Download Dear Chemistry Student, I am excited that you have chosen to

Dear Chemistry Student,
I am excited that you have chosen to challenge yourself by taking on the rigors of AP
Chemistry here at Cathedral Catholic High School. In order to prepare you for the
expected performance outcomes of the course, every one will be expected to complete a
Summer Independent Study Program. Since students entering AP Chemistry will have
had a full year of Chemistry, the summer assignment is intended to help students
maintain old skills and prepare them for the exam that will be given during the first
week of school. In the past, I have found that students who have failed to master the
concepts in the summer assignment struggle during the semester to manage the
workload and maintain a satisfactory grade. A completed summer assignment is the key
to success in this class. Additionally, there are 85 polyatomic ions that will not be
provided during the year and will be tested on directly during the first week of school
and indirectly throughout the remainder of the school year. Some review videos have
been posted onto my You Tube page. Although they are not comprehensive, they do
cover some of the more challenging aspects of the Chemistry 1 curriculum. Another
resource for material you may need help reviewing will be your textbook. Please be
sure to purchase it at the beginning of the summer! I look forward to having you in my
class next year!
- Mrs. Martin
Summer Assignment Due: First Day of Class!
Summer Assignment Exam: First Week of School!
Summer Assignment Review Videos:
https://www.youtube.com/playlist?list=PLwi78F-QlPg-NqpzQhOvKZSHjR4FFcYgy
AP Chemistry Summer Study Assignment 2016
Make sure to complete these ON YOUR OWN PAPER, in order!
Don’t wait until the last minute!!!
The purpose of the summer assignment is three-fold. First, it should serve as a basic review of
Chemistry 1 material, just in case you’ve forgotten some of the information since you took the class.
Two, it will prepare you for the first week of Chemistry class, as we will “hit the ground running”
with a test over the summer assignment (including all 85 polyatomic ions) and quickly move on to
AP Chemistry topics. Lastly, it gives you a week by week breakdown for your summer work.
Students who have slacked off on the summer assignment in the past have performed poorly in the
class itself. Don’t let this be you! This summer assignment is due on the first day of class.
Good luck!
Week 1: Get Organized!
-Purchase your textbook now! You will need it to study and look up concepts that you may not
remember from Chemistry 1. Getting familiar with your book will help you be better prepared for
the rigors of the school year. You can order from Amazon or any other book site. Chemistry-6th
Edition – Zumdahl ISBN-13: 978-0618221561
-Begin memorizing the 85 Polyatomic Ions list. You will need to know both name and ion formulas.
These are the easiest exam points you will earn all year so be sure to make it happen! =)
- Check out Mrs. Martin’s video page on You Tube. There are some review videos that may help
you with various parts of last year’s chemistry content. Additionally, this is where you will be
getting your lecture notes during the school year. Getting familiar now is always a good thing!
https://www.youtube.com/playlist?list=PLwi78F-QlPg-NqpzQhOvKZSHjR4FFcYgy
Week 2: Nomenclature/Lewis Dot Structures/Shapes/Ionic/Covalent Identification
1. Write the formulas for the following compounds:
a. mercury(I) chloride
h. phosphorus tetrachloride
o. potassium chlorate
b. zinc hydroxide
i. barium hydroxide
p. zinc nitrite
c. ferric fluoride
j. potassium permanganate
q. lithium sulfite
d. silver nitrate
k. sulfuric acid
r. strontium bromide
e. calcium bromate
l. lead(II) iodide
s. aluminum oxide
f. acetic acid
m. hydrogen chloride
t. lithium phosphate
g. magnesium bisulfate
n. sodium chlorite
u. sodium bicarbonate
2. Write the name of the following compounds:
a. MgCl2
e. HClO
b. CuSO4
f. Mg(OH)2
c. KMnO4
g. H2O2
d. Na2CO3
h. LiBr
3. Name the following compounds
a. CO2
f. AlCl3
b. O2
g. CrI3
c. KCl
h. N2O5
d. Sn(NO3)4
i. NaOH
e. Na2S
j. CaCO3
i.
j.
k.
l.
