Chapter
4
I.
‐
‐
‐
‐
II.
‐
‐
‐
‐
III.
‐
‐
‐
‐
‐
Nature
of
Aqueous
Solutions
KNOW
Molecular,
Total
Ionic
and
Net
Ionic
KNOW
the
role
of
water
in
solutions
(HOW
DOES
IT
SOLVATE
COMPOUNDS?)
KNOW
difference
between
strong,
weak
and
nonelectrolytes
Calculate
for
Molarity,
moles,
molecular
weight,
grams,
etc.
(FROM
CHAPTER
2
and
3)
and
use
this
in
STOICHIOMETRY
PROBLEMS.
Precipitation
Reactions
Precipitation
reactions
are
double
displacement
reactions
KNOW
how
to
use
the
Solubility
Rules
Table
DO
NOT
MEMORIZE,
WE
WILL
PROVIDE
IT
DURING
THE
EXAM
Use
Precipitation
reactions
in
STOICHIOMETRY
PROBLEMS
Acid‐Base
Reactions
KNOW
the
definition
of
acids
and
bases
KNOW
what
a
NEUTRALIZATION
REACTION
is.
KNOW
the
Strong
acids
and
Strong
bases
KNOW
how
to
use
them
in
molecular,
total
ionic
and
net
ionic
equations
Acid‐base
reaction
is
a
proton
(H+)
transfer
reaction,
acid
is
the
source
of
H+
and
bases
accept
H+.
IMPORTANT
REMINDER
Strong
acids
and
bases
dissociate
completely
MOLECULAR:
HCl
(aq)
+
NaOH
(aq)

H2O(l)
+
NaCl
(aq)
TOTAL
IONIC:
H+(aq)
+
Cl‐
(aq)
+
Na+
(aq)
+
OH‐(aq)

H2O
(l)
+
Na+
(aq)
+
Cl‐
(aq)
NET
IONIC:
H+
(aq)
+
OH‐
(aq)

H2O
(l)
Weak
acids
(like
H2S
and
acetic
acid,
CH3COOH)
and
bases
DO
NOT
DISSOCIATE.
MOLECULAR:
CH3COOH
(aq)
+
NaOH(aq)

CH3COO‐
(aq)
+
H2O(l)
+
Na+
(aq)
TOTAL
IONIC:
CH3COOH
(aq)
+Na+
(aq)
+OH‐(aq)
CH3COO‐
(aq)
+
H2O(l)
+
Na+
(aq)
NET
IONIC:
CH3COOH
(aq)
+
OH‐(aq)

CH3COO‐
(aq)
+
H2O(l)
NOTICE
that
although
CH3COOH
is
in
aqueous
state
(aka
the
“(aq)”
state)
it
didn’t
dissociate
to
CH3COO‐
and
H+
during
the
total
ionic
and
net
ionic
equations.
‐
KNOW
how
to
use
Acid
base
reactions
in
STOICHIOMETRY
PROBLEMS
especially
TITRATION
(Moles
of
acid
will
be
used
up
by
moles
of
base!!)
‐
Moles
acid
is
not
always
equal
to
the
moles
of
the
base;
this
depends
in
the
stoichiometry
of
the
reactions!!
Example
1.
NaOH
+
HCl

H2O
+
NaCl
Moles
HCl
=
Moles
NaOH
Example
2.
2KOH
+
H2SO4

2H2O
+
K2SO4
Moles
H2SO4
=
Moles
KOH
x
1/
2
The
1/2
there
is
the
stoichiometric
ratio
of
KOH
and
H2SO4
IV.
Oxidation‐Reduction
Reactions
‐ KNOW
What
REDOX
means
(LEORA
and
GEROA)
‐ KNOW
how
to
determine
Oxidation
numbers
(MEMORIZE
THE
RULES!!)
‐ KNOW
the
different
ways
in
which
Redox
can
occur
o Redox‐combination
or
Redox‐addition
o Redox‐decomposition
o Redox‐displacement
 Displacement
of
H2
from
water
or
acid
by
metals
• WE
WILL
PROVIDE
YOU
THE
ACTIVITY
SERIES,
NO
NEED
TO
MEMORIZE
• KNOW
how
to
use
the
activity
series
 Displacement
of
Halogens
(MEMORIZE!)
o Redox‐combustion
‐ KNOW
how
to
use
Redox
in
STOICHIOMETRY
PROBLEMS
Chapter
5
I.
Properties
of
Gas
‐ What
differentiates
it
from
liquids
and
solids?
II.
Measuring
Pressure
‐ How
do
we
measure
gas?
Barometer
and
Manometer
‐ Convert
pressure
1
atm
=
1.01325
barr
=
760
mmHg
=
760
torr
=
14.7
psi
=
101325
Pascals
(MEMORIZE!!)
III.
Gas
Laws
‐ KNOW
Them
o Boyle:
P1V1=P2V2
in
constant
n
and
T
o Charles/Gay‐Lusaac:
V1/T1=V2/T2
in
constant
n
and
P
o Amonton:
P1/T1=P2/T2
changes
in
constant
n
and
V
o Avogadro:
V1/n1=V2/n2
changes
in
constant
P
and
T
‐ USE
Them
in
COMBINATION!
IV.
Ideal
Gas
Law
(IGL)
and
its
applications
‐ KNOW
the
formula
PV=nRT
where
R
=
0.0821
L*atm/mol*K
‐ Use
it
in
different
applications
o Getting
density
(m/V)
o Getting
molarity
(n/V)
o Getting
MW
o Dalton’s
Law
of
Partial
Pressures
 PTotal
=
P1
+
P2
+
P3…
 P1
=
X1
PTotal
where
X1
is
mole
fraction
of
component
1
 X1
=
n1/ntotal
NOTE
if
given
in
%
volume
as
in
problem
set
question
#
5.41
treat
%
by
volume
as
Volume
occupied
if
the
specific
gas
is
set
at
the
same
pressure
and
Temp.
A
sample
of
air
contains
78.08%
N2,
20.94
%
O2
and
0.05%
CO2
and
0.93%
Ar
by
volume.
How
man
molecules
of
each
gas
is
present
in
1.00
L
of
sample
at
25
degC
and
1.00
atm.
What
does
%
by
volume
mean?
It
is
the
volume
occupied
of
the
specific
gas
if
it
was
under
the
same
pressure
and
temp
So
for
N2:
Ptotal
V
(of
N2)
=
n(of
N2)
RT
But
we
know
V(of
N2)
=
0.7808
VTotal
and
VTotal
=
1.00
L
So
we
can
get
n(of
N2)
from
this
equation
and
eventually
from
moles
to
number
of
molecules!
DO
THE
SAME
FOR
THE
OTHERS.
o KNOW
how
to
use
IGL
in
STOICHIOMETRY
PROBLEMS
V.
KMT
‐ KNOW
the
Postulates
(DO
NOT
JUST
memorize!
Make
sure
you
ALSO
UNDERSTAND
IT!)
‐ How
does
it
relate
to
Gas
Laws
o Relationship
of
pressures
with
no.
molecules
or
volume
or
temperature
o Temperature
and
KE

