1. Chemical Bonding Chapter 6

2. Molecular Geometry VSEPR Valence – Shell, Electron Pair Repulsion Theory

3. VSEPR How a molecule “looks” in real space (3D). Based upon electron domains (where electrons are) –Bonds are domains (doubles/triples count as one) –Unshared electron pairs are domains –Electron domains repel each other –Unshared pairs repel more than bonding pairs –Domains orient themselves as far away from each other as possible.

4. Development of bond angles Visual Concepts Electron domains or concentration of electrons repel each other to form shape Lone pair geometry Visual Concepts

7. Memorize! Shapes and angles –Linear 180 o –Trigonal planar 120 o –Tetrahedral 109.5 o –Trigonal pyramidal 107.5 –Bent 104.5 –Trigonal bipyramidal 90 o 120 o –Octahedral 90 o

8. Guess the shape!

9. Hybridization When atoms come together in a covalent bond, they overlap orbitals of differing energy creating orbitals of equal energy.

10. Intermolecular Forces

11. Polar Molecule One end negative, one end positive Dipole Molecule that has two poles

13. Different types of intermolecular forces Induced dipole Hydrogen bonding London dispersion Visual Concepts- Induced dipoleVisual Concepts Visual Concepts-Visual Concepts London dispersion