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Explore the Valence-Shell Electron-Repulsion Theory in chemistry, which explains how molecular shapes adjust to keep valence-electron pairs apart. Learn about the nine possible molecular shapes with examples like methane, ammonia, water, and carbon dioxide. Test your knowledge with the 8.3 Section Quiz on molecular orbital, VSEPR theory, and orbital hybridization. Enhance your understanding of molecular bonding and shape prediction. Dive into the fascinating world of molecular geometry!
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Chemistry 8.3 8.3
8.3 VSEPR Theory • VSEPR Theory: The Valence-Shell Electron-Repulsion Theory states that molecular shapes adjust in order for valence-electron pairs to stay as far apart as possible.
8.3 VSEPR Theory • Nine Possible Molecular Shapes: (You will be tested over the first five!)
8.3 VSEPR Theory • Example: Methane Tetrahedral Angle
8.3 VSEPR Theory • Example: Ammonia has one unshared electron Pair. Pyramidal
VSEPR Theory • Example: Water (H2O) has 2 unshared pairs. Bent
VSEPR Theory • Example: Carbon Dioxide – Carbon has no unshared pairs. Linear (180̊)
VSEPR Theory • Example: 3 bonding pairs and 0 unshared pairs. Trigonal Planar
8.3 Section Quiz. • 8.3.
8.3 Section Quiz. • 1. A molecular orbital belongs to a • specific atom. • molecule as a whole. • specific pair of atoms. • central atom.
8.3 Section Quiz. • 2. VSEPR theory enables prediction of 3-dimensional molecular shape because the valence electron pairs • are attracted to each other. • form molecules with only four possible shapes. • stay as far apart as possible. • always form tetrahedral shapes.
8.3 Section Quiz. • 3. Orbital hybridization provides information about • both molecular bonding and molecular shape. • both molecular bonding and bond energy. • neither molecular bonding nor molecular shape. • neither molecular bonding nor bond energy.
