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IIIIII II. Molecular Geometry (p. 183 – 187) Ch. 6 – Molecular Structure

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A. VSEPR Theory n Valence Shell Electron Pair Repulsion Theory n Electron pairs orient themselves in order to minimize repulsive forces.

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A. VSEPR Theory n Types of e - Pairs Bonding pairs - form bonds Lone pairs - nonbonding e - Lone pairs repel more strongly than bonding pairs!!!

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A. VSEPR Theory n Lone pairs reduce the bond angle between atoms. Bond Angle

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n Draw the Lewis Diagram. n Tally up e - pairs on central atom. double/triple bonds = ONE pair n Shape is determined by the # of bonding pairs and lone pairs. Know the 8 common shapes & their bond angles! B. Determining Molecular Shape

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C. Common Molecular Shapes 2 total 2 bond 0 lone LINEAR 180° BeH 2

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3 total 3 bond 0 lone TRIGONAL PLANAR 120° BF 3 C. Common Molecular Shapes

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3 total 2 bond 1 lone BENT <120° SO 2

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4 total 4 bond 0 lone TETRAHEDRAL 109.5° CH 4 C. Common Molecular Shapes

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4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° NH 3 C. Common Molecular Shapes

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4 total 2 bond 2 lone BENT 104.5° H2OH2O C. Common Molecular Shapes

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5 total 5 bond 0 lone TRIGONAL BIPYRAMIDAL 120°/90° PCl 5 C. Common Molecular Shapes

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6 total 6 bond 0 lone OCTAHEDRAL 90° SF 6 C. Common Molecular Shapes

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n PF 3 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° F P F F D. Examples

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n CO 2 O C O 2 total 2 bond 0 lone LINEAR 180° D. Examples

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IIIIII I. Lewis Diagrams Molecular Structure. A. Octet Rule n Remember… Most atoms form bonds in order to have 8 valence electrons.

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