1 / 28

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.

robbin
Télécharger la présentation

Types of Solids

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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. Crystal Lattices • Regular 3-D arrangements of equivalent LATTICE POINTS in space. • Lattice points define UNIT CELLS • smallest repeating internal unit that has the symmetry characteristic of the solid.

  9. Cubic Unit Cells of MetalsFigure 13.24 Simple cubic (SC) Body-centered cubic (BCC) Face-centered cubic (FCC)

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

  11. 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)

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

  13. 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

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

  15. 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

  16. Vapor Pressure vs Temperature

  17. 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

  18. Hg

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

  20. 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

More Related