MnF4
HgO
Al2O3
Fe2O3
k. phosphorus trichloride
l. lithium oxide
m. ammonium phosphate
n. strontium nitrate
o. beryllium chloride
m. AgNO3
n. H2SO4
o. BaS
p. nitrogen oxide
q. hydrogen peroxide
r. ferric sulfate
s. diarsenic trichloride
t. sodium bromide
4.
a.
b.
c.
d.
e.
Name the following compounds.
NaCl
f. KBr
H2SO4
g. S8
CaF2
h. O2
H2 O
i. SO4
N2 O4
j. Os
k.
l.
m.
n.
o.
C5O3
H2 O2
NaH2SO4
SrBr2
CO
p.
q.
r.
s.
t.
CO3
I2
MgCl2
SF5
FeCl3
u. KOH
v. HF
w. HNO3
5. Name the following compounds:
a. H2SO4
b. SCNc. N2
d. Hg2I2
e. ZnS
f. AlPO3
g. KNO3
h. HF
i. CoCO3
j. NaCl
k. Mg(OH)2
l. H3BO3
m. Bi(OH)5
n. AgHCO3
o. NH3
p. AlBr3
q. HCl
r. H2S
s. C4H4
t. LiMnO4
6. Write the name or formula for the following:
a. NaBr
b. Ca(C2H3O2)2
c. P2O5
d. Ti(SO4)2
e. FePO4
f. K3N
g. SO2
h. CuOH
i. Zn(NO2)2
j. V2S3
k. silicon dioxide
l. nickel (III) sulfide
m. manganese (II)
phosphate
n. silver acetate
o. diboron tetrabromide
p. magnesium sulfate
heptahydrate
q. potassium carbonate
r. ammonium oxide
s. tin (IV) selenide
t. carbon tetrachloride
Week 3: Balancing/Writing/Product ID/Rxn Type Chemical Equations/Lewis Dot Structures
7. Predict products and/or write/balance equations for the following, and state what kind of
reaction would occur:
a. calcium carbonate (aq) + magnesium bromate (aq)
b. HNO3 is added to KOH
c. hydrogen is mixed with sodium fluoride
d. AlBr3 is strongly heated (decomposes!)
e. ammonium perchlorate (aq) + Li2O (aq)
f. C6H12 is burned in oxygen
g. balance: CH4 + O2 → CO2 + H2O
h. balance: K + H2O → KOH + H2
i. the reaction of ammonia with iodine to form nitrogen triiodide (NI3) and hydrogen gas
j. the combustion of propane (C3H8)
k. the reaction of nitric acid with potassium hydroxide
l. the reaction of copper (II) oxide with hydrogen to form copper metal and water
m. the reaction of AlBr3 with Mg(OH)2
n. the decomposition of calcium carbonate.
o. lithium hydroxide is added to aluminum sulfate.
p. pentene, C5H10, is burnt in air.
q. sodium is mixed with chlorine.
r. sodium is added to water.
8. Draw the best Lewis Dot Structures for each of the following molecules. Be sure to include
molecular shape, bond angles and formal charges for each and resonance where necessary.
a. NH3 b. SO42- c. CCl4 d. NO3-1 e. SF6 f. XeF4 g. H2S h. CO2 i. O2 j. BF3 k. CClF3 l. XeF2
m. CO32- n. NH4+1 o. PF5
Week 4: The Mole/Stoich/LR/ER/%yield/%comp/EF/MF
9. Answer the questions below using the equation provided. Na + Cl2 → NaCl
a. How many moles of chlorine gas (Cl2) would react with 5 moles of sodium (Na) according to
the chemical equation above? (Balance equation!)
b. Using the equation above, determine the amount of product that can be produced from 24.7 g
Na.
c. How many molecules of product would be produced from 24.7g Na?
10. Chlorine is used by textile manufacturers to bleach cloth. Excess chlorine is destroyed by its
reaction with sodium thiosulfate, Na2S2O3:
Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) → 2NaHSO4(aq) + 8HCl(aq)
a. How many moles of Na2S2O3 are needed to react with 0.12mol of Cl2?
b. How many moles of HCl can form from 0.12mol of Cl2?
c. How many moles of H2O are required for the reaction of 0.12mol of Cl2?
d. How many moles of H2O react if 0.24mol HCl is formed?
