Lecture 5.2- Electron Configurations
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Lecture 5.2- Electron Configurations

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Section 5.2 Lecture for Honors & Prep Chemistry

Section 5.2 Lecture for Honors & Prep Chemistry

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  • This aufbau diagram shows the energy levels of the various atomic orbitals. Orbitals of greater energy are higher on the diagram. Using Tables Which is of higher energy, a 4d or a 5s orbital?

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  • 1. Bellwork- draw orbitals Draw the following atomic orbitals to scale 1s 2s 3s three 2p orbitals Three 3p orbitals
  • 2. Electron configurations show where each electron in an atom is located. Three rules —the aufbau principle, the Pauli exclusion principle, and Hund’s rule— tell you how to find the electron configurations of atoms.
  • 3. According to the aufbau principle, electrons occupy the orbitals of lowest energy first. In the aufbau diagram below, each box represents an atomic orbital.
  • 4. The higher an orbital is on the orbital chart, the higher its energy, so orbitals fill from bottom to top.
  • 5. According to the Pauli exclusion principle, an atomic orbital may hold at most two electrons. To occupy the same orbital, two electrons must have opposite spins.   1 e- in this orbital 2 e-
  • 6. Hund’s rule states that electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible. For orbitals of equal energy, 1 e- per orbital before you double up! 3p  NOT 3p 
  • 7. Fill in an orbital diagram for phosphorus, boron and silicon. Energy level # of e- in that sublevel sublevel type
  • 8. Fill in an orbital diagram for phosphorus, boron and silicon. Energy level # of e- in that sublevel P 1s2 2s2 2p6 3s2 3p3 sublevel type The superscripts will add up to the number of e- in the atom.