A.P. CHEMISTRY
Chapter 4 Schedule-Aqueous Solutions- Term I 2015
DATE
ACTIVITIES
Wed.
9-16
Get Ch.1-3 Tests back;
DUE: Read pg. 136-154 Be sure you’ve thoughtfully read this pages prior to coming to class.
The lecture has been recorded on video and can be found at www.wayzata.k12.mn.us/jodi.grack
Click on the Video link (instead of AP Chem) The Videos are entitled
AP Chemistry Ch 4 Videos
Part 1 - Precipitate Rxns (16 min)
Part 2 – Gas Formation Rxns (new!!!!) – 15 min
Part 3 – Acid Base #1 (14 min); Acid Base #2 (7 min)
Part 4 – Soln Stoich Review
You may either view these ahead of time, during class, or some of each. .
Thurs.
9-17
PROBLEM SET 4.1a DUE- Supplemental Worksheet (only 10 min work time); Quiz tomorrow As students finish.. Label a
50-mL beaker and obtain 1-2
Practice clicker quiz – memorized facts (SA, WA, SB, WB, salt)
grams of brass. Record the
Hand out Molecular WS; may start memorizing (will use two days before test)
mass. Place beaker, brass
Bring Lab Notebooks to use for acid rain demonstration/mini lab.
and watch glass in fume
Lecture pg. 154-162 Assigning Oxidation Numbers
hood.
Fri.
9-18
PROBLEM SET 4.1b DUE Supplemental Worksheet (rxns – esp gas and ox #’s )(~10 min group time)
QUIZ PS 4.1 (You will need to know naming (including acids); have your strong acids memorized, & be adept at writing net ionic eqns
Lecture pg. 162-169 Predicting Redox Rxns
Distribute Lab Manuals; Introduce Lab “How Can Color Be used to Determine the Mass Percent of Copper in Brass?”
Help with balancing net ionic eqn & 3-step mole method (due tomorrow)
Mon.
9-21
DUE: Read Investigation 2 in your lab book and read A-16 to A-19 in the back of your text book
DUE: Lab Day One – Instructor will add Nitric Acid; See white sheet for parts due
Finish Lecture 4.2 (&4.3?) pg. 154-169
Review recognizing and predicting common redox reactions. Practice clicker quiz (ox/red/both)
Discuss Lab “How Can Color Be used to Determine the Mass Percent of Copper in Brass?”
-Spectroscopy (how a spectrophotometer works) Abs vs. %T;
- Beer’s Law
- Serial dilutions
- using volumetric flask (mixing for uniform concentration)
Tues.
9-22
Lab day Two: DUE: Lab Notebook pictures in eBackpack by 7:00 am. (See separate directions.)
I will add the nitric acid and have them react prior to class (takes ~30 minutes)
Complete Lab Steps 3-4 “How Can Color Be used to Determine the Mass Percent of Copper in Brass?” (~40 minutes)
Work time Problem Set 4.2 PROBLEMS, Even #’s 64,68a-e,70a-e,72,74abc,80 & supp’s pp. 170-177 (EC 62,112ab)
(HINT 74c: balance Sulfur by adding H2SO4; sometimes spectator ions will also need to be added)
Wed.
9-23
PROBLEM SET 4.2 DUE (~10-15 min work time); QUIZ; you will need to know common oxidizing/reducing agents and their
products (both formulas and colors).
PROBLEMS, Even #’s 64,68a-e,70a-e,72,74abc,80 & supp’s pp. 170-177 (EC 62,112ab)
(HINT 74c: balance Sulfur by adding H2SO4; sometimes spectator ions will also need to be added)
QUIZ: PS 4.2 (You will need to have your common oxidizing/reducing agents memorized as well as the products
they form.)
Lecture 4.3 – Balancing in Basic solution
Thurs.
