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Intermolecular Forces, Liquids and Solids

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... a fcc structure with 6 atoms in 6 faces, these 6 atoms contribute a net of 3 ... A face centered cubic unit cell has 4 atoms per unit cell ... – PowerPoint PPT presentation

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Title: Intermolecular Forces, Liquids and Solids


1
  • Intermolecular Forces, Liquids and Solids
  • Solids
  • Crystalline solids have an arrangement of ions,
    atoms or molecules that is highly regular and
    form a three dimensional lattice-an orderly
    arrangement of particles that can be reproduced
    by translation in three space.
  • Bulk samples have flat surfaces making definite
    angles with one another.
  • Crystalline solids melt at definite temperatures.
  • Unit cells in crystalline solids
  • The unit cell is the smallest repeating unit that
    can reproduce a lattice by translating the unit
    cell a distance equal to the length of an edge of
    the unit cell.

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  • Intermolecular Forces, Liquids and Solids
  • Crystalline Solids
  • Unit cells in crystalline solids
  • There are 7 basic crystal systems that can define
    14 kinds of unit cells reproducing the
    possible three dimensional lattices.
  • These are the 14 Bravais lattices.
  • The 7 basic crystal systems are shown in Fig.
    13.27, p. 612
  • Three of the lattices have cubic symmetry - see
    Fig. 13.28, p. 613
  • Simple cubic - 1 atom per unit cell atoms in
    contact along edge
  • Body-centered cubic - 2 atoms per unit cell
    atoms in contact along body diagonal
  • The alkali metals are body centered cubic
    (bcc)
  • Face -centered cubic - 4 atoms per unit cell
    atoms in contact along face diagonal
  • Ni, Cu, Al are facecentered cubic (fcc)

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  • Intermolecular Forces, Liquids and Solids
  • Crystalline Solids
  • Calculations involving cubic lattices
  • Atoms at the corners of a cube share their
    volumes with adjacent cubes
  • Eight cubes share the volume of a corner atom
  • If a cubic unit cell has an atom at each corner,
    these 8 corner atoms contribute a net of 1 atom
    to the unit cell
  • For a atom in the face of a cube in a cubic
    structure
  • The atom is shared equally by two cubes
  • For a fcc structure with 6 atoms in 6 faces,
    these 6 atoms contribute a net of 3 atoms to the
    unit cell
  • A simple cubic unit cell has 1 atom per unit cell
  • A face centered cubic unit cell has 4 atoms per
    unit cell
  • A body centered cubic unit cell has 2 atoms per
    unit cell

7
  • Intermolecular Forces, Liquids and Solids
  • Crystalline Solids
  • Atom contacts in cubic unit cells
  • In simple cubic unit cells, the atoms are in
    contact along the cell edge
  • One edge length (EL) contains two atomic radii
  • In face-centered cubic unit cells, the atoms are
    in contact along the face diagonal
  • Using the Pythagorian theorem,
  • For bcc unit cells, the atoms are in contact
    along the body diagnal
  • The Pythagorian theorem must be applied twice

8
  • Intermolecular Forces, Liquids and Solids
  • Crystalline Solids
  • Calculations involving cubic lattices
  • From the cubic unit cell type and edge length,
    the atomic radius may be calculated
  • From the density and the edge length, the cubic
    unit cell type may be determined
  • From the density and unit cell type, the edge
    length may be calculated

9
  • Intermolecular Forces, Liquids and Solids
  • Crystalline Solids
  • Example Cu crystallizes in a fcc unit cell that
    has an edge length of 3.61 Ã…. a. Calculate the
    radius of a Cu atom.

b. Calculate the density of Cu.
10
  • Intermolecular Forces, Liquids and Solids
  • Crystalline Solids
  • CsCl consists of two interpenetrating simple
    cubic lattices - one for Cs and one for Cl-
  • The Cs ion just fits in the octahedral hole in
    the center of the unit cell
  • The corner atoms contribute a net of 1 Cl- ion
  • The center atom is wholly contained in the unit
    cell
  • The structure is consistent with the formula,
    CsCl
  • Perovskite is a mineral of Ca, Ti and O. Its
    formula is
  • 1 Ca2 from the corner atoms
  • 1 Ti from the central Ti atom
  • 6/2 3 Os from the face atoms
  • CaTiO3

11
  • Intermolecular Forces, Liquids and Solids
  • Crystalline Solids
  • Rock salt structure NaCl. See Fig. 13.31, 619
    given on next slide.
  • This structure is 2 interpenetrating FCC
    structures - one each for the Na ions and the
    other for the Cl- ions.
  • The 8 corner Cl- ions contribute 1 net Cl- ions
    to the unit cell
  • the 6 face Cl- ions contribute 3 net Cl- ions to
    the unit cell
  • On each edge is a Na ion, one-fourth belonging
    to the unit cell for a total of 4 Na ions
  • Thus the formula is NaCl
  • MgO also has the rock salt structure - See p. 620

12
Intermolecular Forces, Liquids and Solids Types
of Crystalline Solids
13
  • Intermolecular Forces, Liquids and Solids
  • Phase Diagrams are two or three dimensional plots
    showing conditions under which a particular
    phase (solid, liquid or gas) is stable, the and
    conditions under which phases are in
    equilibrium.
  • In a P-T diagram, areas represent the range of
    pressure and temperature that one of the phases
    of a pure substance is stable.
  • A line in a P-T diagram defines the conditions
    under which equilibrium between two phases
    exists.
  • The line between the solid and liquid shows the
    conditions of pressure and temperature under
    which solid and liquid are in equilibrium.
  • The line between a liquid and gas shows the
    conditions of pressure and temperature under
    which vapor and liquid are in equilibrium.
  • The line between a solid and gas show the
    conditions of pressure and temperature under
    which solid and gas are in equilibrium.
  • A triple point - the intersection of three lines
    - defines the conditions under which
    equilibrium between three phases exits gas,
    liquid and solid are in equilibrium.

14
  • Intermolecular Forces, Liquids and Solids
  • Phase Diagrams
  • The phase diagram of H2O - see Fig. 13.37, p 630.
  • The triple point is at 4.58 torr and 0.01 oC
  • The slope of the solidus line is negative
    indicating that the density of ice is less than
    liquid water.
  • As the pressure increases, the temperature for
    the equilibrium between solid water and liquid
    water decreases as pressure is applied to ice,
    the freezing temperature of ice decreases.
  • The phase diagram of CO2 - see Fig. 13.39, p
    630.
  • The triple point is at 5.11 atm and -56.4 oC.
  • Above 5.11 atm it is possible to have liquid in
    equilibrium with gas and solid in equilibrium
    with liquid.
  • Below 5.11 atm, it is not possible to have liquid
    CO2.
  • At 1 atm, the liquid CO2 cannot exist and an
    equilibrium between gas ad solid exits at a
    temperature of -78.5 oC.
  • The solidus line has a positive slope indicating
    that the solid is more dense than the liquid
    which is the most common behavior of the liquid
    and solid phases of a substance in equilibrium.

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