UNIT 3: Electron Configuration

• Electron Configuration


  ways in which e- are arranged in various orbitals.
• How to find the Electron Configuration of atoms?

  Aufbau Principle

  Pauli Exclusion

  Hund's Rule
• 1. Energy Level
  2. Energy Sublevel
  3. Number of electrons


  Label the following:

  
• Quantum Mechanical Model determines the probability of finding an e- w/in a certain volume of space surrounding the nucleus (represented by a fuzzy cloud).
• fixed energy = energy level
• Excited State


  at what state is this atom?

  
• Ground state


  at what state is this atom?

  
• Orbitals


  region in space where there is a 90% probability of finding e-.
• s-orbitals


  spherical shaped orbitals
• p-orbitals


  dumbbell shaped orbitals
• Aufbau Principle


  e- occupy the orbitals of lowest energy first.
• Pauli Exclusion


  To occupy the same orbital, two e- must have opposite spins.
• Hund's Rule


  e- will not join other e- in an orbital if an orbital of the same energy is available for occupancy.
• Example of Exceptional Electron Configuration

  Copper
• Quantum Numbers

  1. Principal
  2. Azimuthal
  3. Magnetic
  4. Spin
• No. of orbitals each sublevel:

  s = 1

  p = 3

  d = 5

  f = 7
• No. of maximum electrons each sublevels:

  s = 2

  p = 6

  d = 10

  f = 14
• indicates the main energy level

  Principal Quantum #s
• indicates the shape of the orbital.

  Azimuthal Quantum #s
• indicates the orientation of an orbital.

  Magnetic Quantum #s
• indicates the orientation of the e- spin.

  Spin Quantum #s
• Values of Quantum #s:

  1. Principal = 1, 2, 3, 4, 5, 6, 7
  2. Azimuthal = 0, 1, 2, 3
  3. Magnetic = -l, ..., +l
  4. Spin = -1/2, +1/2
• Paramagnetic


  has unpaired e-.
• Diamagnetic


  always has paired e-.