Summer Assignment 2014
AP Chemistry is a very demanding course and you are expected to be prepared to face this task. AP Chemistry will be the FIRST AP Exam next year. By May6, 2013 we need to complete the equivalent of two full semesters of college chemistry + labs that are required by the College Board. In order to be prepared for this challenge it is necessary that you do some review work over the summer. This summer assignment will allow us to have a head start for the college level work required of each of you in the class.
Be prepared…….AP Chem requires 10-12 hours/week of work outside of class. This is only the beginning!!!
Part 1
READ the review material posted on the website.
KNOW the names and chemical element symbols for the first 36 elements in the Periodic Table (check your textbook)
METRICprefixes (Tutorial#1)
CONVERSION factors for the metric system (Tutorial #1)
NAME of all ions posted on the website(Tutorial #3, pages 5 and 6 and your textbook, page 65)and prefixes for naming covalent compounds (textbook, page 60-67,table 2.4). FIRST DAY QUIZ.
MEMORIZE all the solubility rules found in Tutorial #3. Check the website for the Table of solubility rules.
READ over the tutorials posted on the website.
Part 2
COMPLETEAssignments #1,#2, and #3and submit them at the specified times during the summer. Take these assignments seriously. I expect to receive your work on the assigned date. Mail the assignments to my homeor e-mail me (after scanning) at. In addition, email me and let me know that the assignment was sent. I will email a confirmation after receiving the work.
Part 3
REVIEWthe first three chapters in theAP textbook, Chemistry: The Central Science by Brown & LeMay, 10th edition. Read the Chapter and take notes and be sure to use an outline format- no full sentences. It might help you to use the Cornell Note Taking Template.
The outline and questions for each chapter are posted on the website (found at the end of the notes for the specified chapter). Be aware that the answers to the textbook assignment are included in the posted packets. If you have any difficulties with theseassignments make sure to make a note of it and ask questions at the beginning of the school year. I will move through these chapters very quickly, so asking questions in a timely fashion is crucial.
Remember: To receive credit for math problems, you must show all work!!!! Otherwise credit will not be given - even if a numerical answer is “correct”!
If you have any questions, see me before June 19th or e-mail me at . I will be most of the summer, but have internet access.
Cornell Note taking Websites
Review Website:
Summer Assignment Due Dates
Assignment #1: July 11
Assignment #2: August 15
Assignment #3: First day of School and see below
First Day of Class (9/3/2014)
COMPOSITION NOTEBOOK-for laboratory reports (maybe lined or with graphing grids (Staples or any other stationary store, check end of August sales). You will have a lab within the first 2 days of school- bring it day 1!
“Safety Rules and techniques for the Chemistry Lab” worksheet
(complete answers to the best of your knowledge – some may not be possible and you can fill those in as we go over them).
Graphing calculator
Expect a quiz (ions and solubility rules) on DAY 1 and test (Chapters 1,2, and 3)shortly after your return to school. There will be a yearly calendar of tests posted by the middle of August.
If you need help, email. Have a relaxing summer…… see you in September!
Mrs. Jacobus
Summer Assignment #1 (Due July 11, 2014)
Please place all answers on a separate sheet and snail or email itto me on the due dates!
I. Chemical Formulas
1. Write formulas for the following substances:
a. Barium sulfate
b. Ammonium chloride
c. Chlorine monoxide
d. Silicon tetrachloride
e. Magnesium fluoride
f. Sodium oxide
g. Sodium peroxide
h. Copper (I) iodide
i. Zinc sulfide
j. Potassium carbonate
k. Hydrobromic acid
l. Perbromic acid
m. Lead (II) acetate
n. Sodium permanganate
o. Lithium oxalate
p. Potassium cyanide
q. Iron (III) hydroxide
r. Silicon dioxide
s. Nitrogen trifluoride
t. Chromium (III) oxide
u. Calcium chlorate
v. Sodium thiocyanate
w. Cobalt (III) nitrate
x. Nitrous acid
y. Ammonium phosphate
z. Potassium chromate
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2. Name each of the following compounds (Give acid names where appropriate)
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a. CuSO4
b. PCl3
c. Li3N
d. BaSO4
e. N2F4
f. KCl04
g. NaH
h. (NH4)2Cr2O7
i. HNO2(aq)
j. Sr3P2
k. Mg(OH)2
1. Al2S3
m. AgBr
n. P4O10
o. HC2H3O2(aq)
p.CaI2
q.MnO2
r.Li2O
s.FeI3
t.Cu3(PO4)2
u.PCl3
v.NaCN
w.Cs3N
x.Zn(NO3)2
y.N20
z.HF(aq)
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II. Chemical Equations
Determine and write the type of reaction, predict the products, and write a balanced chemical equation for each of the following, as shown in the example:
Example: Solutions of silver nitrate and magnesium iodide are combined.
