Section 1
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Cards (528)
Section 1
(50 cards)
Solute
Substance being dissolved in a solution (lower [ ])
Oxidation is Loss Reduction is Gain
OIL RIG
0
Oxidation # of Compounds
Covalently w/in themselves, Ionicly bonded w/ each other
Polyatomic Ions (bonding)
Monoprotic
Donates a single H+ Ion (... other prefixes also)
+1, except if bonded to Alkali Metal -1
Oxidation # of Hydrogen
p+
proton (symbol)
Atomic Mass Unit
The weighted average of all the isotopes that an atom can have (in g/mol)
Acid + Base --> Salt + Water
Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
precipitate
A solid or gas that can be formed when 2 or more aqueous reactants come together
Bronsted-Lowry Acid
H + donor
Molar Mass of Element/ Total Molar Mass
% Composition Formula
period
Horizontals on the periodic table
Molecule
2 or more covalently bonded atoms
actual yield/theoretical yield x 100%
% yield
End Point
In a titration, the point where the indicator changes (just after moles of solid are equal to moles of base)
Solvent
Substance in which something is dissolved in a solution (higher [ ])
Allotrope
An element with several different forms, each with different properties (i.e. graphite & diamond)
Bronsted-Lowry Base
H+ Acceptor
Ionic Compounds
Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Arrhenius Base
Ionizes to produce OH- Ions
H2, F2, N2, O2, Cl2, Br2, I2
Diatomic Molecules
Molecular
All (though really not all, but for our purposes all) ________ compounds are NOT electrolytes
different # of neutrons
Isotope
Volume Metric Flask & Pipet
Tools NEEDED for dilution
Metalliods
Elements on staircase on periodic table
Ionic
All _________ compounds are electrolytes
n0
neutron (symbol)
Amphoteric
a single substance that may be an acid or a base (i.e. water)
Cation
positive ion
-2, with peroxide -1
Oxidation # of Oxygen
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
How to Find an Empirical Formula Given Percentages
Solution
A homogeneous mixture with 1 phase
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left, Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplying until half reactions are equal 5) Add together & check
How to Balance a Redox Equation
charge
Oxidation # of Polyatomic Ions
Anion
negative ion
1) Convert to moles 2) divide by lowest moles 3) if any halfs, double all values 4) plug into Compound
How to Find an Empirical Formula Given Grams
0
Oxidation # of free elements
# protons (atom is defined by this)
Atomic #
electrolyte
Substance that, when dissolved, is conductive
-1
Oxidation # of Halogens
e-
electron (symbol)
M1V1=M2V2
Formula used when diluting stock solution (to find amount of water or stock needed)
moles of solute/ L of solution
Molarity (M)
charge
Oxidation # of Ions
# protons + # neutrons
Mass #
Molecular Compounds
Compound in which there is a bond between a metal and a non-metal; when naming, pay attention to ionic charges on periodic table (may be reduced)
group
Verticals on the periodic table
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
How to Find a Weighted Average
Arrhenius Acid
Ionizes to produce H+ ions
Section 2
(50 cards)
Oxidizing Agent
The reactant in the reduction reaction that forces the oxidation reaction to occur
Barometer
Instrument used to measure the pressure of atmospheric gas
Endothermic
Absorbs/takes in heat (positive value)
C=(mass)(specific heat)
Heat capacity formula
Open System
Type of system in which the energy and mass may leave or enter
8.314 J/K mol
R in instances that pertain to energy
Thermochemistry
The heat changed in a chemical reaction.
q
Symbol for Total Heat absorbed or released
Calorimeter
A device used to measure Delta H
System
What is defined by you taken from the whole universe
PV=nRT
Ideal Gas Law Formula
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Rate of Diffusion/Effusion formula
Pressure of H2O must be Subtracted
In ideal gas law problem, when it says "atmospheric" ...
AH
Symbol for the heat absorbed or lost molecularly (PER MOLE)
Exothermic
Releases/gives off heat (negative value)
Manometer
Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Reducing Agent
The reactant in the oxidizing reaction that forces the reduction reaction to occur
Temperature
Measure of the average kinetic energy of all the particles in a substance
Force = mass x acceleration
Newton's Second Law
yellow --> green
Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Surroundings
Everything in the universe that is not defined by you as part of the system
rate gas A/rate gas B = square root (mm A/ mm B)
Speed of Diffusion/Effusion formula
Heat Capacity (C)
The amount of energy/heat required to raise some substance 1 degree C
0.0821 atm L/mol K
R in ideal gas law
q H2O = msAT
q H2O = ?
