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Liquids, Solids

liquids - properties explained by intermolecular forces

  • viscosity - resistance of a liquid to flow
    • measured by timing to see how long it takes an amount of liquid to flow through a tube
    • poise (P) - unit of viscosity, g/cm-s
    • lower temperature, larger molecular weight >> lower viscosity
  • surface tension - energy needed to increase surface area by a certain amount
    • cohesion - forces that bind similar molecules to each other
    • adhesion - forces that bind substance to a surface
  • capillary action - rise of liquids up narrow tubes
    • used by plants to move water/nutrients upwards
    • adhesion between liquid and tube increases surface area

solid structures - either crystalline or noncrystalline (amorphous)

  • crystalline solid - molecules arranged in well-defined arrangements
    • have flat surfaces, definite angles, regular shapes
    • brings particles in closest contact >> maximizes attractive forces
    • unit cells - repeating unit of a crystalline solid
    • crystal lattice - 3D array of points representing the crystal
    • primitive cubic - unit cell where lattice points at corners only
    • centered cubic - additional lattice point at center of cell
    • face-centered cubic - additional lattice points at center of each face
  • packing of spheres - each sphere surrounded by 6 others in each layer
    • spheres rest in depressions of surrounding layers
    • hexagonal close packing - 3rd layer repeats the 1st, 4th layer repeats the 2nd
    • cubic close packing - 4th layer repeats the 1st
    • coordination number - number of particles immediately surrounding 1 particle on all sides
  • amorphous solid - no orderly structure, usually made of large complicated substances

bonding in solids - arrangement of particles determines melting point, hardness, etc

  • molecular solids - have molecules/atoms held together by intermolecular forces
    • soft, low melting points
  • covalent-network solids - atoms held together in large networks by covalent bonds
    • much stronger than molecular solids, w/ higher melting points
  • ionic solids - ions held together by ionic bonds
    • strength depends on charges of ions
    • charges/relative sizes determine structure of solid
  • metallic solids - made entirely of metal atoms
    • each atom has 8 or 12 surrounding atoms
    • valence electrons delocalized throughout entire solid
    • mobility of electrons promotes conductivity
Subject: 
Chemistry
Subject X2: 
Chemistry

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