Answer: This is a double replacement reaction.
2AgNO3 + MgI2 2AgI (s) + Mg(NO3)2
1. Ammonium sulfate reacts with barium nitrate.
2. Zinc metal is added to a solution of copper (II) chloride
3. Propane gas (C3H8) is burned in excess oxygen.
4. Dinitrogen tetraoxide gas is added to distilled water.
5. Solid calcium chlorate is heated strongly.
6. Sodium hydroxide solution is added to a solution of iron (III) bromide.
7. Chlorine gas is bubbled through a solution of sodium bromide.
8. Solutions of lead nitrate and calcium iodide are combined.
9. Sulfuric acid is combined with solid magnesium hydroxide.
10. Solid barium oxide is added to distilled water.
11. Isopropyl alcohol (C3H7OH) is burned in air.
12. Iron metal shavings are added to hydrochloric acid.
13. Solid sodium carbonate is heated in a crucible.
14. Solid aluminum hydroxide is added to perchloric acid.
15. Sodium metal is added to distilled water.
III. Metric Conversions, Dimensional Analysis, Atomic Structures
1. A certain brand of coffee is offered for sale at $7.26 for a 3-lb can or $5.42 for a
1-kg can- which is the better buy?
2. A sprinter runs the 100-yd dash in 9.3 s. What would his time be for a 100-m run if he ran at the same rate?
3. An English unit of mass used in pharmaceutical work is the grain (gr). 15 gr = 1.0 g. An aspirin tablet contains 5.0 gr of aspirin. A 145-lb person takes two aspirin tablets.
a) What is the quantity of aspirin taken, expressed in milligrams?
b) What is the dosage rate of the aspirin, expressed in milligrams of aspirin per kilogram of body weight?
4. Many times errors are expressed in terms of percentage. The percentage error is the absolute value of the difference of the accepted value and the experimental value, divided by the accepted value, and multiplied by 100.
Percent Error = |accepted value – experimental value| x 100
accepted value
Calculate the percent error for the following measurements.
a) The density of an aluminum block determined in an experiment was 2.64 g/mL. (Accepted value = 2.70 g/mL)
b) The experimental determination of iron in iron ore was 16.48%. (Accepted value = 16.12%)
c) A balance measured the mass of 1.0000 g standard as 0.9981 g.
5. How many protons, neutrons, and electrons are in each of the following?
6. The density of water is 1.0 g/cm3. Express this value in units of kg/m3 and lb/ft3.
7. Diamonds are measured in carats, and 1 carat = 0.200 g. The density of diamond is 3.51g/cm3. What is the volume of a 5.0 carat diamond?
8. In the opening scenes of the movie “Raiders of the Lost Ark,” Indiana Jones tries to remove a gold idol from a booby-trapped pedestal. He replaces the idol with a bag of sand of approximately equal volume. (Density of gold = 19.32 g/mL; density of sand ≈ 2 g/mL.)
a) Did he have a reasonable chance of not activating the mass-sensitive booby trap?
b) In a later scene he and an unscrupulous guide play catch with the idol. Assume that the volume of the idol is about 1.0 L. If it were solid gold what mass would the idol have? Is playing catch with it plausible? Why or why not?
9. An experiment was performed in which an empty 100 mL graduated cylinder was weighed. It was weighed once again after it had been filled to the 10.0 mL mark with dry sand. A 10 mL pipet was used to transfer 10.00 mL of methanol to the cylinder. The sand-methanol mixture was stirred until bubbles no longer emerged from the mixture and the sand looked uniformly wet. The cylinder was then weighed again. Use the data obtained from this experiment (and displayed below) to find the density of dry sand, the density of methanol, and the density of sand particles. Does the bubbling that occurs when the methanol is added to they dry sand indicate that the sand and methanol are reacting?
Mass of cylinder plus wet sand45.2613 g
Mass of cylinder plus dry sand37.3488 g
Mass of empty cylinder 22.8317 g
Volume of dry sand10.0 mL
Volume of sand + methanol17.6 mL
Volume of methanol 10.00 mL
10) The German chemist Fritz Haber proposed paying off the reparations imposed against Germany after World War I by extracting gold from seawater. Given that (a) the amount of the reparations was 28.8 billion dollars, (b) the value of gold at the time was about $21.25 per troy ounce (12 troy ounces = 1 lb), and (c) gold occurs in seawater to the extent of 4.67 x 1017 atoms per ton of seawater (1 ton = 2000 lb), how many cubic kilometers of seawater would have had to be processed to obtain the required amount of gold? Assume that the density of seawater is 1.03 g/cm3.