and
also
speed
of
particles
of
different
MW.
VI.
Real
Gases
‐ Why
do
gases
deviate
from
Ideal
behavior
‐ van
der
Waals
Equation
(KNOW
and
understand
the
correction
factors!)
Chapter
6
I.
‐
‐
Thermodynamics
and
Thermochemistry
KNOW
how
to
differentiate
SYSTEM
from
SURROUNDINGS
Some
added
info:
o Open
system
–
system
can
transfer
both
energy
(in
the
form
of
heat
and
work)
as
well
as
matter
(in
the
form
of
molecules/moles/mass)
o Isolated
System
–
system
cannot
transfer
energy
and
matter
o Closed
system
–
system
can
transfer
energy
(in
q
and
w)
but
not
matter
o Closed
System
with
adiabatic
boundary–
system
cannot
transfer
energy
as
heat,
all
energy
is
transferred
as
work.
o Closed
system
with
rigid
boundary
–
system
cannot
transfer
energy
as
work,
all
energy
is
transferred
as
heat.
II.
‐
‐
‐
‐
‐
‐
III.
‐
‐
‐
‐
IV.
‐
‐
‐
‐
‐
V.
‐
‐
VI.
‐
‐
‐
Internal
Energy
(and
how
it
changes)
What
is
Internal
energy?
What
is
a
state
function?
Why
can’t
we
measure
exact
values
of
internal
energy?
How
is
the
change
in
internal
energy
of
a
system
manifested?
How
is
energy
transferred?
ΔE
=
q
+w
KNOW
the
SIGN
CONVENTIONS
o ΔE
<0
=
loss
energy
o ΔE
>0
=
gain
energy
o q
<
0
heat
lost
o q
>
0
heat
gained
o w
<
0
work
done
BY
system
o w
>
0
work
done
ON/TO
system
KNOW
the
FIRST
LAW
OF
THERMODYNAMICS
Enthalpy
and
Stoichiometry
How
is
enthalpy
related
to
internal
energy
(NO
NEED
TO
MEMORIZE
FORMULA
just
UNDERSTAND
IT)
WHAT
IS
ENTHALPY?
ΔH
=
qp
KNOW
HOW
Enthalpy
works
as
a
state
function
KNOW
HOW
Enthalpy
works
as
related
to
chemical
reactions.
How
do
we
use
them
in
STOICHIOMETRY?
Calorimetery
What
is
Heat
Capacity
What
is
Specific
Heat
Capacity
and
Molar
Heat
Capacity?
What
does
it
mean
if
one
object
has
a
higher
heat
capacity
than
another?
How
is
heat
capacity
used
in
calculating
change
in
enthalpy
of
solutions?
KNOW
HOW
TO
USE
THE
COFFEE
CUP
CALORIMETER!
o ΔHsys
=
q
sys
=
–q
surr
=
–
m
surr
x
c
surr
x
ΔT
surr
o ΔHrxn
=
q
rxn
=
–q
soln
=
–
m
soln
x
c
soln
x
ΔT
soln
Hess’s
Law
of
Heat
Summation
WHAT
IS
HESS’S
LAW?
DERIVE
the
HEAT
OF
REACTION
ΔHrxn
based
on
the
ΔH
of
other
reactions
Standard
Heats
of
Formation
What
is
the
standard
state?
KNOW
What
is
the
Standard
heat
of
formation
ΔHf0?
o Be
able
to
write
FORMATION
REACTIONS!
o KNOW
THE
STANDARD
STATES
OF
COMMON
ELEMENTS!

State
that
is
most
stable
at
1
atm
and
usually
25
deg
C
KNOW
How
can
you
use
the
ΔHf0
to
calculate
ΔHrxn0