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Lewis Structures and Metallic Bonding

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Lewis Structures and Metallic Bonding Powered By Docstoc
					Tuesday 10/19/10
   Return Naming Compounds Quiz
   Collect Symbol Me Projects
   Lewis structures
   Metallic Bonding
   Hydrogen Bonding
   Jeopardy Review
   Atoms form bonds to gain a full shell of
    valence electrons. (Octet Rule)
   If electrons are not involved in bonding, then
    they are lone pairs.
   Each bond is made up of 2 electrons.
   Count up the total # of valence electrons.
     If it’s an ion, then add or subtract e- as
    needed.
   Connect all the atoms with single bonds.
   Place the remaining electrons as lone pairs
    around the atom.
   Create double or triple bonds if there are not
    enough electrons to go around.
   ALWAYS FOLLOW THE OCTET RULE!!!!
   Draw the Lewis structure for NO3-
   Draw the Lewis structure for CCl3+
   Draw the Lewis structure for CO2
   Draw the Lewis structure for N2O4
   Draw the Lewis structure for C2N24-
   Draw the Lewis structures for PO43-
   Draw the Lewis structure for OCN-
   http://www.youtube.com/watch?v=lkl5cbfqF
    RM&feature=related\

   http://www.youtube.com/watch?v=LGwyBeu
    VjhU

				
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posted:8/10/2012
language:English
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