Pure Substance
A substance with a uniform and constant composition
Element
pure substance composed of only one type of atom
Compound
pure substance made of two or more different elements that are chemically combined in a fixed ratio
Mixture
2 or more pure substances that are physically combined in varying proportions and can be separated physically
Homogeneous mixture
A mixture in which substances are evenly distributed throughout the mixture
heterogeneous mixture
A mixture where the components are not evenly distributed throughout the mixture.
Aqueous solution
When a substance is completely dissolved in water.
Melting point
The temperature at which a solid becomes a liquid
Boiling point
The temperature at which a liquid changes to a gas
STP
standard temperature and pressure
Standard temperature
273K or 0C
Standard Pressure
101.3 kPa or 1 atm
Gas
A state of matter with no definite shape or volume.
Kilopascal (kpa)
Unit of measuring pressure.
Erlenmeyer flask
contain liquids, may be heated, good for swirling, commonly used in titrations
beaker
contain liquids, may be heated
well plate/spot plate
contain small amounts of liquids and solids, observe microscale reactions
graduated cylinders
measure liquid volume, various sizes
test tubes
contain liquids and solids
watch glass
cover beaker or evaporating dish to prevent splattering, sometimes used evaporate solutions.
funnel
transfer and filter solutions
stirring rod
stir solutions; transfer precipitates
dropper pipet or disposable pipet
transfer liquids
mortar and pestle
used grind or pulverize solids
Bunsen burner
heat source
ring stand
support equipment and glassware
ring (iron ring)
support equipment and glassware
crucible tongs
transfer crucibles (and hot glassware)
thermometer
measure temperature
test tube brushes
clean glassware
test tube rack
hold test tubes
spatulas (scoopulas)
transfer solids
burets
measure liquid volume, accurate to the 100th mL, commonly used in titration
hot plate or electric burner
heat source
test tube holder
hold test tubes (held by person)
beaker tongs
hold beaker
goggles
must be worn in lab to protect eyes from splashes
filter paper
special paper used to separate solids from liquids, placed in a funnel
electronic balance (scale)
used to measure mass
Atmospheric pressure
air pressure
Vapor pressure
pressure created from particle collisions on the side of a container
Boiling point (gases unit)
When vapor pressure equals atmospheric temperature.
Kinetic Molecular Theory
Small, hard spheres.
Particle size does not matter compared to distance between particles.
Particles move in random, straight motions.
There are no intermolecular forces between particles.
When particles collide, they transfer energy and bounce apart.
Ideal gas
A gas where all assumptions of the KMT are true. (high temperature & low pressure)
Phase equilibrium
different phases occurring at the same rate.
Intermolecular forces
Forces of attraction between molecules.
Potential energy
Stored energy
Kinetic energy
energy in motion
Thermal energy
random motion of particles
enthalpy
The amount of heat that is released/absorbed.
exothermic
Heat is released
Enthalpy decreases
surrounding environment becomes warmer
endothermic
Heat is absorbed
Enthalpy increases
surrounding environment becomes colder
Entropy
the measure of disorder of a system. (randomness of the system)
Deposition
phase change from a gas to solid
Sublimation
phase change from a solid to gas
Enthalpy
Another term for heat or energy.
Entropy
The randomness or disorder of a system.
Potential energy
Stored energy
Kinetic energy
Energy in motion
Heat
The type of energy that flows from one substance to another due to their temperature differences.
Vaporization
Phase change from liquid to gas.
Condensation
Phase change from gas to liquid.
Heat of Fusion
The amount of heat needed to melt 1 gram of a solid.
Heat of Vaporization
The amount of heat needed to vaporize 1 gram of a liquid.
Specific Heat Capacity
The amount of heat needed to change a substance of 1 gram by 1 degree celsius.
Temperature
Average kinetic energy.
Democritus
Atomos
Dalton
Hard Sphere Model
JJ Thomson
Chocolate Chip Cookie Model or Plum Pudding Model
Rutherford
Nuclear Model
Bohr
Planetary Model
Heisenberg
Quantum Model or Wave Mechanical Model
Charge of Proton
+1
Mass of Proton
1 atomic mass unit
Location of Proton
Nucleus
Charge of neutron
0
Mass of neutron
1 atomic mass unit
Location of neutron
Nucleus
Charge of electron
-1
Mass of electron
1/2000 or 0 amu
Location of electron
orbitals
Charge of Nucleus
Positive
Charge of Atom
0
Atomic #
Intensive property
Does not depend on the amount of mass
Extensive Property
Depends on the amount of mass present in sample