1 / 27

Standing Waves

Explore the fundamentals of electron energy levels and their associated wave forms within atomic structure. This overview covers energy levels that exist and those that are forbidden, highlighted by the phenomenon of standing waves. We delve into the implications of Pauli's Exclusion Principle on electron spins, transitioning energy levels of hydrogen atoms, and how electron configurations are systematically filled across various orbitals—from s, p, d to f. Gain insights into electron configurations, representative notations, and their application in understanding atomic behavior.

nerina
Télécharger la présentation

Standing Waves

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Standing Waves

  2. Wave form for an electron Energy Level that can exist.

  3. Wave form for an electron Energy Level that cannot exist.

  4. Electron spins for Pauli’s Exclusion Principle

  5. Principle Energy Levels

  6. Ground State

  7. Excited State

  8. Ground State

  9. Hydrogen electron transitions within visible light Spectrum

  10. Hydrogen Electron Transitions(All observed changes)

  11. s - orbital

  12. p - orbitals

  13. d - orbitals

  14. f - orbitals

  15. 1st Energy Level has an s-orbital with 1 orientation = 2 e- 2nd Energy Level has an s-orbital with 1 orientation = 2e- p-orbital with 3 orientations = 6e- (total of 8e-) 3rd Energy Level has an s-orbital with 1 orientation = 2e- p-orbital with 3 orientations = 6e- d-orbital with 5 orientations = 10e- (total of 18e-) 4th Energy Level has an s-orbital with 1 orientation = 2e- p-orbital with 3 orientations = 6e- d-orbital with 5 orientations = 10e- f-orbital with 7 orientations = 14e- (total of 32e-)

  16. 5th Energy Level has an s-orbital with 1 orientation = 2e- p-orbital with 3 orientations = 6e- d-orbital with 5 orientations = 10e- f-orbital with 7 orientations = 14e- (total of 32e-) 6th Energy Level has an s-orbital with 1 orientation = 2e- p-orbital with 3 orientations = 6e- d-orbital with 5 orientations = 10e- (total of 18e-) 7th Energy Level has an s-orbital with 1 orientation = 2e- p-orbital with 3 orientations = 6e- (total of 8e-) Total electrons accounted for = 118

  17. Principle Energy Levels with orbitals, showing orbital overlaps

  18. Order of electron fill The resulting order in which electrons will fill the possible sublevels is: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

  19. Sublevel Groupings on the Periodic Table

  20. These electrons can fit in the same orbital because they have opposite spins.

  21. Pauli’s Exclusion Principle Two electrons with the same spin would have an additional magnetic repulsion in addition to their electrical repulsion and would, therefore be excluded from occupying the same orbital.

  22. The p-orbital has 3 orientations. All three orientations are at the same energy. If there were 3 electrons to be placed in the p-orbital, then each would have a different orientation, as illustrated below:

  23. If there were a fourth electron to be placed in this set of orbitals it would pair with one of these, spinning in the opposite direction.

  24. Electron Configuration Notation

  25. Methods for indicating electron placements Isotopic Symbol Electron Configuration Orbital Notation Noble Gas Notation Bohr – Rutherford Model

More Related