12) A water solution that is 15% sucrose, by mass, has a density of 1.059 g/cm3. What mass of sucrose, in grams, is contained in 3.05 L of this solution?
*13). Vanillin ( used to vanilla flavor ice cream and other foods) is the substance whose aroma the human nose detects in the smallest amount. The threshold limit is
2.0 x 10-11 g/liter of air. If the current price of 50 g of vanillin is $112, determine the cost to supply enough vanillin so that the aroma could be detectable in a large aircraft hangar of volume 5.0 x 107 ft3.
*14) A resting adult requires about 240. mL of pure oxygen/min and breathes about 12 times every minute. If inhaled air contains 20.% oxygen by volume and exhaled air 16 %, what is the volume of air/breath? ( Assume that the volume of inhaled air is equal to that of exhaled air.)
Summer Assignment #2: Stoichiometry (Due August 15, 2014)
These problems must be worked out on a separate page and all work shown for credit.
1. Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the compound to be 7.74% H by mass. Find the empirical and molecular formulas of benzene.
2. Find the mass percent of nitrogen in each of the following compounds:
a. NO
b. NO2
c. N2O4
d. N2O
3. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide gas.
a. Write a balanced chemical equation for this reaction.
b. How many grams of calcium oxide will remain after 12.25 g of calcium carbonate is completely decomposed?
c. What volume of carbon dioxide gas is produced from this amount of calcium carbonate? The gas is measured at 0.95 atm and 10˚C.
4. Hydrogen gas and bromine gas react to form hydrogen bromide gas.
a. Write a balanced chemical equation for this reaction.
b. How many grams of hydrogen bromide gas can be produced from 3.2 g of hydrogen gas and 9.5 g of bromine gas?
c. How many grams of which reactant is left unreacted?
d. What volume of HBr, measured at STP, is produced in b)?
5. When ammonia gas (NH3), oxygen gas (O2), and methane gas (CH4) are combined, the products are hydrogen cyanide gas (HCN) and water.
a. Write a balanced chemical equation for this reaction.
b. Calculate the mass of each product produced when 225 g of oxygen gas is reacted with an excess of the other two reactants.
c. If the actual yield of the experiment in b) is 105 g of HCN, calculate the percent yield.
6. A 2.29 g sample of an unknown acid is dissolved in 1.0 L of water. A titration required 25.0 mL of 0.500 M NaOH to completely react with all the acid present. What is the molar mass of the acid?
7. What mass of aluminum hydroxide is produced when 50.0 mL of 0.200 M Al(NO3)3 reacts with 200.0 mL of 0.100 M KOH?
8. Cinnamic acid contains only carbon, hydrogen and oxygen, and is found by analysis to be 73.0% C and 5.4% hydrogen. In a titration, 18.02 mL of 0.135 M NaOH is found to neutralize 0.3602 g of cinnamic acid.
a. Find the empirical formula of this compound.
b. Find the molar mass of this compound.
c. Write the molecular formula for this compound.
9. Potassium nitrate decomposes when heated, forming potassium nitrite and oxygen gas.
a. Write a balanced chemical equation for this reaction.
b. What mass of KNO3 would be needed to produce 18.4 L of oxygen gas, measured at 775 mm Hg and 15˚C?
c. What mass of KNO2 would also be produced?
10. A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 16.01 mg CO2 and 4.37 mg H2O. The molar mass of the compound is 176.1 g/mol. What are the empirical and molecular formulas of the compound?
Summer Assignment #3 (Due September 3, 2014)
Writing Net Ionic Equations (
Your first review assignment was about writing formulas and balancing chemical equations. The AP Chemistry Exam includes three reactions. The equations for these reactions (when appropriate) must be written in net ionic form, be balanced, and you must be able to recognize types of reactions and then predict the products. In addition, you will be asked to answer a few questions about each reaction. In this exercise we will concentrate mostly on writing balanced net ionic equations (only when appropriate) and recognizing the type of the reaction. Use the tutorial posted on the e-board to guide you in this assignment.
Exercise #1: Synthesis and Decomposition Reactions:
Predict and balance the following synthesis and decomposition reactions. Use abbreviations to indicate the phase (aq, s, l, or g) of reactants and products where possible. Write answers on a separate page!
