1 / 26

Section 5.3

Section 5.3. Electron Configurations. Electron Configurations. Atom is in the ground state 3 rules or laws Aufbau principle Pauli Exclusion principle Hund’s Law. Aufbau Principle. Electrons occupy lowest energy orbital available All orbitals of a sublevel are equal energy

hedwig
Download Presentation

Section 5.3

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. Section 5.3 Electron Configurations

  2. Electron Configurations • Atom is in the ground state • 3 rules or laws • Aufbau principle • Pauli Exclusion principle • Hund’s Law

  3. Aufbau Principle • Electrons occupy lowest energy orbital available • All orbitals of a sublevel are equal energy • Sublevels have different energies • s < p < d <f • Orbitals within one principal energy level can overlap orbitals of another

  4. Electron Filling Order Which orbital will fill first, 4s or 3d?

  5. Periodic Table Helps!

  6. Pauli Exclusion Principle • Maximum of 2 electrons in an orbital, but only if they have opposite spin.

  7. Hund’s rule • Electrons with same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbital.

  8. Orbital Filling Order 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

  9. Electron Configurations • Three methods 1. Electron Configuration Notation 2. Noble Gas Notation 3. Orbital Diagrams

  10. Electron Configuration Notation • Ex: N • # of electrons? • Start with the lowest energy, fill to capacity, go to next lowest energy, etc. Stop when you run out of electrons. • Superscripts = total electrons

  11. Electron Configuration Notation • You try … Zinc

  12. Electron Configuration Notation 1s2 2s22p6 3s23p6 4s23d10

  13. Assignment • Write the electron configuration notation for the following elements: • Boron (B), Neon (Ne), Sulfur (S), Magnesium (Mg), Vanadium (V), Silver (Ag)

  14. Noble Gas Notation • Shorthand • Find the noble gas closest to the element (without going over). • Ex: For Gold (79): Xenon (54) • We write [Xe] and start counting from there • The first orbital after xenon is 6s

  15. Noble Gas Notation • [Xe]6s2 4f14 5d9 • Check: (Xe’s atomic number) 54 + 2 + 14 + 9 = 79 (gold’s Atomic number)!

  16. You Try… • Silver

  17. Assignment • P.147 #79

  18. Orbital Diagrams • Draw a line for each orbital • Designate each electron with an arrow • = orbital with 1 electron • = orbital with 2 electrons

  19. Orbital Diagrams • Nitrogen: 1s22s22p3 • Write notation of N • Then we fill them with electrons using the Aufbau principle, Pauli exclusion principle, and Hund’s law

  20. Orbital Diagrams • You try another example: Cu

  21. Orbital Diagrams • Answer

  22. Assignment • Draw orbital diagrams for beryllium, aluminum, nitrogen, and sodium, manganese, germanium, and europium.

  23. Electron Dot Structures • Valence electrons • Electrons in outermost energy level. • Responsible for chemical properties

  24. Electron Dot Structures • Valence electrons only • Place ‘dots’ around element symbol • 4 sides of element = orbitals • Fill these orbitals one at a time (Hund’s)

  25. Electron Dot Structures

  26. Assignment • P.141 #23(yellow box), 26, 28 • P.147 #81

More Related