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Orbital Notation

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ZB Chemistry
ZB Chemistry

The document discusses orbital notation, which visually represents electron configuration by showing the placement and spin of each electron in an atom. It defines key terms like Pauli exclusion principle, Aufbau principle, and Hund's rule that govern how electrons fill atomic orbitals. Examples are given of writing the electron configurations of sodium, boron, titanium, and calcium using orbital notation with half arrows to symbolize individual electrons.

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Orbital Notation Props to Mr. Smyk who gave me this ppt.
What is Orbital Notation Orbital notation is a visual transformation of the electron configuration. Orbital notation shows you where each specific electron is placed (in order) and what it’s “spin” is.
Vocabulary List Check Pauli Exclusion Principle: No two electrons in the same atom can have the same spin quantum number. If one electron has the value of + ½ then the other electron must have the value of − ½ . In Orbital notation this means the arrows representing the electrons must face opposite direction (+ is up, - is down).
Vocabulary List Check Aufbau principle: (you already know the concept) Aufbau is the German word for “building up.” The principle states that electrons fill orbitals that have the lowest energy first. You fill electrons in a certain order. 1 s < 2 s < 2 p < 3 s < 3 p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p
Vocabulary List Check Hund’s Rule: The rule that states that for an atom in the ground state, the number of unpaired electrons is the maximum possible and these unpaired electrons have the same spin. What? You must share your electrons. “Everybody gets one before anyone gets two.”
Meet your next reference sheet The orbital notation reference sheet. This shows each orbital split apart into its 3 dimensional axes. Relax, this is easy.
Write out the electron configuration for Sodium Na, 11e - 1s 2 2s 2 2p 6 3s 1 We are now going to represent each electron as a ‘half arrow”. We must fill in (build up) the electrons as we did previously but show them using arrows on the orbital notation diagram. First one in an orbital is placed up (+ ½ spin)
Write out the electron configuration for Boron B, 5e - 1s 2 2s 2 2p 1 We are now going to represent each electron as a ‘half arrow”. We must fill in (build up) the electrons as we did previously but show them using arrows on the orbital notation diagram. First one in an orbital is placed up (+ ½ spin)
Write out the electron configuration for Titanium Ti, 22e - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2
On your own. Calcium Ca, 20e - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2
Homework Complete the Electron Configuration Homework WKST.

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Orbital Notation

  • 1. Orbital Notation Props to Mr. Smyk who gave me this ppt.
  • 2. What is Orbital Notation Orbital notation is a visual transformation of the electron configuration. Orbital notation shows you where each specific electron is placed (in order) and what it’s “spin” is.
  • 3. Vocabulary List Check Pauli Exclusion Principle: No two electrons in the same atom can have the same spin quantum number. If one electron has the value of + ½ then the other electron must have the value of − ½ . In Orbital notation this means the arrows representing the electrons must face opposite direction (+ is up, - is down).
  • 4. Vocabulary List Check Aufbau principle: (you already know the concept) Aufbau is the German word for “building up.” The principle states that electrons fill orbitals that have the lowest energy first. You fill electrons in a certain order. 1 s < 2 s < 2 p < 3 s < 3 p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p
  • 5. Vocabulary List Check Hund’s Rule: The rule that states that for an atom in the ground state, the number of unpaired electrons is the maximum possible and these unpaired electrons have the same spin. What? You must share your electrons. “Everybody gets one before anyone gets two.”
  • 6. Meet your next reference sheet The orbital notation reference sheet. This shows each orbital split apart into its 3 dimensional axes. Relax, this is easy.
  • 7. Write out the electron configuration for Sodium Na, 11e - 1s 2 2s 2 2p 6 3s 1 We are now going to represent each electron as a ‘half arrow”. We must fill in (build up) the electrons as we did previously but show them using arrows on the orbital notation diagram. First one in an orbital is placed up (+ ½ spin)
  • 8. Write out the electron configuration for Boron B, 5e - 1s 2 2s 2 2p 1 We are now going to represent each electron as a ‘half arrow”. We must fill in (build up) the electrons as we did previously but show them using arrows on the orbital notation diagram. First one in an orbital is placed up (+ ½ spin)
  • 9. Write out the electron configuration for Titanium Ti, 22e - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2
  • 10. On your own. Calcium Ca, 20e - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2
  • 11. Homework Complete the Electron Configuration Homework WKST.