3.3 electron configuration
Upcoming SlideShare
Loading in...5

Like this? Share it with your network


3.3 electron configuration






Total Views
Views on SlideShare
Embed Views



0 Embeds 0

No embeds


Upload Details

Uploaded via as Microsoft PowerPoint

Usage Rights

© All Rights Reserved

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
Post Comment
Edit your comment

3.3 electron configuration Presentation Transcript

  • 1. ElectronElectron ConfigurationConfiguration 3.33.3
  • 2. ModelsModels • 1st model of the atom – Rutherford “plum pudding” • Next model – Bohr, 2 years later – Introduced the idea of energy levels • The difference between 2 energy levels is a quantum of energy.
  • 3. Present ModelPresent Model • Orbitals are like clouds. – Show areas where electrons are likely to be found. • Like the propellers on an airplane or helicopter.
  • 4. Light is a Wave…Light is a Wave… • Light travels in waves. • 2.998 x 108 m/s • ROYGBIV • Different colors have different energies. – Blue end is more energetic than the red end of the spectrum.
  • 5. Light is a particle?Light is a particle? • Einstein said light is a particle. – Observed the photoelectric effect. • When light strikes metal, electrons are released. – This only happens at certain frequencies.
  • 6. Light EmissionLight Emission • When energy is absorbed, electrons can move from a lower energy level to a higher energy level. • Electrons cannot maintain the higher state and fall back to their lower level. When this happens they release the energy they absorbed. – Produces light.
  • 7. StateState • Ground State – State of lowest possible energy – Where e- normally are • Excited State – Where e- moves when energy is absorbed – Can’t stay… – Emits light when falls back to ground state
  • 8. Energy LevelsEnergy Levels • s – Can contain only 2 e- • p – Can contain 6 e- • d – Can contain 10 e- • f – Can contain 14 e-
  • 9. Aufbau PrincipleAufbau Principle • The aufbau (German for “building up”) principle tells us the order to follow when writing energy levels and the e- they contain. • The next slide is extremely important.
  • 10. Aufbau PrincipleAufbau Principle 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 5f14 6s2 6p6 6d10 6f14 7s2 7p6 7d10 7f14
  • 11. PracticePractice Write electron orbital configurations for the elements below: 5 e- 27 e- 18 e- 19 e- 23 e- Stop and go to doc-cam
  • 12. AnswersAnswers B 1s2 2s2 2p1 Co 1s2 2s2 2p6 3s2 3p6 4s2 3d7 Ar 1s2 2s2 2p6 3s2 3p6 K 1s2 2s2 2p6 3s2 3p6 4s1 V 1s2 2s2 2p6 3s2 3p6 4s2 3d3
  • 13. Electrons & the Periodic TableElectrons & the Periodic Table • The periodic table is arranged by increasing atomic number (# of p+). • Each element is 1 proton and electron higher than the one before it. • It is an acceptable shortcut to write the electron configuration for larger elements by noting the symbol of the noble gas on the previous line before it followed by the remaining orbitals. • ???
  • 14. ExamplesExamples • Oxygen 1s2 2s2 2p4 can be written as [He] 2s2 2p4 • Br 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 can be written as [Ar] 4s2 3d10 4p5
  • 15. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 5f14 6s2 6p6 6d10 6f14 7s2 7p6 7d10 7f14