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Modern Chemistry Chapter 6 Chemical Bonding

Modern Chemistry Chapter 6 Chemical Bonding. Sections 1-5 Introduction to Chemical Bonding Covalent Bonding & Molecular Compounds Ionic Bonding & Ionic Compounds Metallic Bonding Molecular Geometry. Chapter Vocabulary. VSEPR theory Hybridization Hybrid orbitals Dipole Hydrogen bonding

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Modern Chemistry Chapter 6 Chemical Bonding

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  1. Modern ChemistryChapter 6Chemical Bonding Sections 1-5 Introduction to Chemical Bonding Covalent Bonding & Molecular Compounds Ionic Bonding & Ionic Compounds Metallic Bonding Molecular Geometry Chapter 6 Section 5 Molecular Geometry pages 197-207

  2. Chapter Vocabulary VSEPR theory Hybridization Hybrid orbitals Dipole Hydrogen bonding London dispersion forces Chapter 6 Section 5 Molecular Geometry pages 197-207

  3. Section 5 Molecular Geometry Chapter 6 Section 5 Molecular Geometry pages 197-207

  4. VSEPR Theory • Valence-Shell Electron-Pair Repulsion • Repulsions between the set of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible. Chapter 6 Section 5 Molecular Geometry pages 197-207

  5. VSPRE & Molecular Geometry p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  6. Geometry & Lone Pairs Chapter 6 Section 5 Molecular Geometry pages 197-207

  7. Molecular Geometry LINEAR Example formula: BeF2 Type of molecule: AB2 Bond angle: 180° Shared pairs on the central atom: 2 Unshared pairs on the central atom: 0 : : :F - Be - F: : : Chapter 6 Section 5 Molecular Geometry pages 197-207

  8. : F: : : :F : Molecular Geometry TRIGONAL PLANAR Example formula: BF3 Type of molecule: AB3 Bond angle: 120° Shared pairs on the central atom: 3 Unshared pairs on the central atom: 0 B :F: : Chapter 6 Section 5 Molecular Geometry pages 197-207

  9. Molecular Geometry H TETRAHEDRAL Example formula: CH4 Type of molecule: AB4 Bond angle: 109.5° Shared pairs on the central atom: 4 Unshared pairs on the central atom: 0 C H H H Chapter 6 Section 5 Molecular Geometry pages 197-207

  10. Molecular Geometry : O : ANGULAR Example formula: H2O Type of molecule: AB2E2 Bond angle: 105° Shared pairs on the central atom: 2 Unshared pairs on the central atom: 2 H H Chapter 6 Section 5 Molecular Geometry pages 197-207

  11. Molecular Geometry : N TRIGONAL PYRAMIDAL Example formula: NH3 Type of molecule: AB3E Bond angle: 107° Shared pairs on the central atom: 3 Unshared pairs on the central atom: 1 H H H Chapter 6 Section 5 Molecular Geometry pages 197-207

  12. Molecular Geometry • Unshared pairs occupies more space around the central atom than shared pairs • Unshared pairs repel other electrons more strongly than shared pairs • Multiple bonds are treated the same as single bonds • Polyatomic ions are treated like molecules. Chapter 6 Section 5 Molecular Geometry pages 197-207

  13. Molecular Geometry • Try • CO2 • ClO31- • Practice Problems page 201 • Try • CF4 • NO3 1- Chapter 6 Section 5 Molecular Geometry pages 197-207

  14. Hybridization • The mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energy • Example CH4 C = ____ 1s 2s 2p ____ 1s sp3 Chapter 6 Section 5 Molecular Geometry pages 197-207

  15. Hybridization • s and p orbitals have different shapes • The 2s & 2p hybridize to make four identical orbitals • named sp3 • The 3 is from the three p orbitals used • But the 1 is not written for the s Chapter 6 Section 5 Molecular Geometry pages 197-207

  16. Hybridization • All sp3 orbitals have the same energy • Higher than 2s but • Lower than 2p • Hybrid orbitals – orbitals of equal energy produced by the combination of two or more orbitals. Chapter 6 Section 5 Molecular Geometry pages 197-207

  17. Hybridization N = ___ 1s 2s 2p ___ 1s sp3 O = __ 1s 2s 2p __ 1s sp3 Chapter 6 Section 5 Molecular Geometry pages 197-207

  18. Uses one p orbital Uses two p orbitals Hybridization Be =  1s 2s ____ 1s sp B = _____ 1s 2s 2p _____ 1s sp2 Chapter 6 Section 5 Molecular Geometry pages 197-207

