGY DECREASESATOMIC RADIUS

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