Download welcome to ap chemistry - Garnet Valley School District

Welcome to AP Chemistry!
I am delighted that you have chosen to take AP chemistry this fall. It is a
challenging course and a strong foundation is necessary for your success.
The material included in the summer work packet will enable you to
cover the basics of chemistry, which are covered in chapters 1, 2, 3 and 4
of the textbook: Chemistry: A Molecular Approach by Nivaldo J. Tro.
The topics covered are chemical formulas, equation writing and
balancing, formula and reaction stoichiometry, gas laws and solutions.
This will be review for some of you, but new for others so spend plenty of
time making sure you understand this material during the summer.
The work is split into two assignments: One for all students and an
additional one for students who have not taken Honors Chemistry. The
work is split into a weekly schedule, but you may also complete it at your
own pace. However, I would recommend you do not procrastinate, and
that you give yourself time to review what you have learned over the
summer prior to your return to school. We will go over this material
very quickly in class before moving on to new topics.
Please contact me if you are struggling to understand the chemistry or if
you have any other questions. I will be around most of the summer
except for the last week of June and the last two weeks of July. I am
looking forward to working with you next school year.
Have a great summer!
Yours sincerely,
Dr. Liz Bish
[email protected]
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Summer Assignment for Students who have not taken
Honors Chemistry
This assignment is due on September 8, 2015.
Textbook: Living By Chemistry
Author: Angelica M. Stacy
Copyright: 2010
Read through the material in the textbook and answer the section and review questions
as listed below. You may also work through the lesson questions, if necessary, to ensure
you understand the concepts covered. For calculations show all your work.
Week 1: Unit 1 Alchemy: Matter, atomic structure and bonding
Page 21: questions 1 – 6
Page 51: questions 1 – 4
Page 84: questions 1 – 4
Page 123: questions 1 – 6
Page 140: questions 1 – 4
Alchemy Review, pages 141 - 142: questions 1 – 12
Week 2: Unit 2 Smells: Molecular structure and properties
Read Lessons 3, 4, 5, 10, 11, 15, 16, and 17 and answer the questions for
those lessons.
Week 3: Unit 3 Weather: Phase changes and behavior of gases
Page 288: questions 1 – 5
Page 321: questions 1 – 5
Page 343: questions 1, 3, 4 and 5
Weather Review, pages 345 - 346: questions 1 – 13
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Week 4: Unit 4 Toxins: Stoichiometry, solution chemistry, and acids and bases
Page 373: questions 1,3 and 4
Page 398 - 399: questions 1, 3, 4, 5, and 6
Page 418: questions 1 – 8
Page 449: questions 1 – 5
Page 470: questions 1 – 3
Toxins Review, pages 471 - 472: questions 1 – 12
Week 5: Unit 5 Fire: Energy, thermodynamics, and oxidation-reduction
Page 502 - 503: questions 1 – 8
Page 520: questions 1 – 4
Page 540 - 541: questions 1 – 6
Page 564: questions 1 – 5
Fire Review, pages 565 - 566: questions 1 – 15
Week 6: Unit 6 Showtime: Reversible reactions and chemical equilibrium
Page 595: questions 1 – 5
Page 612 - 613: questions 1 – 5
Showtime Review, pages 614 - 615: questions 1 – 10
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Summer Assignment for All Students Taking AP Chemistry
This assignment is due on Tuesday September 8, 2015.
The summer work will be assessed with an Honors level test on Friday September 11,
2013. After further study, review, and problem practice, an AP level test on this
material will be given on September25, 2013.
Textbook: Chemistry: A Molecular Approach
Author: Nivaldo J. Tro
Copyright: 2014
Review and then complete one chapter per week.


Review: Complete “Chemistry 1 Review” (separate document) and the Reactions
Review”
Memorize: The “Common Ions” sheet and the “Solubility Rules” on page 161 in
“Tro”.

Chapter 1: Matter, Measurement, and Problem Solving
Pages 1 to 43: Complete the
“Chapter in Review – Self Assessment Quiz” (page 34)
“Review Questions” 1 – 31 (pages 36 – 37)
“Problems by Topic” 33 – 87 odd numbers only and as many unit
conversions as you need to. (pages 37 – 40)
“Conceptual Problems” 141, 142, 143, 145, and 147 (pages 42 – 43)
The answers to the blue questions are in the back of the book. Use them only as
a comparison; it is important for you to know how to do the problems. Show all
work.

Chapter 2: Atoms and Elements
Pages 44 to 85: Complete the
“Chapter in Review – Self Assessment Quiz” (pages 75 – 76)
“Review Questions” 1 – 28 (pages 78 – 79)
“Problems by Topic” 29 – 93 odd numbers only (pages 79 – 82)
“Conceptual Problems” 131, 133, and 135 (page 84)
The answers to the blue questions are in the back of the book. Use them only as
a comparison; it is important for you to know how to do the problems. Show all
work.
4

Chapter 3: Molecules, Compounds and Chemical Equations
Pages 86 to 137: Complete the
“Chapter in Review – Self Assessment Quiz” (pages 126 – 127)
“Review Questions” 1 – 19 (page 130),
“Problems by Topic” 23 – 109 odd numbers only (pages 130 – 134)
“Conceptual Problems” 155, 157, and 159 (page 136)
The answers to the blue questions are in the back of the book. Use them only as
a comparison; it is important for you to know how to do the problems. Show all
work.

