AP Summer Assignment Packet 2
2013-14
Mrs. Varma-Kumar
AP Chemistry Summer Assignment Packet 2
DUE DATE: Tuesday, September 10th, 2013
FIRST TEST DATE: Friday, September 13th, 2013
Welcome to AP Chemistry. This is the first set of MANY assignments you will complete for this
course. Please answer each question below as completely as you can, showing ALL mathematical
calculations as appropriate. Your answers MUST be hand written in blue or black ink on the answer
sheets (pages 8-16) that follow the question packet. This packet will be collected and graded.
You are welcome to use multiple resources of your choice. Attempt to complete the packet on your
own. If you choose to work with another member of your class, each one of you is responsible for
handing in your own packet, AND for knowing ALL the material (i.e. “I’ll do the first half and you do
the other half, and we’ll copy” does NOT help either one of you). My recommendation is to read
Chapter 1-3 (and work on AP Summer Assignment 1) first, and then work on this packet.
Also remember, this is the easy stuff—a review of what you already know from Honors/Academy
Chemistry, therefore you should have no trouble completing the assignment accurately. Having said
that, it is possible that there will be some material that was not covered in Honors/Academy
Chemistry, or compounds that you are unfamiliar with. It is still your responsibility to find and
learn that material as you complete the assignment. Do keep in mind that I would not assign
something that you couldn’t otherwise complete with a little effort. Remember also that you will be
graded on accuracy, as well as completion.
Your first graded test will include ALL material below, along with the second assignment, and will be
given on FRIDAY, SEPTEMBER 13, 2013
Feel free to contact me with any questions via email at yvarma@marsd.k12.nj.us or via phone at
732-469-5609. Please call at a reasonable time and recognize that if you leave a voicemail, your call
will be returned but may not be returned immediately. Please be sure to identify yourself clearly,
and leave your phone number.
Good Luck!!
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AP Summer Assignment Packet 2
2013-14
Mrs. Varma-Kumar
PROBLEMS
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
c. cm3
d. mm
e. kg/m3
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
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AP Summer Assignment Packet 2
2013-14
Mrs. Varma-Kumar
5. 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
6. Record the following in correct scientific notation:
a. 350,000,000 cal
b. 0.0000721 mol
c. 0.0000000809 Ǻ
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.
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Mrs. Varma-Kumar
h. Forming of frost on a cold night.
i. Bleaching of hair with hydrogen peroxide.
j. A copper wire is hammered flat.
12. Calculate the mass of O2 produced if 2.50 g KClO3 are completely 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 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 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
l. I2
20. State the contribution of the following chemist in one line.
a. Democritus b. Mendeleev c. Henry Becquerel
d. Roentgen
f.Faraday
g. Chadwick
h. Millikan
i. Proust
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.
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e. J.J Thompson
j. Cavendish
AP Summer Assignment Packet 2
2013-14
Mrs. Varma-Kumar
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?
28. What mass of copper is required to replace silver from 4.00g 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
d. Sodium Oxide
e. Calcium Sulfate
g. Magnesium Acetate
h. Potassium cyanide
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 131I has how many
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
b. Baking soda
c. Osmium Metal (Os)
34. Convert the following to moles
a. 3.86 grams of Carbon dioxide.
b. 6.0 x 10 5g of Hydrazine (N2 H4), 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?
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c. Sodium Chloride
f. Sodium Nitrite
i. Zinc (II) Nitrate
AP Summer Assignment Packet 2
2013-14
Mrs. Varma-Kumar
36. Complete the list ionic compounds ( name or formula)
a. Cupric Hydroxide
b. Strontium Chromate
c. Ammonium Per chlorate
d. NaHCO3
e. Fe2 (CO3)3
f. Sodium Hydroxide.
g. Potassium Chloride.
37. Determine the formula mass for the following:
a. N2O5
b. CuSO4
c. Ca(HCO3)2
d. CaSO4. 2 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, and 68.7 % F
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. 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. Reaction of magnesium Oxide with Iron to form Iron (III) Oxide and Magnesium.
c. The decomposition of dinitrogen Oxide gas to its elements.
d. The reaction of Calcium Carbide solid with water to form calcium hydroxide and acetylene
(C2H2) gas.
e. The reaction of solid calcium cyan amide (CaCN2) with water to from calcium carbonate
and ammonia gas.
f. Ethane burns in air (Oxygen).
g. Hydrogen reacts with oxygen to from Water.
h. Nitrogen gas reacts with Hydrogen to form Ammonia.
i. Hydrogen reacts with Iodine gas to form Hydrogen Iodide.
j. Sodium reacts with Iodine gas to form Sodium Iodide.
k. Sodium Oxide reacts with water to form sodium hydroxide and hydrogen.
l. Carbon dioxide combines with water to form carbonic acid.
m. Magnesium and nitrogen gas combine to form magnesium nitride.
n. Conc. Hydrochloric acid reacts with Conc. Sodium hydroxide to form sodium chloride and
water.
42. Define limiting reagent, theoretical yield, and actual yield.
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AP Summer Assignment Packet 2
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Mrs. Varma-Kumar
43 Define the following terms:
a. Electrochemistry
b. Electrolysis
c. Voltaic Cell
44. Name the five different types of chemical reaction and their general formulas.
45. Define solubility. Prepare AND MEMORIZE a list of solubility rules for ionic compounds in
water. (IMPORTANT)
46. Name the following:
a. CO2
b. P4S10
c. NI3
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d. PCl5
e. CCl4
f. SF6
AP Summer Assignment Packet 2
2013-14
Mrs. Varma-Kumar
AP CHEMISTRY SUMMER ASSIGNMENT PACKET 2
ANSWER FORM (this part will be collected and graded)
Due Date: Tuesday, September 10th, 2013
ALL answers to the 46 questions above must be filled in the appropriate spaces below. If more
space is required to show work (calculations etc.) or to fully answer a question, please use
supplemental lined paper or the BACK of the answer sheet and identify the question AND part (as
appropriate) clearly.
1.
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g. _________
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AP Summer Assignment Packet 2
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Mrs. Varma-Kumar
6.
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Mrs. Varma-Kumar
13.
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AP Summer Assignment Packet 2
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Mrs. Varma-Kumar
16. _______________
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Mrs. Varma-Kumar
22. __________________
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ACID: __________________________________________________________________
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Mrs. Varma-Kumar
29.
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Mrs. Varma-Kumar
d. __________________
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Mrs. Varma-Kumar
f.
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Mrs. Varma-Kumar
a.
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