1. Electronic Structure and Periodic Properties Electron Configuration Orbital Size Effective Nuclear Charge

2. Shells, Subshells, Orbitals

3. Organization of the Periodic Table

6. Effective Nuclear Charger Z* = Z eff = Z – S Shielding: 1.electrons with greater n = 0 2.electrons with same n = 0.35 (except d and f, =1) 3.electrons with n one lower, = 0.85 (except d and f, =1) 4.electrons with n two or more lower = 1 P = 1s 2 2s 2 2p 6 3s 2 3p 3 shielding = 2x1 8 x 0.85 4x0.35 = 5.1 Z* = 15 – 10.2 = 4.8

7. Trends in Z*: Do Li through Ne: Do C, Si, Ge:

8. Periodic Properties Overall Trend: Electrons held most tightly in upper left of periodic table