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Chapter 1 & 2 Review Sheets (Part I)

# Chapter 1 & 2 Review Sheets (Part I) - Lewis Dot...

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O C N H S Cl Br I F B Si Number of bonds typically made for selected atoms P Lewis Dot Structures Note: Bonds can also be double and triple in some cases H H O H H O Step 1 Step 2 Step 4 H H H H C H H H H C Step 3 H H O H H H H C Step 5 H H C C O Cl H H H C C O Cl H H H C C O Cl H 8=8 8=8 24=24 8 electrons 8 electrons 24 electrons # of atoms # atoms × valence # total 2 Hydrogens 2 × 1 2 1 Oxygen 1 × 6 6 8 # of atoms # atoms × valence # total 4 Hydrogens 4 × 1 4 1 Carbon 1 × 4 4 8 # of atoms # atoms × valence # total 3 Hydrogens 5 × 1 3 2 Carbons 2 × 4 8 1 Oxygen 1 × 6 6 1 Chlorine 1 × 7 7 24 Method Step 1 : Draw a “molecular skeleton” and connect all of the atoms by single bonds Step 2 : Identify the atomic group of each atom, for example carbon is a group IV atom and chlorine is a group VII atom. The atomic group is also the number of valence electrons that each atom has, therefore carbon has 4 and chlorine has 7 etc. Step 3 : Fill in all other valence electrons for all atoms in addition to the bonding electrons already added. First fill in lone pairs then add radicals for the moment. Step 4 : Determine weather the octet rule is satisfied for all of the atoms, remember hydrogen only needs two electrons to complete a 1s orbital. Add electrons to bonds where they will satisfy the octet rule by combining the radials you have written in step 3.

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