Solids

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Calculate DHo, DGo, DSo for N2O5 H2O HNO3
Cpd N2O5 H2O HNO3 DHfo -11.3
-285.8 -174.1 DGfo -10.4 -237.2
-151.5
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AP Chm HW

• Problems 7 9
• Page 268

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Solids
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Molecular Solids

• Covalently bound molecules held together by
  intermolecular forces

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Molecular Solids

• Non-conductors
• Insoluble in water mostly
• Low MP BP
• Held by intermolecular F

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Intermolecular Forces

• Instantaneous weak forces that hold one molecule
  to another or to another part of itself

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Intermolecular Forces

• H-bond
• Dipole-dipole
• Dipole-induced dipole
• London dispersion

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Network Molecular Solids

• Bound by a continuous network of covalent bonds
• High MP, insoluble, non-conductor

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Ionic Solids

• Ions or ionic compounds held together by
  electrostatic charge
• Fattraction Kq1q2/d2

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Ionic Solids

• Non-conductors as solids
• Conductors in solution
• Soluble in water mostly
• Very high MP BP
• Brittle

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Metallic Solids

• Conductors, insoluble in water mostly, high MP
  BP, held by gravitational type force
• Fattraction Gm1m2/d2

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Crystal

• Solid
• Any substance that has a well defined crystal
  structure

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Crystal Lattice

• The three dimensional arrangement of unit cells
  in a crystal structure

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Unit Cell

• The smallest repeating unit that a crystal
  structure can be divided into

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Drill

• Describe unit cells crystal lattice

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Crystal Structures

• Cubic Monoclinic
• Tetragonal Triclinic
• Orthorhombic
• Hexagonal Rhombohedral

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Cubic

• All angles 90o
• All sides are
• All faces are squares

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Tetragonal

• All angles 90o
• 2 side sets are , third ?
• 1 set of opposing squares
• 2 sets opposing rectangles

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Orthorhombic

• All angles 90o
• all 3 side sets are ?
• 3 unequal sets opposing rectangles

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Hexagonal

• All angles 90o or 120o
• 1 set of opposing hexagons
• 3 sets opposing rectangles

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Monoclinic

• 2 sets of angles 90o
• third set ?90o
• 1 set of opposing parallel
• 2 sets opposing rectangles

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Triclinic

• No angles 90o
• 3 unequal sets of opposing parallelograms

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Rhombohedral

• No angles 90o
• All sides
• 3 sets of opposing congruent rhombuses

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Simple Cube

• Unit cell with one atom at each vertex
• 1 atom/cell

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Body Centered Cube

• BCC
• Unit cell with one atom at each vertex one atom
  in the center of the cube
• 2 atoms/cell

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Face Centered Cube

• FCC or CCP
• Unit cell with one atom at each vertex one atom
  on each face of the cube
• 4 atoms/cell

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• The density of iron in its normal state of BCC is
  7.86 g/mL.
• Calculate its density in the FCC state

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Drill

• List describe the 7 crystal structures

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Hydrated Crystal

• A solid with water in the crystal
• CuSO45H2O

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Anhydrous Solid

• A crystal without water

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Hygroscopic

• Crystals that absorb moisture from the air

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Deliquescent

• Crystals that absorb enough moisture from the air
  to liquify

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Efflorescent

• Crystals that give up water to the surroundings

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Polymorphous

• When a single substance can have multiple crystal
  structures

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Isomorphous

• When different substances have the same crystal
  structure

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Amorphous Solid

• A solid w/o a well defined crystal structure
• Super-cooled liquid

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Liquid Crystals

• Part solid part liquid
• Has a well defined crystal structure in 1 or 2
  but not all 3 dimensions

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Smectic

• Liquid crystal that have a well defined crystal
  structure in 2 dimensions

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Nematic

• Liquid crystals that have a well defined crystal
  structure in only 1 dimension

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Liquid

• A substance that holds together loosely, but has
  no structure in any dimension

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Solid

• Definite size shape
• Particles vibrate about fixed points

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Liquid

• Definite size but no shape
• Particles vibrate about moving points

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Gas

• No definite size or shape
• Particles move at random

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Drill

• Name describe each of the 7 crystal structures

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Melting Point

• Temperature at which the solid phase liquid
  phase are at equilibrium
• MP FP are equal

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Melting Point

• Temperature at which the vapor pressure of a
  solid the vapor pressure of its liquid phase

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Boiling Point

• Temperature at which the liquid phase gaseous
  phase are at equilibrium

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Boiling Point

• Temperature at which the vapor pressure of a
  liquid the vapor pressure of its gaseous phase
  or atmospheric P

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Adhesion

• The attraction of particles from different
  substances to each other

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Cohesion

• The attraction of particles of the same substance
  towards each other

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Capillarity

• The movement of a liquid up a thin tube due to
  adhesion cohesion

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Surface Tension

• Pressure on the surface of a liquid caused by the
  uneven forces acting on the surface molecules

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Vapor Pressure

• The pressure caused by the evaporated particles
  in the vapor above a liquid

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Intermolecular Forces

• Weak temporary attractions between atoms from one
  molecule to another or another part of a larger
  molecule

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Intermolecular Forces

• Hydrogen-bond
• Dipole-dipole
• Dipole-induced dipole
• London dispersion forces

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Hydrogen Bond

• Strongest of the intermolecular forces
• Occurs when H is bound to one highly EN element
  connects to another

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Dipole-Dipole

• When two polar molecules connect

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Dipole-Induced Dipole

• When a polar molecule gets near a non-polar one,
  it induces the non-polar one to become polar
  thus, they connect

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London Dispersion

• Instantaneous attraction for fractions of seconds
  in which non-polar molecules connect
• Very weak force

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Predict explain the MP trends of1) Li,
Na, K, Rb2) F2, Cl2, Br2, I2 3) LiF, NaCl,
KBr, RbI
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Phase Diagram

• Graphic representation of all the phases of a
  substance with respect to temperature pressure

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Approximate MP BP
1 atm
100 K
400 K
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Phase Diagrams
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Describe conditions at each number
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AP Chm HW

• Problems
• 27, 51, 53
• Pages 269 270

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Define solids, liquids, gases, melting Boiling
points
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Determine the phase changes for the 3 arrows
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