Constant Pressure
Coffee Cup Calorimeter
force x distance = work done
Energy (definition)
high pressure, low temperature
Non-Ideal Gas Conditions
Constant Volume
Bomb Calorimeter
Equivalence Point
In a titration, the point where moles of acid are equal to moles of base (just before the indicator changes color)
P1V1/N1T1=P2V2/N2T2
Combined Gas Law Formula
Closed System
Type of system in which the energy may escape, but the mass is conserved
Average KE = 1/2(mass)(average speed of all particles)
Average Kinetic Energy Formula
Atmospheric Pressure
the weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
P of a =(X of a)(total pressure)
Dalton's Law of Partial Pressures (to find partial pressure formula)
Delta H or Enthalpy Change
Measure of the change in enthalpy
0
If heat capacity isn't mentioned, you can assume that q of cal is = ?
M = square root (3RT/mm)
Kinetic Energy of an individual particle formula
0 degrees C, 1 atm
STP
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
Idea Gas Law (actual rules)
1 atm = 760 mmHg = 101.3 kPa
Pressure Units/Conversions
Specific Heat (s)
The energy required to raise 1 g of substance 1 degree C
Temperature
Kinetic Energy is proportional to ______
q cal = CAT
q cal = ?
q rxn = -(q of H2O + q of cal)
q rxn = ?
purple --> pink
Colors of Reaction when (MnO4 -) --> (Mn2+)
X of a = moles a/total moles
Mole Fraction
Calorimetry
The measurement of heat changes
Isolated System
Type of system in which nothing is transfered (no mass or energy); ideal
H
Symbol for Enthalpy
Section 3
(50 cards)
State Functions
Function in which it doesn't matter HOW the changes take place, only that they do; you can use to formula Final - Initial ( i.e. energy, pressure, volume, temperature, sort of moles)
Positive work value; work done on system
When gas compresses ...
London dispersion forces
larger molecules which have higher mass and therefore electron density have stronger...
+ ∆S
diatomic molecules forming mixed molecules, e.g. H2 + I2 -> 2HI, means...
w =-(P)(Change in V)
work = ?
0
AH of formation for a substance in its stablest form (how it is found in nature)
see-saw
AX4E
AH = q/moles
Delta H (AH) = ?
vapor pressure
stronger IMF= lower... weaker IMF= higher...
∆H | ∆S is spontaneous...at low temperatures
- | -
An = (moles of products that are gasses) - (moles of reactants that are gasses)
Change in moles (An) =?
N=N.(0.5)^time/time half-life
half-life equation
Multiplying
When _____ significant digits, round answer to least significant digit
∆H | ∆S is spontaneous...never
+ | -
square planar
AX4E2
trigonal bipyramidal
AX5
AE = q + w
Change in Energy (AE) = ? (in terms of work)
are not
For significant digits, leading zeros ____ significant
∆H | ∆S is spontaneous...at high temperatures
+ | +
octahedral
AX6
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Dirrect Method Formula
AE= AH - RTAn
Change in Energy = ? (in terms of constant pressure; for gasses)
endless
Significant Digits of counted things
viscosity
thickness
+ ∆S
greater # of moles of gas formed and greater volume formed cause...
are
For significant digits, trailing zeros _____ significant
London dispersion forces
universal IMF for nonpolar molecules
Dipole-dipole forces
IMF that exists in polar molecules
effects of IMF
boiling point, melting point, viscosity, vapor pressure, surface tension
Hydrogen bonding
IMF that occurs with FON
isothermal
change that occurs at constant temperature
T-shape
AX3E2
∆H | ∆S is spontaneous...always
- | +
boiling point
point at which vapor pressure=air pressure above
Adding
When ____ significant digits, round answer to least decimal place
+ ∆S
gas > liquid > solid and (aq)>(s) cause...
