AP Chemistry – Summer Study Guide
Future AP Chemistry Student:
Attached you will find summer work which will review topics that were learned in Honors Chemistry.
It is imperative that you review during the summer. We will begin by applying the concepts you have
already mastered this past year and begin looking at problems in a new and exciting way. You may
use any resource needed to complete this review packet. You may work with your peers; in fact, I
encourage you to do so. Keep in mind that copying from your peers will do you no good, as you will
ultimately be responsible for knowing this material.
It is expected that ALL work is shown and completed on notebook paper, NOT on these worksheets. I
will be collecting your work during the first week of school and it will be graded.
If you have any questions, please e-mail me at Sfiligoj@hudson.edu and I will get back to you. If you
would like to check out a text book to use over the summer, please stop by C100, as you will have to
turn in your Honors Chemistry textbook at the end of this year.
Enjoy your summer,
Mrs. Sfiligoj
Help Sessions this summer: Please attend any or all of these to help you work through this study
guide.
Where: Panera Hudson
When: Tues, June 17th
Tues, July 8th
Tues, Jul 29th
Time: 10:00am- 12:00pm
Directions: Below you will find topics that are a review of material you learned in Chemistry.
Beneath each topic are a series of questions pertaining to the topic. Answer each of the
questions with the following in mind: show all work, label all numbers with units and
species (ex: 3 grams of NaCl), and provide your answer with correct units and
significant figures…On another sheet of paper…i.e. not in this packet!
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AP Chemistry Summer Study Guide
1. Measurement (Zumdahl-Zumdahl Section 1.3-1.8)
A. Write the appropriate symbol in the blank, <, =, >
1. 303m_____303 X 103km
2. 500g_____0.500kg
3. 1.50cm3_____1.50 X 103 nm3
B. Explain how a volume measurement is made when measuring water in a
graduated cylinder.
C. Identify the best piece of lab equipment and process that would be used to
measure the following:
1. Mass of a solid crystal reagent which is in excess.
2. Mass of a solid precipitate
3. Create 500ml of a 1M HCl solution from 2M stock
4. Volume of 15ml of a 0.05M NaCl solution
2. Significant Figure (Zumdahl-Zumdahl Section 1.5)
A. Round off the following quantities to the indicated number of significant
figures.
1. 7.4855 grams (3 significant figures)
2. 298.693 cm (5 significant figures)
3. 11.968 lbs. (1 significant figure)
4. 345 oz. (2 significant figures)
B. Calculate the following to the correct number of significant figures.
1. X = 128.5 + 2116.44 – 2244.47
2. X = 0.004010 X 2.0000 X 50054
3. X = 12.6 + 0.3 + 256.5/ 1003.7
4. X = 12.20 – (1.60 + 4(0.36))1/2/ 1.3409
3. Dimensional Analysis (Zumdahl-Zumdahl Section 1.6)
A. A metal slug weighing 25.17 grams is added to a flask with a volume of 59.7mL.
It is found that 43.7 grams of methanol (density = 0.791 g/mL) must be added to the
metal to fill the flask. What is the density of the metal?
B. A solid with an irregular shape and a mass of 11.33 grams is added to a graduated
cylinder filled with water (density = 1.00 g/mL) to the 35.0mL mark. After the solid
sinks to the bottom, the water level is read to be at the 42.3mL mark. What is the
density of the solid?
C. Air is 21% oxygen by volume. Oxygen has a density of 1.31 g/L. What is the
volume, in liters, of a room that holds enough air to contain 55 kilograms of oxygen?
4. Periodic Table & Atom: Protons, Neutrons, Electrons (Zumdahl-Zumdahl Sections
2.1-2.5, 3.1, 7.8, 7.11-7.13)
A. Who discovered the electron? Describe the experiment that led to the deduction
that electrons are negatively charged.
B. Selenium is widely sold as a dietary supplement. It is advertised to “protect”
women from breast cancer. Write the nuclear symbol for naturally occurring
selenium. It has 34 protons and 46 neutrons.
C. Complete the following table using the periodic table if necessary.
Nuclear
Charge
Number of
Number of
Number of
Symbol
Protons
Neutrons
Electrons
79
0
35Br
-3
7
7
+5
33
42
90
4+
40Zr
D. Strontium has four isotopes with the following masses: 83.9134 (0.56%), 85.9094
(9.86%), 86.9089 (7.00%), and 87.9056 (82.58%). Calculate the atomic mass of
strontium.
E. Define an isotope. What is the same and what is different?
F. Complete the table below.
Element
Electron Configuration
Mg
1s22s22p63s23p64s23d104p65s24d3
Br
1s22s22p63s23p64s23d104p65s24d105p66s25d106p1
G. Complete the table below.
Element
Orbital Diagram
Ti
Xe
C
Sc
H. Define ionization energy. Arrange the following elements in order based on
increasing ionization energy: Na, Mg, K
I. Define atomic radius. Arrange the following elements in order based on decreasing
atomic radii: Cl, S, Ca
J. Define electronegativity. Arrange the following elements in order based on
increasing electronegativity: Be, Mg, Ca.