1. A sample of calcium carbonate is heated.
2. Sulfur dioxide is bubbled through water.
3. Solid potassium oxide is added to a container of carbon dioxide gas.
4. Liquid hydrogen peroxide is warmed.
5. Solid lithium oxide is added to water.
6. Molten aluminum chloride is electrolyzed.
7. A pea-sized piece of sodium is added to a container of iodine vapor.
8. A sample of carbonic acid is heated.
9. A sample of potassium chlorate is heated.
Exercise #2: Single Replacement Reactions
Using the activity series, predict and balance the following single replacement reactions. Use abbreviations to indicate the appropriate phase of reactants and products where possible. Write answers on a separate page! Note: Not all reactions will occur. For those, write “No Reaction.” (
1. A piece of copper is dropped into a container of water.
2. Liquid bromine is added to a container of sodium iodide crystals.
3. An aluminum strip is immersed in a solution of silver nitrate.
4. Zinc pellets are added to a sulfuric acid solution.
5. Fluorine gas is bubbled into a solution of silver nitrate.
6. Magnesium turnings are added to a solution of lead (II) acetate.
7. Iodine crystals are added to a solution of sodium chloride.
8. Calcium metal is added to a solution of nitrous acid.
9. A pea-sized piece of lithium is added to water.
10. A solution of iron (III) chloride is poured over a piece of platinum wire.
Exercise 3- Formation of a Precipitate
Predict and balance the following metathesis reactions based on the solubility of the products. Use the abbreviations (aq) and (s) for the reactants and the products. All reactants are aqueous. Write answers on a separate page! Note: Some of these reactions do not go to completion! Correct molecular formulas must be written for both reactants and products before an equation may be balanced.
1. silver nitrate + potassium chromate
2. ammonium chloride + cobalt (II) sulfate
3. lithium hydroxide + sodium chromate
4. zinc acetate + cesium hydroxide
5. ammonium sulfide + lead (II) sulfide
6. iron (III) sulfate + barium iodide
7. chromium (III) bromide + sodium nitrate
8. rubidium phosphate + titanium (IV) nitrate
9. ammonium carbonate + nickel (II) chloride
10. tin (IV) nitrate + potassium sulfite
Exercise 4- Formation of a Gas
Predict and balance the following metathesis reaction based on the solubility of the products. Use the abbreviations (aq), (s), (l), and (g) for the reactants and the products. All reactants are aqueous unless otherwise stated. Write answers on a separate page!
1. ammonium sulfate and potassium hydroxide are mixed together
2. ammonium sulfide is reacted with hydrochloric acid
3. cobalt (II) chloride is combined with silver nitrate
4. solid calcium carbonate is reacted with sulfuric acid
5. potassium sulfite is reacted with hydrobromic acid
6. potassium sulfide is reacted with nitric acid
7. ammonium iodide + magnesium sulfate
8. solid titanium (IV) carbonate + hydrochloric acid
9. solid calcium sulfite + acetic acid
10. strontium hydroxide + ammonium sulfide
Exercise 5: Mixed Methathesis Reaction (Double Replacement) Problems
Predict and balance the following metathesis reactions based on the solubility of the products. Use the abbreviations (aq), (s), (l), (g) for the reactants and the products. All reactants are aqueous unless otherwise stated. Write answers on a separate page!
1. carbon dioxide gas is bubbled through a solution of lithium hydroxide
2. sodium nitrite is reacted with hydrochloric acid
3. carbon dioxide gas is reacted with solid potassium oxide
4. solid magnesium oxide is reacted with solid potassium oxide
5. equal numbers of moles of potassium hydroxide and phosphoric acid react
6. sodium fluoride reacts with dilute nitric acid
7. ammonium carbonate + potassium bromide
8. oxalic acid (0.1 M) reacts with an equal volume of cesium hydroxide (0.1 M)
9. silver nitrate + sodium chromate
Exercise 6: Mixed Reactions (All Types)
Write balanced molecular, overall ionic equations for the following reactions. Write answers on a separate page!
1. aqueous nickel (II) nitrate + aqueous cesium hydroxide
2. equal volumes of equal molar concentrations of sulfuric acid and sodium hydroxide
3. solid potassium chlorate is strongly heated
4. potassium tartrate solution + water
5. solid lithium metal is added to water
6. aqueous solutions of magnesium nitrate and sodium bromide are mixed together
7. aqueous solutions of oxalic acid and excess potassium hydroxide
8. solid cobalt (II) hydroxide + hydroiodic acid
9. aqueous solutions of manganese (II) sulfate undergoing hydrolysis
10. aqueous sodium carbonate + chlorous acid
11. aqueous solutions of potassium phosphate and excess hydrobromic acid
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