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Understanding Molecular Shapes and Hybridization in Covalent Compounds

This educational resource explores the VSEPR (Valence Shell Electron Pair Repulsion) theory, which helps predict molecular shapes and bond angles based on electron pair repulsion. Learn how hybridization, a process where atomic orbitals mix to form equivalent hybrid orbitals, contributes to the geometry of molecules. This guide examines how factors like lone pairs and bond types diminish or enhance spatial configurations, ultimately affecting the physical and chemical properties of substances. Perfect for students seeking insight into molecular structure and bonding.

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Understanding Molecular Shapes and Hybridization in Covalent Compounds

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  1. Molecular Shapes Covalent Compounds

  2. Learning Goals • Summarizethe VSEPR bonding theory. • Predictthe shape of, and the bond angles in, a molecule. • Definehybridization.

  3. VSEPR Model • The shape of a molecule determines many of its physical and chemical properties.

  4. VSEPR Model • Molecular geometry (shape) can be determined with the Valence Shell Electron Pair Repulsion model, or VSEPR model which minimizes the repulsion of shared and unshared atoms around the central atom.

  5. VSEPR Model • Electron pairs repel each other and cause molecules to be in fixed positions relative to each other.

  6. VSEPR Model • Unshared electron pairs also determine the shape of a molecule. • Electron pairs are located in a molecule as far apart as they can be.

  7. Hybridization • Hybridizationis a process in which atomic orbitals mix and form new, identical hybrid orbitals.

  8. Hybridization • Carbon often undergoes hybridization, which forms an sp3 orbital formed from one s orbital and three p orbitals. • Lone pairs also occupy hybrid orbitals.

  9. Hybridization • Single, double, and triple bonds occupy only one hybrid orbital (CO2 with two double bonds forms an sp hybrid orbital).

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