Mcat Chemistry Equation Sheet Page 2
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ACID-BASE EQUILIBRIA
Chemical Reaction: some bonds break, and new
ln
2
=
[A] = 0.5[A]
,
t
bonds form
0
1
2 /
k
S
F
:
TATE
UNCTION
S
-O
R
E
:
A property that depends only on the state of the
A
A
:
ECOND
RDER
ATE
XPRESSION
RRHENIUS
CID
2
Rate = k[A]
, this can be converted to
system
Anything that produces hydrogen ions in aqueous
P
F
:
solution
ATH
UNCTION
1
1
−
=
kt
Arrhenius Base:
A property that depends on how a change takes
[A]
[A]
place
Anything that produces hydroxide ions in aqueous
0
Molar Heat Capacity:
solution
B
:
IMOLECULAR ELEMENTARY REACTION
A + B → products
The amount of heat needed to raise the temperature
B
-L
A
:
RØNSTED
OWRY
CID
Elementary rate = k[A][B]
of 1 mol of substance by 1 Kelvin (1K)
A species that donates a proton is an acid
U
:
NIMOLECULAR ELEMENTARY REACTION
B
-L
B
:
C → products
W
(
):
RØNSTED
OWRY
ASE
Elementary rate = k[C]
ORK
W
A species that accepts a proton is a base
Energy used to move an object against an opposing
F
S
R
-D
:
IRST
TEP IS
ATE
ETERMINING
Amphiprotic Species: a chemical species that can
force, w= Fd
The predicted rate law for the overall reaction is the
both donate and accept protons
F
L
T
:
rate expression for that first step
IRST
AW OF
HERMODYNAMICS
∆
Lewis Acid:
A
E
(E
):
E
= q
+ w
CTIVATION
NERGY
sys
sys
sys
A
Anything that accepts a pair of electrons
Energy barrier, the minimum energy that must be
Exothermic Process:
Lewis Base:
supplied before the reaction can occur
If the chemicals release heat, this heat gain raises
Anything that donates a pair of electrons
Activated Complex: the molecular arrangement at
the temperature of the surroundings
W
E
C
(K
):
ATER
QUILIBRIUM
ONSTANT
the point of highest energy along the energy level
E
P
:
W
NDOTHERMIC
ROCESS
−
−14
+
K
= [H
O
][OH
] = 1.00×10
(at 298 K)
diagram
If the chemicals absorb heat, this heat loss lowers
w
3
S
A
:
TRONG
CIDS
the temperature of the surroundings
Acids that donate protons to water molecules
∆T, q = nC
∆
q
= C
T
CHEMICAL EQUILIBRIUM
calorimeter
cal
quantitatively
E
:
NTHALPY
Strong Base:
A thermodynamic quantity whose change equals the
A substance that generates hydroxide ions
heat flow at constant pressure,
E
C
:
QUILIBRIUM
ONSTANT
quantitatively in aqueous solution.
∆H = ∆E + ∆(PV)
[ ] [ ]
d
e
H S
:
D
E
P
CALES
eq
eq
=
o
−
∆
S
E
F
:
pH = −log[H
] pOH = −log[OH
= −log K
K
+
TANDARD
NTHALPY OF
ORMATION
H
O
] pK
[ ] [ ]
eq
f
3
a
a
a
b
A
B
= −log K
pK
pH + pOH = 14.00 K
K
= K
pK
+
eq
eq
Enthalpy change accompanying the formation of
b
b
a
b
w
a
pK
= 14.00
one mole of a chemical substance from pure
K
applied only at equilibrium, K
is independent of
b
eq
eq
elements in their most stable forms under standard
W
A
:
initial conditions, K
is related to the stoichiometry.
EAK
CID
eq
conditions
Acid that reaches equilibrium when only a small
P
L
S
:
URE
IQUID AND
OLID
H
’ L
:
ESS
AW
fraction of its molecules transfer protons to water
The concentrations of pure liquids or solids are
The enthalpy change for any overall process is
W
B
:
EAK
ASE
always equal to their standard concentrations,
equal to the sum of enthalpy changes for any set of
Generates hydroxide ions by accepting protons from
therefore division by standard concentration results
steps that leads from the reactants to the products
water but reaches equilibrium when only a fraction
in a value of 1
M
H
S
:
of its molecules have done so
OLAR
EAT OF
OLUTION
L
K
:
ARGE
EQ
Measures net energy flow that occurs as substance
A
A
E
:
PPLICATIONS OF
QUEOUS
QUILIBRIA
Indicates that the reaction goes virtually to
dissolves
B
S
:
completion
UFFER
OLUTION
M
H
V
:
OLAR
EAT OF
APORIZATION
Contains both a weak acid and its conjugate base
L
C
’
P
:
E
HÂTELIER
S
RINCIPLE
The heat needed to vaporize one mole of a
as major species in solution,
When a change is imposed on a system at
[ ]
substance at its normal boiling point
⎛
−
⎞
equilibrium, the system will react in the direction that
A
M
H
F
:
⎜ ⎜
⎟ ⎟
=
+
OLAR
EAT OF
USION
initial
pH
p
K
log
reduces the amount of change.
[ ]
Heat needed to melt one mole of a substance at its
a
⎝
⎠
H
A
T
:
EMPERATURE
initial
normal melting point
The only variable that causes a change in the value
S
:
B
C
:
UBLIMATION
UFFER
APACITY
of K
an increase in temperature always shifts the
−
+
A phase change in which a solid converts directly to
eq,
The amount of added H
O
or OH
the buffer
3
equilibrium position in the endothermic direction.
a vapour without passing through the liquid phase,
solution can tolerate without exceeding a specified
∆E
= ∆H
− RT
pH range.
vap
vap
vap
THERMODYNAMICS
CHEMICAL KINETICS
S
L
T
:
ECOND
AW OF
HERMODYNAMICS
C
S
:
LOSED
YSTEM
Any spontaneous process increases the disorder of
Exchanges energy but not matter with its
the universe
R
M
:
EACTION
ECHANISM
surroundings
E
:
NTROPY
The exact molecular pathway that starting materials
I
S
:
SOLATED
YSTEM
The state function that provides a quantitative
follow on their way to becoming products
Exchanges neither matter nor energy with the
measure of disorder and is symbolized S,
R
-D
S
:
ATE
ETERMINING
TEP
surroundings
q
The slowest elementary step in a mechanism
∆
=
T
S
V
:
TATE
ARIABLES
S
F
-O
R
L
:
T
IRST
RDER
ATE
AW
Conditions that must be specified to establish the
Rate = k[A], where A is a reactant in the overall
state of a system, pressure (P), volume (V),
Entropy Change of the Universe:
reaction, this can be converted to
temperature (T), and amounts of substances (n)
Total entropy change,
⎛
⎞
∆S
= ∆S
+ ∆S
P
C
S
:
[A]
HYSICAL
HANGE OF
TATE
⎜ ⎜
⎟ ⎟
=
universe
system
surroundings
0
ln
kt
Some of the state variables changes, but the
R
E
:
EACTION
NTROPIES
⎝
⎠
[A]
∑
∑
chemical composition of the system stays the same
∆
=
∆
−
∆
o
o
o
S
coeff
S
coeff
S
ST
H
-L
(
), 1
O
:
ALF
IFE
T
RDER
C
C
S
:
reaction
p
r
1/2
HEMICAL
HANGE OF
TATE
When half the original concentration has been
The amounts of reactants and products change
consumed,
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