AP Chemistry Summer Assignment
Future AP Chemistry Student,
Welcome to AP Chemistry. I am eagerly anticipating a great year of Chemistry. In
order to ensure the best start for everyone next fall, I have prepared a Summer
Assignment that reviews basic chemistry concepts. There is a multitude of
tremendous chemistry resources available via the Internet. With the ready access
to hundreds of websites either in your home or at the local library, I am confident
that you will have sufficient resources to prepare adequately for the fall semester.
There are a few old chemistry textbooks which can be picked up for your
reference. The reference text book for this course is Chemistry by Zumdahl,
Steven, and Susan Zumdahl. Published by Houghton Mifflin. A suggested study
book that is available from Mr. Edelman upon request is 5 Steps to a 5 AP
Chemistry,
You may contact me by email: (mredelman@ca.rr.com) this summer. I will do my
best to answer your questions ASAP. Taking a college level course in high school
is difficult, requires dedication, and is a great investment in your education so
prepare yourself for the future. Arrive ready to learn!!!
Part 1: Letter of Introduction (20 Points)
Your first digital assignment is to successfully send an email to your favorite AP Chemistry Teacher
by Sunday June 8th following these steps.
a) Use written, full sentences. Do not abbreviate words like you are on the Twitter machine or Myspace with a
friend.
Use spell check!
b) Make the Subject: AP Chem.: Introduction to “ < Insert your name here>”
c) Begin the email with a formal salutation, like “Mr. Edelman,”
d) Now introduce yourself (your name) and tell me a little about yourself like:
What do you like to do (hobbies, sports, music, interests, etc)? Do you have a job? Tell me a little bit about
what is important to you- friends, family, pets, etc. What are your strengths/weaknesses academically?
What is your career goal? Is this your first AP course? Why are you taking this class? What are your study
skills? Etc. Anything interesting?
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Part 2: Chemistry:Basics (30 points each)
Follow the instructions below to access chapter 1 Chemical Foundations and chapter 2 Atoms, Molecules, and
Ions both of which are pdf files. . Feel free to view the videos which will enhance learning process. Practice
solving the problems in the chapters.
The videos are found at the following website:
http://apchemistrynmsi.wikispaces.com/AP+Chemistry+Class+Lecture+Notes
+AND+instructional+videos
Utilize Internet Resources to complete the following problems. The URLs below represent a
fraction of the available chemistry addresses available. Please feel free to expand the list
and find other web sites that help prepare you for the coming year. We recommend that
you complete as many online quizzes as possible, take detailed notes, and practice the
items indicated in the packet.
Completed work must be submitted by the appointed dates. Late work will not be
accepted and could result in your removal from the class before school starts. The
goal of these assignments is to give you a basic introduction/review to things that
should be in your Chemistry toolkit when we start.
Let me know if there are any problems in submitting the assignment on time. A list of
books prescribed by the College Board has been provided for your reference. You do
not need all the books to complete the assignment. Any basic chemistry textbook can
help you find the information needed to complete the summer assignment.
General Chemistry Sites:
http://chemteam.info/ChemTeamIndex.ht
ml www.chemfiesta.com
www.chemistrygeek.com
http://www.collegeboard.com/ap/students/chemistry/index.html
www.chemmybear.com
Quizzes (multiple choice and free response):
http://www.adriandingleschemistrypages.com/apquiz.html
Study Cards:
http://www.chemmybear.com/stdycrds.html#APChem
How to submit each assignment? Send by email only.
You can copy and paste the questions for each assignment and submit.
For problems that need to be solved mathematically, scan your work and copy and paste. Or take a picture
Of your work and copy and paste into your work document. Title each assingnment as is. Ex: Assignment #1
2
Assignment #1 (Due: June 30th)
1.
Write the most common guidelines to determine significant figures (digits) with an example?
2.
Use factor labeling method to convert the following:
a. 515 m = ___ miles.
b. 200 in = ____ meters
c. 325 days = _____ seconds.
d. 20 gallons = _____ ml
e. 3 meters into centimeters
f. 10 kilometers into meters
g. 15,050 milligrams into grams
h. 3,264 milliliters into liters I . 9,674,444 grams into kilograms
3.
Classify each of the following as units of mass, volume, length, density, energy, or pressure.
a. mg
b. mL
3
c. cm
d. mm
3
e. kg/m
f. kJ
g. atm
h. cal.
4.
Most laboratory experiments are performed at room temperature at 25˚C. Express this temperature in:
a.
˚F
b.
K
5.
How many
a.
b.
c.
d.
e.
f.
g.
h.
i.
significant figures are in each of the following?
1.92 mm
0.030100 kJ
23
6.022 x10 atoms
460.00 L
3
0.00036 cm
100
1001
0.001
0.0101
6.
