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Types of Solids

Types of Solids. Chap. 13: Day 4b. Metallic and Ionic Solids Sections 13.6-8. Properties of Solids. 1. Molecules, atoms or ions locked into a CRYSTAL LATTICE 2. Particles are CLOSE together 3. STRONG IM forces 4. Highly ordered, rigid, incompressible. ZnS, zinc sulfide.

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Types of Solids

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  1. Types of Solids Chap. 13: Day 4b

  2. Metallic and Ionic SolidsSections 13.6-8

  3. Properties of Solids 1. Molecules, atoms or ions locked into a CRYSTAL LATTICE 2. Particles are CLOSE together 3. STRONG IM forces 4. Highly ordered, rigid, incompressible ZnS, zinc sulfide

  4. Types of SolidsTable 13.6 TYPE FORCE Properties . Ionic Ionic Hard, brittle, High MP poor conductor Metallic Electrostatic Malleable, Range of MP good conductor Molecular Dipole Soft, Low of MP Ind. Dipole poor conductor Network Extended Range of MP & hardness covalent poor conductor

  5. Network Solids Diamond Graphite

  6. Network Solids A comparison of diamond (pure carbon) with silicon.

  7. Atom Packing in Unit Cells Assume atoms are hard spheres and that crystals are built by PACKING of these spheres as efficiently as possible.

  8. PROPERTIES OF LIQUIDS Chap. 13: Day 4a

  9. Intermolecular Forces • The forces BETWEEN molecules. Holds the molecules together. At a set temperature: • What phase has the strongest force? • Solids • What phase has the weakest forces? • Gases (vapor)

  10. Viscosity • the resistance of a fluid to flow Thick fluids have high viscosity

  11. Liquid Properties • Surface Tension- Abilityofliquid molecules to hold on to each other. • Apparent “skin” affect • Ex. Over filling a liquid in a glass with out the liquid spilling

  12. Hg

  13. Liquid Properties • Capillary Rise- the tendency of a liquid to rise in a small diameter tube due to the surface tension of the liquid.

  14. Vapor Pressure • The pressure exerted by a vapor in equilibrium with its liquid state. • The pressure at which liquid changes to vapor • Liquids with high vapor pressures turn into vapors very easily. (Volatile) Ex. Gasoline, perfume

  15. Once equilibrium is reached, the vapor particles will begin to condense back to a liquid

  16. Boiling Point • The temperature at which the vapor pressure of the liquid equals the atmospheric pressure • The entire liquid is changing state, not just the surface. • Water boils at 1000C at standard P

  17. Vapor Pressure vs Temperature

  18. PHASE CHANGES: TWO ways to change PHASE • Temperature Pressure

  19. Almeltingpoints SOLID LIQUID

  20. Boiling points: Liquid to Vapor LIQUID GAS Water

  21. Phase Diagrams

  22. TRANSITIONS BETWEEN PHASESSection 13.10 Lines connect all conditions of T and P where EQUILIBRIUM exists between the phases on either side of the line. (At equilibrium particles move from liquid to gas as fast as they move from gas to liquid, for example.)

  23. Phase Equilibria — Water Gas-Liquid Solid-liquid Gas-Solid

  24. Triple Point — Water At the TRIPLE POINTall three phases are in equilibrium.

  25. Phases Diagrams—Important Points for Water T(˚C) P(mmHg) Normal boil point 100 760 Normal freeze point 0 760 Triple point 0.0098 4.58

  26. Critical T and P As P and T increase, you finally reach the CRITICAL T and P Above critical T no liquid exists no matter how high the pressure.

  27. Critical T and P Tc(oC) Pc(atm) M (g/mol) H2O 374 218 (18) P Freon-12 112 41 (121) NP (CCl2F2) CO2 31 73 (44) NP CH4 -82 46 (16) NP Notice that Tc and Pc depend on intermolecular forces.

  28. Phase Diagram for Water

  29. Solid-Liquid Equilibria Raising the pressure at constant T causes water to melt. The NEGATIVE SLOPE of the S/L line is unique to H2O. Almost everything else has positive slope.

  30. STRONGForces lead to…. Nonvolatile Substances Highboiling points Low evaporation rates Lowvapor P at room temperature WEAK Forces lead to.. Volatile substances Low boiling points High evaporation rates High vapor P at room temperature INTERMOLECULAR FORCES

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