1 / 18

chemistry

chemistry. 5.2. Electron Configurations. The ways in which electrons are arranged in various orbitals around the nuclei of atoms are called electron configurations.

heberte
Download Presentation

chemistry

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. chemistry

  2. 5.2 Electron Configurations • The ways in which electrons are arranged in various orbitals around the nuclei of atoms are called electron configurations. • Three rules—the aufbau principle, the Pauli exclusion principle, and Hund’s rule—tell you how to find the electron configurations of atoms.

  3. 5.2 Electron Configurations • Aufbau Principle • According to the aufbau principle, electrons occupy the orbitals of lowest energy first. In the aufbau diagram below, each box represents an atomic orbital.

  4. 5.2 Electron Configurations • Pauli Exclusion Principle • According to the Pauli exclusion principle, no two electrons in an atom can have the same four quantum numbers. • What does that mean?

  5. Quantum Numbers: like addresses for electrons • (n) size of cloud (all w same n are in same energy level) • (l) shape of cloud (depends on orbital) • (m) orientation (depends on orbital) • (s) spin (clockwise or counterclockwise)

  6. 5.2 Electron Configurations • Hund’s Rule • Hund’s rule states that electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible.

  7. 5.2 Electron Configurations • Orbital Filling Diagram

  8. 1s22s22p63s23p3

  9. 5.2 Exceptional Electron Configurations • Exceptional Electron Configurations • Why do actual electron configurations for some elements differ from those assigned using the aufbau principle?

  10. 5.2 Exceptional Electron Configurations • Some actual electron configurations differ from those assigned using the aufbau principle because half-filled sublevels are not as stable as filled sublevels, but they are more stable than other configurations.

  11. 5.2 Exceptional Electron Configurations • Exceptions to the aufbau principle are due to subtle electron-electron interactions in orbitals with very similar energies. • Copper has an electron configuration that is an exception to the aufbau principle.

  12. Exception

  13. 5.2 Section Quiz. • 5.2.

  14. 5.2 Section Quiz. • 1. Identify the element that corresponds to the following electron configuration: 1s22s22p5. • F • Cl • Ne • O

  15. 5.2 Section Quiz. • 2. Write the electron configuration for the atom N. • 1s22s22p5 • 1s22s22p3 • 1s22s1p2 • 1s22s22p1

  16. 5.2 Section Quiz. • 3. The electron configurations for some elements differ from those predicted by the aufbau principle because the • the lowest energy level is completely filled. • none of the energy levels are completely filled. • half-filled sublevels are less stable than filled energy levels. • half-filled sublevels are more stable than some other arrangements. `

  17. END OF SHOW

More Related