5. Nomenclature (Zumdahl-Zumdahl Section 2.8)
A. Complete the table below
Name
ICl3
N2O5
PH3
HNO2
HNO3
HCl
K2Cr2O7
Fe2(SO3)3
NaClO
MgCl2
B. Complete the table below.
Name
Iron (III) carbonate
Sulfur hexafluoride
Silicon dioxide
Hypochlorous acid
Oxalic acid
Carbon monoxide
Sulfur trioxide
Copper (II) sulfate
Barium oxide
Titanium (IV) oxide
Formula
Formula
C. Criticize each of the following statements.
1. In an ionic compound the number of cations is always equal to the number
of anions.
2. The molecular formula for strontium bromide is SrBr2.
3. The mass number is always equal to the atomic number.
4. For any ion, the number of electrons is always more than the number of
protons.
7. Molar Mass (Zumdahl-Zumdahl Section 3.3-3.4)
A. Complete the following table for TNT, C7H5(NO2)3.
Number of Grams
Number of Moles
Number of
Molecules
127.2
1.248
4.32 X 1022
Number of N
Atoms
5.55 X 1019
B. Calculate the molar mass of the following:
1. cane sugar, C12H22O11
2. laughing gas, N2O
3. vitamin A, C20H30O
8. Percent Composition (Zumdahl-Zumdahl Section 3.6)
A. Turquoise has the following chemical formula: CuAl6(PO4)4(OH)8*4H2O.
Calculate the mass percent of each element in turquoise.
B. A tablet of Tylenol has a mass of 0.611 grams. It contains 251mg of its active
ingredient, acetaminophen, C8H9NO2.
1. What is the mass percent of acetaminophen in a tablet of Tylenol?
2. Assume that all the nitrogen in the tablet is in the acetaminophen. How
many grams of nitrogen are present in a tablet of Tylenol?
9. Simplest & Molecular Formulas (Zumdahl-Zumdahl Section 3.7)
A. Determine the simplest formula of the following compounds:
1. the food enhancer MSG which has the composition 35.51%C, 4.77%
H, 37.85% O, 8.29% N, and 13.6% Na.
2. Zircon, a diamond like mineral, which has the composition 34.91% O,
15.32% Si, and 49.76%Zr.
3. Nicotine which has the composition 74.0% C, 8.65% H, and 17.4% N.
B. Explain how you would find the molecular formula given the simplest formula and
the molar mass.
10. Balancing Equations (Zumdahl-Zumdahl Section 3.9)
A. Balance the following equations:
1. H2S + SO2  S + H2O
2. CH4 + NH3 + O2  HCN + H2O
3. Fe2O3 + H2  Fe + H2O
11. Stoichiometry (Zumdahl-Zumdahl Section 3.10)
A. Diborane, B2H6, can be prepared by the following reaction:
3NaBH4 + 4BF3  2B2H6 + 3NaBF4
1. How many moles of NaBH4 react with 1.299 moles of BF3?
2. How many moles of B2H6 can be obtained from 0.893 moles of NaBH4?
3. If 1.987 moles of B2H6 is obtained, how many moles of NaBF4 are
produced?
4. How many moles of BF3 are required to produce 4.992 moles of NaBF4?
12. Limiting Reagents & Theoretical Yield (Zumdahl-Zumdahl Section 3.10)
A. The Space Shuttle uses aluminum metal and ammonium perchlorate in its reusable
booster rockets. The products of the reaction are aluminum oxide, aluminum chloride,
nitrogen oxide gas, and steam. The reaction mixture contains 7.00 grams of aluminum
and 9.32 grams of ammonium perchlorate.
1. Write the balanced equation for the reaction.
2. What is the theoretical yield of aluminum oxide?
3. If 1.56 grams of aluminum oxide is formed, what is the percent yield?
4. How many grams of excess reactant remain?
B. Oxyacetylene torches used for welding reach temperatures near 2000oC. The
reaction involved in the combustion of acetylene is
2C2H2 + 5O2  4CO2 + 2H2O
1. Starting with 175 grams of both acetylene and oxygen, what is the
theoretical yield, in grams, of carbon dioxide?
2. If 68.5L (density = 1.85 g/L) of carbon dioxide is produced, what is the
percent yield at the same conditions of temperature and pressue?
13. Molarity (Zumdahl-Zumdahl Section 4.1)
A. A reagent bottle is labeled 0.450M K2CO3.
1. How many moles of K2CO3 are present in 45.6mL of this solution?
2. How many milliliters of this solution are required to furnish 0.800 moles of
K2CO3?