11. Determine the empirical formula of a compound with the following composition by mass: 48.0
% C, 8.0 % H, 28.0 % N and 16.0 % O. If this compound has a molar mass of 200 g/mol , what is its
molecular formula?
12. Determine the empirical formula of a compound with 20.8 % hydrogen, 36.3 % oxygen, and 42.9
% carbon
13. Determine the molecular formula of CHO, given the molecular mass of 174.9 amu.
14. Calculate the number of molecules in 325 grams of lithium oxide.
15. If 4.50 g of Li reacts with 4.5 g of O2, what mass of lithium oxide is produced?
16. If 27.3g of C8H18 are combusted, what mass of water will be produced?
17. The actual yield of a solution is 3.0 x 103, the theoretical yield is 3.5 x 103, what is the percent
yield?
18. A compound is found to contain 71.9% potassium and 28.1% sulfur. Find the empirical formula.
19. How many grams of NO can be produced from 65 grams of NH3? 4NH3 + 5O2 →4NO + 6H2O
20. HCl + NaOH → NaCl + H2O
a. Given that there is 2 moles of HCl and 2.5 moles of NaOH reacting, find the limiting
reactant (hint: write a balanced equation).
21. 2HNO3(aq) + 3H2S(g) -> 2NO(g) + 4H2O(l) +3S(s)
In the reaction above, 4.62g HNO3(aq) and 1.84g H2S(g) are mixed. How many grams of NO(g) is
formed?
22. A compound containing carbon, hydrogen, and oxygen is 52.11% carbon, 13.14% hydrogen, and
34.75% oxygen. What is the empirical formula of this compound?
23. Calculate the indicated quantity for each of the given chemical reactions:
a. Theoretical yield= 1.0g, percent yield= 90.0%, actual yield= ?
b. Theoretical yield= 3.45g, percent yield= 48.0%, actual yield= ?
24. Give the empirical formula for a compound made up of, 24% C, 48%O, and 28% N.
25. Determine the percentage of sodium in sodium sulfate.
26. Draw the periodic trend of electron affinity.
27. Calculate the percent composition of the elements in HNO3.
28. Given the equation, 2Fe+ 3Cu(OH)2 → 2Fe(OH)3 + 3Cu,
a. If 1 mole of iron reacts completely, how many grams of Cu is formed?
If 28.4 grams of Fe(OH)3 is produced, how many grams of Fe reacted?
29. Aluminum hydroxide reacts completely with acetic acid (HC2H3O2)
a. Write the reaction.
b. If 100 grams of aluminum hydroxide reacts with 100 mL of 3 M acetic acid, what is the
limiting reactant?
30. Ba2+ + 2Cl+ à BaCl2
According to the reaction above, how many grams of chlorine are required to completely react
to form 208.2g of barium chloride.
Week 5: Gas Laws
31. What is the equation for the combined gas law
32. What is the equation for Boyle’s Law?
33. What is the equation for Charle’s Law?
34. What is the equation for Gay-Lussac’s Law?
35. What is the equation for the Combined gas law?
36. What is the equation for the Ideal gas law?
37. When 5.0 moles of O2 are confined to a 24 liter container at 87°C, the pressure is 6.0 atm. If the
oxygen is allowed to isothermally expand to 36 liters, what is the new pressure?
38. A 502.8g sample of X2(g) has a volume 9.0 L at 10 atm and 102°C. What is element X?
39. If a baloon with a volume of 12.2 L is at 22.5 oC what will be its new volume when placed in a
freezer at 0 oC?
40. If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its
volume is 4.8 L, what will the new pressure inside the piston be?
41. A toy balloon has an internal pressure of 1.05 atm and a volume of 5.0 L. If the temperature
where the balloon is released is 20°C, what will happen to the volume when the balloon rises to
an altitude where the pressure is 0.65 atm and the temperature is –15°C?
42. Calculate the pressure of 2 moles of a gas at 20°C with a volume of 200mL.
43. If there is a solid, rigid container holding 3 moles of N2 gas at 760 torr and 25oC, and then the
container is heated to 50oC, what is the new pressure of the gas in atm?
