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Chemical Bonding
Chapter 6
Molecular Geometry
VSEPR
Valence – Shell, Electron Pair Repulsion
Theory
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.
• Development of bond anglesVisual Concepts
• Electron domains or concentration of electrons repel each other to form shape
• Lone pair geometryVisual Concepts
Vsepr.mov
Memorize!
• Shapes and angles– Linear 180o
– Trigonal planar 120o
– Tetrahedral 109.5o
– Trigonal pyramidal 107.5– Bent 104.5– Trigonal bipyramidal 90o 120o
– Octahedral 90o
Guess the shape!
Hybridization• When atoms come together in a covalent bond,
they overlap orbitals of differing energy creating orbitals of equal energy.
Intermolecular Forces
Polar Molecule • One end negative, one end positive
Dipole• Molecule that has two poles
Different types of intermolecular forces
• Induced dipole• Hydrogen bonding• London dispersion
• Visual Concepts- Induced dipole
• Visual Concepts- London dispersion
Hydrogen Bonding.MOV