Lecture 21: Chemical Bonding
Reading: Zumdahl 13.113.2
Read all sections of Ch 13 this is different than
what the reading schedule says in the syllabus;
sections 13.6 and 13.7 will not be addressed
specifically in lecture but you should still read them
Lecture 17: Quantum Mechanics
Reading: Zumdahl 12.5 & 12.6
Problems for Extra Practice
47, 49 (Chapter 12)
Outline
Bohrs Model of the hydrogen atom (12.4)
QuantumMechanical model of the atom (12.5)
The particle in a box (12.6)
The wave equation for t
Lecture 14: The Nernst Equation
Reading: Zumdahl 11.4 & 11.7
Outline
How does Ecell depend on concentration?
(11.4)
Nernst equation
Concentration Cells
Electrolytic cells: an example of
nonspontaneous electron flow (11.7)
Problems for Extra Practice
Lecture 13: Cell Potential and G
Announcements:
HW #4 due today (by 11pm)!
HW #5 posted, due Nov. 10
Reading: Zumdahl 11.3 & 11.4
Outline
Line notation for electrochemical cells (not in book)
Cell potential, electrical work, and free energy (11.3,
Lecture 10: Free Energy and Equilibrium
Announcements
HW#3 Due Today (11:00 PM)
Review sheet posted on web
Reading: Zumdahl 10.10 and 10.11
Outline
Free energy and pressure (10.10)
Equilibrium is achieved when the total Gibbs
energy for a system is
Lecture 9: Gibbs Free Energy
Reading: Zumdahl 10.7, 10.8 and 10.9
Outline
Define Gibbs free energy (10.7)a
formulation of Suniv in terms of system
variables
Free energy and chemical reactions (10.9)
Second Law of Thermodynamics
The entropy of the univ
Lecture 7: Thermo. Def. of Entropy
Reading: Zumdahl 10.5 and 10.6
Outline
Entropy and the second law of thermodynamics
(10.5); How do we increase entropy?
Entropy changes in the surroundings and the effect of
temperature on spontaneity (10.6)
Entropy
Lecture 7: Thermo. Def. of Entropy
Reading: Zumdahl 10.2, 10.3 and 10.13
Outline
Isothermal processes; Isothermal gas
expansion and work, Reversible processes
(10.2)
Entropy is a state function
General Expression for Entropy
Note that in the previous
Lecture 6: Intro to Entropy
Reading: Zumdahl 10.1 and 10.3
Outline
Reaction spontaneity (10.1)
Statistical interpretation of entropy and Boltzmanns
formula (10.3)
Announcements
Announcements
HW #2 Due today
HW #3 Posted Due on Friday, Oct. 22
Offi
Lecture 5: Standard Enthalpies
Reading: Zumdahl 9.5, 9.6
Outline
Hesss Law (9.5)
Examples of using Hesss Law
Standard Enthalpies (9.6)
What is a standard enthalpy?
Defining standard states
Using standard enthalpies to determine H
rxn
Heats of for
Lecture 4: Calorimetry & Hess Law
Reading: Zumdahl 9.4, 9.5
Outline
Calorimetry (9.4)
Examples of calorimetry calculations
Hesss Law (9.5)
Motivation for and definition of Hesss Law
Examples of using Hesss Law
What do we know so far?
(Summary of wh
Lecture 3: Thermodynamics of
Ideal Gases & Calorimetry
Announcements
Calculators
Homework
Reading: Zumdahl 9.3, 9.4
Outline
Define the manner in which substances store heat energy:
heat capacity (CV, CP)
Mathematical form for E and H using CV and C
Lecture 2: Enthalpy
Reading: Zumdahl 9.2, 9.3
Outline
Define a new thermo variable: enthalpy (H), the
heat transferred at constant pressure
Define the manner in which substances store
heat energy: heat capacity (CV, CP)
Mathematical form for E and H
Lecture 1: Energy
Reading: Zumdahl 9.1
Outline:
General properties/trends of Kinetic and Potential
Energy
Molecular kinetic energy and molecular potential
energy; Internal energy
Conservation of energy; system vs. surroundings
Methods of transferrin
CHEMISTRY 152 A
Autumn 2010
Lectures:
Mon., Wed., and Fri.
1:30 pm 2:20 pm
Class:
Lab:
Dr. Leah Miller
Dr. Andrea Carroll
TAs:
Jonathan Cox
Mike Carroll
Abhinav Dhall
Chelsea Hess
Course Objectives Chemistry 152
Second course in the intro. Chemistry
seri
E = q + w
w = Pext V
E = nCv T
H = nC P T
P
wrev = nRT ln 1
P
2
S = k B ln( )
H = E + P V
V final
wrev = nRT ln
V
initial
A!
=
ai !
i
S =
V final
S = nR ln
V
initial
dqrev qrev
=
T
T
T final
S = nCV ln
T
initial
aA
aA + bB
o
H rxn =
n H
o
f
E = q + w
w = Pext V
E = nCv T
H = nC P T
P
wrev = nRT ln 1
P
2
S = k B ln( )
H = E + P V
V final
wrev = nRT ln
V
initial
A!
=
ai !
i
S =
V final
S = nR ln
V
initial
dqrev qrev
=
T
T
T final
S = nCV ln
T
initial
ln (K ) =
H o 1 S o
+
R T
R
E = q + w
w = Pext V
E = nCv T
H = nC P T
V final
wrev = nRT ln
V
initial
H = E + P V
P
wrev = nRT ln 1
P
2
S = k B ln( )
=
A!
ai !
S =
dqrev qrev
=
T
T
i
V final
S = nR ln
V
initial
T
S = nC P ln final
T
initial
G o = H o TS o
G = G o + RT ln
CHEM 152A Autumn 2010
Review of material covered since Exam 2
Chapter 12 Quantum Mechanics and Atomic Theory
Section 12.10 Electron Spin and the Pauli Principle

Define the fourth quantum number, electron spin quantum number (ms) and know the allowed
val
Intro. Chemistry Lab and
Lecture Policies
Undergraduate Support Services
303 Bagley Hall
Overview
Lecture Policies
Excused Absences
from Exams
Homework and Quizzes
Laboratory Policies
Proper Attire
Prelab and Lab Report Policies
Excused Absences an
CHEM 152A Autumn 2010
Review for Exam 2
Chapter 11: Electrochemistry
Section 11.1 Galvanic Cells


Be able to define oxidation, reduction, oxidizing agent and reducing agent
Balance redox reactions using the halfreaction method
Galvanic cell
o Know the
CHEM 152A Autumn 2010
Review for Exam 1
Chapter 9: Energy, Enthalpy and Thermochemistry
Section 9.1 The Nature of Energy

General properties/trends of Kinetic and Potential Energy
Molecular kinetic energy and molecular potential energy; internal energy
C
Formulas, Chemical Equations and more.
The mole: Atoms are very tiny and lightmore convenient to
consider a collection of them:
1 mole = 6.022 x 1023 units of something
= Avogadros number (NA)
This is the number of atoms in exactly 12.000 g of 12C.
Atomic