Unit 1 Review of Chem. 1 Basics
Assignment 1:
Physical Separations of Matter vs. Chemical Changes
Read sec 1.1 – 1.3 pp. 2-14 in Brown & Lemay Textbook
1.1: The Study of Chemistry
1.2: Classifications of Matter
1.3: Properties of Matter
Assignment 2:
Atomic Structure & The Periodic Table
Read sec 2.1 – 2.7 pp. 38-59
Solve Textbook Problems 2.49, 2.53 and 2.60
2.2: The Discovery of Atomic Structure
2.3: The Modern View of Atomic Structure
2.4: Atomic Weights
2.5: The Periodic Table
2.6: Molecules and Molecular Compounds
2.7: Ions and Ionic Compounds
Assignment 3:
Chemical Names and Formulas
Read sec 2.8 & 2.9 pp. 59-67
Solve Textbook Problems 2.65, 2.68, 2.70, 2.74 and 2.78
2.8: Naming Inorganic Compounds
2.9: Some Simple Organic Compounds
Assignment 4:
Periodic Trends & Chemical Reactions (PPT Slides 52-75)
Read sec 7.2 – 7.5 pp.251 – 264
Solve Textbook Problems 7.16, 7.28, 7.42 and 7.96
7.2
7.3
7.4
7.5
Assignment 5:
Effective Nuclear Charge
Sizes of Atoms and Ions
Ionization Energy
Electron Affinities
Nuclear Chemistry (PPT Slides 32-50)
Read sec 21.1 – 21.3 pp. 251-268
Solve Textbook Problems 21.28 and 21.30
21.1 Radioactivity
21.2 Patterns of Nuclear Stability
21.3 Nuclear Transmutations
Assignment 6:
Math Relationships in Chemistry
Read sec 1.5 – 1.6 pp. 20-30
Solve Textbook Problems 1.40, 1.49, 1.56 & 1.82
Solve 1999 AP Exam Problem #5
1.5: Uncertainty of Measurement
1.6: Dimensional Analysis
Assignment 7:
Mole Relationships
Read sec 3.1 – 3.5 pp. 78-96 and sec 4.5 pp. 139-143
Solve Textbook Problems 3.24, 3.36, 3.58, 4.68 and 4.76
Solve 2005 AP Exam Problem #2
3.1: Chemical Equations
3.2: Some Simple Patterns of Chemical Reactivity
3.3: Formula Weights
3.4: Avogadro's Number and the Mole
3.5: Empirical Formulas from Analyses
4.5: Concentrations of Solutions
Assignment 8:
Stoichiometry, Limiting Factors and % Yield
Read sec 3.6 - 3.7 pp. 96-103
Solve Textbook Problems 3.70, 3.93, 3.98 and 3.102
Solve 2006 AP Exam Problem #3
3.6: Quantitative Information from Balanced Eqns.
3.7: Limiting Reactants
Assignment 9:
Stoichiometry and PV=nRT
Read sec 10.3 – 10.6 pp. 387-402
Solve Textbook Problems 10.57 and 10.62
Solve 2003 AP Exam Problem #2
10.3: The Gas Laws
10.4: The Ideal-Gas Equation
10.5: Further Applications of the Ideal-Gas Eqn.
10.6: Gas Mixtures and Partial Pressures
Assignment 10:
Titration Experiments & Stoichiometry
Read sec 4.6 pp. 144-148
Solve Textbook Problems 4.90 and 4.107
Solve 2000 AP Exam Problem #3
4.6: Solution Stoichiometry and Chemical Analysis
Assignment 11:
Go to the website listed below to run an acid-base titration simulation, using NaOH as the base and
phenolphthalein as the indicator. As a pre-lab exercise, complete the calculations for a sample
experiment.
http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/stoichiometry/aci
d_base.html
Assignment 12:
Lab Experiment: “Standardization of NaOH”
Complete formal lab report with data, spreadsheet analysis, and conclusions
Begin growth and recovery of green Fe Complex Crystals
Assignment 13:
Preparing Solutions and Expressing Concentrations
Read sec 13.4 pp. 526-530
Solve Textbook Problems 13.54 and 13.56
13.4: Ways of Expressing Concentration
Assignment 14:
Examples of AP Multiple Choice Questions – Test taking strategies and math estimation skills without
a calculator; What information should you memorize?