44. If there is a 5.00L container holding O2 gas at standard temperature and pressure, how many
grams of O2 are in the container?
Week 6: Solutions
45. What is the equation for molarity?
46. What is the equation for molality?
47. What is the equaiton for dilutions?
48. The molarity of a solution is 0.75M. How many moles of the solute is needed in 500mL of
solvent?
49. What is the molarity of a solution containing 0.32 moles of NaCl in 3.4 liters?
50. How many moles of KBr are in 25.0 mL of a 1.23 M KBr solution?
51. Determine molarity of 11.4 g of ammonia in 200. mL of water.
52. What is the concentration of a solution made by diluting 40 mL of 9 M H2SO4 to a total volume
of 600 mL?
53. What volume of a 5.0M solution is needed to make 20.0L of .50M of the same solution?
54. How many moles of NaOH are there in 500 mL of a 2.0 M solution?
55. If 80.2g of calcium are added to 10000mL of water, what is the molarity of the resulting
solution?
56. If 167.385mL of water are added to 86.3L of ammonium nitrate solution, what is the resulting
volume in liters? (sig figs)
57. How many milliliters of a 2.0 M H2SO4 is needed to make 45.0 mL of a 0.10 M H2SO4 solution?
58. 16.7 grams of substance X is dissolved in 100 mL water and gives a molarity of 2.5 M. What is
the molecular mass of substance X?
Week 7: Acids and Bases
51. According to Bronsted-Lowry, what are acids?
52. According to Bronsted-Lowry, what are bases?
53. What does amphoteric mean?
54. What is the value of Kw?
55. The [H3O+] is 0.0543 M. What is the pOH?
56. What is [H3O+] in a solution with a pH of 3?
57. The pH of a solution is 7.8. What is the pOH and [H3O+]?
58. Calculate the pH of each solution:
a. [H+] = 1.4 x 10-3 M
b. [H+] = 2.5 x 10-10 M
c. [H+] = 6.1 M
d. [OH-] = 3.5 x 10-2 M
e. [OH-] = 8 x 10-11 M
f. [OH-] = 5.0 M
Week 8: Chemical Changes, Sig Figs, Density, Periodic Trends.
59.
60.
61.
62.
What type of bond is NaCl?
List the seven diatomic elements.
What is the difference between polar and non-polar bonds?
Which of the following is a chemical change?
a. Metal melting into a molten liquid
b. Metal rusting
c. Water expanding as it freezes
d. Ink spreading on paper
e. Cutting paper in half
63. Which of the following is true?
a. chemical changes change the properties of the substance
b. physical changes change the properties of the substance
c. chemical changes always change colors
d. physical changes involve color changes
e. chemical changes is filtering two substances
64. Chemical or physical: ice melting.
65. Metals _____________ electrons. (Gain or lose)
66. Nonmetals ___________ electrons. (Gain or lose)
67. A brick of salt measuring 10.0 cm x 10.0 cm x 2.0 cm weighs 433 grams. What is its density?
68. How many sig figs are in the following number 5700?
69. Is O2 a compound or an element?
70. Is melting ice a physical or a chemical change?
71. Give the definition of a mixture.
72. Is magnesium or chlorine more electronegative?
List the seven diatomic elements.
How many sig figs are in the number 33,516?
Convert 0.25 nanometers to cm.
Write the long electron configuration for chlorine.
What volume of silver metal will weigh exactly 2500.0 grams? The density of silver is 10.5
g/cm3.
78. Draw the periodic trend of ionization energy.
79. What is density equal to?
80. What is the density of 57.8g of NaCl in 147.4mL of water?
83. The density of chlorine is 35.9 g/mL. If you have 20 mL, what is the weight of the sample?
84. Write the electron configuration of nitrogen.
85. Write the noble gas electron configuration of chlorine.
73.
74.
75.
76.
77.
86. Classify each as a solution, colloid or suspension (heterogeneous mixture), element, or
compound:
a. salt water
b. milk
c. sodium
d. carbon monoxide
e. muddy water
f. sweet tea
87. How many electrons are in the valence shell of
a. the halogens
d. boron
b. oxygen
e. neon
c. the alkali metals
f. the alkaline earth metals
g. carbon
h. nitrogen
88. Write the electron configuration for the element copper.
89. What is the weight of the ethyl alcohol that exactly fills a 200.0 mL container? The density of
ethyl alcohol is 0.789 g/mL.
