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# 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 π = = ÷ L n = nh /2π Angular momentum is quantized Energy is quantized Radius is quantized n = 1, 2, 3 ... Momentum too
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 π = l 10

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ACT For which state of hydrogen is the orbital angular momentum required to be zero? 1. n=1 2. n=2 3. n=3 The allowed values of l are 0, 1, 2, …, n-1. When n=1, l must be zero. 12 75% 15% 10%
l   =0 is “ s state l   =1 is “ p state l   =2 is “ d state l   =3 is “ f state

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

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