lecture25 - Physics 102: Lecture 25 Periodic Table, Atomic...

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Periodic Table, Atomic Structure Physics 102: Lecture 25
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From last lecture – Bohr model ( 29 2 4 2 2 2 2 2 13.6 eV where / 2 2 n mk e Z Z E h n n π × = - ≈ - h h ( 29 2 2 2 2 1 0.0529 nm 2 n h n n r mke Z Z = = ÷ L n = nh /2π Angular momentum is quantized Energy is quantized Radius is quantized n = 1, 2, 3 . .. Momentum too
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Quantum Numbers Each electron in an atom is labeled by 4 #’s n = Principal Quantum Number (1, 2, 3, …) Determines energy (Bohr) m s = Spin Quantum Number (-½ , +½) “Up Spin” or “Down Spin” l = Orbital Quantum Number (0, 1, 2, … n-1) Determines angular momentum l   < n always true! m l = Magnetic Quantum Number (- l , … 0, … ) Component of l | m l | <= l always true! ( 1) 2 h L π = + l l 2 z h L m = l 10
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For which state of hydrogen is the orbital angular momentum required to be zero? 1.
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This note was uploaded on 01/25/2012 for the course PHYS 102 taught by Professor Lee during the Spring '08 term at University of Illinois, Urbana Champaign.

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lecture25 - Physics 102: Lecture 25 Periodic Table, Atomic...

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