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Electron Structure

Electron Structure. The Quantum Number The electron’s “hood”. Electron Structure. The Quantum Number The electron’s “hood” 3 dimensional address. Electron Structure. The Quantum Number Attraction versus repulsion determines region, shape of region and spin of electron

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Electron Structure

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  1. Electron Structure • The Quantum Number • The electron’s “hood”

  2. Electron Structure • The Quantum Number • The electron’s “hood” • 3 dimensional address

  3. Electron Structure • The Quantum Number • Attraction versus repulsion determines region, shape of region and spin of electron • No electron can have the same 4 quantum numbers (Pauli Exclusion Principle)

  4. Electron Structure • The Quantum Number • Principal energy level (n) • 2 dimensional representation

  5. Electron Structure • The Quantum Number • Principal energy level (n) • Real pattern far different- both wave and particle • L number (azimuthal) – shape and orbital

  6. Electron Structure • The Quantum Number • Magnetic or m number • Spatial orientation of the orbital within atom • Starts with negative of l and goes to positive • E.g. l=2, m=-2,-1,0,1,2

  7. Electron Structure • The Quantum Number • Electron-spin quantum number • AKA magnetic (ms) number • Illustration – Helium (He) atom • Two electrons in one cloud • Opposite “spin” or magnetic qualities • + ½ (Arrow up) or -1/2 (arrow down)

  8. Electron Structure • The Quantum Number n=1, l=0, m=0 • 1s2 • s=+½,-½   

  9. Electron Structure • This is the helium atom. It has 2 electrons. These are able to share the same s orbital because of opposite spins. The "2" in "1s2" means there are 2 electrons in that orbital. "s" orbitals can only hold 2 electrons, so that's as high as you will ever see it. The 1 in "1s2" means this is the s orbital belonging to the n=1 shell. n=1, l=0, m=0 • 1s2, s=+½ , -½  

  10. Electron Structure • Pauli Exclusion Principle • Each orbital can contain only one electron with each kind of spin • If two electrons are in an orbital they must have different ms values

  11. Electron Structure

  12. Electron Structure • Diagonal fill rule • s levels fill first, p next , d after p and f last of all

  13. Electron Structure • Hund’s Rule

  14. Electron Structure • Aufbau principle

  15. Electron Configuration & The Periodic Table

  16. Orbital Notation

  17. Orbital Notation Longhand notation for Li: 1s2 2s1 Shorthand notation for Li: [He]2s1 Be: [He]2s2 B: [He]2s22p1 See table 4-5 p. 90 Hund’s rule example: C

  18. Atomic Number & Mass Atomic Mass = sum of mass of protons + mass of neutrons

  19. Atomic Number & Mass http://jefflittle.edu.glogster.com/the-periodic-table/

  20. The Periodic Table http://jefflittle.edu.glogster.com/the-periodic-table/

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