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