9-24
Lab Day Three:
Group A (tables 2,4,6)
Complete Lab Steps 5-11 “How Can Color Be used to Determine the Mass Percent of Copper in Brass?”
Table 2 and 4a start by using the spectrophotometer; table 6 and 4b start with the visual method
Computers will be available to do graphing after lab. See Mrs. Grack for help with excel spreadsheets/graphs.
Anything that is not completed will need to be done outside of class.
One partner must enter the % Cu for both methods into the shared Google Doc from your instructor by midnight tomorrow
Group B (tables 1,3,5,7)
PROBLEM SET 4.3 DUE (~25 minutes group time); QUIZ
PROB’S, Even #’s 58 (net ionic only), 66,74de,76,82,88; & Supp’s EC #92,110,112f pg. 170-177
Pick-up Redox Lab packet after quiz. Start pre-lab if time.
Fri.
9-25
Lab Day Three:
Group B (tables 1,3,5,7)
Complete Lab Steps 5-11 “How Can Color Be used to Determine the Mass Percent of Copper in Brass?”
Table 1 and 3 start by using the spectrophotometer; table 5 and 7 start with the visual method
Computers will be available to do graphing after lab. See Mrs. Grack for help with excel spreadsheets/graphs.
Anything that is not completed will need to be done outside of class.
One partner must enter the % Cu for both methods into the shared Google Doc from your instructor midnight tonight.
Group A (tables 2,4,6)
PROBLEM SET 4.3a DUE (~25 minutes group time); QUIZ
PROB’S, Even #’s 58 (net ionic only), 66,74de,76,82,88; & Supp’s EC #92,110,112f pg. 170-177
Pick-up Redox Lab packet after quiz. Start pre-lab if time.
Mon.
9-28
DUE: Redox pre-lab (1-3)
Complete Part I of Redox Titration – Standardization of KMnO4 (Must finish; solutions need to be fresh!)
Tues.
9-29
Collect Lab notebooks (%Cu in Brass Lab); all calcs 1-5, argumentation & documentation; post-lab calcs, error
analysis, & concludion (see white sheet)
Finish Redox Lab – Part II Determing the Concentration of Oxalic Acid; turn in data summary to teacher
Predicting Reactions – Molecular Equations
Hungry Dragon Demo
Wed.
9-30
DUE: PS 4.4b Predicting Rxns AND Error Analysis (1-4) for Redox Lab
DUE: Packet w/ data tables, Calculations, and conclusion
Study for test; review solubility rules (1-2), strong acids/acid naming; recognizing rxn types; common ox/red agents
Finish Redox lab;.
Thurs.
10-1
Collect Redox Lab
TEST: Chapter 4 “Aqueous Solutions,” %Cu in Brass Lab and Redox Titration Lab
~34 pt. Free Response (~19 predicting rxns, 15 pt lab); 15 Multiple Choice (2 pt. each) = 64 total points
Note: Students find this exam to be one of the most challenging. You need to practice until you feel proficient at each skill – writing net ionic equations
for all reaction types, completing difficult stoichiometry problems, assigning oxidation numbers and balancing redox reactions (in neutral, acidic or
basic soln). You also need to study your labs. You may not have done your lab work independently (cooperation is expected in lab groups) – make
sure you did are aware of your own understanding of the labs. Look through you pre-lab work, your calculations, and your post-lab questions. You
will be asked to complete calculations like those done in lab. You will also be asked to identify colors of solutions/chemicals used/seen in lab.
