lect_17dec1f09

lect_17dec1f09 - Outline 17 1-DEC-2009 1 Review orbitals...

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1 Outline 17 1-DEC-2009 1. Review- Ψ , orbitals , Quantum #’s- n, , m , shapes 2. Multi-Electron Atoms (Ch. 8) (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 are 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 . 6. 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) ; steps of 1 (Shape) n values for given n Magnetic Moment Quantum Number possible values for a given ℓ. m = - , -1, 0, 1,…., ; steps of 1, (Orientation) (2 +1 ) values for given n 2 values of m for given n One orbital for each m value!
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6 Quantum Numbers and Atomic Orbitals Ψ n, , m Ψ 1,0,0 = 1s Ψ 2,0,0 = 2s Ψ 2,1,-1 ; Ψ 2,1, 0 ; Ψ 2,1, 1 = 2p x ; 2p y ; 2p z Ψ 3,0,0 = 3s Ψ 3,1,-1 ; Ψ 3,1, 0 ; Ψ 3,1, 1 = 3p x ; 3p y ; 3p z Ψ 3,2,-2 ; Ψ 3,2, -1 ; Ψ 3,1,0 ; Ψ 3,2,1 ; Ψ 3,2, 2 = = 3d xy ; 3d yz ; 3d z2 ; 3d xz ; 3d x2-y2
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8 Orbitals and Periodic Table Illustrates Building Up Order KEY SLIDE
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9 Name________ Sample Quiz 21 TA_______ 1. (2) When n = 2 write the possible values of . 2. (2) When =1 write the possible values of m . . 3. (1) For a given n value, how many orbitals are there when = 1?
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10 s ( ℓ=0) orbitals; m = 0 so 1 orbital (for given n) Review.
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11 2 p ( ℓ=1) orbitals; m = -1,0,1 so 3 orbitals. Review.
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3d ( ℓ=2) orbitals; m = -2,-1,0,1, 2 so 5 orbitals. Review.
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This note was uploaded on 10/14/2011 for the course CHEM 1A taught by Professor Okamura during the Spring '08 term at UC Riverside.

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lect_17dec1f09 - Outline 17 1-DEC-2009 1 Review orbitals...

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