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Hog Hilton Part I

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					Good morning! Today is November 17, 2010 (B day)

TURN IN ELECTRON CONFIGURATIONS WORKSHEET!

                         ChemCatalyst

Answer the following questions in your notebook:
1. What are the only possible values that the spin quantum
   number, ms, can have?
2. Complete the table below:

            l    Letter/shape   ALL possible values of ml
         l=0
         l=1
         l=2
         l=3
Electron Orbital Diagrams
             Objective
• To compare and contrast the energies
  of the electron orbitals on the same
  energy level and on different energy
  levels
     Electron Configuration
• Shows the value of 2 quantum numbers
  – Principal
  – Azimuthal

• Does not show the value of the other
  quantum numbers
  – Magnetic
  – Spin
  Magnetic Quantum Number
• ml

• Equal to –l to l

• Tells how many ways the orbital can be
  oriented (positioned)
         Magnetic Quantum Number
     l       Letter/shape      ALL possible values of ml
    l=0           s                      0
    l=1           p                   -1, 0, 1
    l=2           d               -2, -1, 0, 1, 2
    l=3           f            -3, -2, -1, 0, 1, 2, 3

•   One way to orient “s”
•   Three ways to orient “p”
•   Five ways to orient “d”
•   7 ways to orient “f”
   Electron Configuration Layout
7p ___ ___ ___
6d ___ ___ ___ ___ ___
5f ___ ___ ___ ___ ___ ___ ___
7s ___
6p ___ ___ ___
5d ___ ___ ___ ___ ___
4f ___ ___ ___ ___ ___ ___ ___
6s ___
5p ___ ___ ___
4d ___ ___ ___ ___ ___
5s ___
4p ___ ___ ___
3d ___ ___ ___ ___ ___
4s ____
3p ___ ___ ___
3s ___
2p ___ ___ ___
2s ___
1s ___
             The Layout
• Shows the electron configuration
  arranged vertically

  – Energy increases as you move up
       Spin Quantum Number
• ms

• Equal to -½ or ½
        Filling the Diagram
• Use arrows

  – ↑and ↓


• Based on 3 rules
          Aufbau Principle
• Electrons enter orbitals of lowest
  energy first
      Pauli Exclusion Principle
• An atomic orbital may only hold 2 electrons

• Electrons must have opposite spins

  – ms = ½ or -½


  – Denoted by direction of arrows
                 Hund’s Rule
• Every orbital of the same energy is singly
  occupied before any orbital is doubly occupied

  – Add up arrows first singly

  – Add down arrows to double

				
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