90. How many sig figs are in the number 7.080 x 10-7?
91. Answer with the correct number of sig figs: (37.14 cm)(0.1458 cm)
92. Answer with the correct number of sig figs: 4.57 mL + 89.14 mL
93. Find the density of a sample that weighs 6.39g with the volume of 15mL.
94. If the density of a sample is 15.24 g/mL and the volume is 25mL. Find the mass in grams.
95. Give the longhand electron configuration for Os.
96. The following electron configuration is for what element? 1s22s22p63s23p64s23d104p65s24d4
97. Which one have the highest ionization: N O F Cl
98. How many sig figs are in each of these numbers:
a. 1.543
c.
10250
e.
0.02750
b. 0.003
d.
1.57x1012
f.
27.861
99. What is the full electron and noble gas electron configuration of Sn?
a. Out of the elements Rb, Fe, F, and Se, which one has the highest:
a. atomic radius
b. electronegativity
c. electron affinity
d. ionization energy
100. Write the electron configuration for the following:
a. Ca+2
b. Cl-1
c. Co+1
101. Write the noble gas configuration for:
a. O-2
b. U
102. How many sig figs do each of the following numbers have?
a. 101.000
b. 1012300
c. 0.000032
103. Which has the smallest atomic radius? Ca+2, Na+1, O-2, or Ne
104. Which is most electronegative? C, N, O, F?
c. W
d. 1.09800
e. 0.900
-2-
GO ON TO THE NEXT PAGE.
All My Ions
A List of 85 Ions to MEMORIZE
Cations
Aluminum
Ammonium
Antimony
Al3+
NH4+
(III) Sb3+
(V) Sb5+
Arsenic
(III) As3+
(V) As5+
Barium
Ba2+
Bismuth
(III) Bi3+
(V) Bi5+
Calcium
Ca2+
Cadmium
Cd2+
Chromium (II) or chromous Cr2+
(III) or chromic
Cr3+
Cobalt (II) or cobaltous
(III) or cobaltic
Co2+
Co3+
Copper (I) or cuprous
(II) or cupric
Cu+
Cu2+
Hydrogen
H+
Hydronium H3O+
Iron (II) or ferrous Fe2+
(III) or ferric
Fe3+
week 1
Lead (II) or plumbous
(IV) or plumbic
Lithium
Magnesium
Manganese
Li+
Mg2+
(II) Mn2+
(IV) Mn4+
Mercury (I) or mercurous
(II) or mercuric
Hg2+
Nickel
Potassium
Silver
Sodium
Strontium
(II) Ni2+
(III) Ni3+
K+
Ag+
Na+
Sr2+
Tin (II) or stannous Sn2+
(IV) or stannic
Sn4+
Zinc
Pb2+
Pb4+
Zn2+
Hg22+
Anions
Acetate
C2H3O2Arsenate
AsO43Bicarbonate HCO3Binoxalate
HC2O4Bisulfate
HSO4Bisulfide
HSBisulfite
HSO3Borate
BO33Bromate
BrO3Bromide
BrBromite
BrO2Carbonate
CO32Chlorate
ClO3Chloride
ClChlorite
ClO2Chromate
CrO42Cyanide
CNDichromate Cr2O72Dihydrogen phosphate
H2PO4Ferrocyanide Fe(CN)64Ferricyanide Fe(CN)63Fluoride
FHydroxide
OHHypobromite BrOHypochlorite ClOHypoiodite
IOIodate
IO3Iodide
IIodite
IO2Nitride
N3Nitrate
NO3Nitrite
NO2Oxalate
C2O42Oxide
O2Perbromate BrO4Perchlorate ClO4Permanganate
MnO42Peroxide
O2
Phosphate
PO43Phosphide
P3Phosphite
PO33Sulfate
SO42Sulfide
S2Sulfite
SO32Tartrate
C4H4O62Thiocyanate SCNThiosulfate
S2O32-
week 2
week 3
week 4