Lecture_17_103111 - Lecture 17 Molecular Geometry Goals Use...

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Lecture 17: Molecular Geometry Goals: Use molecular models to help visualize the structure of simple molecules. Outline (Timberlake 5.5, 5.7, 5.8): - Experiment 3: Molecular Geometry - Covalent Compounds (5.5) - Electronegativity and Bond Polarity (5.7) - Shapes and Polarity of Molecules (5.8) Problems for Extra Practice: 5.69, 5.71, 5.73, 5.75, 5.79
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Lewis Structure: Valence Electrons 1s 2 2s 2 2p 2 2s 2 2p 2 6 electrons 4 electrons 4 electrons Electron configuration valence electrons Lewis structure C
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Electron Dot Structures • Atoms are represented by atomic symbols surrounded by valence electrons. • Electron pairs between atoms indicate bond formation. Bonding Pair Lone Pair (6 x) Valence electrons are where the action is… when we write electron dot structures we use valence electron “spackle” to construct molecules. F C F F
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Covalent bonds form • when atoms share electrons to complete octets • between two nonmetal atoms from from Groups 4A(14), 5A(15), 6A(16), and 7A(17) Covalent Bonds
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Learning Check • Draw the Lewis structure for CCl 4
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Single and Multiple Bonds • In a single bond , one pair of electrons is shared. • In a double bond , two pairs of electrons are shared. • In a triple bond , three pairs of electrons are shared. C Cl Cl Cl Cl C Cl Cl Cl Cl O O O O N N N N
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Lewis Structures: Polyatomic Ions • Charge must be considered when determining the total number of electrons – For each positive charge, subtract and electron – For each negative charge, add an electron
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Lewis Structures: Polyatomic Ions • Charge must be considered when determining the total number of electrons – For each positive charge, subtract and electron – For each negative charge, add an electron
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Lecture_17_103111 - Lecture 17 Molecular Geometry Goals Use...

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