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Atomic Structure (II)

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Bernard Ng
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Quantum Numbers © my-chem-tutor.blogspot.com ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],f d p s Subshell 3 2 1 0 l
[object Object],[object Object],[object Object],[object Object],Prentice Hall © 2005
p orbitals s orbital Prentice Hall © 2005
d orbitals Prentice Hall © 2005
Order of filling orbitals © my-chem-tutor.blogspot.com [1] Fill orbitals with lower energy 1st [Aufbau Principle] [2] Each orbital can accommodate 2 electrons [Pauli Exclusion Principle] [3] Where there is a choice between orbitals of equal energy, fill the orbitals singly 1st [Hund’s Rule] (minimise electron repulsion) 4s orbital is lower in E than 3d ( when unfilled )!
Electronic configuration © my-chem-tutor.blogspot.com Examples: Ca O Cl Si Na 20 40 11 23 8 35 16 17 28 14 B 5 11 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 4 1s 2 2s 2 2p 5 1s 2 2s 2 2p 6 3s 2 3p 2 1s 2 2s 2 2p 1

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Atomic Structure (II)

  • 1.
  • 2.
  • 3. p orbitals s orbital Prentice Hall © 2005
  • 4. d orbitals Prentice Hall © 2005
  • 5. Order of filling orbitals © my-chem-tutor.blogspot.com [1] Fill orbitals with lower energy 1st [Aufbau Principle] [2] Each orbital can accommodate 2 electrons [Pauli Exclusion Principle] [3] Where there is a choice between orbitals of equal energy, fill the orbitals singly 1st [Hund’s Rule] (minimise electron repulsion) 4s orbital is lower in E than 3d ( when unfilled )!
  • 6. Electronic configuration © my-chem-tutor.blogspot.com Examples: Ca O Cl Si Na 20 40 11 23 8 35 16 17 28 14 B 5 11 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 4 1s 2 2s 2 2p 5 1s 2 2s 2 2p 6 3s 2 3p 2 1s 2 2s 2 2p 1