AP Chem Daily Assignments

AP Chemistry Text Book  Chemistry 7th Edition  Zumdahl / Zumdahl


 Course Syllabus                                         Scoring Guide for Labs

 AP Credit for your University                       Required Materials for Class

Link for all AP Exam dates

2017 AP Score Distributions

AP Chemistry sample test & Key  Pg 117-149

AP Scoring Rubric to the "Big Ideas"  pg 151-159

P-Table & Formula sheet Pg 160-162


Chapter 1   Chemical Foundations                Lab on Gravimetric Analysis & Chromatography

Student Learning Outcomes      Students will be able to:

1. Use Metric Prefixes to convert units   2. Use Significant Figures in Calculations   3.  Determine the effects of accuracy & precision

4. Use Dimensional Analysis to convert units  5. Density     6. Know how and when to use different separation techniques such as distillation, chromatography, filtration gravimetic analysis, evaporation

Ch. 1 Problems #21, 23, 28, 29, 31, 32, 50, 54, 60, 67, 82


Kindt Video on Metric Conversions

Scientific Notation

Significant Figures

Accuracy vs Precision

Dimensional Analysis

Separtation Techniques


Other video Links for Chapter 1

How to determine Significant Figures.



Why are Significant Figures Important?


Significant Figures with the Atlantic Pacific Rule


Metric conversion "loop Chart"


Dimensional Analysis


Solutions & Separation Techniques (Chromatography, Distillation)



 Chapter 2  Atoms, Molecules, and Ions

Student Learning Outcomes      Students will be able to:

1. Apply Dalton's atomic Theory to chemical ratios, 2. Explain implications of Rutherford's foil experiment, 3. Classifications on the P-Table 4. Name Binary Compounds (Memorize Polyatomic Ions Table 2.5) 5. Know formulas for common acids and bases

Chapter 2 Problems:  16, 21, 23, 27, 42, 44, 50, 52, 56, 58, 62, 64, 66, 69


Kindt Video on Rutherford's Gold Foil Experiment

Intro to the Periodic Table

Polyatomic Ions to know for AP Chemistry

Naming Binary Compounds


Other Video Links

Naming Compounds Part 1


Naming Compounds Part 2



More Practice Naming Compounds with Polyatomic Ions



                                                                                                      Chapter 1 & 2 Exam 


 Chapter 3   Stoichiometry                 Lab on Balanced Chemical Equations

Student Learning Outcomes      Students will be able to:

1. Use moles to calculate the percent composition in compounds  2. Determine the molectular & empirical formula

3. Write balanced chemical equations  4. Calculate yield with limiting reagents 

Chapter 3 Problems:








Chapter 4 Types of Chemical Reactions & Solution Stoichiometry     Lab on Titrations

Student Learning Outcomes      Students will be able to:

1. Identify properties of electrolytes  2. Calculate the molarity of a solution  3. Write a net Ionic Equation

4. Know the types of compounds that form precipitates  5. Calculate the mass in a precipitation reaction  5. Acid - Base Titraion calculations with endpoints  6. Assign oxidation numbers  7. Be able to identify the type of reaction:

Chapter 4 Problems:



How to determine oxidation numbers






 Chapter 3 & 4 Exam


Chapter 5  Gases         Butane Lighter Lab

Student Learning Outcomes      Students will be able to:

1. Convert units of pressure  2. Apply Boyle's Law, Charles's Law, and Avogadro's Law  3. Be able to apply the Ideal Gas Law

4. List the postulates of an ideal gas and know when and why something is not an ideal gas  5. Use stoichiometry in a gas law problem

6. Apply Dalton's Law of Partial Pressure to a gas  7. Apply Graham's law of Effusion to HCl & NH3

Chapter 5 Problems:







Chapter 5 Test


 Chapter 6   Thermochemistry                                   Specific Heat of a Metal Lab

Student Learning Outcomes      Students will be able to:

1. Calculate the Enthalpy in a chemical reaction  2. Calculate the heat in a Calorimetry reaction  3. Apply Hess's law in a reaction



Chapter 6 Problems:



Chapter 6 Test


Chapter 7    Atomic Structure & Periodicity  (Quantum Chemistry)     Brass & Copper Spec 20 Lab

Student Learning Outcomes      Students will be able to:

