AP Chemistry Summer Assignment
WARNING: AP Chemistry is an ADVANCED PLACEMENT course that will give you the experience of a
college course during your high school career. It is the equivalent of taking a full year of a college course at a
university.
DO NOT continue with AP CHEM if any of the following criteria apply to you (Be Honest):
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Don’t have a strong work ethic
Don’t study or complete assignments on time
Not willing to seek additional help outside of
class when needed
Not able to handle feeling frustrated with
difficult concepts
Don’t fully read instructions/directions/text
Cannot manage or prioritize your time
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Not interested in attending college
Not willing to put in late hours, sacrifice social
activities, etc. to succeed
Blame others for areas that you fail in, do not
take ownership of your mistakes
Not willing/able to seek out/learn information
that I do not know on your own
 This is not meant to discourage you from challenging yourself with this AP course, but a reality
check of the hard work and dedication that will be required of you to succeed.
So Why Summer Work?
This class covers a full year of chemistry at a university. Let's take a look at an example. At my college (Cal Poly)
Chemistry 127,128, and 129 meets for 3hrs/week for lecture and 3hrs/week for lab. Each quarter is 10 weeks long
(not including finals) so that is 90 hours of lecture and 90 hours of lab for a total of 180 hours in class.
At Laurel High School we start the first week in August and the AP test is on the first Monday in May. That is 33
weeks not including winter and spring break. We meet for 4 hours per week (assuming we don't lose time to
assemblies, bad weather, holidays, etc. - which we do). That is a total of 125 hours in class.
The difference is ~55 hours less time – to cover the same amount of material; that has to be made up
during the summer, at home, on Saturdays, and during breaks via homework assignments, studying, projects, etc.
CONSEQUENCES for not COMPLETING the summer assignment
- If this is not turned in fully completed by the 1st day of school at the beginning of the AP Chem class period you will
be dropped from the course and will have to change your schedule.
- You are expected to have a firm understanding of this material from the first day of school. These topics will be
quickly reviewed then used at a deeper, more complex level. We don’t have time for me to teach it to you.
- If you struggle greatly with this assignment you may want to rethink taking this course.
- This assignment will take time to complete, it cannot get done the day or even just the week before school starts.
TO REMAIN IN AP CHEM…
- If you complete this assignment you are still not guaranteed to remain in AP CHEM
- To show that you thoroughly understood the topics in the assignments and are capable of succeeding you must earn
a minimum score on the pre test that will be given the first week of school. Those who do not pass with the minimum
required score will be dropped from AP CHEM and have to change their schedule.
ATTITUDE IS EVERYTHING!
As I have explained AP CHEM is a tough, challenging course, but it can also be a fun, exciting course that will better
prepare you for your college career. The more you are prepared and putting forth effort to comprehend the
material the more we can do to enjoy it such as labs, activities, and special projects.
REQUIRED MATERIALS: Paper, pencil, periodic table, calculator, computer/internet access
NO COPYING: if any plagiarized work is used, you will be immediately dropped from the course.
AP CHEM SUMMER ASSIGNMENT CHECKLIST:
READ ALL DIRECTIONS CAREFULLY – it is your responsibility to read and complete all
directions as stated. If you skim directions and do something wrong, that is on you!
 PART 1: REMIND SIGN UP
o Can do text messages OR e-mail
 PART 2: TEXTBOOK ASSIGNMENTS
Checkout an AP Chemistry Book from the library to have over break – this is checked out in YOUR NAME
so it is YOUR RESPONSIBILITY to keep up with it and return it when the time comes.
o Read & Outline Chapters 1-2: (Look online for proper outlining styles and formats; You can
YouTube “How to Outline Your Textbook”; ONLY write the down the key points/facts/vocab NOT
every detail.
