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Chapter 9

Chapter 9. Directions for drawing Lewis Structures: 1. Draw skeleton structure 2. Count valence electrons – add or subtract if charged 3. Deduct 2 electrons for each single bond then distribute remaining electrons to complete octet rule. Molecular Structure. Lewis-Electron Dot Diagram

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Chapter 9

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  1. Chapter 9 Directions for drawing Lewis Structures: 1. Draw skeleton structure 2. Count valence electrons – add or subtract if charged 3. Deduct 2 electrons for each single bond then distribute remaining electrons to complete octet rule Molecular Structure

  2. Lewis-Electron Dot Diagram .. H-N-H H Shared pairs Unshared pairs Electron pair repulsion- electron pairs spread as far apart as possible to minimize repulsive forces.

  3. Hybrid Orbitals carbon sp3 hybrid orbitals Sigma Bonds- 2 orbitals form a bond which lies directly on the bond axis. σ Pi Bond- If 2 p orbitals overlap along an axis in an end-to-end fashion, a sigma bond forms. If 2 p orbitals overlap sideways a pi bond is formed. π ethene Double Bond- 2 pairs of electrons are shared between the bonding atoms

  4. Triple Bond 1 sigma bond 2 pi bonds Multiple bonds are: * less flexible * shorter * stronger Unsaturated / Saturated

  5. Single Bonds: -ane Double Bonds: -ene Triple Bonds: -yne Multiple Bonds Molecular Shape

  6. H2 HCl O3 AlH3 H2CO PFs SeF4 I F3 XeCl2 lCl5 C2H2 L.S. B.A. Shape Polar?

  7. Benzene: C6H6 delocalizedπ electrons results in greater stability ……………………………. Isomers: 2 or more substances with the same molecular formula but different structures Structural Geometric

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