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Honors Chemistry Section 4.3

Honors Chemistry Section 4.3. Electron Configurations. Electron Configuration is the arrangement of electrons in an atom Every atom has a unique electron configuration Atoms tend to lowest E state, so normally exist in ground state. Electron Configuration.

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Honors Chemistry Section 4.3

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  1. Honors ChemistrySection 4.3 Electron Configurations

  2. Electron Configuration is the arrangement of electrons in an atom • Every atom has a unique electron configuration • Atoms tend to lowest E state, so normally exist in ground state Electron Configuration

  3. Aufbau Principle – Electrons occupy the lowest energy orbital available to them • Pauli Exclusion Principle – No two electrons can have the same 4 quantum numbers • Hund’s Rule – Orbitals of equal energy (called degenerate orbitals) are each occupied by one electron, before any is occupied by a second electron. All single electrons have the same spin. Rules for Electron Configuration

  4. Orbital Energies

  5. Hydrogen • ↿ 1s • Helium • ↿⇂ 1s • Oxygen • ↿⇂ ↿⇂ ↿⇂↿⇂ ↿⇂ 1s 2s 2px 2py 2pz Orbital Notation

  6. Hydrogen • 1s1 • Helium • 1s2 • Oxygen • 1s2 2s2 2p4 Electron Configuration

  7. Filling Order – Memory Aid

  8. What is the electron configuration of Carbon? • Write the electron configuration and orbital notation for Sulfur Practice

  9. Highest Occupied Level – The highest main energy level (highest n value) that contains an electron • Outer shell electrons – electrons in the Highest Occupied Level • Inner shell electrons – all those electrons EXCEPT those in the Highest Occupied Level • Example – Carbon • 2 inner shell electrons • 4 outer shell electrons Definitions

  10. Noble gas – Has full s and p orbitals • Noble gas configuration • [symbol] stand for the complete electron configuration of the specified noble gas • Add electrons after noble gas required for element. • Na – [Ne] 3s1 Noble Gases

  11. All noble gases have full outer main energy levels • He – 2 electrons (Energy Level n=1) • All others – 8 electrons (Energy Level n = 2 to 7) Important Note

  12. Filling Orbtials and the Periodic Table

  13. Fill 4s first • Then next lowest energy 3d – it fills next • Followed by 4p Fourth Period

  14. Chromium • Expected - [Ar] 3d4 4s2 • Actual - [Ar] 3d5 4s1 • Why? • Two half filled orbitals have more stability and lower energy than one full and one partially full • Copper • Expected - [Ar] 3d8 4s2 • Actual - [Ar] 3d10 4s0 • Why? • A full d orbital and unfilled s orbital have more stability and lower energy than one full and one partially full 4th Period Exceptions to the Expected Filling Order – KNOW THESE!!!!

  15. Deviates from Nb to Ag 5th Block Exceptions to the Expected Filling Order

  16. What element has 2 electrons in the p orbitals in the 2nd Energy Level? • What is the maximum number of electrons that can be found on the second energy level? • What element in the third period has the same outer electron configuration as the element in #1? Practice

  17. What element has 5 electrons in the p sublevel on the third energy level? • How many total electrons does this element have on the third energy level? • What element in the 4th Period has the same outer configuration as this element? More Practice

  18. What element has the configuration [Ne]3s1? • How many inner shell electrons does this element have? • What is the Noble Gas configuration for Al? • How many outer shell electrons? • How many inner shell electrons? Even More Practice

  19. Write the electron configuration and Noble Gas configuration for Ti. • How many electron containing orbitals in Ti? • How many orbitals in Ti are completely filled? Are you Ready for More?

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