Chemistry Unit 6

• Temperature


  Measure of kinetic energy of atoms/molecules in a substance.
• Heat


  Kinetic energy transferred from one object to another.
• Kinetic Energy


  - Energy that comes from motion

  - Formula: KE-1/2mv2
• Solid


  -Particles packed tightly together + vibrating

  -Low entropy (randomness of movement)

  -definite/well defined shape and volume

  -low energy
• Liquid


  -Particles packed closely but can still pass through (think school hallways)

  -Medium entropy (randomness of motion)

  -impressible

  -definite/well defined volume

  -indefinite shape

  -medium energy
• Gas


  -Particles are very far away from each other

  -High entropy (randomness)

  -compressible

  -Don't touch each other, if they do they bounce off each other

  -Indefinite shape and volume

  -High energy
• Plasma


  -All the same qualities of gas, but their is enough energy that e's get stripped off.

  -high entropy (randomness)

  -Very high energy --> particles ionize
• Inside a florescent light-bulb (when on), the flame portion of a fire, lighting, a grape cut mostly in half in a microwave...


  Examples of Plasma
• States of matter


  solid, liquid, gas and plasma
• Matter


  Anything that has mass and takes up space; 'stuff
• intramolecular forces


  forces within molecules. Forces caused by the attraction and repulsion of charged particles/ hold molecules together within a molecule (Ionic bonds-metals+nonmetals, covalent bond-sharing of electrons, metallic bonding)
• intermolecular forces


  forces of attraction between molecules (LDF, dipole-dipole interactions, hydrogen bonding).
• Polarizability


  the tendency of an electron cloud to distort
• More molar mass and more electrons means...

  increased polarizability
• Temperature vs Heat


  Heat is energy transferred from a hotter system to a cooler system while temp is measure of average KE of substances.
• Kinetic Molecular Theory


  -Gas particles are in constant motion and exhibit perfectly elastic collisions (no loss in KE)

  -How Gassous materials behave
• Electrons consitantly moving around, when more dense in one area it causes...

  Temporary dipoles
• Melting


  solid to liquid
• Freezing


  liquid to solid
• Evaporating


  Liquid to gas
• Vaporization


  Liquid to gas (Slower than boiling)
• Condensing


  Gas to liquid
• Sublimination


  solid to gas
• Deposition


  gas to solid
• The higher the mass/boiling point/surface area...

  highest London dispersion forces
• Entropy


  Randomness of Particles
• Triple points


  A substance is the temperature and pressure conditions at which the substance can exist in equilibrium as a solid, liquid, or gas
• Boiling


  Liquid to gas (rapid compared to evaporation at boiling point)
• Density


  mass/volume- how much "stuff" is in a given volume
• Ideal Gas


  a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory (KMT)

  -has no volume

  -no forces between particles

  -collide perfectly elastically (No loss in KE or velocity)
• Latent heat of fusion


  heat released by freezing
• Latent heat of vaporization


  heat required to vaporize
• Conduction


  Heat transfer by touch
• Convection


  Heat transfer through water or gas
• Radiation


  When waves are absorbed, reflected, or transmitted.
• Ionization


  the process of adding or removing electrons from an atom or molecule, which gives the atom or molecule a net charge; taking valence electrons of an atom

  *Gas to plasma
• Deionization


  Removal of ions from a solution, return of valence electrons to atom

  *changing from plasma state to a gas
• Critical point


  the temperature and pressure at which the gas and liquid states of a substance become identical and form one phase
• If an object has high temp the particles have a ______ KE


  High (hotter objects have higher KE and temp; cooler objects have lower KE and temp).
• Energy Transfer Rules


  Heat always goes from whatever is hot into whats cold