 Ch. 1  25, 27, 28, 39, 41, 45, 49, 57, 61, 76
 Ch. 2  21-25, 31, 32, 49, 50, 61-70, 73, 87
 PART 3: MEMORIZATION
o Symbols and Names of Elements #1-90
o Polyatomic Ions: formulas, names, and their charges
 PART 4: CHEM 1 REVIEW WORKSHEETS
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1. Significant Figures and Dimensional Analysis
2. Structure of the Atom and the Periodic Table
3. Naming Inorganic Compounds
4. Atomic and Molecular Masses
5. Balancing Equations & Patterns of Reactivity
6. The Mole
7. Empirical and Molecular Formulas
8. Chemical Equations and Calculations
9. Limiting Reactants & Theoretical Yield
10. Personal Statement
RESOURCES IF YOU NEED HELP/REVIEW/EXAMPLES:
 Videos (search by topic on YouTube):
o Khan Academy
o Brightstorm
o Bozeman Science
o Tyler Dewitt
 Textbook
o Use index to look up location of the material
 Google
o Search topic for how to's
o Search for worksheets for examples/more practice
 Contact me
o Email me: rhooper@laurelschools.org (I should get back to you in a day or two)
o Phone: 601-340-4044
o Help Sessions – I will be at the school for summer school from 8:30-11:30am during the
week throughout the month of June
PART 2: REMIND SIGN UP
PART 3: MEMORIZATION
Name
Sym
Hydrogen
H
Chromium
Cr
Silver
Ag
Ytterbium
Yb
Helium
He
Manganese
Mn
Cadmium
Cd
Lutetium
Lu
Lithium
Li
Iron
Fe
Indium
In
Hafnium
Hf
Beryllium
Be
Cobalt
Co
Tin
Sn
Tantalum
Ta
Boron
B
Nickel
Ni
Antimony
Sb
Tungsten
W
Carbon
C
Copper
Cu
Tellurium
Te
Rhenium
Re
Nitrogen
N
Zinc
Zn
Iodine
I
Osmium
Os
Oxygen
O
Gallium
Ga
Xenon
Xe
Iridium
Ir
Fluorine
F
Germanium
Ge
Caesium (Cesium)
Cs
Platinum
Pt
Neon
Ne
Arsenic
As
Barium
Ba
Gold
Au
Sodium
Na
Selenium
Se
Lanthanum
La
Mercury
Hg
Magnesium
Mg
Bromine
Br
Cerium
Ce
Thallium
Tl
Aluminum
Al
Krypton
Kr
Praseodymium
Pr
Lead
Pb
Silicon
Si
Rubidium
Rb
Neodymium
Nd
Bismuth
Bi
Phosphorus
P
Strontium
Sr
Promethium
Pm
Polonium
Po
Sulfur (Sulphur)
S
Yttrium
Y
Samarium
Sm
Astatine
At
Chlorine
Cl
Zirconium
Zr
Europium
Eu
Radon
Rn
Argon
Ar
Niobium
Nb
Gadolinium
Gd
Francium
Fr
Potassium
K
Molybdenum
Mo
Terbium
Tb
Radium
Ra
Calcium
Ca
Technetium
Tc
Dysprosium
Dy
Actinium
Ac
Scandium
Sc
Ruthenium
Ru
Holmium
Ho
Thorium
Th
Titanium
Ti
Rhodium
Rh
Erbium
Er
Vanadium
V
Palladium
Pd
Thulium
Tm
Polyatomic Ions List
 FLASH CARDS & FREQUENT PRACTICE WORK BEST TO MEMORIZE THESE
 MUST KNOW THE SYMBOLS AND THE CHARGES!
 LOOK ONLINE FOR “HOW TO USE FLASHCARDS” EFFECTIVELY
+ 1 Ions
Name
-2 Ions
NH4+1
ammonium ion
CO3-2
carbonate
CrO4-2
chromate
-1 Ions
Cr2O7-2 dichromate
CN-1
cyanide
O2-2
peroxide
OH-1
hydroxide
SO3-2
sulfite
ClO-1
hypochlorite
SO4-2
sulfate
ClO2-1
chlorite
C2O4-2
oxalate
ClO3-1
chlorate
ClO4-1
perchlorate
-3 Ions
C2H3O2-1 / CH3COO-1 acetate
PO4-3
phosphate
MnO4-1
permanganate
BO3-3
borate
NO2-1
nitrite
NO3-1
nitrate
+2 Ions
HCO3-1
bicarbonate
Hg2+2
mercury (I)
Hg+2
mercury (II)
or
hydrogen carbonate
SCN-
thiocyanate
Name: ________________________________
PART 4
DIRECTIONS: For each problem below show your work. Always use units and box your final answer.
