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Download September 26 - Mr. Searcy Chemistry 20
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September 26 Chemistry 20 Schrodinger’s Equation Aufbau Principle Each electron occupies the lowest energy orbital available. All orbitals related to an energy sublevel are of equal energy. Energy sublevels within a principle energy level have different energies. From low to high, s-p-d-f Orbitals between different principle energy levels may overlap. Pauli exclusion Principle Electrons have specified spins A maximum of two electrons may occupy a single orbital Hund’s Rule Electrons with the same spin must occupy each orbital, before electrons with opposite spins may be added to that orbital. Examples Write the electron configuration for the following elements a) b) c) Ne Mg P Noble-Gas Configuration We can write electron configurations with shorthand. Note that sodium’s electron configuration contains the electron configuration for Neon in it. Sodium: 1s22s22p63s1 Neon: 1s22s22p6 We can write Sodium’s configuration using noble gas configuration. [Ne]3s1 Lewis Diagrams Show the symbol, and the valence electrons Number of valence electrons can be found by looking at the highest level s and p orbitals. Valence electrons are shown as dots, placed on the four sides of the symbol Lewis Diagrams Example: Chlorine Chlorines electron configuration: 1s22s22p63s23p5 Chlorine therefore has 7 valence electrons.
