1. A.P. Exam Review
Regular Review Day 5

2. Big Idea #5
The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.

3. DH = qp Internal Energy, E Enthalpy, H H = E + PV = + q w heat + _
Chapter A.P. Chemistry
Thermochemistry
CHANGES IN...
WHAT THEY BOTH HAVE IN COMMON
CHANGES IN...
Internal Energy, E
Total amount of K.E. and P.E.
Extensive
Total capacity for heat exchange
Enthalpy, H
State Functions
H = E + PV DE = q w
DH = DE + DPV
PERSPECTIVE IS IMPORTANT!!
heat
…flow of energy due to temp. diff.’s
DH = qp + _
Flowing in
work
…force x distance (moving things)
FINDING THIS
System
Surroundings
Flowing out +
Done to
VS.
Calorimetry _
(Everything Else) 1.
(Your Focus)
Done by
q = m c DT
w = -PDV
1 mole of a substance formed from its elements in std. states 2.
Given the eq.’s
AN EXPANDING GAS
Heats of Formation.
HESS’S LAW
DH = Snprod.DHf – Snreact.DHf
Write your own 3.

4. + - = + - DSuniv Thermodynamics -DHsys T DSsys DSsurr
Chapter 16 – A.P. Chemistry
Thermodynamics
Because of:
Occurs only with outside intervention
The 2nd Law
Occurs w/o outside intervention
The entropy of the univ. is increasing
spontaneous
nonspontaneous +
DSuniv -
-DHsys
Which is equal to: 1. 2. 3.
phases T
# of gaseous particles
A measure of disorder
The change in the entropy of the universe = +
DSsys
DSsurr
rankings
complexity of particles
measurable because of or
3rd Law
The little superscript zeros mean:
standard
DSuniv = DSsys – DH/T
Changed to
DG° = DH° – TDS°
Change in free energy
Which can be changed to:
Which says:
-TDSuniv = DH – TDS
= DG
Standard ________ in ______________
Standard ________ in ___________
Standard ________ in __________
The entropy of a perfect crystal is zero
change free energy
change enthalpy
change entropy -
form that is usable
Which must be ___ for spontaneous processes
and for which info is easily found.
But what if we are not at standard conditions?
←Q is the reaction quotient…the mass action expression w/ init. conditions
DG = DG° + RTlnQ
DG° = -RTlnK
DG = 0
0 = DG° + RTlnK or
And if we are at equilibrium?

6. 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.

7. Kc Q Ksp Kp Q K Q K Q K reverse Kc (RT)Dn = Kp forward at eq. opposing
Ch. 13 A.P. Chem
When two ____________ processes equal
eachother in ________
rate
Chemical Equilibrium
establishing it
manipulating it
quantifying it
Reactions are _________
reversible
Le Chatelier’s Principle
__________________________________________
Consequences at Equilibrium
Mass Action Expression
An equilibrium system that is stressed will respond to a stress in such a way to counteract the stress
[P]x/[R]y
Rates of forward and reverse are
Equilibrium
Nonequilibrium
same/constant
Conc. Changes
maybe!! Kc Q
[ ]’s are
same/constant
stoich. and intitial [ ]
[ ]’s are dictated by
Temp. Changes
__________
Ksp
Compare rxtion favored
Volume (Pressure) Changes Kp Q K
reverse
If ___ > ___ ________
Kc (RT)Dn = Kp Q K
forward
If ___ < ___ ________ Q K
at eq.
If ___ = ___ ________

8. Molar Solubility

11. pH Ka Kb Kw Ch. 14/15 A.P. Chemistry ACIDS AND BASES x = Titration
Covalent (acidic)
Ionic (basic)
Nature of Them
As Equilibrium Rxtns. pH
Salts
Oxides
neutral
acidic
Practical Definitions
Conceptual Definitions
Conjugate Pairs
Dissociation Constants
Defined: -log [H3O+]
Calculations
basic
ACIDS
Arrhenius Ka x Kb = Kw
Strong Species
Weak Species
Polyprotic Acids
Sour
Turns litmus red
Reacts with metals to produce H2
A: Liberates H+ ions in sol’n
B: Liberates OH- ions in sol’n
[H+]
[OH-]
[the autoionization of water]
Easiest… concentration on bottle dictates [H3O+]
Harder… Use Ka or Kb values
B-L
Tells about: Strength
A: proton donor
B: proton acceptor
Sol’ns which resist changes in pH with small additions of acids or bases
BASES
Volumetric analysis to determine unknown [ ]’s…
% Dissociation
Changes with dilution
Bitter
Turns litmus blue
slippery
Lewis
Electron Withdrawing Capacity explains this
A: electron pair acceptor
B: electron pair donor
Titration
SA/SB
Henderson-Hasselbalch Eq.
Calculations
How they work
Indicators… used to find end point of titration
pH curves
WA/SB
Buffers
Range pKa ± 1
WB/SA

12. hypoiodous acid (formula-wise) is HIO(aq)
(Hydrogen compounds dissolved in water)
Naming Acids
(simple description)
Rules
Generally Binary Acid
Hydro-
Anion-
-ic
Acid 1.
Without Oxygen
Root Name from Where?
Prefix?
Suffix?
Yes!
Yes!
Generally containing a polyatomic ion
-ic (ate) or
-----
Polyatomic ion-
-ous (ite)
Acid 2.
With Oxygen
Root Name from Where?
Prefix?
Suffix?
No!!
HI(aq) is
hydriodic acid
Depends on the 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)