Attach all additional papers with any work shown, clearly numbered.
Anything you get stuck on you can review online via these YouTube channels:
- Khan Academy
- Brightstorm
- Tyler Dewitt
- Bozemann Science
AP Chemistry Worksheet 1: Significant Figures and Dimensional Analysis
1. Round each of the following numbers to four significant figures, and express the result in scientific notation:
2.
a. 300.235800
_______________
b. 456,500
_______________
c. 0.006543210
_______________
d. 0.000957830
_______________
e. – 0.035000
_______________
Carry out the following operations, and express the answers with the appropriate number of significant
figures:
a. 1.24056 + 75.80
_______________
b. 23/67 - 75
_______________
c. 890,000 x 112.3
_______________
d. 78,132 / 2.50
_______________
3. Perform the following conversions: (You need to go online to look up some conversion factors between
metric and English units.)
a. 8.60 mi to m
_______________
b. 3.00 days to s
_______________
c. $1.55/gal to dollars per liter
_______________
d. 75.00 mi/hr to m/s
_______________
e. 55.35 ft3 to cm3
_______________
4. The density of pure silver is 10.5 g/cm3 at 20oC. If 5.25 g of pure silver pellets are added to a graduated
cylinder containing 11.2 mL of water, to what volume level will the water in the cylinder rise? (Water: 1 mL=
1 cm3)
5. The density of air at ordinary atmospheric pressure and 25oC is 1.19 g/L. What is the mass, in kilograms, of
the air in a room that measures 12.5 x 15.5 x 8.0 ft?
AP Chemistry Worksheet 2: Structure of the Atom and the Periodic Table
1. What were the main points of Dalton’s Atomic Theory? Which of these points are still accepted today? Which ones do
we no longer accept, and why?
2. Summarize the evidence used by J.J. Thomson to argue that cathode rays consist of negatively charged particles.
3. Let’s pretend you are holding two atoms of carbon that are isotopes. Describe what the two atoms have in common
and what they have different.
4. Fill in the gaps in the following table, assuming each column represents a neutral atom:
Symbol
39
19K
Protons
25
Neutrons
30
Electrons
82
64
48
56
Mass #
137
207
5. Write the correct symbol, with both superscripts and subscripts, for each of the following :
(a)
the isotope of sodium with mass 23
_______________
(b)
the atom of vanadium that contains 28 neutrons
_______________
(c)
the isotope of chlorine with mass 37
_______________
(d)
an atom of magnesium that has an equal number of protons and neutrons
_______________
6. Give the name and the common charge for elements
found in each of these groups of the Periodic Table:
7. Describe where each type of element
is found on the Periodic Table.
(a)
Group 1
(a) Metals
(b)
Group 2
(b) Non-metals
(c)
Group 17
(c) Transition metals
(d)
Group 18
(d) Lanthanides
(e) Actinides
AP Chemistry Worksheet 3: Naming Inorganic Compounds
1. Give the name for each of the following ionic compounds:
a. AlF3
f.
b. Fe(OH)2
g. Ca(C2H3O2)2
c.
h. Cr2(CO3)3
Cu(NO3)2
Hg2S
d. Ba(ClO4)2
i.
K2CrO4
e. Li3PO4
j.
(NH4)2SO4
2. Write the chemical formula for each of the following compounds:
a. copper (I) oxide
e. mercury (I) bromide
b. potassium peroxide
f.
c.
g. sodium hypobromite
aluminum hydroxide
iron (III) carbonate
d. zinc nitrate
3. Give the name or chemical formula, as appropriate, for each of the following acids:
a. HBrO3
d. hypochlorous acid
b. HBr
e. iodic acid
c.
f.
