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Chapter 8: Covalent Bonding

CHEMISTRY Matter and Change. Chapter 8: Covalent Bonding. Molecular Shapes. SECTION 8.4. Summarize the VSEPR bonding theory. atomic orbital: the region around an atom’s nucleus that defines an electron’s probable location. Predict the shape of, and the bond angles in, a molecule.

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Chapter 8: Covalent Bonding

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  1. CHEMISTRY Matter and Change Chapter 8: Covalent Bonding

  2. Molecular Shapes SECTION8.4 • Summarizethe VSEPR bonding theory. atomic orbital:the region around an atom’s nucleus that defines an electron’s probable location • Predictthe shape of, and the bond angles in, a molecule. • Definehybridization. VSEPR model hybridization The VSEPR model is used to determine molecular shape.

  3. Molecular Shapes SECTION8.4 VSEPR Model: • The premise of VSEPR is that the valence electron pairs surrounding an atom mutually repel each other, and will therefore adopt an arrangement that minimizes this repulsion, thus determining the molecular geometry.  • The shape of a molecule determines many of its physical and chemical properties. • 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 electron pairs around the central atom. • Shape of the molecule determined by : shared and unshared electron pairs around the central atom.

  4. Molecular Shapes SECTION8.4 VSEPR Model(cont.) • Electron pairs repel each other and cause molecules to be in fixed positions relative to each other. The angle formed by two terminal atoms and the central atom is a bond angle • What are the two things that predicted by VESPR? • Unshared electron pairs also determine the shape of a molecule. • Electron pairs are located in a molecule as far apart as they can be.

  5. Molecular Shapes SECTION8.4 Hybridization • Hybridizationis a process in which atomic orbitals mix and form new, identical hybrid orbitals. • Carbon often undergoes hybridization, which forms an sp3 orbital formed from one s orbital and three p orbitals. • Lone pairs also occupy hybrid orbitals.

  6. Molecular Shapes SECTION8.4 Hybridization (cont.) • Single, double, and triple bonds occupy only one hybrid orbital (CO2 with two double bonds forms an sp hybrid orbital).

  7. Molecular Shapes SECTION8.4 Hybridization(cont.)

  8. Molecular Shapes SECTION8.4 Hybridization(cont.)

  9. Molecular Shapes SECTION8.4 Hybridization(cont.)

  10. Section Check SECTION8.4 The two lone pairs of electrons on a water molecule do what to the bond angle between the hydrogen atoms and the oxygen atom? A.They attract the hydrogen atoms and increase the angle greater than 109.5°. B.They occupy more space and squeeze the hydrogen atoms closer together. C.They do no affect the bond angle. D.They create resonance structures with more than one correct angle.

  11. Section Check SECTION8.4 The sp3 hybrid orbital in CH4 has what shape? A.linear B.trigonal planar C.tetrahedral D.octahedral

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