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CHAPTER 4.6

CHAPTER 4.6. Nature of SOLIDS. Bonding in Solids. Physical properties of a solid depend on: kind of particle they are composed from. the attractive forces found between the particles  intermolecular/ intramolecular

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CHAPTER 4.6

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  1. CHAPTER 4.6 Nature of SOLIDS

  2. Bonding in Solids • Physical properties of a solid depend on: • kind of particle they are composed from. • the attractive forces found between the particles intermolecular/intramolecular • distance between particles held by intramolecular forces is always smaller/stronger than intermolecular forces

  3. PLACEMAT ACTIVITY - instructions • You will work in groups of 2 or 4 individuals. • Each group will collect a big chart paper and 2 or 4 markers. • You will divide the chart paper into 4 equal sized blocks. • Each member will pick one of the following topics and complete a graphic organizer shown on the next slide: • Molecular solids Covalent solids • Ionic solids Metallic solids • After completing the placemat, pair with another group and compare your info with them.

  4. PLACEMAT FORMAT

  5. Bonding in Solids • There are four types of solid: • Molecular (formed from atoms or molecules) - usually soft with low melting points and poor conductivity. • Covalent network (formed from atoms) - very hard with very high melting points and poor conductivity. • Ionic (formed from ions) - hard, brittle, high melting points and poor conductivity. • Metallic (formed from metal atoms) - soft or hard, high melting points, good conductivity, malleable and ductile.

  6. Bonding in Solids • 1) Molecular Solids • Intermolecular forces: dipole-dipole (HCl, SO2), London dispersion (He, CH4) and H-bonds (H2O, HF); range of properties depends on bonding!

  7. Bonding in Solids • 1) Molecular Solids • Intermolecular forces: dipole-dipole (HCl, SO2), London dispersion (He, CH4) and H-bonds (H2O, HF); range of properties depends on bonding!

  8. Bonding in Solids • 1) Molecular Solids • Intermolecular forces: dipole-dipole (HCl, SO2), London dispersion (He, CH4) and H-bonds (H2O, HF); range of properties depends on bonding!

  9. Bonding in Solids • 1) Molecular Solids • Intermolecular forces: dipole-dipole (HCl, SO2), London dispersion (He, CH4) and H-bonds (H2O, HF); range of properties depends on bonding!

  10. Bonding in Solids • 1) Molecular Solids • Intermolecular forces: dipole-dipole (HCl, SO2), London dispersion (He, CH4) and H-bonds (H2O, HF); range of properties depends on bonding!

  11. Bonding in Solids • 2) Covalent Network Solids • Atoms held together in large networks of covalent bonds. • Examples: diamond, graphite, quartz (SiO2), silicon carbide (SiC), and boron nitride (BN).

  12. Bonding in Solids • 2) Covalent Network Solids • Atoms held together in large networks of covalent bonds. • Examples: diamond, graphite, quartz (SiO2), silicon carbide (SiC), and boron nitride (BN).

  13. Bonding in Solids • 2) Covalent Network Solids • Atoms held together in large networks of covalent bonds. • Examples: diamond, graphite, quartz (SiO2), silicon carbide (SiC), and boron nitride (BN).

  14. Bonding in Solids • 2) Covalent Network Solids • Atoms held together in large networks of covalent bonds. • Examples: diamond, graphite, quartz (SiO2), silicon carbide (SiC), and boron nitride (BN).

  15. Bonding in Solids • 2) Covalent Network Solids • Atoms held together in large networks of covalent bonds. • Examples: diamond, graphite, quartz (SiO2), silicon carbide (SiC), and boron nitride (BN).

  16. Bonding in Solids • 2) Covalent Network Solids • Atoms held together in large networks of covalent bonds. • Examples: diamond, graphite, quartz (SiO2), silicon carbide (SiC), and boron nitride (BN).

  17. Bonding in Solids • 2) Covalent Network Solids • Atoms held together in large networks of covalent bonds. • Examples: diamond, graphite, quartz (SiO2), silicon carbide (SiC), and boron nitride (BN).

  18. Bonding in Solids • 2) Covalent Network Solids • Carbon as diamond and graphite… • In diamond: • each C atom is covalently bonded to four other carbons; • each C atom is tetrahedral (sp3 orbitals); • there is a three-dimensional array of atoms. • PROPERTIES • hard • high melting point (3550 °C) • non-conducting

  19. Bonding in Solids Covalent Network Solids

  20. Bonding in Solids • Covalent Network Solids • In graphite • each C atom is in a layer and covalently bonded to 3 other carbons (sp2 hybrid orbitals) in a planar hexagonal ring; • layers of interconnected rings are placed on top of each other; • the distance between layers is large (3.41 Å vs 1.42 Å between covalently bonded carbons); • layers are held together by van der Waal’s forces and overlap of p orbitals forming “pi” bonds • one valence electron per C is still available; • electrons move in delocalized orbitals (good conductor).

  21. Bonding in Solids • Covalent Network Solids • In graphite • PROPERTIES • soft • high melting point • conducting (since electrons move in delocalized orbitals)

  22. Bonding in Solids • 3) Ionic Solids • Ions (spherical) held together by electrostatic forces of attraction:

  23. Bonding in Solids • 3) Ionic Solids • Ions (spherical) held together by electrostatic forces of attraction:

  24. Bonding in Solids • 3) Ionic Solids • Ions (spherical) held together by electrostatic forces of attraction:

  25. Bonding in Solids • 3) Ionic Solids • Ions (spherical) held together by electrostatic forces of attraction:

  26. Bonding in Solids • 3) Ionic Solids • Ions (spherical) held together by electrostatic forces of attraction:

  27. Bonding in Solids • 3) Ionic Solids • Ions (spherical) held together by electrostatic forces of attraction:

  28. Bonding in Solids • 3) Ionic Solids • Ions (spherical) held together by electrostatic forces of attraction:

  29. Bonding in Solids Ionic Solids

  30. Bonding in Solids • 4) Metallic Solids • Problem: the bonding is too strong for London dispersion and there are not enough electrons for covalent bonds. • Resolution: the metal nuclei float in a sea of electrons  metallic bonds

  31. Bonding in Solids Metallic Solids

  32. Bonding in Solids 4) Metallic Solids

  33. Bonding in Solids 4) Metallic Solids

  34. Bonding in Solids 4) Metallic Solids

  35. Bonding in Solids 4) Metallic Solids

  36. Bonding in Solids 4) Metallic Solids

  37. Bonding in Solids 4) Metallic Solids

  38. Bonding in Solids 4) Metallic Solids

  39. Bonding in Solids 4) Metallic Solids

  40. Bonding in Solids 4) Metallic Solids

  41. Bonding in Solids • 5) Amorphous Solids • solids whose particles are not arranged in a definite pattern • e.g. glass • consists of long molecules that are tangled and disorganized • these molecules are unable to untangle to form a crystal structure

  42. Bonding in Solids Summary

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