  19. Hybridization p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  20. Hybrid Orbital Animation p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  21. Comparing Molecular & Ionic Compounds p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  22. Molecule Polarity δ+ δ- • Dipole: created by equal but opposite charges that are separated by a short distance H - Cl 2.1 3.0 Lower EN Higher EN polar bond = dipole Chapter 6 Section 5 Molecular Geometry pages 197-207

  23. Molecule Polarity • Molecule polarity for compounds with more than one bond depends on … bond polarityand molecule geometry. Chapter 6 Section 5 Molecular Geometry pages 197-207

  24. : N H H H Molecule Polarity • Draw the Lewis Structure true to shape. Example NH3 Chapter 6 Section 5 Molecular Geometry pages 197-207

  25. Molecule Polarity • Find all the partial positive and negatives for each atom in the molecule δ- 3.0 : N 2.1 H H H δ+ δ+ δ+ Look at each bond. High EN = δ- Low EN = δ+ Chapter 6 Section 5 Molecular Geometry pages 197-207

  26. Molecule Polarity • Look at around the “outside” of the molecule. δ- : N H H H δ+ δ+ δ+ • All the same δ = NP; Different δ = P Chapter 6 Section 5 Molecular Geometry pages 197-207

  27. H C H H H Molecule Polarity • Draw the Lewis Structure true to shape. Example CH4 Chapter 6 Section 5 Molecular Geometry pages 197-207

  28. H C H H H Molecule Polarity • Find all the partial positive and negatives for each atom in the molecule δ+ 2.1 2.5 δ- 2.1 δ+ δ+ 2.1 2.1 δ+ High EN = δ- Low EN = δ+ Look at each bond. Chapter 6 Section 5 Molecular Geometry pages 197-207

  29. H C H H H Molecule Polarity • Look at around the “outside” of the molecule. δ+ δ- δ+ δ+ δ+ • All the same δ = NP; Different δ = P • Carbon is not on the “outside”. Chapter 6 Section 5 Molecular Geometry pages 197-207

  30. Intermolecular Forces • The force of attraction between molecules to make (solids or) liquids • Boiling point is a good measure of the strength of intermolecular forces • Weaker than covalent bonds, ionic bonds and metallic bonds Chapter 6 Section 5 Molecular Geometry pages 197-207

  31. δ+ δ+ δ- δ- H - Cl H - Cl Molecule Polarity Dipole-dipole force: the force of attraction between polar molecules Chapter 6 Section 5 Molecular Geometry pages 197-207

  32. Dipole Dipole Animation p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  33. Comparing Dipole Dipole Forces p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  34. Hydrogen Bonding • H-F, H-O or H-N bonds have a large electronegativity difference • These bonds are very polar. • Molecules with these bonds have very strong dipole-dipole forces Chapter 6 Section 5 Molecular Geometry pages 197-207

  35. Hydrogen Bonding p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  36. Hydrogen Bonding • The intermolecular force in which a Hydrogen atom that is bonded toNitrogen or Oxygen or Fluorineis attracted to an unshared pair of electronsof the N, O or F of another molecule Chapter 6 Section 5 Molecular Geometry pages 197-207

  37. Hydrogen Bonding • Compare PH3 & NH3H2O & H2S Page 204 Chapter 6 Section 5 Molecular Geometry pages 197-207

  38. Dipole Induced Dipole p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  39. Induced Dipole • Polar molecules cause a dipole in a nonpolar molecule H δ+ δ+ δ- : : : O O O δ- : : : H δ+ Chapter 6 Section 5 Molecular Geometry pages 197-207

  40. London Dispersion Forces • Nonpolar molecules don’t have dipoles • However at any instance the electron distribution may be uneven. • An instantaneous dipole can occur and induce dipoles in other molecules Chapter 6 Section 5 Molecular Geometry pages 197-207

  41. London Dispersion Force p. xx Chapter 6 Section 5 Molecular Geometry pages 197-207

  42. London Dispersion Forces • London dispersion forces – the intermolecular attraction resulting from the constant motion of electrons and the creation of instantaneous dipoles • Very weak intermolecular forces • London forces increase with increasing atomic or molar mass. Chapter 6 Section 5 Molecular Geometry pages 197-207

  43. Lewis Structures Practice • C2H4 • BeF2 • AsH3 • IBr • CHCl3 • CN 1- • N2O2 Chapter 6 Section 5 Molecular Geometry pages 197-207

  44. Lewis Structures Practice • C2Cl4 • SCl2 • AsF5 • CI2Cl2 • BF3 • NO 1- • CH2O • IO31- Chapter 6 Section 5 Molecular Geometry pages 197-207

  45. Section 5 Homework Chapter 6 Section 5 Worksheet Chapter 6 Section 5 Molecular Geometry pages 197-207

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