1 / 17

Chapter 6

Chapter 6. Electron Configurations. Electron Configurations Every electron has a name. Name of each electron unique Name consists of four numbers: n,l,m l ,m s We must learn to name our electrons Unlike people, there is a lot in the “ name ” of an electron. Electron Configurations.

matthewbrady
Download Presentation

Chapter 6

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. Chapter 6 Electron Configurations

  2. Electron Configurations Every electron has a name • Name of each electron unique • Name consists of four numbers: • n,l,ml,ms • We must learn to name our electrons • Unlike people, there is a lot in the “name” of an electron.

  3. Electron Configurations • Distribution of all electrons in an atom • Consist of • Number denoting the energy level

  4. Electron Configurations • Distribution of all electrons in an atom • Consist of • Number denoting the energy level • Letter denoting the type of orbital

  5. Electron Configurations • Distribution of all electrons in an atom. • Consist of • Number denoting the energy level. • Letter denoting the type of orbital. • Superscript denoting the number of electrons in those orbitals.

  6. Orbital Diagrams • Each box represents one orbital. • Half-arrows represent the electrons. • The direction of the arrow represents the spin of the electron. 1s22s1

  7. Hund’s Rule(of maximum multiplicity) “For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized.” NOT:

  8. Electron configurations

  9. Why do we accept this wacko stuff? It predicts the periodicity of the periodic table!! • We fill orbitals in increasing order of energy. • Different blocks on the periodic table, then correspond to different types of orbitals.

  10. Why do we accept this wacko stuff? It predicts the periodicity of the periodic table!! • Remember: The periodic table was arranged the way it was based on chemical properties. • Totally empirical, until now. Based only on observation.

  11. Periodic Table • Periodic table tells you about the last electron that went in!!! • Periodic table also makes it easy to do electron configurations.

  12. Short cut for writing electron configurations

  13. Electron configurations of the elements

  14. Some Anomalies Some irregularities occur when there are enough electrons to half-fill s and d orbitals on a given row.

  15. Some Anomalies For instance, the electron configuration for Chromium, is [Ar] 4s1 3d5 rather than the expected [Ar] 4s2 3d4.

  16. Some Anomalies • This occurs because the 4s and 3d orbitals are very close in energy. • These anomalies occur in f-block atoms, as well.

  17. Writing Configurations for transition metal cations • Write the electron configuration first, then remove the s electrons then the d electrons to get the positive charge. • Example : Fe = [Ar]4s23d6, Fe+2 = [Ar] 3d6

More Related