Mar19 - !" # !) # $ % & ' ( & *'...

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Unformatted text preview: !" # !) # $ % & ' ( & *' Frequency Exam 2 90 80 70 60 50 40 30 20 10 0 90 10 20 30 40 50 60 70 80 M or e Chemistry 114 General College Chemistry II % & ( + Bin Instructor: Dr. Gregory Jursich Email: jursich@uic.edu BioE Office: 233 SEO Office: Phone: 312-413-8641 Office: 3235 SEL Office Phone: 312-996-3178 Lab: 1215 SEL Lab Phone: 312-996-8373 Office Hours: MWF 12:00 12:45 pm and 2:15-2:45 pm or by appointment Office Hour Location: 233 SEO , 4 3 2 1 4s 4p 4d 4f (ml=0) (ml=+1,0,-1) (ml=+2,+1,0,-1,-2) (ml=+3,+2,+1,0,-1,-2,-3) Principal QN, n 3s (ml=0) 3p (ml=+1,0,1) 3d (ml=+2,+1,0,-1,-2) 2s (ml=0) (ml= +1,0,-1) 2p (ml=0) 1s 0 1 2 3 Angular Momentum QN, l Angular Momentum, l=0 , Orbital Representation n=1,2,3 & l=0 ml=0 only no nodal planes; only radial nodes not trajectory orbits as indicated by Bohr orbital are wavefunctions with amplitudes and nodes "s" Orbitals Angular Momentum, l=1 , Orbital Representation () "p" Orbitals n=2 & l=1 ml=-1,0,1 each with one angular plane and no radial node note: angular node refers to nodal plane Angular Momentum, l=3 , Orbital Representation () "d" Orbitals n=3 & l=2 ml = -2,-1,0,1,2 each with two angular nodes and no radial node ! n = 1,2,3 l=0 " n = 2,3 l=1 # 2$ 3px orbital 3p n=3, l=2 (3-1-1) or 1 radial node (1) angular node n=3, l=2 % ! ! ' ( *+ , - , & & ) complete description of one e- atom or ion n , l , ml , ms . 0 Key Topics: % 2 '/ 1 5 #3 & 4$ ' ' , . 0 Key Topics: ' ) 2 ) )' '/ 1 / 2 6 ! / '/ ! Exact solutions to Schrodinger Equation not possible for many electron atoms due to electron-electron repulsion * * ' 7 ) * ) # ' $ * ) 8 # && & $ * % ' - , * / * -#9, $" ' / H atom Orbitals 4 Energy 3 2 QN, n 1 4s 3s 2s 4p 3p 2p 4d 3d 4f 1s 0 1 2 QN, l 3 Multi-electron atom Orbitals 6 5 4 4s Energy 3 2 QN, n 1 1s 3s 2s 6s 5s 5p 4p 3p 2p 5d 4d 3d 4f 0 1 2 QN, l 3 " # $ 4 ! ' # $4 ' / 2 4 ) % ) # $: / ; " ' 8 '( 2 Multi-electron atom Orbitals 6 5 4 4s Energy 3 2 QN, n 1 1s 3s 2s 6s 5s 5p 4p 3p 2p 5d 4d 3d 4f electron configurations: S (16 e-) 1s22s22p63s23p4 0 1 2 QN, l 3 Filling Order of Orbitals in Multi-Electron Atoms electron configurations: Mg: (12 e-) 1s22s22p63s2 S (16 e-) 1s22s22p63s23p4 Ge (32 e-) 1s22s22p63s23p64s23d104p2 Mg Ge S To form cations from elements remove 1 or more e- from subshell of highest n [or highest (n + l)]. 4< = - ---> 4+ < = 3s 2s 1s 3p 2p 3s 2s 1s 3p 2p / ! ! ( # 2 ' 5$ 6 ( ( 5 ' # 2' 25 '5 2 -' $ ( # 8 ...
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This note was uploaded on 04/07/2008 for the course CHEM 114 taught by Professor Jursich during the Spring '08 term at Ill. Chicago.

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