∆Hvap
energy needed to vaporize a mole of a liquid
bond energy
energy needed to break a bond
critical point
temperature-pressure point after which gas can no longer form liquid
Negative work value; work done by system
When gas expands ...
triple point
temperature-pressure combination at which solid, liquid, and gas states appear
sublimation
phase change from solid to gas
solid CO2
chemical composition of dry ice
square pyramidal
AX5E
adiabatic
change without heat transfer between the system and its surroundings
equilibrium
happens at lines in phase change charts
deposition
phase change from gas to solid
fusion
melting
endless
Significant Digits of Conversion Factors
methods of increasing rate
raising heat, adding catalyst, heighten concentration, bigger surface area
Section 4
(50 cards)
-ous acid
if anion ends in -ite, acid name ends in...
rate law
this MUST be determined experimentally
g solute/g solvent x 100
mass percent
blue-green
when n=4 ->2, color=
s (fourth quantum number)
variable for spin of electron (+.5 or -.5)
hept-
(organics) seven carbons
violet
when n=6 ->2, color=
p
l=1
non-
(organics) nine carbons
oct-
(organics) eight carbons
Balmer Series
spectrum of light when an electron drops to energy level n=2
4.184
specific heat of water
hex-
(organics) six carbons
but-
(organics) four carbons
prop-
(organics) three carbons
hydro-ic acid
if anion ends in -ide, acid name ends in
f
l=3
eth-
(organics) two carbons
Diffusion
mixing of gases
spontaneous
If K>1, then Gº<0 and reaction will be...at chemical equilibrium
p orbitals
these orbitals are perpendicular
d
l=2
dec-
(organics) ten carbons
Boltzmann distribution
states molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
d orbitals
these orbitals are diagonal
m (third quantum number)
variable for orientation of orbital (-1 through +1)
not spontaneous
If K<1, then Gº>0 and reaction will be...at chemical equilibrium
blue-violet
when n=5 ->2, color=
third
AP doesn't deal with ...-order reaction, don't pick it!
heat capacity
amount of heat needed to change a system by 1˚C
-ic acid
if anion ends in -ate, acid name ends in...
like
like dissolves...
specific heat
heat needed to change 1 g of substance to 1˚C
meth-
(organics) one carbon
zero
[A] vs. time is a ...-order reaction
first
ln[A] vs. time is a ...-order reaction
n (first quantum number)
variable for energy of e-, goes from 1,2,3 on up
C + 273
calculation from K to C
red
when n=3 ->2, color=
Effusion
passage of gas through tiny orifice
s orbitals
these orbitals are spherical
entropy (S)
degree of disorder in a system
moles solute/kg solvent
molality =
increasing
entropy in the universe is always...
l (second quantum number)
variable for type of orbital
second
1/[A] vs. time is a ...-order reaction
ionic
... compounds are most conductive
s
l=0
pent-
(organics) five carbons
electron affinity
energy involved in gaining an electron to become a negative ion
Section 5
(50 cards)
red
color of Li (flame test)
-oic acid
carboxylic acid ending
Ag+, Pb2+, Hg2+, Sr2+, Ca2+, Ba2+
all cations are soluble with sulfate EXCEPT
yellow
color of Na (flame test)
Arrhenius equation
to find activation energy use the...
Alkaline earth metals
Group 2 metals
hydrocarbons
carbon & hydrogen compounds
insoluble
hydroxides are soluble or insoluble?
phosphate, sulfide, carbonate, sulfate
generally insoluble anions (names)
-oate
ester suffix
0
∆Hº of pure elements=
purple
color of K (flame test)
red
color of Sr (flame test)
allotrope
different form of same element
-ol
ending for alcohols
alkane
(organics) single-bonded compound
acid
nonmetal oxide + H2O ->
geometric isomers
two molecules with identical connectivity but different geometries
Alkali metals
Group 1 metals
hydrolysis
organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
blue
color of Cs (flame test)
condensation
organic reaction in which two functional groups come together, resulting in the release of water
Limiting reactant
reactant that's completely used up in a chemical reaction
diamagnetic
elements which have all electrons paired and relatively unaffected by magnetic fields
base
metal oxide + H20 ->
amine
organic w/ -NH2
-one
ketone suffix
ether
organic w/ -O-
carbohydrates
carbon, hydrogen, oxygen compounds
oxide gas and water
oxoacid solution (such as HSO4-) forms...
Ag+, Pb2+, Hg2+
all cations are soluble with bromide, chloride and iodide EXCEPT
Law of Conservation of Mass
mass reactants= mass products
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
equation to find Ea from reaction rate constants at two different temperatures
Transition metals
elements in groups 3-12
red/orange
color of Ca (flame test)
k=Ae^(-Ea/RT)
Arrhenius equation
alkyne
(organics) triple-bonded compound
activated complex (transition state)
peak of energy diagram
complex ions
transition metals with ammonia, hydroxide, cyanide or thiocyanate form...