H3PO4
sulfurous acid
4. Give the name or chemical formula, as appropriate, for each of the following molecular substances:
a. SF6
d. dinitrogen tetroxide
b. IF5
e. hydrogen cyanide
c.
f.
XeO3
tetraphosphorous hexasulfide
5. Write the balanced chemical equation for each reaction given below.
a. Zinc carbonate can be heated to form zinc oxide and carbon dioxide
b. On treatment with hydrofluoric acid, silicon dioxide forms silicon tetrafluoride and water.
c.
Sulfur dioxide reacts with water to form sulfurous acid.
d. Liquid butane fuel (C4H10) burns in the presence of oxygen gas.
e. Perchloric acid reacts with cadmium to form cadmium perchlorate and a gas.
f.
A solution of sodium bromide reactions with a solution of vanadium (III) nitrate to form a brightly colored
precipitate.
AP Chemistry Worksheet 4: Atomic and Molecular Masses
For each problem below, write the equation and show your work. Always use units and box in your final answer.
1. What isotope is used as the standard in establishing the atomic mass scale?
2. The atomic weight of magnesium is reported as 24.3, yet no atom of magnesium has the mass of 24.3 amu. Explain.
3. Only two isotopes of copper occur naturally, Cu-63 (abundance 69.09 percent) and Cu-65 (abundance 30.91 percent).
Calculate the average atomic mass of copper.
4. Determine the molar mass of each of the following compounds:
a. N2O5
b. FeCO3
c.
Ca(C2H3O2)2
d. (NH4)3PO4
e. sodium nitrate
f.
copper (II) sulfate
g. disilicon hexabromide
5. Calculate the percentage by mass of oxygen in the following compounds:
a. NO2
b. CH3COOCH3
c.
Cr(NO3) 3
d. (NH4) 2CO3
AP Chemistry Worksheet 5: Balancing Equations & Patterns of Reactivity
NOTE: You may have to research the 5 types of chemical reactions we went over in class to properly figure out
the products of some of these reactions.
1. Balance the following equations:
a.
CO (g)
+
O2( g)
b.
N2O5 (g)
c.
PCl5 (l)
+
H2O (l)
-->
H3PO4 (aq)
d.
CH4 (g)
+
Br2 (g)
-->
CBr4 (l)
e.
C5H10O2 (l)
f.
Cr(OH) 3 (s)
+
-->
H2O (l)
+
+
CO2 (g)
-->
O2 (g)
-->
HClO4 (aq)
HNO3 (aq)
+
CO2 (g)
-->
+
HCl (aq)
HBr (g)
+
H2O (l)
Cr(ClO4) 3 (aq)
+
H2O (l)
2. Write balanced chemical equations to correspond to each of the following descriptions (include phases):
a. Solid calcium carbide, CaC2, reacts with water to form an aqueous solution of calcium hydroxide and acetylene
gas, C2H2.
b. When solid potassium chlorate is heated, it decomposes to form solid potassium chloride and oxygen gas.
c.
Solid zinc metal reacts with sulfuric acid to form hydrogen gas and an aqueous solution of zinc sulfate.
d. When liquid phosphorous trichloride is added to water, it reacts to form a solution of phosphorous acid and
hydrochloric acid.
e. When hydrogen sulfide gas is passes over solid hot iron (III) hydroxide, the reaction produces solid iron (III)
sulfide and gaseous water.
3. a. What products form when a hydrocarbon is completely combusted in air?
b. Write a balanced chemical equation for the combustion of octane, C8H18 (l), in air.
c.
How can you determine the chemical formula of the product formed when the metallic element calcium
combines with the nonmetallic element oxygen, O2?
d. Write the balanced chemical equation for the reaction described in (c).
4. Write a balanced chemical equation for the reaction that occurs when
a. the hydrocarbon heptane, C7H16 (l), is combusted in air
b. the gasoline additive MTBE (methyl tertiary-butyl ether), C5H12O (l), burns in air
c.
