CHEM-TO-GO LESSON 9: ORBITAL DIAGRAMS CONVERSATION STARTER Materials: 1)Orbital diagram video notes and color-coded periodic table 2)Clean sheet of paper for additional diagrams 3)Pencil

Practice of Electron Configuration Write the full electron configuration and noble gas notation for the following: 1)Boron 2)Nickel 3)Strontium 4)Iodine 5)Barium 6)Platinum Illustrate your understanding of the concept by answering the following questions about each: 1)Number of electrons 2)Number of energy levels 3)Number of valence electrons

Collaborative Application Students will apply knowledge in a predictable situation. Important information about an atom’s electrons: 1)Number of electrons 2)Number of energy levels 3)Number of valence electrons 4)Number of unpaired electrons 5)Number of empty sublevels on an energy level 6)Number of empty orbitals in a sublevel

Collaborative Application Five Minute Practice: Draw the orbital diagrams for the following elements: Chlorine and Titanium Five Minute Practice: Who’s rule is broken in these diagrams? )Number of electrons 2)Number of energy levels 3)Number of valence electrons 4)Number of unpaired electrons 5)Number of empty sublevels on an energy level 6)Number of empty orbitals in a sublevel

Assimilation of Knowledge KEY IDEA: Two groups of elements on the periodic table BREAK aufbau’s principle regularly to achieve a more stable configuration. Who are these rebels?  Chromium family  Copper family Why?  Full orbitals = STABLE  ½ Full orbitals = ~ stable  Empty orbitals = UNstable