Record the
a.
b.
c.
d.
following in correct scientific notation:
350,000,000 cal
0.0000721 mol
0.0000000809 Ǻ
765,400,000,000 atoms
7.
Calculate the following to the correct number of significant figures.
3
a.
b.
c.
d.
e.
f.
g.
8.
9.
1.27 g / 5.296 cm
12.235 g / 1.01 L
12.2 g + 0.38 g
17.3 g + 2.785 g
2.1 x 3.21
200.1 x 120
17.6 + 2.838 + 2.3 + 110.77
Give the chemical symbols for the following elements:
a. Carbon
b. sulfur
c. Titanium
d. Nitrogen
e. Helium
Write the names for each of the elements symbols:
a. Na
b. Au c. Ag d. Sn e. Fe f. Hg g. K
3
10. A solid white substance A is heated strongly in the absence of air. It decomposes to form a new
white substance B and a gas C. The gas has exactly the same properties as the product obtained
when carbon is burned in an excess of oxygen. Based on these observations, can we determine
whether solids A and B and the gas C are elements or compounds? Explain your conclusions for
each substance.
11. Label each
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
of the following as either a physical process or a chemical process.
Corrosion of aluminum metal.
Melting of ice.
Pulverizing an aspirin.
Digesting a candy bar.
Explosion of nitroglycerin.
Milk turning sour.
Burning of paper.
Forming of frost on a cold night.
Bleaching of hair with hydrogen peroxide.
A copper wire is hammered flat.
Assignment #2 (Due: July 9nd )
12. Calculate the mass of O2 produced if 2.50 g KClO3 are completely decomposed by heating in the
following reaction:
2KClO3 →
2KCl + 3O2
13. Write the formula of the following compounds? (Use criss- cross method)
a. Calcium sulfate. b. Ammonium Phosphate
c. Lithium Nitrite
d. potassium perchlorate.
e. Barium Oxide
f. Zinc sulfide.
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14. Convert 3.57 atm to: (Using factor-labeling method)
a. mm Hg
b. pascals
15. Define the words: atomic number, atomic mass, mass number, molecular formula, structural formula,
empirical formula, isotopes, cation, anion, metalloid, allotrope, stoichiometry.
16. White gold is an alloy that typically contains 60.0% by mass gold and the remainder is platinum. If
175 g of gold are available, how many grams of platinum are required to combine with the gold to
form this alloy?
17. What is the empirical formula of a compound that contains 53.73% Fe and 46.27% of S ?
18. Determine the number of molecules in 2.23 mol of nitrogen (N2) molecules.
19. List the following has diatomic molecule, Molecular compound, Ionic compound, Atomic element.
a. F2
b. Cl2 c. C
d. NaCl
e. KF f. CO2 g. H2 h. Ag i. Rust (Fe2O3)
j. MgO
k. O2
l. I2
20. State the contribution of the following chemist in one line.
a. Democritus
b. Mendeleev
c. Henry Becquerel
e. J.J Thompson f.Faraday
g. Chadwick
j. Cavendish k. Madam Curie
21. What is the difference between
a. Chlorine atom and Chloride ion?
d. Roentgen
h. Millikan
i. Proust
b. Sodium atom and sodium ion.
22. How many grams of nitrogen are present in 2.3 moles of nitrogen gas (N2)?
23. Calculate the mass in grams of each of the following:
23
a. 6.02 x 10 atoms of Mg.
23
b. 3.01 x 10 Formula units of CaCl2.
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24. How do you distinguish:
a. An element from a compound.
b. An element from a mixture.
c. A true solution from a heterogeneous mixture.
d. Distillation from filtration.
25. An extensive property is one that depends on the amount of the sample. Which of the following
Properties are extensive?
a. volume b. density
c. temperature d. energy
e. melting point.
26. Define Acid, base and salt? Give some examples of each.
27. What is the difference between the Bronsted-Lowry, Lewis and Arrhenius definition of a base? An
Acid?
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Assignment #3 (Due: July 23th)
28. What mass of copper is required to replace silver from 4.00g of silver nitrate dissolved in water?
Cu(s) + AgNO3(aq) → Cu(NO3)2(s) + Ag(s).
29. Write the chemical formulas for the following compounds:
a. Calcium Carbonate b. Ammonium Phosphate c. Sodium Chloride d. Sodium Oxide e.
Calcium Sulfate f. Sodium Nitrite g. Magnesium Acetate h. Potassium cyanide i. Zinc (II) Nitrate
j. Iron (III) Phosphate k. Nickel (II) Fluoride
30. Define a. Law of conservation of mass.
b. Law of multiple proportion.