Rb (s) reacts with water
d. Mg(s) reacts with Cl2 (g)
5. Balance the following equations, and indicate what type of reaction each one is:
a.
Al (s)
+
b.
C2H4 (g)
c.
Li(s)
d.
PbCO3 (s)
-->
e.
C7H8O2 (l)
+
+
Cl2 (g)
+
-->
O2 (g)
N2 (g)
AlCl3 (s)
-->
-->
CO2 (g)
+
H2O (l)
Li3N (s)
PbO (s)
O2 (g)
____________________
-->
+
____________________
____________________
CO2 (g)
CO2 (g)
+
____________________
H2O (l)
____________________
AP Chemistry Worksheet 6: The Mole
1. The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet, is C14H18N2O5.
a. What is the molar mass of aspartame?
b. How many moles of aspartame are present in 1.00 mg of aspartame? (1000 mg = 1g)
c.
How many molecules of aspartame are present in 1.00 mg of aspartame?
d. How many hydrogen atoms are present in 1.00 mg of aspartame?
2. A sample of glucose, C6H12O6, contains 2.03 x 1021 atoms of carbon.
a. How many atoms of hydrogen does it contain?
b. How many molecules of glucose does it contain?
c.
How many moles of glucose does it contain?
d. What is the mass of the sample in grams?
3. Calculate the following amounts:
a. How many moles of chloride ions are in 0.0750 g of magnesium chloride?
b. What is the mass, in grams, of 3.50 x 10-3 mol of aluminum sulfate?
c.
What is the mass, in grams, of 1.75 x 1020 molecules of caffeine, C8H10N4O2?
d. What is the molar mass of cholesterol if 0.00105 mol weigh 0.406 g?
4. Calculate the number of molecules in:
a. 0.0666 mol propane, C3H8, a hydrocarbon fuel
b. A 50.0 mg tablet of acetaminophen, C8H9O2N, an analgesic solid under the name of Tylenol
c.
A tablespoon of table sugar, C12H22O11, weighing 10.5 g
5. The allowable concentration level of vinyl chloride, C2H3Cl, in the atmosphere in a chemical plant is 2.0 x 10-6 g/L.
a. How many moles of vinyl chloride in each liter does this represent?
b. How many molecules per liter is this?
AP Chemistry Worksheet 7: Empirical and Molecular Formulas
For each problem below, write the equation and show your work. Always use units and box in your final answer.
1. Determine the empirical formula of each of the following compounds if a sample contains
a. 0.104 mol K, 0.052 mol C, and 0.156 mol O
b. 5.28 g Sn and 3.37 g F
c.
87.5 percent N and 12.5 percent H by mass
2. Determine the empirical formulas of the compounds with the following compositions by mass
a. 10.4 percent C, 27.8 percent S, and 61.7 percent Cl
b. 21.7 percent C, 9.6 percent O, and 68.7 percent F
3. What is the molecular formula of each of the following compounds?
a. empirical formula CH2, molar mass = 84 g/mol
b. empirical formula NH2Cl, molar mass = 51.5 g/mol
4. Determine the empirical and molecular formulas of each of the following substances:
a. Ibuprofen, a headache remedy contains 75.69 percent C, 8.80 percent H, and 15.51 percent O by mass; molar
mass about 206 g
b. Benzene contains only carbon and hydrogen and is 7.74% hydrogen by mass. The molar mass of benzene is
78.1 g/mol.
5. Many homes in rural America are heated by propane gas, a compound that contains only carbon and hydrogen.
Complete combustion of a sample of propane produced 2.641 g of carbon dioxide and 1.442 g of water as the only
products. Find the empirical formula of propane. (Hint: Figure out how many moles of C and H were produced. They
all came from the fuel.)
6. (This is probably the hardest problem in the whole packet!) Menthol, the substance we can smell in mentholated
cough drops, is composed of C, H, and O. A 0.1005 g sample of menthol is combusted, producing 0.2829 g of CO2
and 0.1159 g of H2O.
a. What is the empirical formula for menthol?
b. If the compound has a molar mass of 156 g/mol, what is its molecular formula?
