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• Principal Quantum Number, n
• Azimuthal Quantum Number, l
• Magnetic Quantum Number, ml
Exercise
• What are the similarities and differences
between the hydrogen atom 1s and 2s
orbitals?
• For n=4 what are the ...
Main
Energy
Level
No. of
Sublevel
Identity of
Sublevels
No. of
Orbitals
(n2)
Max. No. of
Electrons
(2n2)
1 1 1s 1 2
2 2
2s...
Electron Spin Quantum Number, m
• Two possible values are allowed
+ ½ and - ½
• Opposite directions
Can two electrons in an atom have the
same set of quantum numbers?
Pauli Exclusion Principle
• No two electrons in an atom can have the
same set of four quantum numbers, n, l, ml,
and ms.
•...
Electron Configuration
• The way in which electrons are distributed
among the various orbitals of an atom
Aufbau Principle
• Electrons occupy orbitals of lower energy first.
The relation between orbital filling and the periodic
table
The relation between orbital filling and the periodic
table
Hund’s Rule
• For degenerate orbitals, the lowest energy is
attained when the number of electrons with
the same spin is ma...
Orbital Diagram
Anomalous Electron Configuration
Example:
Chromium
Copper
• Consequence of the closeness of the 3d and
4s orbital energies.
• Minor departures from the expected
• Not of great chem...
Seat work
Write the electron configuration and the
electron orbital diagram for the following
elements.
1. Cl
2. Os
3. Cs
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
Electron configuration
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Electron configuration Slide 1 Electron configuration Slide 2 Electron configuration Slide 3 Electron configuration Slide 4 Electron configuration Slide 5 Electron configuration Slide 6 Electron configuration Slide 7 Electron configuration Slide 8 Electron configuration Slide 9 Electron configuration Slide 10 Electron configuration Slide 11 Electron configuration Slide 12 Electron configuration Slide 13 Electron configuration Slide 14 Electron configuration Slide 15 Electron configuration Slide 16 Electron configuration Slide 17 Electron configuration Slide 18 Electron configuration Slide 19 Electron configuration Slide 20 Electron configuration Slide 21 Electron configuration Slide 22 Electron configuration Slide 23 Electron configuration Slide 24 Electron configuration Slide 25 Electron configuration Slide 26 Electron configuration Slide 27 Electron configuration Slide 28 Electron configuration Slide 29

Electron configuration

  1. 1. • Principal Quantum Number, n • Azimuthal Quantum Number, l • Magnetic Quantum Number, ml
  2. 2. Exercise • What are the similarities and differences between the hydrogen atom 1s and 2s orbitals? • For n=4 what are the possible values of l and m? • give the values for n, l, m for a. 2p b. 5d c. 5f
  3. 3. Main Energy Level No. of Sublevel Identity of Sublevels No. of Orbitals (n2) Max. No. of Electrons (2n2) 1 1 1s 1 2 2 2 2s 2p 1 3 2 6 3 3 3s 3p 3d 1 3 5 2 6 10 4 4 4s 4p 4d 4f 1 3 5 7 2 6 10 14
  4. 4. Electron Spin Quantum Number, m • Two possible values are allowed + ½ and - ½ • Opposite directions
  5. 5. Can two electrons in an atom have the same set of quantum numbers?
  6. 6. Pauli Exclusion Principle • No two electrons in an atom can have the same set of four quantum numbers, n, l, ml, and ms. • An orbital can hold a maximum of two electrons and they must have opposite spins.
  7. 7. Electron Configuration • The way in which electrons are distributed among the various orbitals of an atom
  8. 8. Aufbau Principle • Electrons occupy orbitals of lower energy first.
  9. 9. The relation between orbital filling and the periodic table
  10. 10. The relation between orbital filling and the periodic table
  11. 11. Hund’s Rule • For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized.
  12. 12. Orbital Diagram
  13. 13. Anomalous Electron Configuration Example: Chromium Copper
  14. 14. • Consequence of the closeness of the 3d and 4s orbital energies. • Minor departures from the expected • Not of great chemical significance
  15. 15. Seat work Write the electron configuration and the electron orbital diagram for the following elements. 1. Cl 2. Os 3. Cs
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