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Unformatted text preview: 1 1 Lecture 8 Chapter 6 square4 Electron configurations ( from last notes) square4 Electron configurations and the periodic table square4 Chemical periodicity 1 2 Electron Configurations of Simple Ions square4 Anions: Electrons added to form anions follow the Aufbau rule, Hunds rule and the Pauli Exclusion principle F + e- F- 1s 2 2s 2 2p 5 1s 2 2s 2 2p 6 3 Electron Configuration of Simple Ions square4 Cations Electrons are lost from an orbital in the highest n subshell Na Na + + e- 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 4 Paramagnetic / Diamagnetic Atoms and Ions square4 Paramagnetic square4 atoms and ions whose electron arrangement results in one or more unpaired electrons square4 paramagnetic materials are attracted into a magnetic field square4 Diamagnetic square4 atoms and ions whose electron arrangement results in all electrons paired in orbitals square4 diamagnetic materials are not attracted into a magnetic field 2 2 Ground State vs Excited State square4 Ground state electron configuration: square4 the electrons are in the orbitals of lowest possible energy following the Aufbau principle and Hunds rule square4 This is the normal or resting state of an atom or ion square4 Excited state square4 electrons can absorb energy and move into a higher energy orbital; the atom (or ion) will be in an excited state square4 An atom in an excited state will lose energy in the form of light as an electron moves from a higher energy orbital to an available orbital of lower energy 5 6 Some terminology square4 Distinguishing Electron square4 the last electron added to the electron configuration when the configuration is written following the Aufbau principle...
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- Spring '11