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 the local library, I am confident that you will
have sufficient resources to prepare adequately for the fall semester. The reference textbook for this
course is Chemistry: The Central Science, 10th edition, Brown, LeMay and Bursten, Prentice-Hall, 2006.
Additional Online General Chemistry Sites:
http://chemteam.info/ChemTeamIndex.html
www.chemfiesta.com
www.chemistrygeek.com
http://www.collegeboard.com/ap/students/chemistry/index.html
www.chemmybear.com
You may contact me by email: bgreyson@sdb.k12.wi.us this summer. I will do my best to answer your
questions ASAP. You can also follow me on Twitter @BarbGreyson for occasional updates and for
reminders about the two Pizza Hut work sessions.
AP Chemistry is an equivalent course to Introductory Chemistry in college. Taking a college level course
in high school is difficult, requires dedication, and is a great investment in your education to prepare
yourself for the future. Arrive ready to learn!
Assignment 1: Letter of Introduction (10 points)
Due date: Friday, June 27
Your first digital assignment is to successfully send an email to your AP Chemistry teacher.
Draft an email following these rules:
a. Use written, full sentences. Do not abbreviate words like you are on the Twitter with a friend.
b. Use spell check.
c. Make the Subject: AP Chem.: Introduction to “<Insert you name here>”
d. Begin the email with a formal salutation, like “Mrs. Greyson,”
e. 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 the class? What are you study skills? Etc. Anything interesting?
f. Due date: Friday, June 27
Assignment #2:
Due: Wednesday, July 9th
Read Ch. 1 BLB and complete the following problems.
On Wednesday, July 9, the AP Chemistry class will be meeting at the Beloit Pizza Hut from 12:002:00pm. The address of this location is: 2787 Prairie Ave. Beloit, WI
I will be providing pizza for everyone who attends this meeting (If you want additional food or a
beverage, you will need to buy it yourself). At this first meeting we will have a quiet space to read and
work on Assignment #2. You will have the opportunity to ask questions and work with your friends to
finish the assignment…all while enjoying some pizza! Alternatively, you may also choose to complete
the assignment on your own and submit the answers electronically by attaching it to an email by
8:00pm on Wednesday, July 9.
1. Write the most common guidelines to determine significant figures (digits) with 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
c. cm3
d. mm
e. kg/m3
f. kJ
g. atm
h. cal.
4. Most laboratory experiments are performed at room temperature at 25oC. Express this
temperature in:
a. oF
b. K
5. How many significant figures are in each of the following?
a. 1.92 mm
b. 0.030100 kJ
c. 6.022 x 1023 atoms
d. 460.00 L
e. 0.00036 cm3
f. 100
g. 1011
h. 0.001
i. 0.0101
6. Record the following in correct scientific notation:
a.
350,000,000 cal
b.
0.0000721 mol
c.
0.0000000809 Å
d.
765,400,000,000 atoms
7. Calculate the following to the correct number of significant figures.
a.
1.27 g / 5.296 cm3
b.
12.235 g / 1.01 L
c.
12.2 g + 0.38 g
d.
17.3 g + 2.785 g
e.
2.1 x 3.21
f.
200.1 x 120
g.
17.6 + 2.838 + 2.3 + 110.77
8. Give the chemical symbols for the following elements:
a. Carbon
b. Sulfur
c. Titanium
d. Nitrogen
e. Helium
9. Write the Latin and common names for each of the elements symbols:
a. Na b. Au c. Ag d. Sn e. Fe f. Hg g. K
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 of the following as either a physical process or a chemical process.
a. Corrosion of aluminum metal.
b. Melting of ice.
c. Pulverizing an aspirin.
d. Digesting a candy bar.
e. Explosion of nitroglycerin.
f. Milk turning sour.
g. Burning of paper.
h. Forming of frost on a cold night.
i. Bleaching of hair with hydrogen peroxide.
j. A copper wire is hammered flat.
Assignment #3:
Due: Wednesday, August 13th
Read Ch. 2 BLB and complete the following problems.
On Wednesday, August 13th, the AP Chemistry class will be meeting at the Beloit Pizza Hut from 12:002:00pm. The address of this location is: 2787 Prairie Ave. Beloit, WI
I will be providing pizza for everyone who attends this meeting (If you want additional food or a
beverage, you will need to buy it yourself). At this second meeting we will have a quiet space to read and
work on Assignment #3. You will have the opportunity to ask questions and work with your friends to
finish the assignment…all while enjoying some pizza! Alternatively, you may also choose to complete
the assignment on your own and submit the answers electronically by attaching it to an email by
8:00pm on Wednesday, August 13th.
12. Calculate the mass of O2 produced if 2.50 g KClO3 are complete decomposed by heating.
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
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
a 175 g of gold is 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 compounds 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 as: 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
20. State the contribution of each of the following chemists in one line.
a. Democritus
b. Mendeleev
c. Henry Becquerel
d. Roentgen
e. J.J. Thompson
f. Faraday
g. Chadwick
h. Millikan
i. Proust
j. Cavendish
k. Madam Curie
21. What is the difference between
a. Chlorine atom and chloride ion?
b. Sodium atom and sodium ion?
22. How many grams of nitrogen are present in 2.3 moles of nitrogen gas?
23. Calculate the mass in grams of each of the following:
a. 6.02 x 1023 atoms of Mg.
b. 3.01 x 1023 formula units of CaCl2
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. Define and give 2 examples of:
a. acid
b. base
c. salt
26. What is the difference between the Bronsted-Lowry, Lewis and Arrhenius definition of base?
27. What is the difference between the Bronsted-Lowry, Lewis and Arrhenius definition of acid?
Assignment #4
Due: Monday, Sept. 1 (First Day of School)
28. What mass of copper is required to replace silver from 4.00 g of silver nitrate dissolved in water?
Cu(s) + AgNO3
Cu(NO3)2 + Ag
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.
31. An isotope of Iodine used in thyroid disorders is 131
I How many:
153
a. protons are in its nucleus?
b. neutrons are in its nucleus?
c. electrons are in an Iodine atom?
d. Neutrons and protons are in the I-1 formed from this isotope?
32. Mercury has an atomic mass of 200.59 amu. Calculate the
a. mass of 3.0 x 1010 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)
34. Convert the following to moles
a. 3.86 grams of Carbon dioxide
b. 6.0 x 105 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 of ionic compounds (name or formula)
a. Cupric hydroxide
b. Strontium chromate
c. Ammonium perchlorate
d. NaHCO3
e. Fe2(CO3)3
f. Sodium hydroxide
37. Determine the formula mass for the following:
a. N2O5
b. CuSO4
c. Ca(HCO3)2
d. CaSO4
e. H2O
38. Calculate the percentage by mass of the following compounds:
a. SO3
b. CH3COOCH3
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, 68.7 % F