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Electronic Structure and Periodic Properties

This article explores the electronic structure and periodic properties, focusing on electron configuration, orbital size, and effective nuclear charge (Z*). It details how shielding affects Z*, which is calculated using the formula Z* = Z - S, where S is the shielding constant. The article examines trends in Z* from lithium to neon and across elements like carbon, silicon, and germanium. It highlights how electrons are held most tightly in the upper left of the periodic table, outlining the implications for chemical properties and reactivity.

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Electronic Structure and Periodic Properties

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

  2. Shells, Subshells, Orbitals

  3. Organization of the Periodic Table

  4. Effective Nuclear Charger Z* = Zeff = Z – S Shielding: electrons with greater n = 0 electrons with same n = 0.35 (except d and f, =1) electrons with n one lower, = 0.85 (except d and f, =1) electrons with n two or more lower = 1 P = 1s2 2s2 2p6 3s2 3p3 shielding = 2x1 8 x 0.85 4x0.35 = 5.1 Z* = 15 – 10.2 = 4.8

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

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

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