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Chemistry 1 Chapter 4

by: Courtney Beckwood

Chemistry 1 Chapter 4 CHEM 1110 - 02

Marketplace > University of Memphis > CHEM 1110 - 02 > Chemistry 1 Chapter 4
Courtney Beckwood
University of Memphis

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These are the Chapter 4 notes of Chemistry 1, which covers The Periodic Properties of the Elements
General Chemistry I Lecture
Henry Kurtz
Class Notes
Chemistry, Courtney Beckwood, memphis
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This 2 page Class Notes was uploaded by Courtney Beckwood on Saturday February 20, 2016. The Class Notes belongs to CHEM 1110 - 02 at University of Memphis taught by Henry Kurtz in Spring 2016. Since its upload, it has received 33 views.


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Date Created: 02/20/16
Chapter 4 Energy Levels with the same n split in multi-electron atoms  Farther away the electron is away from the nucleus, the smaller the charge Energy Levels of Multi-Electron Atoms  S < p < d < f…  1s < 2s < 2p < 3s < 3p < … Filling Orbitals with Electrons  Fill for lowest total energy  Electron configurations (list of filled orbitals)  Several ways o H = 1s, He = 1s , Li = 1s 2s, … o Boxes and lines with arrows for spin representation  Two electrons in same orbital with different spins o Pauli Exclusion Principle – no two electrons may have the same 4 quantum numbers  Orbitals with the same energy are degenerate  Hunds Rule (maximize unpaired electrons) o Unpaired electrons have net magnetic moment – Paramagnetic  Strength of attraction related to how many unpaired electrons o Configurations with all pairs electrons have no net magnetic moment – Diamagnetic  No attraction  Effective nuclear charge (Z effthe positive charge felt by an electron. o Zeff Z – number of inner or core electrons o Out of every element on the periodic table, for each row, the alkali metals (far left elements) have the greatest radius while the noble gases (far right elements) have the smallest radius.  Cations: atoms with a positive net charge. Anions: atoms with a negative net charge.  Isoelectronic: have the same ground-state electron configuration o Ex: Na , Al , F , O , and N all have the same ground-state electron configuration as Ne  Ionization Energy: minimum energy required to remove an electron from a gaseous atom in its ground state (Where I1 < I2 < I3) o o For ionization energy, the noble gases (far right electrons) have the highest energy while the alkali metals (far left elements) have the lowest.


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