AP Chemistry Information and Summer Assignment 2017
Congratulations on your decision to take Advanced Placement Chemistry. This class has the potential to be one of the most fun and rewarding classes that you will take in high school. However, please be advised that many people have found AP Chemistry to be a particularly challenging course with a particularly challenging exam, even when compared with other AP courses and AP exams.
Remember also that AP classes are taught as college courses. This means that:
I will do as much as I can to help you learn, but you and you alone are responsible for learning and understanding everything covered in class.
I will tell you when everything is due, but I won’t chase after you. If you were absent and you need to turn in an assignment late, you need to remember to show it to me; do not assume I will ask you for it.
If you are having trouble with something, you need to be proactive about learning it, either by coming in for help before school, consulting with your classmates, or by getting outside help (Internet).
The goals of this summer assignment are to make sure you haven’t completely forgotten General Chemistry, to give you a “warm-up” for AP Chemistry, and to prepare you to be serious about doing work. This assignment is due Tuesday, Sept. 5th. Do not wait until September to start this assignment!!!
You may work with friends in the class, as long as you list the names of the people you worked with and each person turns in a separate copy. You may also ask me for help by email at or visit at school on August 29th-31st.
For each problem, you must show all the steps that lead from the question to the answer.
Please answer on a separate piece of paper.
1. Use factor labelmethod to convert the following:
a. 515 m = ___ miles.
b. 200.0 in = ____ meters
c. 10 kilometers into meters
d. 15,050 milligrams into grams
e. 3,264 milliliters into liters
f . 9,674,444 grams into kilograms
2. Classify each of the following as units of mass, volume, length, density, energy, or pressure.
a. mg b. mL c. cm3d. mm
e. kg/m3f. kJ g. atmh. cal.
3. A cylinder rod formed from silicon is 16.8 cm long and has a mass of 2.17 kg. The density of silicon is 2.33 g/cm3. What is the diameter of the cylinder? (the volume of cylinder is given by πr2h, where r is the radius and h is the length)
4. How many significant figures are in each of the following?
a. 1.92 mm b. 0.030100 kJ
c. 6.022 x1023 atoms d. 460.00 L
e. 0.00036 cm3 f. 100
g. 1001 h. 0.001
i. 0.0101
5. Record the following in correct scientific notation:
a. 350,000,000 cal
b. 0.0000721 mol
c. 0.0000000809 grams
d. 765,400,000,000 atoms
6. 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. 200.1 x 120
e. 17.6 + 2.838 + 2.3 + 110.77
7. 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.
8. Label each of the following as either a physical process or a chemical process.
a. Corrosion of aluminum metal.b. Milk turning sour.
c. Melting of ice.d. Burning of paper.
9. Calculate the mass of O2 produced if 2.50 g KClO3 are completely decomposed by heating.
10. Write the formula of the following compounds?
a. calcium sulfate. d. potassium perchlorate.
b. ammonium phosphate e. barium fluoride
c. lithium nitrite f. aluminum sulfide.
11. Convert 3.57 atm to: (Using factor-label method)
a. mm Hg b. kilopascalsc. Torr
12. Determine number of protons, electrons and neutrons in each of the following neutral atoms.
- K-39 b. Na-23. c. Pb-208d. P-33
13. 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?
14. Determine the number of molecules in 2.23 mol of nitrogen (N2) molecules.
15. List the following as diatomic molecule, Molecular compound, Ionic compound, Atomic element.
a.F2b. Cl2c. C d. NaCl e. KF f. CO2
g. H2h. Ag i. Rust (Fe2O3) j. MgO k. O2l. I2
16. In an experiment, a student gently heated a hydrated copper compound to remove the water of hydration. The following data was recorded:
mass of crucible, cover, and contents before heating 23.54 g.
mass of empty crucible and cover 18.82 g.
mass of crucible, cover, and contents after heating to constant mass 20.94 g.
Calculate the experimental percent of water in the compound.
17. A hydrated compound has an analysis of 18.29% Ca, 32.37% Cl, and 49.34% water. What is its formula?
18. What mass of copper is required to extract silver from 4.00g of silver nitrate dissolved in water? (Balance equation)
Cu(s) + AgNO3 → Cu(NO3)2 + Ag.
19. Initially 1.50moles of N2(g) and 3.50moles of H2(g) were added to a 1-L container at 700°C according to the reaction N2(g) + 3H2(g) 2NH3(g). As a result of the reaction the equilibrium concentration of NH3(g) became 0.540M. What is the value of the equilibrium constant for this reaction at 700°C.
20. Write a balanced equation for the following:
a. Reaction of boron trifluoride gas with water to give liquid hydrogen fluoride and solid boric acid, (H3BO3).
b. The decomposition of dinitrogen monoxide gas to its elements.
c. The reaction of calcium carbide (CaC2) solid with water to form calcium hydroxide and acetylene (C2H2) gas.
d. Ethane burns in air (oxygen).
e. Carbon dioxide combines with water to form carbonic acid.
f. Magnesium and nitrogen gas combine to form magnesium nitride.
g. Hydrochloric acid reacts withsodium hydroxide to form sodium chloride and water.
21. Find the Oxidation number of
a. Carbon in CO2.
b. Sulfur in H2SO4.
c. Phosphorus in PO43-
d. Manganese in MnO42-
22. Which of the following statements are always true? Never true? Not always true?
a. A compound with the molecular formula C6H6 has the same simplest formula.
b. The mass percent of copper in CuO is less than in Cu2O.
c. The limiting reactant is the one present in the smallest number of grams.
d. Since C3H6O3 and C6H12O6 reduce to the same formula, they represent the same compound.
23. How much heat is required to raise the temperature of 100.0 grams of water from 14.0°C to 82.0°C?
24. A piece of unknown metal with mass 14.9 g is heated to 1000.0°C and dropped into 75.0 g of water at 200°C. The final temperature of the system is 345°C. What is the specific heat of the metal?
25. Calculate the molarity of a solution that contains 20.0grams of sodium hydroxide in 200ml?