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This 2 page Class Notes was uploaded by Candace Brooks on Sunday February 8, 2015. The Class Notes belongs to CH 101 at University of Alabama - Tuscaloosa taught by Paul Rupar in Spring2015. Since its upload, it has received 151 views.
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Date Created: 02/08/15
Chapter 3 The Shapes of Atomic Orbitals o O the s orbital 0 one value for ml I ml0 0 Each principal energy level has one s orbital 0 Lowest energy orbital in a principal energy state 0 Spherical o 1 p orbital o mgt1 you have 3 quotpquot orbitals 0 corresponds to ml 101 shaped like infinity aligned through axis 000 two lobed o l2 d orbitals ngt2l2 0 ml 21012 0 four of the d orbitals are lined in a different plane I dxy dyz dxz d x squared y squared 0 mainly four lobed o l3 f orbitals o ngt3 7 quotfquot orbitals o ml3210123 o eight lobed Chapter 4 Periodic Table and Electron Configuration 0 Sublevel Energy Splitting in Multielectron atoms 0 What factors influence how an electron interacts with the nucleus 0 Pauli Exclusion o No two electrons can have the same four quadrants numbers 0 Only two electrons allowed per orbital n L nl m12 12 0 Aufbau Principle 0 Electrons fill the lowest energy level possible 0 Hund s Rule 0 When filling orbitals of the same energy place one electron in each orbital before completing pairs
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