Law of Multiple Proportions
atoms combine in fixed whole # ratios
paramagnetic
elements which have unpaired electrons and highly affected by magnetic fields
Density
mass/volume
Amino-
amine prefix
alcohol
organic w/ -OH group
base and hydrogen gas
pure metal or metal hydride + H20 ->
mol
6.022x10^23
methoxy-
ether prefix
alkene
(organics) double-bonded compound
-al
aldehyde suffix
green/yellow
color of Ba (flame test)
Section 6
(50 cards)
% error
theoretical yield-experimental yield/theoretical yieldx100
√3kT/m
speed per molecule of gas
Strong acid weak base rxn
H⁺+NH₃→NH₄
end point
point at which the titrated solution changes color
linear
AX₂, AX₂E₃
titrant
buret solution used in titration
oxidizing agent
the reactant that is being reduced, brings about oxidation
Pressure
force per unit area
strong bases
Group 1 and heavier Group 2 bases
Molality
mol/kg of solvent, used in calculating colligative properties
3.0x10⁸m/s
speed of light, C
Theoretical yield
amount of product produced when limiting reactant is used up
1/2mv²
Kinetic Energy per molecule
E
#NAME?
soluble
Group 1, Ammonium, Nitrates, Acetates, Sulfates, Halides
Pauli Exclusion Principle
each orbital can hold two e⁻s each w/ opposite spins
wavelength
determined by the formula h/m(in kg)v, (v=velocity)
indicator
a weak acid that changes color at or near the equivalence point
Molarity
mol/L, concentration of a solution
3/2RT
Kinetic Energy per mol
Aufbau Principle
e⁻s fill the lowest energy orbital first, then work their way up
analyte
solution in flask being titrated
% yield
experimental yield/theoretical yieldx100
√3RT/M(in kg)
average speed of gas
Standard Temperature and Pressure
0.00°C, 1 atm
reduction agent
the reactant that is being oxidized, brings about reduction
tetrahedral
AX₄
strong acids
HCl, HBr, HI, HNO₃, HClO₄, H₂SO₄
strong acid strong base rxn
H⁺+OH⁻→H₂O
weak acid strong base rxn
HF+ OH⁻→H₂O
Graham's Law
effusion of a gas is inversely proportional to the square root of the molar mass
insoluble
Carbonates, Hydroxides, Oxides, Phosphates, Sulfides
standard solution
a solution used in titrations whose concentration is known
6.63x10⁻³⁴Js
Planck's constant, used to calculate energy w/frequency
Heisenberg Uncertainty Principle
we cannot simultaneously determine an atom's exact path or location
oxidation
loss of electrons, increase in oxidation #
mol Fraction
mols A/ total mols, XA
1 atm
760 mmHg, 760 torr
equivalence point
point where acid completely neutralizes base
trigonal planar
AX₃
excess reactant
reactant which doesn't get used up completely in a chemical reaction
lambda
wavelength symbol
22.4L
volume of gas @STP
r₁/r₂
=√M₂/M₁
Dalton's Law
Ptotal=Pa+Pb+Pc....
reduction
gain of electrons, decrease in oxidation #
Hund's Rule
within a sublevel, place one e⁻ per orbital before pairing them
nu
frequency symbol
1.38x10⁻²³J/K
Boltzmann constant, used in calculating speed of gas per molecule
experimental yield
the actual amount of product produced in an experiment
Section 7
(50 cards)
heat of vaporization
energy required for liquid→gas
square pyramidal
AX₅E
trigonal bipyramidal
AX₅
deposition
gas to solid
work
all forms of energy except for heat
ΔTf= kf x molality
freezing point depression formula
condensation
gas to liquid
0.512°C
kb of water
melting
solid to liquid
supercritical fluid
substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
pi=(nRT)/v
osmotic pressure formula
permanent gases
substances w/ critical temperatures below 25°C
boiling point
point at which liquid→gas occurs
surroundings
the rest of the universe (in thermodynamics)
triple bond
1 sigma bond, 2 pi bonds
P₁= X₁P₁°
Raoult's Law, relations between vapor pressure and concentrations
1.86°C
kf of water
cohesion
molecules' tendency to stick to one another
seesaw
AX₄E
single bond
1 sigma bond
Colligative properties
vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure
freezing
liquid to solid
vaporization
liquid to gas
Bond enthalpy
ΔH when 1 mol of bonds is broken in the gaseous state
melting point
point at which solid→liquid occurs
catalyst
lowers activation energy
system
the part of the universe one is focused upon (in thermodynamics)
heat capacity
heat required to raise the system 1°C
