lect_25nov26f08

Lect_25nov26f08 - Outline 25 26-NOV-2008 1 Review orbitals Quantum#s n m shapes 2 Multi-Electron Atoms(a Wave functions(approx e spin ms Pauli(b

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1 Outline 25 26-NOV-2008 1. Review- Ψ , orbitals , Quantum #’s- n, , m , shapes 2. Multi-Electron Atoms (a) Wave functions (approx), e - spin, m s , Pauli (b) Electrostatics & Energy Level Splitting Pauli Exclusion Principle, Aufbau prinzip, Hund’s Rule, Examples
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2 Quantum corral. 48 Fe atoms on Cu surface. Note wavelike ripple of trapped electrons. Photo courtesy IBM Almaden Research Center; research by Dr. Don Eigler and co-workers. Electron wave property.
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3 Orbital (P)Review 1. Electrons in H atom associated with math functions, ORBITALS - not orbits. 2. Orbitals NOT physical objects but regions in space (3-dimensions) where electron probably found. 3. Orbital described by SET of three numbers, [ n, , m ]. 4. Only certain sets possible.
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4 Orbital (P)Review (cont.) 5. Orbital energy & size associated with n . “Shape” (s,p,d,f) given by . “Orientation” given by m . 1. Each e - associated with orbital described by set of three quantum #s, plus (new in Ch. 8) spin quantum #, m s (-1/2, +1/2). 7. Extend these ideas to multi-electron atoms. Ch. 8 8. NO two electrons may have same set of four quantum #s, [ n, , m , m s ] . Ch. 8, Pauli Principle.
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5 Quantum #’s Review The n, , m are related. Principle Quantum Number possible values. n = 1, 2, 3, 4……. (integers) (Size, Energy) Angular Momentum Quantum Number possible values for a given n. = 0, 1,…., (n -1) ;
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This note was uploaded on 02/18/2009 for the course CHEM 1A taught by Professor Okamura during the Fall '08 term at UC Riverside.

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Lect_25nov26f08 - Outline 25 26-NOV-2008 1 Review orbitals Quantum#s n m shapes 2 Multi-Electron Atoms(a Wave functions(approx e spin ms Pauli(b

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