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• What are the two main types of solids?

  Crystalline solid and Amorphous solid
• What are the types of crystalline solids?


  • Ionic solids
  • Molecular solids
  • Covalent network solids
  • Metallic solids
• What is an example of a molecular crystalline solid?


  H2O
• What type of attraction holds ionic solids together?


  Electrostatic attractions
• What is an example of an ionic solid?


  NaCl
• What is the structure of metallic solids described as?


  Sea of electrons
• What is an example of a network covalent solid?


  SiO2
• What are the properties of ionic compounds?


  • Strong bonds leading to high melting points
  • Good conductors of electricity and heat only in solution or molten
  • Conductivity occurs through the motion of charged particles
• What defines a giant covalent structure?


  • Atoms bonded by covalent bonds
  • Continuous network extending throughout the material
  • Examples: SiO2 and Diamond
• What are the three different forms of carbon allotropes?


  Amorphous (coal), Crystalline (graphite and diamond)
• What hybridization is present in graphite?


  Sp2 hybridized Carbon
• Why does graphite have a slippery feel?


  Due to delocalized electrons flowing between aligned p orbitals
• What hybridization is present in diamond?


  Sp3 hybridized Carbon
• What is the conductivity of diamond?


  Poor conductor
• What are the properties of metallic bonds?


  • Conduct heat and electricity
  • Malleable and ductile
  • High melting and boiling points
• What characterizes molecular solids?


  • Made of only non-metals
  • Distinct individually-bonded molecules
  • Attracted by weak intermolecular forces
  • Generally low melting and boiling points
• How are molecules arranged in a molecular solid?


  In a 3D lattice structure
• What are the three main types of intermolecular forces (IMF)?


  1. London Dispersion Forces (weakest)
  2. Dipole-dipole attraction (intermediate)
  3. Hydrogen Bond (strongest)
• What is a hydrogen bond?


  Attraction between hydrogen on one molecule and F, N, or O of another molecule
• What are dipole-dipole interactions?


  Interactions present between polar molecules
• What is a dipole-induced dipole interaction?


  Attractive forces between polar and nonpolar molecules
• What are ion-dipole interactions?


  Interactions present between ions and polar molecules
• How do ion-dipole interactions occur in solution?


  Water dipoles interact with ions, causing them to separate
• What causes London Dispersion Forces (LDF)?


  Temporary dipoles caused by movement of electrons in the molecule

  
• Why can LDF be strong in large molecules?


  They increase with the contact area and polarizability of the molecule
• What are the properties of liquids?

  • Surface tension
  • Capillary action
  • Viscosity
  • Vapor pressure
• What is surface tension in liquids?


  The resistance to an increase in surface area due to cohesive forces
• What is capillary action?


  The spontaneous rising of a liquid in a narrow tube
• What is viscosity?


  The resistance of flow in a liquid
• What is vapor pressure?


  The pressure exerted by the vapor over the liquid at equilibrium
• How does intermolecular force affect vapor pressure?


  Higher IMF leads to lower vapor pressure
• What is the boiling point of a liquid?


  The constant temperature when added energy is used to vaporize the liquid
• What is the relationship between vapor pressure and atmospheric pressure at boiling point?


  Vapor pressure of liquid equals the pressure of surrounding atmosphere
• higher molar mass = stronger IMF = lowers vapor pressure
• like dissolves like

  P and P, Np and NP
• base reacts with acid