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Electron Configuration of Ions

Electron Configuration of Ions. Electron Configuration Exceptions. A filled or exactly half- filled d-subshell is very stable Half-filled: d 5 Filled : d 10. Electron Configuration Exceptions. A filled or exactly half-filled d-subshell is very stable Half-filled: d 5 Filled: d 10

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Electron Configuration of Ions

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  1. Electron Configuration of Ions

  2. Electron Configuration Exceptions A filled or exactly half-filled d-subshell is very stable Half-filled:d5 Filled: d10

  3. Electron Configuration Exceptions • A filled or exactly half-filled d-subshell is very stable • Half-filled: d5 • Filled: d10 Example: Chromium: [Ar] 4s2 3d4

  4. Electron Configuration Exceptions • A filled or exactly half-filled d-subshell is very stable • Half-filled: d5 • Filled: d10 Example: Chromium: [Ar] 4s2 3d4 [Ar] 4s1 3d5 Copper:

  5. Electron Configuration Exceptions • A filled or exactly half-filled d-subshell is very stable • Half-filled: d5 • Filled: d10 Example: Chromium: [Ar] 4s2 3d4 [Ar] 4s13d5 Copper: [Ar] 4s2 3d9 

  6. Electron Configuration Exceptions • A filled or exactly half-filled d-subshell is very stable • Half-filled: d5 • Filled: d10 Example: Chromium: [Ar] 4s2 3d4 [Ar] 4s13d5 Copper: [Ar] 4s2 3d9  [Ar] 4s13d10

  7. Electron Configuration Exceptions • A filled or exactly half-filled d-subshell is very stable • Half-filled: d5 • Filled: d10 Example: Chromium: [Ar] 4s2 3d4 [Ar] 4s13d5 Copper: [Ar] 4s2 3d9  [Ar] 4s13d10 Molybdenum: [Kr] 5s2 4d4 

  8. Electron Configuration Exceptions • A filled or exactly half-filled d-subshell is very stable • Half-filled: d5 • Filled: d10 Example: Chromium: [Ar] 4s2 3d4 [Ar] 4s1 3d5 Copper: [Ar] 4s2 3d9  [Ar] 4s13d10 Molybdenum: [Kr] 5s2 4d4  [Kr] 5s14d5

  9. Electron Configurations for Ions • NEGATIVE IONS • Add electrons to the last unfilled subshell Example: Oxygen: (add two electrons) [He] 2s2 2p4 + 2 electrons 

  10. Electron Configurations for Ions • NEGATIVE IONS • Add electrons to the last unfilled subshell Example: Oxygen: (add two electrons) [He] 2s2 2p4 + 2 electrons  [He] 2s2 2p6

  11. Electron Configurations for Ions • NEGATIVE IONS • Add electrons to the last unfilled subshell Example: Oxygen: (add two electrons) [He] 2s2 2p4 + 2 electrons  [He] 2s2 2p6 Sulphur: (add one electron) [Ne] 3s2 3p4 + electron 

  12. Electron Configurations for Ions • NEGATIVE IONS • Add electrons to the last unfilled subshell Example: Oxygen: (add two electrons) [He] 2s2 2p4 + 2 electrons  [He] 2s2 2p6 Sulphur: (add one electron) [Ne] 3s2 3p4 + electron  [Ne] 3s2 3p5

  13. Electron Configurations for Ions • POSITIVE IONS • Two Rules: • Electrons in the outermost shell (largest n-value) are removed first. • If there are electrons in both the s- and p-orbitals of the outermost shell, the electrons in the p-orbitals are removed first. Write the core notation for the atom, then remove electrons in the order: p-electrons before s-electrons before d-electrons

  14. Electron Configurations for Ions Example: Tin2+: (remove 2 electrons) [Kr] 5s2 4d10 5p2

  15. Electron Configurations for Ions Example: Tin2+: (remove 2 electrons) [Kr] 5s2 4d10 5p2 [Kr] 5s2 4d10 Tin4+: (remove 4 electrons) [Kr] 5s2 4d10 5p2

  16. Electron Configurations for Ions Example: Tin2+: (remove 2 electrons) [Kr] 5s2 4d10 5p2 [Kr] 5s2 4d10 Tin4+: (remove 4 electrons) [Kr] 5s2 4d10 5p2 [Kr] 4d10 Vanadium2+: (remove 2 electrons) [Ar] 4s2 3d3

  17. Electron Configurations for Ions Example: Tin2+: (remove 2 electrons) [Kr] 5s2 4d10 5p2 [Kr] 5s2 4d10 Tin4+: (remove 4 electrons) [Kr] 5s2 4d10 5p2 [Kr] 4d10 Vanadium2+: (remove 2 electrons) [Ar] 4s2 3d3 [Ar] 3d3

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