Summer Assignment
2016 - 2017
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Future AP Chemistry Students—
I want to be the first to welcome you to AP Chemistry as you finish up your last couple
of days of school. Behind this letter you will find your summer work. It is a review over
material that you covered in class this year. Use the materials from this year to help you
answer the questions. This will help us prepare for the first exam, which will cover the first
three chapters, on Wednesday, August 31st. Please don’t go home today and do the packet.
Take some time off!!! You deserve it. Plus, it is a review to get many of the ideas you learned
this year back in your head before the start of school. That won’t happen if you do it during the
next few weeks of summer vacation. The packet is due on Friday, August 19th. I also expect
you to come back with you knowing what the polyatomic ions are that you memorized in PreAP Chemistry. There will be a quiz over these ions on the first day of class! I attached the list in
case you need it to study. We will spend the week of school covering material from Chapters 13 and then we will test on the 31st.
Also, I would like you to sign up for Edmodo. The course code is below. Please sign up
BEFORE school ends. The code locks within two weeks. That is the place where I will be able to
communicate with you this summer. My plan is also to put some tutorial videos on some of the
main topics to help you with your homework as the summer goes along. With that I would also
like you to sign up for Mastering Chemistry before school starts. I will put that information on
Edmodo in July.
Enjoy your summer vacation and if you have any questions, don’t hesitate to contact me
by email or through Edmodo.
Sincerely,
Mr. Mooney
Contact Information—
Email: [email protected]
Edmodo Course Code: v8f8tx
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AP Chemistry – Summer Review Assignment
1. Significant Figures
I.
II.
Determine the number of significant figures in each of the following numbers:
1. 5.432 g
11. 2500 cm
2. 40.319 g
12. 2500.0 cm
3. 146 cm3
13. 1.04 x 1014 g
4. 3.285 cm
14. 3.58 x 10-9nm
5. 0.189 lb
15. 48.57193 lb
6. 429.3 g
16. 8365.6 g
7. 2873.0 cm3
17. 0.002300 mg
8. 99.9 mL
18. 7.500 x 108 oz
9. 0.000235 g
19. 3.92 x 10-4 g
10. 144 lb
20. 1.000 x 103 lb
Add & Subtraction
1. 12 cm + 0.031 cm + 7.969 cm =
2. 0.085 cm + 0.062 cm + 0.14 cm =
3. 3.419 g + 3.912 g + 7.0518 g + 0.00013 g =
4. 1.8 x 10-5 cm + 3.25 x 10-4 cm + 4.6 x 10-5 cm =
5. 0.0653 g + 0.08538 g + 0.07654 g + 0.0432 g =
6. 145.63 mL – 28.9 mL =
III.
Multiply & Divide
1. 5.00 mm x 7.3216 mm =
2. 282.2 km x 3.0 km =
3. 9.13 x 10-4 cm x 1.2 x 10-3 cm =
4. 8.071 cm2 / 4.216 cm =
5. 6.058 mm2 / 0.85 mm =
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Convert the following:
a. 50 km to m
b. 47.9 ML to L
c.
578 ms to s
d. 1.55 X 102 kg to milligrams
e. 87.4 cm2 to mm2
f.
IV.
0.0962 km/min to m/s
Density
a. The mass of 325 mL of liquid methanol is found to be 257 g. What is its density?
b. A block of lead is 1.20 cm X 2.41 cm X 1.80 cm and has a mass of 59.01 g. What is the
density of lead?
c.
What is the mass, in grams, of 30 mL of syrup that has a density of 1.32 g/mL?
d. A square of aluminum foil (d= 2.70 g/cm3) is 5.10 cm on a side and has a mass of 1.762 g.
Calculate the thickness of the foil, in millimeters.
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2. Atomic Structure
I.
Complete the table:
Symbol
Atomic
Number
Mass Number
# protons
# neutrons
# electrons
12
6
C
48
64
197

