1 / 17

Electron Configurations

Electron Configurations. Chapter 5. Heisenberg Uncertainty Principle. 1927 – German Physicist Werner Heisenberg States that it is nearly impossible to know for sure the exact location and the precise velocity of a subatomic particle at the same time. Explanation.

georgio-betagh
Download Presentation

Electron Configurations

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. Electron Configurations Chapter 5

  2. Heisenberg Uncertainty Principle 1927 – German Physicist Werner Heisenberg States that it is nearly impossible to know for sure the exact location and the precise velocity of a subatomic particle at the same time

  3. Explanation To “see” an electron, we pass photons through it (light is deflected back) but we can’t know it’s true velocity since when the photons hit it, the velocity changes

  4. Schrödinger ●Treated electrons as waves ● developed a complex mathematical formula to identify the position of an electron

  5. Wave Mechanical Model • Quantum Mechanical Model • Mathematical model – based on probability • Predicts energy levels for an atom that can be pictured like Bohr’s orbits • Only the PROBABILITY of finding an electron in a certain region of the atom is known

  6. Energy Levels • The largest area where electrons can be found (state) • Maximum of 7 PELs • Each PEL has one or more sublevels in it

  7. Sublevels • Smaller areas within an Energy Level (“city”) • # of sublevels in a PEL = PEL # • 4 types of sublevels • s • p • d • f

  8. Sublevels • PEL# of sublevelstype of sublevel 1 1 s 2 2 s,p 3 3 s,p,d 4 4 s,p,d,f 5 5 s,p,d,f…

  9. Orbital • Region within a sublevel where electrons can be found Sublevel# of orbitals s 1 p 3 d 5 f 7

  10. Principles • Pauli Exclusion Principle – A maximum of 2 e- can occupy an orbital • Aufbau Principle – Each e- enters an orbital of the lowest energy level first • Hund’s Rule – before a second e- can be placed in any orbital, all the orbitals of that sublevel must contain at least one e-

  11. Orbital Diagrams • Visual representation of how e- are placed in orbitals • In an orbital e- have opposite spins • Electrons are represented by arrows

  12. Aufbau Diagram

  13. Electron Configurations • The “address” of where e- can be found • Notation tells us the PEL, type of sublevel and the # of e- in that sublevel • Ex: 1s22s22p4

  14. Valence Valence Energy Levels – outermost energy level of an atom where electrons can be found Valence Electrons – electrons found in the valence energy level - maximum of 8 valence e-

  15. Dot Diagrams

More Related