Electronic configuration

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Electronic configuration

  1. 1. ELECTRONIC CONFIGURATION<br />
  2. 2. ELECTRONIC CONFIGURATION<br />-arrangement of electrons in the space around the nucleus of an atom.<br />-distribution of electrons in the orbitals of an atom.<br />
  3. 3. ELECTRONIC CONFIGURATION<br />ENERGY LEVEL (electron shell)<br />-orbit where electrons spin around the nucleus of an atom.<br />
  4. 4. ELECTRONIC CONFIGURATION<br />
  5. 5. ELECTRONIC CONFIGURATION<br />ENERGY SUBLEVEL (subshell)<br />-energy subdivision of a principal energy level.<br />-designated by: <br />s(sharp) <br />p (principal) <br />d (diffuse) <br />f (fundamental) <br />
  6. 6. Mnemonic Device for Electronic Configuration<br />
  7. 7. Electronic configuration of:<br />IodineI53<br />= 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5<br />
  8. 8. Electronic configuration of:<br />Silicon Si14<br />= 1s2 2s2 2p6 3s2 3p2<br />LeadPb82<br />= 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p2<br />
  9. 9. RULES <br />AND <br />CONCEPTS<br />
  10. 10. AUFBAU’S PRINCIPLE<br />-”aufbau” –building up<br />-principle of electrons filling up the orbitals in order of increasing energy.<br />
  11. 11. PAULI’S EXCLUSION PRINCIPLE<br />-an orbital may be occupied by a maximum of two (2) electrons.<br />-the maximum number of electrons in each of the sublevels and orbitals:<br />
  12. 12.
  13. 13. HUND’S RULE<br />-if electrons have more than one equivalent orbital available, they will half-fill each of the equivalent orbitals before filling the second half of each.<br />
  14. 14. Example: Electronic configuration of: 14N = 1s2 2s2 2p37<br />
  15. 15. Electronic configuration of:56Fe= 1s22s2 2p6 3s2 3p6 4s2 3d 626<br />

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