Assignment 15:
Lab Experiment: Dehydrate green Fe Complex crystals & determine % water in hydrate
Complete lab calculations and error analysis
Assignment 16:
Lab Practical: “Making Solutions for Iodine Clock Reaction”
Complete lab calculations and error analysis
Assignment 17:
Unit 1 Test – Nomenclature, Math & Mole Ratios, and Stoichiometry
Due Dates and Presentation Dates are the same!
Unit 1:
Due
Dates for Presentation Problems, Labs & Tests
Due Dates
Textbook Problems
1/7
2.49, 2.53, 2.60
1/7
2.65, 2.68, 2.70, 2.74,
2.78
1/8
AP Exam
Questions
1.40, 1.49,
1.56, 1.82
1/8
3.24, 3.36, 3.58, 4.68
and 4.76
3.70, 3.93,
3.98, 3.102
2005 #2
10.57, 10.62
2003 #2
1/9
Tests & Quizzes
7.16, 7.28, 7.42, 7.96
1/8
1/9
Lab Reports
1999 #5
2006 #3
TI83 analysis of NaOH
titration workpage
1/9
4.90, 4.107
1/10
21.28, 21.30,
13.54, 13.56
All Unit HW Problems
due
1/11
2000 #3
% Water in green
crystal journal due
Standardize NaOH
formal lab report
Lab Practical:
Making Solutions
Unit 1 Re-test
Due Dates and
Presentation
Dates
1/7
1/7
1/8
1/8
1/8
1/9
1/9
1/9
1/10
1/11
Textbook Problems
Group 1
2.49, 2.53, 2.60
Group 2
2.65, 2.68, 2.70, 2.74, 2.78
Group 3
7.16, 7.28, 7.42, 7.96
Group 4
1.40, 1.49, 1.56, 1.82
Group 6
3.24, 3.36, 3.58, 4.68 and 4.76
Group 1
3.70, 3.93, 3.98, 3.102
Group 3
10.57, 10.62
Group 5
4.90, 4.107
Group 7
13.54, 13.56,
21.28, 21.30
All Problems Due
AP Exam Questions
Group 5
1999 #5
Group 7
2005 #2
Group 2
2006 #3
Group 4
2003 #2
Group 6
2000 #3
Welcome to AP Chem/Chem 2 Hon – Your 1st Lab Experiment
Problem: You will be given a sample of a mixture that contains calcium carbonate, potassium carbonate, and sodium
chloride. Your goal is to devise an experimental procedure that will allow you to quantitatively separate the
components and determine their percent composition by mass in the mixture.
Procedure: It’s up to you to determine the most efficient and economical methods that will achieve the objectives given
in the problem. Consider using the common glassware, equipment, and chemicals that were utilized during your lab
experiences in the Chem I class to decide what should be available. (You could check your Chem I lab notebook if you
can’t remember!) Also, evaluate any chemical reagents you may wish to use based upon their availability, cost, and safe
handling procedures. A free site where you can obtain this information is http://www.sciencestuff.com/msds/
Welcome Back! On the first day of school, you will be randomly assigned to a lab group. Be prepared to share your
ideas and do some brain-storming to agree upon a plan of attack to solve this problem. You will then submit a group
proposal, which I will evaluate based upon safety, available chemicals and equipment, and feasibility. Either your plan
will be approved and experimentation may begin or your group may require further modifications before you may
actually start the experiment.
The Final Analysis: Upon completion of the experiment, you will submit a final report, summarizing your approved
procedure, data, calculations, and conclusions. Your results will be compared to the known percent by mass
composition of your mixture to determine the accuracy of your analysis.
“Chance favors the prepared mind.” Louis Pasteur