Studied by 13 people
combustion/synthesis (9)
2 or more substances combine to form a single substance (A + B → AB)
decomposition (9)
a single reactant is broken down into 2 or more products (AB → A + B)
single replacement/single displacement (9)
a single element replaces a second element in a compound (A + Bx → B + Ax)
double replacement/double displacement (9)
positive ions between 2 reacting compounds exchange places (Ax + By → Ay + Bx)
combustion (9)
an element or a compound reacts with oxygen (X + O2 → ?)
to predict products… (9)
identify the reaction type and use general formula
to convert moles to particles (10)
moles x (6.022 x 10^23) = particles
to convert grams to moles (10)
grams / molar mass = moles
limiting reagent (11)
determines the amount of product that can be found
excess reagent (11)
the reactant that is not completely used up
theoretical yield (11)
100% of expected mass
actual yield (11)
amount of mass actually formed
5 points of kinetic theory (12)
gas is made of particles
all particles move in constant random motion
all collisions are elastic
higher temperature = more energy
larger molecules move slower than smaller ones at the same temperature
unit of temperature (12)
273 Kelvin (K) and 0 Celsius (C)
SI unit for pressure (12)
atm
STP (12)
101.3 kPa or 1 atm & 0 Celsius or 273 Kelvin
absolute zero (12)
point where you have no energy
how is kinetic energy related to temperature? (12)
at higher temperatures there is a wide range of energies, and at lower temperatures the range of kinetic energy is close to the same
how is pressure affected by altitude? (12)
air exerts pressure because of gravity and decreases as you go up in elevation
evaporation (12)
process of turning liquid to vapor (open vessel)
cooling process
vaporization (12)
conversion of a liquid to a gas or vapor
warming process
vapor pressure (12)
force exerted by a gas above a liquid
helps prevent evaporation and boiling
boiling point (12)
the temperature at which a liquid boils
with altitude, boiling point lowers because it needs less kinetic energy
melting point (12)
temperature that a solid turns into a liquid
crystals (12)
solid, orderly, repeating structure
crystal allotropes (12)
carbon = graphite is thin sheets
diamond = tetrahedral shape, rigid compact array
buchminster fullerine = 60 carbon hollow sphere
amorphous solid (12)
solid that does not form crystals
sublimation (12)
changing from a solid to a vapor without changing into a liquid
variables that describe a gas (13)
pressure, volume, temperature, and number of moles
Boyle’s law (13)
(pressure - volume relationship) at constant temperature the volume of a gas varies inversely with pressure
Charles’s law (13)
(temperature - volume relationship) at constant pressure the volume of a gas is directly proportional with temperature
Gay-Lussac’s law (13)
(temperature - pressure relationship) at constant volume pressure is directly proportional to Kelvin temperature of gas
combined gas law (13)
using the three gas la ( ws we are able to see that there is a relationship between pressure, volume, and temperature
hold one of three variables constant
ideal gas law (13)
has 3 of the variables that act on a gas
increase in moles = increase in pressure and volume
Dalton’s law (13)
at constant volume and temperature total pressure exerted by a mixture is equal to the sum of the partial pressures of component gases
Graham’s law of effusion (13)
the rate of effusion of a gas is inversely proportional to the square root of its molar mass
gases of lower molar mass effuse faster
solution (14)
mixture of small particles
solvent (14)
dissolving medium
solute (14)
substance being dissolved
suspension (14)
mixture where the particles will settle out if left undisturbed
mixture (14)
2 or more substances physically combined
colloid (14)
mixture of intermediate sized particles
solubility (14)
amount of solute that can dissolve in a solvent (higher temp = more solubility)
unsaturated (14)
more solute can dissolve in the substance but if more is added it disappears
saturated (14)
no more solute can dissolve but if more is added will sink to the bottom
supersaturated (14)
special situation where solvent holds more solute than it should and requires a series of steps to create
Henry’s law (14)
solubility 1/pressure 1 = solubility 2/pressure 2
electrolytes in solution (14)
(ionic compounds) number of particles is based on the number of separate ions a compound dissolves apart into
nonelectrolytes in solution (14)
(covalent compounds) number of particles per compound and always equal to 1
boiling point eleration (14)
boiling point of a solvent increases when a solute is dissolved in it
freezing point depression (14)
freezing point of a solvent decreases when a solute is dissolved in it
heat (15)
energy that flows from one object to another
Hess’s law (15)
most reactions occur in a series of steps
endothermic (15)
a reaction that absorbs energy and feels cold
equation: A + B + heat → C + D or A + B → C + D AH = +
exothermic (15)
a reaction that releases energy and feels warm
equation: A + B → C + D + heat or A + B → C + D AH = -
heat capacity (15)
the amount of heat required to change the temperature of a given amount of matter by 1 degree
specific heat (15)
the amount of energy required to raise 1 gram of a substance by 1 degree C
spontaneous reactions (15)
free energy (15)
maximum amount of energy that can be used to do useful work
relationship between directly proportional and inversely proportional (13)
inversely proportional has one that goes up and goes down and directly proportional has either both go up or both go down
how to differentiate between colloid and suspension (14)
suspension has multiple phases and colloids have one
colloid uses the tyndall effect and suspension does not
what is conserved in a reaction (11)
mass and particles
spontaneous process (15)
any chemical of physical change that, once begun, occurs with not outside intervention
2 things that determine spontaneous processes (15)
entropy - measure of disorder in a system
enthalpy - the heat of a system when it is under constant pressure
convert moles to volume (10)
1 mol = 22.4 L
5 things that affect the rate of solution (14)
agitation, temperature, surface area, pressure, and saturation
reaction (15)
deltaH rxn
formation (15)
deltaH f degrees = 0
fusion (15)
heat required to melt 1 mol of a substance
solution (15)
deltaH when dissolved
combustion (15)
deltaH of reaction where combustion occurs
Note 
Flashcard (43)