3. Assuming no volume change, how many grams of K2CO3 do you need to
add to 2.00L of this solution to obtain a 1.000M solution of K2CO3?
4. If 50.0mL of this solution is added to enough water to make 125mL of
solution, what is the molarity of the diluted solution?
14. Ideal Gas Law (Zumdahl-Zumdahl Section 5.3)
A. A piece of dry ice, CO2, has a mass of 22.50 grams. It is dropped into an
evacuated 2.50L flask. What is the pressure in the flask at -0.4oC?
B. Use the ideal gas law to complete the following table.
Pressure
Volume
Temperature
Moles
o
1.75L
19 C
1.66
0.895atm
6oC
433mmHg
92.4mL
0.395
o
1.1atm
8.66L
25 C
Grams
14.0
15. Light (speed, frequency, wavelength) (Zumdahl-Zumdahl Section 7.1)
A. A photon of violet light has a wavelength of 423nm. Calculate
1. the frequency
2. the energy in joules pre photon
3. the energy in kilojoules per mole
B. Describe the relationship between wavelength and frequency.
C. Describe the relationship between energy and frequency.
D. Explain which color of light in the visible spectrum has the highest energy.
E. Explain which color of light in the visible spectrum has the longest wavelength.
16. Lewis Dot Structures (Zumdahl-Zumdahl Section 8.10)
A. Complete the table below:
Formula
Lewis Dot
3-D Shape/ AXE
Shape Name
Structure
Formula
CCl4
NCl3
CO2
SO3
Angles
Formula
Polar Bonds
(Y/N)
Polar
molecule
(Y/N)
Hybridization Number of 
/  bonds
Type(s) of
IMF
CCl4
NCl3
CO2
SO3
17. Redox Reactions (Zumdahl-Zumdahl Section 4.9-4.10) (NEW)
A. Assign oxidation numbers to each element in the following examples.
1. P2O5
2. NH3
3. CO324. SnO2
5. NaMnO4
B. Explain the difference between oxidation and reduction and write a half reaction to
represent each.
C. Write a half-reaction to represent sodium being oxidized.
D. Write a half reaction to represent fluorine being reduced.
18. Kinetics (Zumdahl-Zumdahl Section (Zumdahl-Zumdahl Section 12.2-12.3)
A. The equation for the reaction between iodide and bromate ions in acidic solution is
6I- + BrO31- + 6H+  3I2 + Br1- + 3H2O
[I-]
[BrO31-]
[H+]
0.0020
0.0040
0.0020
0.0020
0.0080
0.0080
0.0160
0.0080
0.020
0.020
0.020
0.040
Initial Rate
(mol/L*s)
8.89 X 10-5
1.78 X 10-4
1.78 X 10-4
3.56 X 10-4
1. What is the order of the reaction with respect to each reactant.
2. Write the rate expression for the reaction.
3. Calculate the rate constant with appropriate units.
19. Equilibrium (Zumdahl-Zumdahl Section 13.1-13.2)
A. Write the mass action expressions for the following reactions:
1. I2(g) + 5F2(g)  2IF5(g)
2. CO(g) + 2H2(g)  CH3OH(l)
3. 2H2S(g) + 3O2(g)  2H2O(l) + 2SO2(g)
4. SnO2(s) + 2H2(g)  Sn(s) + 2H2O(l)
B. A gaseous reaction mixture contains 0.30 atm SO2, 0.16atm Cl2, and 0.50 atm
SOCl2 in a 2.0L flask. K = 0.011 for the equilibrium system
SO2Cl2(g)  SO2(g) + Cl2(g)
1. Is the system at equilibrium? Explain.
2. If it is not at equilibrium, in which direction will the system move to reach
equilibrium?
20. Acids and Bases (Zumdahl-Zumdahl Section 14.1-14.3) (NEW)
A. Find the pH and pOH of solutions with H+ ion concentrations of:
1. 6.0M
2. 4.6 X 10-8M
3. 7.2 X 10-14M
B Write the net ionic neutralization reactions for each of the following:
1. Hydrocyanic acid is mixed with sodium hydroxide
2. Phosphoric Acid is mixed with ammonia
3. Hydrofluoric acid is mixed with methylamine
4. Sulfuric acid is mixed with ammonia
21. Nuclear Reactions (Zumdahl-Zumdahl Section 19.1-19.7) (NEW)
A. Define emission reaction and bombardment reactions
B. Write the symbols for the following and explain how the number of protons and
mass number changes when the particle is a reactant, and as a product.
Alpha, Beta, Gamma, Proton, Neutron
C. Write balanced reactions for the following:
1. U-238 undergoes alpha emission
2. Th-185 undergoes beta emission
3. Cl-35 is bombarded with a neutron
4. Ni-63 is bombarded with a proton