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Periodic Table

Periodic Table. The Bohr model of hydrogen provided a single quantum number n . Principal quantum number One-dimensional solution Schr ö dinger’s equation for a real atom is 3-D. Two other quantum numbers Orbital angular momentum Orbital magnetic number. Quantum Numbers. 1. 2. 3.

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Periodic Table

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  1. Periodic Table

  2. The Bohr model of hydrogen provided a single quantum number n. Principal quantum number One-dimensional solution Schrödinger’s equation for a real atom is 3-D. Two other quantum numbers Orbital angular momentum Orbital magnetic number Quantum Numbers 1 2 3 Shells for the principal quantum number n

  3. The orbital angular momentum l is quantized in steps of h. Values from 0 to n-1 The values are named based on early spectroscopy. n shells 1=K, 2=L, 3=M, 4=N, 5=O l shells 0=s, 1=p, 2=d, 3=f, 4=g Orbital Shells A. Clark, Chemical Computing Group

  4. Spectral lines from atoms in a strong magnetic field are split. Zeeman effect Magnetic moment of orbiting electron Orbital magnetic number ml lines up with applied field. Values from –l to l Lz is with respect to field Zeeman Effect

  5. Electrons possess intrinsic angular momentum. Spin angular momentum s Spin magnetic number ms Electron spin s can only have one value: 1/2. ms = +1/2 or -1/2 Spin up or spin down No two atomic electrons can occupy the same set of quantum numbers. Pauli exclusion principle Applies to fermions Photons are spin 1 Spin

  6. Electron Configurations • Electrons in atoms populate the lowest energies first. • Two electrons per state for spin • Atoms have unique ground states. • Hydrogen has 1 1s electron • Helium adds another 1s • Lithium must start 2s shell • Boron starts 2p shell which holds 6 electrons H He Li Be B C N O

  7. Germanium (Ge) has an atomic number of 32. Find the shell configuration for the ground state. Start counting shells from the lowest state. n = 1, l = 0: 1s – 2 electrons n = 2, l = 0: 2s – 2 electrons n = 2, l = 1: 2p – 6 electrons n = 3, l = 0: 3s – 2 electrons n = 3, l = 1: 3p – 6 electrons n = 3, l = 2: 3d – 10 electrons n = 4, l = 0: 4s – 2 electrons n = 4, l = 1: 4p – 2 electrons Total 2+2+6+2+6+10+2+2=32 Germanium

  8. Organized Table • The periodic table was organized to explain chemical properties. • Quantum physics explained structure

  9. Subshell: S G F D P Period 1 1s 2 2s 2p 3 3s 3p 4 4s 3d 4p 5 5s 4d 5p 6 6s 4f 5d 6p 7 7s 5f 6d 7p 8 8s 5g 6f 7d 8p The shells don’t fill up in exact order. Energy levels are determined by quantum calculations. General patterns exist Energy Levels next

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