131
31. An isotope of Iodine used in thyroid disorders is I
has how many
a. Protons are in its nucleus?
b. Neutrons are in its nucleus?
c. Electrons are in an Iodine atom?
-1
d. Neutrons and protons are in the I formed from this isotope?
32. Mercury has an atomic mass of 200.59 amu. Calculate the
23
a. Mass of 3.0 x 10 atoms.
b. Number of atoms in one nanogram of Mercury.
33. Calculate the molar masses ( g/ mol) of
a. Ammonia ( NH3) b. Baking soda ( NaHCO3)) c. Osmium Metal (Os)
34. Convert the following to moles
a. 3.86 grams of Carbon dioxide.
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b. 6.0 x 10 g of Hydrazine (N2H4), a rocket propellant.
35. The molecular formula of morphine, a pain-killing narcotic, is C17H19NO3.
a. What is the molar mass?
b. What fraction of atoms in morphine is accounted for by carbon?
c. Which element contributes least to the molar mass?
36. Complete the list ionic compounds ( name or formula)
a. Cupric Hydroxide
b. Strontium Chromate
c. Ammonium Per chlorate
d. NaHCO3
e.
f.
g.
Fe2(CO3)3
Sodium Hydroxide.
Potassium Chloride.
5
37. Determine the formula mass for the following:
a. N2O5
b. CuSO4
C. Ca(HCO3)2 d. CaSO4.·2 H2O (water is connected)
38. Calculate the percentage by mass of the following compounds:
a. SO3
b. C2H3O3
c. Ammonium Nitrate.
39. Determine the empirical formula of the compounds with the following compositions by mass:
a. 10.4% C, 27. 8% S , 61. 7 % Cl
b. 21.7 % C, 9.6 % O, and 68.7 % F
Assignment #4 (Due: August 7th)
40. Write balanced chemical equations for the reactions of sodium with the following nonmetals to form
ionic solids.
a. Nitrogen b. Oxygen
c. Sulfur
d. Bromine
41. Balance the following equations as indicated.
a. __ AlF3 + __ Mg3N2  __ AlN + __ MgF2
.
b. __ C4H8 + __ O2  __ CO2 + __ H2O
c. __ Pb3(PO4)4+ __ Cr2S3  __ PbS2+ __ CrPO4
d. __ Fe2(SO4)3 + __ HCl  __ FeCl3+ __ H2O + __ SO3
e. __ C12H24 + __ O2  __ CO2 + __ H2O
f. __ Al + __O2  __ Al2O3
g. __ C9H16 + __ O2  __ CO2 + __ H2O
h. __ Cr(SO3)2 + __ H2  __ SO2 + __ Cr + __ H2O
i. __ C4H8O4 + __ O2  __ CO2 + __ H2O.
41. Define limiting reagent, theoretical yield, and actual yield.
43 Define the following terms:
a. Electrochemistry
b. Electrolysis
c. Voltaic Cell
44. Name the five different types of chemical reaction and give their general formulas.
45. Define solubility. Prepare a list of solubility rules for ionic compounds in water. ( online
resources)
(IMPORTANT)
45. Classify each of the substances as being soluble or insoluble in water.
6
a.
b.
c.
d.
e.
f.
g.
h.
KBr =
PbCO3 =
BSO3 =
zinc hydroxide =
sodium acetate =
silver iodide =
cadmium (II) sulfide =
zinc carbonate =
i.
j.
k.
l.
m.
n.
o.
p.
silver acetate =
copper (II) sulfide =
Mg3(PO4)2 =
KOH =
NiCl2 =
NH4OH =
Hg2SO4 =
PbI2 =
.
46. Identify the two new compounds which form if the solutions, as suggested by the following table, were mixed.
CIRCLE the names of the compounds which would precipitate from the solutions.
KBr
Na2CO3
CaS
NH4OH
AgNO3
BaCl2
Al(NO3)3
CuSO4
47. Define Oxidation number. Find the Oxidation number of
a. Carbon in CO2.
b. Sulfur in H2SO4.
c. Phosphorus in PO43d. Manganese in MnO42.
48. Define strong electrolyte, weak electrolyte, precipitation reactions and solubility?
49. Define the terms: Exothermic, endothermic reactions? How much heat in joules is required to raise the
o
o
temperature of 100g of water from 25 C to 100 C?
0
50. A piece of unknown metal with mass 14.9 g is heated to 100 C and dropped into 75.0 g of water at
0
20 C. The final temperature of the system is 28 degree Celsius. What is the specific heat of the metal?
51. What is a solute and solvent? Define Molarity, Molality, mole-fraction and Mass percent of a solution?
52. Calculate the molarity of a solution that contains 20.0grams of sodium hydroxide in 200ml?
53. How many grams of solute are present in 50.0 ml of 0.360 M sodium chloride?
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