----------------------------------------------------------------------------------------------------------------------------- -----------------------------TEST NOTES:
1) Predicting Reactions: There will be a predicting reactions portion of the test. (You will get 8 reactions = 19 points)
a. Precipitate
b. Gas Formation
c. Acid/Base (Acids could be strong or weak; know how to write acid formulas given the name)
d. Redox
e. Combination
Note: Emphasis will be placed on
i. Metal oxide + water  base
the first four (a-d) reaction types.
ii. Nonmetal oxide + water  acid
iii. Metal oxide + nonmetal oxide  salt
f. Decomposition (see pink Molecular reactions sheet)
2) Multiple Choice (15 problems, 2 pts each = 30 points)
a. Stoichiometry – there are a significant number of “hard” stoichiometry problems. Make sure you’ve learned
strategies involved in solving stoichiometry problems in a proficient way.
b. Redox balancing – there are a significant number of redox equations to balance. Be sure you feel comfortable
enough with them to balance them proficiently.
c. Predicting Reactions – there will be some predicting reactions and descriptive chemistry as well.
3) Free Response – The free response questions will emphasize the two recent labs and will have one question that asks you
to analyze data from a lab you have not completed.
- % Cu in Brass
- Redox Titration.
***********************SEE REVIEW SHEET FOR MORE DETAILS**********************************
Essentials Question(s):
• How can you predict and write net ionic reactions for the following reaction types: acid/base,
precipitate, gas formation and oxidation/reduction?
• How can you complete stoichiometric calculations using volumes and molarity, including the use of
limiting reactants?
Chapter 4 Unit Objectives
Problem Set 4.1 – Aqueous Reactions – (precipitates, gas formation, acid-base) and Stoichiometry
1) Students will be able to write the net ionic equation for a precipitate reaction.
a) Solid ionic reactants are written together. (e.g. solid _____)
b) Aqueous ionic reactants are written as ions. (e.g. a “solution” of ____)
c) Soluble ionic products are written as ions.
d) Insoluble (low solubility) ionic products are written together.
e) All nitrate salts are soluble. MEMORIZE
f) All alkali and ammonium salts are soluble. MEMORIZE
2) Students will be able to write the net ionic equation for a gas formation reaction.
a) Rules above still apply.
b) H2CO3, H2SO3, NH4OH are unstable and decompose into water and CO2, SO2, and NH3 respectively. MEMORIZE
c) H2S is a gas. MEMORIZE
d) Gaseous compounds/elements are written as is (no ions present).
3) Students will be able to write the net ionic equation for an acid-base reaction.
a) Rules above still apply.
b) Strong acids written as ions. (HCl, HBr, HI, HClO4, HNO3, H2SO4, HClO3, HIO4)MEMORIZE
c) Weak acids written as molecules.
d) Water is a weak acid.
e) NH3 is a molecular weak base and written as NH3. MEMORIZE
f) All other bases (for now) are metal hydroxides which are ionic (see rules 1a,b,c,d)
4) Students will be able to complete stoichiometric calculations for reactions in aqueous solution.
a) Balanced equations are needed.
b) Follow 3-step mole method.
c) M = n/V (volume in liters)
d) Determine limiting reactants when given amounts of both reactants.
Problem Set 4.2,3– Redox Reactions –
1) Students will be able to assign oxidation numbers to atoms in elements, ions, or compounds.
2) Students will be able to balance redox reactions in neutral, acidic, or basic (4.3 only) solution.
3) Students will be able to identify common oxidizing and reducing agents and use them to predict the products in redox reactions.
a. MnO4- (purple) is reduced to Mn2+ (pale pink) in acidic solution.
b. MnO4- (purple) is reduced to MnO2 (black solid) in basic solution.
c. Cr2O72- (orange) is reducted to Cr3+ (green) in acidic solution.
d. Metals can be oxidized to metal ions. (Metal ions can be reduced back to metals.)
e. Metallic ions can be reduced to metallous ions or further to metals.
f. Metallous ions may be oxidized or reduced.
g. Halides are oxidized to halogens.
h. Halogens can be oxidized to hypohalits ions to halite ions to halate ions, to perhalate ions.
i. Any –ite polyatomic ion can be oxidized to an -ate polyatomic ion.
j. All of the above oxidations(d,e,g,i) can take place in the reverse direction as reductions (e.g. metal ions can be reduced
to metals).