79
23
+1
___Na
30
66
28
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II.
What are isotopes? Given an example
III.
What are ions? How are they formed? Give 2 examples.
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3. Formulas and Nomenclature
I. Name the following compounds.
1. HCl
15. NaC2H3O2
2. KOH
16. FeCO3
3. HgOH
17. Zn(NO3)2
4. KCl
18. NH4IO3
5. FeCl3
19. LiH
6. HNO3
20. KHCO3
7. Cu2O
21. K2Cr2O7
8. NH4OH
22. Sn(ClO)4
9. Al2(SO4)3
23. K2SiO3
10. N2O5
24. P3N5
11. NaOH
25. H2SO3
12. CO2
26. SnI4
13. HF
27. MoCl5
14. Pb(OH)2
28. Pb(CO3)2
II. Write the correct formula for each of the following.
1. sodium hydroxide
14. manganese (II) hydroxide
2. calcium oxide
15. aluminum phosphate
3. carbon monoxide
16. tin (II) hydroxide
4. lithium sulfate
17. zinc hydroxide
5. sulfuric acid
18. ammonium carbonate
6. iron (II) oxide
19. lead (IV) chloride
7. lead (IV) chloride
20. hydrochloric acid
8. nickel (I) bromide
21. zinc acetate
9. zinc hydroxide
22. nickel (II) chloride
10. diphosphorus pentoxide
23. sodium hydrogen carbonate
11. aluminum phosphate
24. aluminum bisulfate
12. hypochlorous acid
25. nitric acid
13. sulfur dioxide
26. cadmium nitrite
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4. Percentage Composition
I.
Find the percentage composition of each of the following compounds
1. HBr
6. NH4Br
2. KI
7. Ca(NO3)2
3. CO
8. K3PO4
4. SO2
9. Zn3(PO4)2
5. K2S
10. NH3
11. What is the percentage of carbon in calcium carbonate?
12. What is the percentage of hydrogen in Ca(C2H3O2)2?
13. How much phosphorus is there in 500.0 g of calcium phosphate?
14. How much iron can be obtained from 100.0 grams of Fe3O4?
15. What is the percentage of bismuth in sodium bismuthate, NaBiO3?
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5. Basic Stoichiometry and Chemical Calculations
I.
Balance:
___ Fe + ___ O2
___ SiCl4
→
+ ___ H2O
___ PCl3 +
___ CaO
___ H2O
+ ___ P4O10
___ C2H6 +
___ O2
___ Fe2O3
→
___ SiO2 + ___ HCl
→
___ H3PO3 + ___ HCl
→
→
___ H3PO4 + ___ NaCN
___ Ca3(PO4)2
___ CO2
→
___ HCN + ___ Na3PO4
___ Ba(NO3)2 + ___ Al2(SO4)3
___ FeCl3 + ___ NaOH
II.
→
+ ___ H2O
→
___ BaSO4 + ___ Al(NO3)3
___ Fe(OH)3
+ ___ NaCl
Find the molecular weight for each of the compounds shown below:
1. H3PO4
2. Sb(NO3)3
3. NaIO4
III.
Mole Conversions
1. What is the mass of 0.250 mole of sodium? How many sodium atoms is this?
2. How many molecules of carbon dioxide are in 225g?
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3. How many molecules of water are in 4.68 mole water?
4. What is the mass of 1.75 X 1034 aluminum atoms?
6. Determining Empirical and Molecular Formulas
I.
Finding the Empirical Formula from the Percent Composition
1) Cyclohexanol, used in the manufacture of plastics, has the mass percent composition:
71.95% carbon, 12.08% hydrogen and 15.97% oxygen. What is its empirical formula?
2) TNT has the mass percent composition: 37.00% C, 2.20% H, 18.50% N, and 42.23% O, by
mass. Find its empirical formula.
II.
Determining the Molecular Formula
1. The empirical formula of paradichlorobenzene, used as a moth repellant, is C3H2Cl. Its
molecular mass is 147 u. What is its molecular formula?
2. Resorcinol, used in the manufacture of resins, drugs and other products is 65.44% C, 5.49% H
with the remainder being oxygen. Its molecular mass is 110.0 amu. What is its molecular
formula?
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III.
Non-limiting reactant/non-solution Stoichiometry
1. The final step in the production of nitric acid involves the reaction of nitrogen dioxide with
water. Another product is nitrogen monoxide. How many grams of nitric acid are
produced for every 100.0 g of nitrogen dioxide that reacts?
2. Upon being strongly heated or subjected to severe mechanical shock, ammonium nitrate
decomposes into nitrogen and oxygen gases and water vapor. If 75.5 grams of ammonium
nitrate decomposes, how many grams of each product is made?
3. Lead(II) oxide reacts with ammonia (NH3), forming solid lead, nitrogen gas and liquid
water.
a. How many grams of ammonia are consumed in the reaction of 75.0 g lead(II) oxide?
b. If 56.4 g of lead are produced, how many grams of nitrogen are also formed?
Questions:
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Atomic Ions to Know

Alkali Metals (1+)
o Li+, Na+, K+, Rb+, Cs+

Halogens
o F-, Cl-, Br-, I-

Alkaline Earth Metals (2+)
o Be2+, Mg2+, Ca2+, Sr2+, Ba2+

Calcogens (Oxygen Family)
o O2-, S2-, Se2-

Aluminum (3+)


Silver (1+)
Nitrogen Family (3-)
o N3-, P3-

Zinc, Cadmium (2+)

Carbon Family (4-)
o C4-
Polyatomic Ions to Know
 Chlorate (ClO3-)
 Carbonate (CO32-)
 Chlorite (ClO2-)
 Phosphate (PO43-)
 Iodate (IO3-)
 Phosphite (PO33-)
 Iodite (IO2-)
 Ammonium (NH4+)
 Nitrate (NO3-)
 Acetate(C2H3O2-)
 Nitrite (NO2-)
 Chromate (CrO42-)
 Sulfate (SO42-)
 Dichromate (Cr2O72-)
 Sulfite (SO32-)
 Permaganate (MnO4-)
 Hydroxide (OH-)
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