adhesion
molecules' tendency to stick to the container
Q<K
forward rxn occurs when
trigonal pyramidal
AX₃E
LeChatelier's Principle
If a system @equilibrium is stressed, the system will shift so as to reestablish equilibrium
square planar
AX₄E₂
Q>K
reverse rxn occurs when
endothermic
positive enthalpy, heat flows into system
Cg=kPg
Henry's Law, solubility of gases is directly proportional to the partial pressure of the gas
rate
how fast or slow a reaction occurs, becomes slower as it reaches equilibrium
Van't Hoff factor
for colligative properties for electrolytes, the # of mols of ions/ mols of solute
exothermic
negative enthalpy, heat flows into surroundings
ΔTb= kb x molality
boiling point elevation formula
activation energy
the minimum energy that molecules must possess for collisions to be effective, Ea
t-shape
AX₃E₂
London dispersion forces
weakest IMFs, found in all molecules
bent
AX₂E, AX₂E₂
double bond
1 sigma bond, 1 pi bond
Hydrogen bonding
unusually strong dipole forces found when H is bonded to N, O, or F
heat of fusion
energy required for melting to occur
viscosity
resistance to flow
sublimation
solid to gas
octahedral
AX₆
Section 8
(50 cards)
nitrate
NO₃¹⁻
chloride
Cl¹⁻
carbonate
CO₃²⁻
no precipitate forms
if Q<Ksp
bromate
BrO₃¹⁻
a precipitate forms
if Q>Ksp
Weight
amount of gravitational force exerted on an object
96,500
Faraday's constant
sulfite
SO₃²⁻
2nd law of thermodynamics
the total entropy is always increasing, all systems tend towards maximum entropy
cyanide
CN¹⁻
ammonium
NH₄¹⁺
Buffer
a solution that resists a change in pH, contains both a weak acid and its conjugate base
1st law of thermodynamics
the total energy of the universe is constant, all systems tend towards minimum energy
chromate
CrO₄²⁻
conjugate acid
the chemical formed when a base accepts a proton
phosphate
PO₄³⁻
chlorate
ClO₃²⁻
3rd law of thermodynamics
the entropy of a pure perfectly formed crystal @0K is 0
Scientific Method
a method of investigation involving observation and theory to test scientific hypotheses
dichromate
Cr₂O₇²⁻
voltaic cells
uses a spontaneous redox rxn to generate electrical energy, consists of 2 half cells
Law of Conservation of Mass
matter can't be created nor destroyed
chlorite
ClO₂¹⁻
acetate
C₂H₃O₂¹⁻
hydroxide
OH¹⁻
sulfate
SO₄²⁻
conjugate base
the chemical formed when an acid donates a proton
iodide
I¹⁻
oxide
O²⁻
Nernst Equation
Ecell= E°cell -RT/nF x lnQ
cathode
half cell in which reduction occurs
sulfide
S²⁻
Arrhenius base
puts OH⁻ into solution
nitrite
NO₂¹⁻
flouride
F¹⁻
Bronsted-Lowry acid
proton donors
Mass
a measure of resistance of an object to a change in its state of motion
anode
half cell in which oxidation occurs
Arrhenius acid
puts H⁺ into solution
permanganate
MnO₄¹⁻
5% rule
x can be ignored when % ionization is <5%
1.0x10⁻¹⁴
Kw
entropy
a measure of randomness or disorder
Bronsted-Lowry base
proton acceptors, must have an unshared pair of e⁻s
Matter
anything occupying space and with mass
perchlorate
ClO₄¹⁻
salt bridge
connects the 2 half cells in a voltaic cell
oxalate
C₂O₄²⁻
spontaneity
the likelihood that a rxn will occur "by itself"
Section 9
(50 cards)
Acids
substances that form H+ when dissolved in water; proton donors
First-Order Rate Law
r=k[A]
A monoatomic cation takes name from
its element
Law of Multiple Proportions
when two elements form a series of compounds, the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Integrated First-Order Rate Law
ln[A]=-kt + ln[A]0
Normality
(N) number of equivalents per liter of solution
R=
0.0826Latm/Kmol
Percent Yield
Actual Yield/Theoretical Yield*100%
R=
8.31J/Kmol
Law of Definite Proportion
a given compound always has exactly the same proportion of elements by mass
Net Ionic Equation
only contains ions that change in reaction
Finding Empirical Formulas
1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary, multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Molality
mol of solute/kg of solvent
Overall Reaction Order
n+m (these are orders of reactants)
Beta Particles-
high-speed electrons
Chemical Kinetics
studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Dalton's Law of Partial Pressures
Ptotal=P1+P2+P3+...
