II. Molecular Geometry (p. 183 – 187)

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Presentation transcript:

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

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

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

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

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

C. Common Molecular Shapes 2 total 2 bond 0 lone BeH2 LINEAR 180°

C. Common Molecular Shapes 3 total 3 bond 0 lone BF3 TRIGONAL PLANAR 120°

C. Common Molecular Shapes 3 total 2 bond 1 lone SO2 BENT <120°

C. Common Molecular Shapes 4 total 4 bond 0 lone CH4 TETRAHEDRAL 109.5°

C. Common Molecular Shapes 4 total 3 bond 1 lone NH3 TRIGONAL PYRAMIDAL 107°

C. Common Molecular Shapes 4 total 2 bond 2 lone H2O BENT 104.5°

C. Common Molecular Shapes 5 total 5 bond 0 lone PCl5 TRIGONAL BIPYRAMIDAL 120°/90°

C. Common Molecular Shapes 6 total 6 bond 0 lone SF6 OCTAHEDRAL 90°

D. Examples F P F F PF3 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107°

D. Examples O C O CO2 2 total 2 bond 0 lone LINEAR 180°