Download Chapter 9 – Molecular Geometry and hybridization I. Molecular

Chapter 9 – Molecular Geometry and hybridization
I. Molecular Shapes
II. Polarity
III. sigma and pi bonds (sp hybridization)
Chapter 14 - Kinetics
I. Collision Theory
II. Factors that affect reaction rates
A. Potential energy graph
B. Kinetic energy graph
III. Instantaneous rate - determined from the slope of the curve (concentration vs. time) at a particular time
IV. Average rate of reaction = ∆[Product]/∆time
V. Reaction rates and Stoichiometry
VI. Writing rate expression (rate law) Rate = k[A]m[B]n
VII. Calculating rate constant with proper units
VIII. Determining reaction orders from data and overall reaction order (m + n)
A. Reaction order graphs
IX. Reaction mechanisms
A. Rate determining step
B. Determining the rate law for a multistep mechanism
X. Using Integrated first order rate law
ln[A]t = -kt + ln[A]0
XI. Catalysts
Chapter 15 – Equilibrium
I. Dynamic equilibrium – characteristics of an equilibrium state
II. Graphs:
III. EQ constant (Kc = Keq)
aA + bB
Kc = [D]d [E]e
[A]a [B]b
IV. Magnitude of Keq
dD + eE
V. Le Chatelier’s Principle – predict shifts
VI. EQ Law
Qc = [D]d[E]e
[A]a[B]b
VII. “ICE” problems
Chapter 16 – Acid-Base Equilibria
I.
II.
Acid-Base Theories
A. Arrhenius
B. Bronsted-Lowry
1. Conjugate pairs
C. Lewis
Acid Reactions
III.
Net Ionic Equations
IV.
Strong & Weak Acids and Bases (Table/Figure 16.3 & Exercise 16.3)
V.
pH and pOH scales
A. pH = -log [H+]
B. [H+] = 10-pH
C. pOH = -log [OH-]
D. [OH-] = 10-pOH
E. [H+] [OH-] = 1 x 10-14
VI.
Kw : Ionization of Water
A. [H+] [OH-] = Kw
VII.
Ka and Kb
A. Ka = [H3O+] [A-]
[HA]
B. Kb = [BH-] [OH-]
[B]
Acid dissociation constant
Base dissociation constant
VIII.
ICE problems with Ka and Kb
IX.
pKa and pKb relationships with strong and weak acids and bases
Chapter 20 – Electrochemistry
I.
Assigning oxidation numbers
II.
Identifying oxidation and reduction
III.
Balancing redox half reactions
IV.
Activity Series Table
V.
Voltaic Cell
1.
2.
3.
4.
5.
Spontaneous reaction where chemical energy is converted to electrical energy
An Ox & a Big Red Cat – Anode is negative, Cathode is positive
Metal at Anode is listed higher on Table J
Electrons flow from Anode to Cathode
Salt bridge – flow of ions – keeps charge from building up in one cell
VI.
Standard reduction potentials table and calculating voltage
VII.
Electrolytic Cell
1. Non-spontaneous reaction – needs outside source of energy (electrical energy is
converted to chemical energy)
2. Anode is positive, Cathode is negative
3. Electrons flow from Anode to Cathode
4. Electroplating, electrolysis
5. Anode is the metal that is used for plating; Cathode is the object being plated
6. No salt bridge