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Electron Configurations
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  1. Electron Configurations Page 35 of Scientific Notebook

  2. SPI’s & CLE’s: • SPI 3221.1.2 Describe an elements atomic make-up • SPI 3221.1.3 Describe an atoms composition and electron composition. • CLE 3221.2.1 Investigate the characteristic properties of matter.

  3. Objective: • TLW evaluate electrons by writing electron configurations and orbital diagrams • TLW review electrons and light • TLW evaluate and understand atoms, electrons, and electron configurations • TLW determine the importance of electron configurations to the world in which we live • TLW link electrons and electron configuration to matter, composition, and reactions.

  4. What are electron Configurations? • A written arrangement of electrons in an atom. • Shorthand notation of where the electrons are in an atom. • Electrons in an atom tend to have arrangements that have the lowest possible energies.

  5. What is the Principal Quantum number(n)? • A number that specifies the size and energy of atomic orbitals. • The number can be a 1-7. • Each quantum number can have orbitals • There are s- oribitals, p-orbitals, d-orbitals, and f-orbitals(rememeber orbitals are where electrons are located)

  6. What is the Aufbau Principle? States that electrons fill orbitals that have the lowest energy first.

  7. What is the Pauli Exclusion Principle? States that two, but no more than two, electrons can occupy a singe orbital.

  8. What is Hund’s Rule? States that the orbitals of the same quantum numbers are each occupied by one electron before any pairing occurs (Electrons are represented by arrows).

  9. Electron Review(don’t write) • Why are Electron Configurations important? • Shows us were electrons are located. • Identifies Valence Electrons • What is meant by the Duality of light/electrons? • Behave like particles • Behave like waves

  10. What are valence electrons? • Electrons in the outermost shell • Electrons that participate in chemical reactions Why is this important?

  11. ELECTRON CONFIGURATION • Electron are represented by arrows • Shell: 1s > 2s > 2p > 3s > 3p > 4s >3d • S- 2 p - 6 d - 10 f - 14 Page 36

  12. Orbitals(Energy Sublevels) Page 36

  13. Guided Practice: • Electron Configuration 1s 2s 2p 3s 3p • Orbital Diagram _ _ _ _ _ _ _ _ _ 1s 2s 2p 3s 3p

  14. Independent Practice:

  15. Electron Review • Why are Electron Configurations important? • Shows us were electrons are located. • Identifies Valence Electrons • What is meant by the Duality of light/electrons? • Behave like particles • Behave like waves

  16. Enrichment: Which of the following “rules” is being violated in each electron configuration below? Explain your answer for each. Hund’s Rule, Pauli Exclusion Principle, Aufbau Principle  __ __ 1s 2s 2p Hund’s Rule

  17. Just One More • Write the Electron Configuration and Orbital Diagram for Calcium.