AP Chemistry Worksheet 8: Chemical Equations and Calculations
1. Why is it essential to use balanced chemical equations in solving stoichiometry problems?
2. The fermentation of glucose, C6H12O6, produces ethyl alcohol, C2H5OH, and CO2 as shown here:
C6H12O6 (aq)
-->
2 C2H5OH(aq)
+
2 CO2 (g)
a. How many moles of CO2 are produced when 0.300 mol of C6H12O6 reacts in this fashion?
b. How many grams of C6H12O6 are needed to form 2.00 g of C2H5OH?
c.
How many molecules of CO2 form when 2.00 g of C2H5OH are produced?
3. Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide.
a. Write the balanced chemical equation for this reaction.
b. How many grams of aluminum hydroxide are obtained from 10.5 g of aluminum sulfide?
4. Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements:
2 NaN3 (s) -->
Na(s)
+
3 N2 (g)
a. How many moles of N2 are produced by the decomposition of 1.50 moles of NaN3?
b. How many grams of NaN3 are required to form 5.00 g of nitrogen gas?
c.
How many grams of NaN3 are required to produce 10.0 L of nitrogen gas if the gas has a density of 1.25 g/L?
5. A piece of aluminum foil 0.550 mm thick and 1.00 cm square is allowed to react with bromine to form aluminum
bromide.
a. How many moles of aluminum were used? (The density of aluminum is 2.699 g/cm3.)
b. How many grams of aluminum bromide form, assuming that the aluminum reacts completely?
AP Chemistry Worksheet 9: Limiting Reactants & Theoretical Yield
1. A manufacturer of bicycles has 50 wheels, 30 frames, and 24 seats.
a. How many bicycles can be manufactured using these parts?
b.
How many parts of each kind are left over?
c.
Which part is like a limiting reactant in that it limits the production of bicycles?
2. The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium
bicarbonate, NaHCO3, and citric acid, H3C6H5O7:
3 NaHCO3 (aq) + H3C6H5O7 (aq) --> 3 CO2 (g) + 3 H2O(l) + Na3C6H5O7 (aq)
In a certain experiment 1.00 g of sodium bicarbonate and 1.00 g of citric acid are allowed to react.
a.
Which reactant is the limiting reactant? You must show work to support your answer.
b.
How many grams of carbon dioxide form?
c.
How much of the limiting reactant is left when the reaction is complete?
d.
How much of the excess reactant remains after the reaction is complete?
3. When hydrogen sulfide gas is bubbled into a solution of sodium hydroxide, the reaction forms sodium sulfide and
water. How many grams of sodium sulfide are formed if 2.50 g of hydrogen sulfide is bubbled into a solution containing
1.85 g of sodium hydroxide, assuming that the limiting reagent is completely consumed?
4. Solutions of sulfuric acid and lead (II) acetate react to form solid lead (II) sulfate and a solution of acetic acid. If 10.0 g
of sulfuric acid and 10.0 g of lead (II) acetate are mixed, calculate the number of grams of sulfuric acid, lead (II)
acetate, lead (II) sulfate, and acetic acid present in the mixture after the reaction is complete.
5. A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr.
a.
What is the theoretical yield of bromobenzene in this reaction when 30.0 g of benzene reacts with 65.0 g of
bromine?
b.
If the actual yield of bromobenzene was 56.7 g, what was the percent yield?
AP Chemistry Worksheet 10: Personal Statement
1. Write a paragraph to tell me about your Chemistry experience last year. What did you like and dislike? What were you
good at and not so good at? What teaching and learning techniques work well for you?
2. Write another paragraph to tell me about your hopes for AP Chemistry. What made you decide to take this class?
How much effort are you willing to give to the class? What do you hope to take away from it?
(turn over for one last question!)
3. Write one last paragraph (5 full sentences) to tell me about yourself. How would you describe yourself? What do you
like to do? What are you involved in? What kind of goals do you have in your life?