Chem

• Matter


  Anything that occupies space and has mass
• Light and sound are NOT examples of matter
• Solid


  • Particle distance very close
  • Molecular arrangement regular
  • Shape well defined
  • Mass definite
  • Volume definite
  • Speed slowest
  • Intermolecular force of attraction very strong
  • Density high
  • Compressibility incompressible
• Liquid


  • Particle distance less close
  • Molecular arrangement irregular
  • Shape of the container
  • Mass definite
  • Volume definite
  • Speed fast
  • Intermolecular force of attraction less strong
  • Density moderate
  • Compressibility almost incompressible
• Gas


  • Particle distance far
  • Molecular arrangement irregular
  • No shape
  • Mass definite
  • Volume indefinite
  • Speed fastest
  • Intermolecular force of attraction weak
  • Density low
  • Compressibility highly incompressible
• Kinetic molecular theory

  Matter is made of particles that are constantly in motion
• Kinetic energy


  Directly proportional to temperature
• Liquid particles

  Have more kinetic energy since they can freely flow, molecules are so close together that there is very little empty space
• Amount of space in between particles


  Related to the substance's state of matter
• Solid particles


  • Very limited spaces in between particles
• Phase changes


  Happen when the temperature of the substance changes sufficiently
• Solid


  • Rigid position, long-range order, almost incompressible, possesses a definite shape and volume
• Liquid


  • Molecules so close together that there is very little empty space, molecules can move past one another freely
• Endothermic


  Absorption of heat (melting, evaporation, and sublimation)
• Exothermic


  Release/removal of heat (freezing, condensation, and deposition)
• London dispersion forces


  Weakest intermolecular force, temporary attractive force due to the formation of temporary dipoles in a nonpolar molecule
• Dipole-dipole forces


  Attractive forces between polar molecules, the partial negative side of one molecule is attracted to the partial positive side of another molecule, the larger the dipole moment, the stronger the attraction
• Hydrogen bond

  A special type of dipole-dipole interaction between the hydrogen atom in a polar bond
• Ion-dipole


  Electrostatic interactions between the fixed dipole in one molecule and an ion
• Surface tension


  The tendency of fluid surfaces to shrink into the minimum surface area possible, directly proportional to the intermolecular force of attraction, inversely proportional to temperature
• Viscosity


  Resistance of fluids to flow, directly proportional to intermolecular force of attraction, inversely proportional to temperature
• Vapor pressure


  Pressure exerted by a vapor with its condensed phases (solid or liquid) in a closed system at a given temperature, inversely proportional to intermolecular force of attraction
• Boiling point


  The temperature at which liquid vapor pressure equals atmospheric pressure, inversely proportional to intermolecular force of attraction
• Molar heat of vaporization


  Total amount of heat required to turn a particular amount of liquid into vapor without any rise in the temperature of the fluid, directly proportional to intermolecular force of attraction
• Water has high boiling point and exists as liquid in room temperature
• Water has high specific heat which requires large amount of heat to vaporize
• Water is the only substance that contracts when cooled, ice is less dense than liquid water thus it floats
• Water has high heat of vaporization, this causes a large drop in temperature
• Water has high surface tension, this allows water to move from roots to the top of tall tree
• CRYSTALLINE SOLIDS - arranged in fixed geometric patterns or lattices. The ordered arrangement of their units maximizes the space they occupy and are essentially incompressible. Often exhibit anisotropic properties.
• AMORPHOUS SOLIDS - have a random orientation of particles. Super-cooled liquids where molecules are arranged in a random manner. Do not have long-range order. Generally exhibit isotropic properties.
• CRYSTAL LATTICES - the regular repeating structure of a crystalline solid. UNIT CELL - the smallest subunit of a crystal lattice that can be repeated over and over to make the entire crystal. CRYSTALLIZATION - disordered state (usually a liquid or gas) to a highly ordered state (a solid with a welldefined and repeating crystal lattice structure). VITRIFICATION - the constituent particles (atoms, molecules, or ions) of the liquid are cooled so quickly that they do not have enough time to form a crystalline structure. As a result, the material solidifies into an amorphous solid.
• PHASE CHANGES - transformations of matter from one physical state to another.

  • transformations of matter from one physical state to another
• PHASE DIAGRAM - graphical representation of the physical states of a substance under different conditions of temperature and pressure.
• MELTING/FREEZING CURVE - The curve on the phase diagram which represents the transition between liquid and solid states. VAPORIZATION/CONDENSATION CURVE - The curve on the phase diagram which represents the transition between gaseous and liquid states. SUBLIMATION/DEPOSITION CURVE – the curve on a phase diagram which represents the transition between gaseous and solid states. TRIPLE POINT - the point on a phase diagram at which the three states of matter coexist.
• CRITICAL POINT- temperature and pressure above which a gas cannot be condensed into a liquid. SUPERCRITICAL FLUID - substance at a temperature and pressure higher than its critical point; exhibits properties intermediate between those of gaseous and liquid states
• CONCENTRATION - is the measure of how much of a given substance is mixed with another substance. CONCENTRATED SOLUTION - is one in which there is a large amount of solute in a given amount of solvent. DILUTE SOLUTION - is one in which there is a small amount of solute in a given amount of solvent. SOLUTE - A substance that is dissolved in a solution. SOLVENT - Dissolves Solute. SOLUTIONS – homogeneous mixtures. It may be solids dissolved in liquids or gases dissolved in liquids
• Fill in the blank.

  A) Triple point

  B) critical point

  C) gas

  D) liquid

  E) solid

  F) temperature

  G) pressure