STP
0°C and 1 atm
Second-Order Half Life
1/([A]0*k)
Root Mean Square Velocity
u(rms)=(3RT/M)^1/2
Decrease Volume and Increase Temperature
Increase Pressure
1atm=?mmHg/Torr
760mmHg/Torr
Integrated Zero-Order Rate Law
[A]=-kt + [A]0
In covalent bonds, prefixes are used to tell
amount of atoms present
Alpha Particles-
2+ charge
Molal BP Elevation Constant
▲T=k*m(solute)
Molal FP Depression Constant
▲T=k*m(solute)
Osmotic Pressure
Osmotic pressure=MRT
A monoatomic anion is named by taking
its root and adding -ide
First-Order Half Life
.69/k
Molarity
moles of solute/volume of soln(L)
Zero-Order Half Life
[A]0/2k
1atm=?Pa
101,325 Pa
Gamma Ray-
high-energy light
Ideal Gas Law
PV=nRT
Radioactivity
Spontaneous emission of radiation
Integrated Rate Law
expresses how the concentrations depend on time
Zero-Order Rate Law
r=k
Bases
Substances that form OH- when dissolved in water; proton acceptors
Naming Binary Ionic Compounds
Cation first, anion second
van't Hoff Factor
i=moles of particles/moles of solute dissolved
Enthalpy of Solution
▲Hsoln=▲H1+▲H2+▲H3+...
Isotopes
atoms with the same number of protons but a different number of neutrons
Increase Temperature
Increase Volume
Integrated Second-Order Rate Law
1/[A]=kt + 1/[A]0
Chemical Bonds
Force that holds atoms together
Joule
SI unit of energy; Kg*m^2/s^2
Kinetic Molecular Theory-FOR IDEAL GASES!!!
1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion, which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Second-Order Rate Law
r=k[A]^2
If needed, indicate charge of metal(cation) by
a Roman numeral
Section 10
(50 cards)
Speed of light
c=2.9979*10^8 m/s
Equilibrium constant
K
Q>K
shift to left (Q?K)
Principal Quantum Number
(n) has values 1,2,3,...; tells energy levels
▲Ssurr
-▲H/T
Work
force acting over distance
Heat
the transfer of energy between two objects due to temperature difference
Reaction Quotient
(Q) does the same as equilibrium expression, except it uses initial concentrations
Le Chatelier's Principle
if a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change
Equilibrium Expression
K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Law of Conservation of Energy
energy can't be created nor destroyed
Theory of Relativity
E=mc^2
Buffered Solution
a solution that resists a change in its pH
Hess's Law
in going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
Nodes
where there are no electrons
▲E
q+w
Molar Heat Capacity
J/°Cmol or J/Kmol
Quantum Numbers
describe various properties of one orbital
▲G°
▲H°-T▲S°
Volt
unit of electrical potential; J/C
ℓ=0
s orbital
▲Suniv
▲Ssys+▲Ssurr
Electron Spin Quantum Number
(msubs) can only be +1/2 or -1/2
Q=K
at equilibrium (Q?K)
Galvanic Cell
a device in which chemical energy is changed to electrical energy
Pauli Exclusion Principle
in a given atom no two electrons can have the same set of four quantum numbers
Acid Dissociation Constant
Ka=[products]^m/[reactants]^n
▲H°reaction
Σn▲H°(products)-Σn▲H°(reactants)
Cell Potential
(Ecell) driving force of the electrons
w(max)
=▲G (work)
Solubility Product
(Ksp) an equilibrium expression
ℓ=1
p orbital
Quantum Model
electrons in a hydrogen atom move around the nucleus only in circular orbits
ℓ=4
g orbital
G
G°+RTln(Q)
c=
λv
Hund's Rule
the lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
ℓ=3
f orbital
Entropy
(S) the driving force for a spontaneous is an increase in entropy of the universe
Q<K
shift to right (Q?K)
▲G
▲H-T▲S
Quantum Mechanical Model
involves quantum numbers
pH=
=log[H+]
Cathode
where reduction occurs
Angular Momentum Quantum Number
(ℓ), has values from 0 to (n-1); tells shape of atomic orbitals
Anode
where oxidation occurs
Specific Heat Capacity
J/°Cg or J/Kg
Aufbau Principle
as protons are added to the nucleus, electrons are similarly added
Magnetic Quantum Number
(mℓ) has values from -ℓ to ℓ, including zero; tells orientation of the orbital relative to other orbitals
ℓ=2
d orbital
Section 11
(28 cards)