159_fall_07_chapt_10_supplement

159_fall_07_chapt_10_supplement - Chapter 10 The Shapes of...

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Ch 10 1 Chapter 10 The Shapes of Molecules
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Ch 10 2 The Shapes of Molecules 10.1 Depicting Molecules and Ions with Lewis Structures 10.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory and Molecular Shape 10.3 Molecular Shape and Molecular Polarity
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Ch 10 3 Drawing Lewis Structure Step 1- Place the atoms relative to each other. Place the atom with lower group number in the center (lower EN). If the group number is the same, place the atom with the higher period number in the center. H can never be a central atom Step 2 - Determine the total number of valence e’s available Step 3 - Draw a single bond from each surrounding atom to the central atom and subtract two valence electrons for each bond Step 4 - Distribute the remaining e’s in pairs so that each atom ends up with 8 e’s (or 2 for H). First place lone pairs on the surrounding more electronegative atoms to give each an octet. If any e’s remain, place them around the central atom. Then check that each one has 8e’s Step 5 : If after Step 4, a central atom still does not have an octet, make a multiple bond by changing a lone pair from one of the surrounding atoms into a bonding pair to the central atom EXCEPTIONS Incomplete Octets Be 4 electrons, B 5 electrons Odd-Electron Molecules Ex/ Expanded Octets – starting with the end of third period NO O .. .. .. .. : .
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Ch 10 4 Step 1- Place the atoms relative to each other F F N F Step 2 – Det the total no of valence e’s N = 5 e’s and 3xF = 3x7=21 e’s, total 26 e’s Step 3 – Draw a single bond from each surrounding atom to the central atom and subtract two electrons for each bond F F N F 26 e’s – 6 e’s = 20 e’s Step 4 – Distribute the remaining electrons in pairs so that each atom ends up with 8 e’s (or 2 for H atom).
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159_fall_07_chapt_10_supplement - Chapter 10 The Shapes of...

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