chm115_lecture10 - 19-1Chemistry 115Lecture 10...

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Unformatted text preview: 19-1Chemistry 115Lecture 10 OutlineChapter 6Quick summary of key pointsChapter 7Multiple Electrons in OrbitalsPauli Exclusion principleAufbau PrincipleRecitation: Many electron atomsQuantum numbers, orbitals, Electron spinAufbau principle, Trends in atomic propertiesHW 5:Due Friday, Feb 18, 11pmSymbolSymbolValuesValuesDescriptionDescriptionn (major)n (major)1, 2, 3, ..1, 2, 3, ..Orbital size Orbital size and energy and energy where E = -R(1/nwhere E = -R(1/n2))ll(angular)(angular)0, 1, 2, .. n-10, 1, 2, .. n-1Orbital shape Orbital shape or type or type (subshell) (subshell) mml(magnetic)(magnetic)--ll..0..+..0..+llOrbital Orbital orientationorientation# of orbitals in subshell = 2# of orbitals in subshell = 2ll+ 1+ 1QUANTUM NUMBERSQUANTUM NUMBERSTypes of Atomic OrbitalsSee Active Figure 6.1418-419-5Concept Questions1. What is the sublevel name for the following combination of quantum numbers: n= 3, l = 2?A) 3sB) 2dC) 3pD) 3d2. Which of the following quantum numbers is not correct for the 4f orbital?A) n=4B) l = 3C) ml= -4D) all are correct19-6Chapter 7Periodic chart first correctly described by Mendeleev (1871)Based on ordering of atomic masseslater corrected to Atomic number ZPut elements with common reactivity in columns Predicted Ge properties 15 years before its discoveryFor many electron atoms, Schrodingers equation gives good approx.But we need to make 3 modifications:1) More complex orbital energy picture2) Limit to number of electrons in each orbital (Pauli Exclusion Principle)3) Add 4thQuantum Number, called spin19-7For hydrogen, n alone determines the energyFor all other atoms, two important differences:Higher positive charge on the nucleusMore than one electronWe can predict the position of any level, but we have to account for these differences:Higher charge increases binding energyOther electrons tend to neutralize this effect,But incompletely 19-8Orbital energies: Electron penetrationalters energy between S, P and D orbitals:2S electron spends more time away from nucleus than 2P, but penetrates nearer to the nucleus, thus increasing its attraction. Result: 2S has lower energy than 2P19-9Results:Energy to remove the the top electron (IP)depends on whats belowThe energy of any givenorbital depends on bothits radius and its shape:Notice difference between S, P, D orbitals.(more later)Important for periodicityOrbital Energy Diagramfor a many-electron atom19-10Were going to build up the structure of atoms by adding electrons to orbitalsQuestion can we put more thanone electron per orbital?...
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This note was uploaded on 04/09/2011 for the course CHM 115 taught by Professor Towns during the Spring '08 term at Purdue University-West Lafayette.

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chm115_lecture10 - 19-1Chemistry 115Lecture 10...

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