1. Apply the relationship between wavelenght, frequency, and energy of a photon  2. Diagram and explain the Bohr model

3. Give the quantum shells for an atom  4. Identify atoms from a PES diagram  5. Explain periodic trends in ionization energy &

atomic radius


Chapter 7 Problems:


 Chapter 7 Test


Chapter 8 & 9    Bonding Concepts

Student Learning Outcomes      Students will be able to:

1. Identiy the types of bonds  2. Apply electronegativity & Polarity to bonding  3. Draw the dipole moments in a bond

4. Predict the relative sizes of ions  5. Calculate lattice energy  6. Explain a covalent bond  7. Calculate delta H from bond energy

8. Draw a lewis dot structure  9. Calculate formal charge  10. Use the VSEPR model to determine the geometry

From Chapter 9 Explain what Hypbridization is and why an atom is hybridized  SP  SP2  SP3  SP3d & SP3d2

Chapter 8 problems:



Chemical Bonds

Ionic Bonding  Text Book Pages 330 - 353

Covalent Bonding  Text Book 391 – 403

Network Covalent Bonding (Strongest bond like Diamond & Quartz) Pg 444 – 448

Lewis Dot Structures & Resonance  Page 354 – 366

Molecular Geometry & the VSEPR Model  pg 367-378


Bond Angles & Molecular Geometry  pg 367 – 378

Metallic Bonding with Interstitutial & Substitutal Alloys


Chapter 8 & 9 Exam


Chapter 10  (Intermolecular Forecs) Liquids & Solids      &          Chapter 11 Properties of Solutions

Student Learning Outcomes      Students will be able to:

1. Identify the intermolecular forces (Dipole-Dipole, Hydrogen Bondin, London dispersion)  2. Explain the cause of surface tension and capillary action  3. Diagram and explain Bonding in metals (closest packing)  4. Diagram and explain the silicate tetrahedral

5. Be able to use a phase diagram 

From Chapter 11: 

6. Factors affecting solubility (Lake Nyos 1986)  7. Identify factors Boiling-Point Elevation & Freezing-Point Depression 

8. Explain what a Colloid is


Chapter 10 Problems


Intermolecular Forces
Hydrogen Bonding & common mistakes to avoid

Dipole forces or polarity in molecules

Intermolecular forces (give properties for solid liquid gases such as MP. BP


London Dispersion Forces





 Comprehensive Semester Exam






2nd Semester Outline:  Ch 12 Kinetics   Ch 13 Equilibrium   Ch 14 Acids & Bases    Ch15 Aqueous Equilibriua    Ch 17 Electrochemistry


Introduction to Chapter 12  Chemical Kinetics  Crystal Violet Lab

Student Learning Outcomes      Students will be able to:

Homework  Read Chapter 12 



The Rate Constant K


 Reaction Path & the Arrhenius Equation


 Activation Energy in a Chemical Reaction


 Multi Step Reactions


 The Rate Limiting Step



32 min video reviewing AP Chem unit on Chemical Kinetics



Chapter 13 Chemical Equilibrium

Student Learning Outcomes      Students will be able to:

Equilibrium, Le Chatelier's Principle, Acid Bases, Solubility, Buffers

Video #1  Le Chatelier’s Principle


Video #2 Chemical Equilibrium


Video #3 Reaction Quotient


#4 Equilibrium Disturbances


#5 ICE tables for Equilibrium equations


#6 Delta G & the Equilibrium Constant


 #7 More ICE table practice


#8 Solubility and Ksp


Even More ICE tables




Chpater 14 Acids & Bases  & Chapter 15 Aqueous Equilibria

Student Learning Outcomes      Students will be able to:

Acids Bases pH


Acid Base Equilibrium


pH and Buffers


Buffers with Henderson Hasselbalch Equation


More Henderson Hasselbalch Equation


Buffers  MIT Lecture


Derivation of Henderson Hasselbalch





Chapter 17 Electrochemistry

Student Learning Outcomes      Students will be able to:

Redox Reaction




What’s the anode, cathode, and salt bridge?


Introduction to Electrochemistry


Finding the E cell of a reaction


 The Nerst Equation





The AP Exam   Part 1 90 min:  60 Mult. Choice Questions  No Calculator

                   Part 2 90 min: Free Response  1, 2, 3 Long form quest (20 min each) 4, 5, 6, 7 Short Ans question (approx 5 min each)

Percent Breakdown from past exams:  76% = 5   62% = 4    48% = 3    34% = 2     0 - 33% = 1