Meeting%2033%20F%202010

Meeting%2033%20F%202010 - Meeting 33 - Chapter 10 Bonding...

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1 Meeting 33 - Chapter 10 Bonding Theory and Molecular Structure We want to answer such questions as: Why CO 2 is linear, while H 2 O is bent? Why are HCCl 3 molecules polar, while CCl 4 molecules are non-polar? Why is there is only one Butane isomer and two isomers of 2-butene? To understand the structure and properties of molecules we will need two theories of bonding. These are Valence-Bond (VB) theory (VB) and Molecular Orbital (MO) theory. We begin by examining the structure of molecules using VSEPR, valence-shell electron-pair repulsion to determine the shapes of molecules.
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2 Shapes of molecules Lewis structures only indicate the connectivity of bonded atoms and account for all the valence electrons. Lewis structures tell us nothing about the shape of the molecule VSEPR will give us information regarding molecular shape. VSEPR assumes that the main determinant of molecular shape is the repulsive force among negatively charged valence shell electrons. It also assumes that valence-shell electron pairs move as far apart as possible.
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3 A third assumption is that lone pairs occupy more space than bonded pairs. Examples of VSEPR: some common shapes of molecules (a nifty use of balloons) :
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4 Also Linear as with CO 2 , which has 2 electron groups about the central C atom. Q: what are the bond angles for the i
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Meeting%2033%20F%202010 - Meeting 33 - Chapter 10 Bonding...

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