Transcript A.P. Exam Review - Mt. Lebanon School District

A.P. Exam Review
Regular Review Day 5
Big Idea #5
The laws of thermodynamics
describe the essential role of
energy and explain and predict
the direction of changes in
matter.
Chapter 6
A.P. Chemistry
Thermochemistry
WHAT THEY BOTH
HAVE IN COMMON
amount Extensive Total capacity
Internal Total
Enthalpy
for heat
of K.E. and State
Energy, P.E.
,H
Functions exchange
EDE q w
H = E + PV
=
+
PERSPECTIVE IS
IMPORTANT!!
heat…flow of energy due
+ in to temp. diff.’s
Flowing
_
work…force x distance (moving things)
Flowing out
System VS. Surroundings
Done to+
(Everything
_
(Your Focus)
Done by
Else)
w = -PDV 1 mole of a substance
AN EXPANDING GAS formed from its
elements in std. states
Heats of Formation.
DH = Snprod.DHf – Snreact.DHf
DH = DE + DPV
DH = qp
FINDING THIS
1.Calorimetry
q = m c DT
2. Given the eq.’s
HESS’S LAW
3. Write your own
Chapter 16 – A.P. Chemistry
Thermodynamics
Occurs only with outside
intervention
Occurs w/o outside
intervention
spontaneous
1. phases
2. # of gaseous
particles
3. complexity of
particles
3rd Law
+
nonspontaneous
DSuniv
A measure The change
of disorder in the entropy
of the
universe
The little superscript zeros
mean: standard
Which is equal to: -DHsys
T
=
DSsys
+
Changed to
DSuniv = DSsys – DH/T
Which can be changed to:
Which says:
Standard
Standard
Standard
The entropy of a change
univ =
change
change
________ in
________ in
________ in
perfect crystal is ______________
___________ entropy
__________
free energy enthalpy
zero
and for which info
But what if we are not at standard conditions?
is easily found.
←Q is the reaction quotient…the mass
=
action expression w/ init. conditions
DG DG° + RTlnQ
And if we are at equilibrium?DG = 0
DSsurr
or
form that is usable
DG° = DH° – TDS°
-
-TDS
0 = DG° + RTlnK
Change in
free energy
DH – TDS = DG
-
Which must be ___ for
spontaneous processes
or
DG° = -RTlnK
Big Idea #6
Any bond or intermolecular
attraction that can be formed
can be broken. The two
processes are in a dynamic
competition, sensitive to initial
conditions and external
perturbations.
opposing processes equal
When two ____________
Ch. 13 A.P. Chem
rate
eachother in ________
Chemical Equilibrium
quantifying it
Le Chatelier’s Principle
Reactions are _________
reversible
Consequences
at Equilibrium
Rates of
forward and
reverse are
Equilibrium
[ ]’s are
dictated by
______________
An
equilibrium system that is
stressed
will respond to a
______________
stress in such a way to
______________
counteract
the stress
Nonequilibrium
same/constant
Conc. Changes
maybe!!
[ ]’s are
Mass Action
Expression [P]x/[R]y
same/constant
stoich. and
intitial
[ ]
__________
Kc (RT)Dn = Kp
Kc
Q
Ksp Compare
If ___
> ___
Q
K
Kp If ___
Q < ___
K
Temp. Changes
rxtion favored
Volume
reverse (Pressure)
________
forward Changes
________
at eq.
If ___
Q = ___
K ________
Molar Solubility
Ch. 14/15
A.P. Chemistry
Nature of Them
Practical
Definitions
Conceptual
Definitions
Conjugate
Pairs
•Sour
A: Liberates H+
ions in sol’n
B: Liberates OHions in sol’n
B-L
Defined:
-log [H3O+]
Dissociation
Constants
Strong
Species
Easiest…
Ka x Kb = Kw
[H+]
[OH-]
Tells about:
[the autoionization
of water]
Salts
neutral
acidic
basic
Calculations
Weak
Species
Harder…
concentration
on bottle
dictates [H3O+]
Strength
Oxides
Polyprotic
Acids
Use Ka or Kb
values
A: proton donor
BASES
B: proton
acceptor
•Bitter
Lewis
•Turns litmus blue
•slippery
SA/SB
WA/SB
WB/SA
Volumetric
analysis to
determine
unknown [ ]’s…
A: electron pair
acceptor
B: electron pair
donor
Titration
pH curves
% Dissociation
Changes
with dilution
Electron Withdrawing Capacity
explains this
Henderson-Hasselbalch Eq.
Indicators… used to
find end point of titration
Range
pKa ± 1
Buffers
Sol’ns which resist changes in pH
with small additions of acids or bases
Arrhenius
•Reacts with
metals to
produce H2
pH
As Equilibrium Rxtns.
ACIDS
•Turns litmus red
Covalent (acidic)
Ionic (basic)
ACIDS AND BASES
Naming Acids
Generally Binary Acid
1.
Without Oxygen
Generally containing a
polyatomic ion
2. With Oxygen
(Hydrogen compounds dissolved in water)
(simple description)
Rules
HydroPrefix?
Yes!
----Prefix?
No!!
Anion-
Root Name
from
Where?
-ic
Acid
Suffix? Yes!
-ic (ate) or
Polyatomic ion- -ous (ite) Acid
Root Name
from
Where?
Suffix?
Depends on the
HI(aq) is hydriodic acid
ending of the
polyatomic ion
HIO2(aq) is iodous acid
hypoiodous acid (formula-wise) is HIO(aq)
Hydrogen periodate (dissolved in water) is
periodic acid (with a formula of) HIO4(aq)