Chapter 4:
Pages 138 to 193: Complete the
“Chapter in Review – Self Assessment Quiz” (pages 182 – 183)
“Review Questions” 1 – 24 (page 186),
“Problems by Topic” 25 – 97 odd numbers (pages 186 – 190)
“Cumulative Problems” 99 – 123 (pages 190 – 191)
“Conceptual Problems” 135, and 137 (page 192)
The answers to the blue questions are in the back of the book. Use them only as
a comparison; it is important for you to know how to do the problems. Show all
work.
5
Chemistry 1 Review
1. Write the names of the following compounds
a)
XeF4
b)
Ca(OH)2
c)
H2SO4
d)
K2CO3
e)
N2O3
f)
CuBr2
g)
Mn(SO4)2
h)
SCl6
i)
HNO3
j)
KMnO4
2. Write the formulas of the following compounds
a) silver chromate
f) strontium cyanide
b) sodium phosphate
g) sulfur dioxide
c) acetic acid
h) potassium phosphide
d) iron (III) oxide
i) manganese (IV) hydroxide
e) phosphorus pentoxide
j) ammonium sulfate
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3. The total pressure of a mixture of gases (H2, CO2, and O2) is 235 kPa. The partial
pressures of CO2 and O2 are 102.3 kPa and 58.2 kPa respectively. What is the
partial pressure of the H2?
4. What is the pH of the following solutions:
a) [H+] is 3.6 x10-12
b) [H+] is 3.4 x10-5
c) [OH-] is 1.0 x10-7
d) [OH-] is 8.2 x10-3
e) [OH-] is 2.1 x10-10
5. Are the solutions in question 4 neutral, acidic, or basic?
6. Calculate the percent composition of Cu3(PO4)2
7. How many moles are there in 0.34L of nitrogen gas?
8. Write the formulas for the following compounds:
a) diphosphorus pentoxide
e) silver carbonate
b) cupric phosphate
f) tin (II) chloride
c) calcium fluoride
g) magnesium hydroxide
d) nickel nitrite
h) chloric acid
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9. If a solution has a pOH of 4 what is the pH?
10. Make sure the answers to the following calculations have the correct number
of significant figures and the correct units.
a) 3.2105cm x 4.56cm
b) 4.5g / 2.34 mL
c) 5.67cm x 0.002 cm x 3.6 cm
11. Classify these processes as exothermic or endothermic.
a)
burning alcohol
b)
photosynthesis
c)
baking a potato
d)
freezing ice cream
12. There are five naturally occurring isotopes of the element A. The relative
abundance and mass of each are as follows:
48.89%, 33.929 amu
27.81%, 35.926 amu
4.11%, 36.927 amu
18.75%, 37.925 amu
0.62%, 39.925 amu
Calculate the average atomic mass of A.
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13. A sample of oxygen at 24°C has a volume of 1.32 L and a pressure of
756mmHg. What is the mass of the oxygen?
14. Why does ammonia have a much higher boiling point (-33 C) than methane
(-164C) although their molar masses are almost the same?
15. In a solution the concentration of hydrogen ions, [H+], is 1x10-12. What is the
concentration of hydroxide ions, [OH-]? Is the solution neutral, acidic or basic?
16. What is meant by 3p3?
17. How many molecules are there in:
a) 0.86 moles of CH4
b) 46.3 g of SO3
c) 71.85 g of C6H12O6
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18. Round the following to the correct number of significant figures:
a) 0.00342892
(3 sig. fig.)
b) 3423
(2 sig. fig.)
c) 144.98
(1 sig. fig.)
19. How much copper (I) chloride can be produced beginning with 75.0g of
copper (I) oxide?
Cu2O + 2HCl  2CuCl + H2O
20. What pressure in atmospheres does a gas exert at 385mm Hg?
21. The unbalanced equation for the reaction of ammonia and chlorine gas is
NH3(g) + Cl2(g)  NH4Cl (s) + NCl3(g)
45.6g of ammonia reacts with 68.5 g of chlorine.
a) Balance the equation.
b) Which is the limiting reagent?
c) What is the theoretical yield of ammonium chloride?
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22. How much faster does helium diffuse compared to oxygen?
23. How much 0.3 M H2SO4 is needed to neutralize 34.0 mL of a 0.25 M solution of
NaOH?
24. What are the three rules that govern the filling of atomic orbitals by electrons?
25. 34 mL of nitrogen gas is collected over water at 20°C. The barometric pressure
is 1.06 atm. What is the pressure of the dry nitrogen? Calculate the mass of the
dry nitrogen. Vapor pressure of water at 20°C is 17.5 mm Hg.
26. Which of the following substances dissolve in water? Why?
a)
CH4
b)
MgSO4
c)
Cane sugar
27. The density of osmium, which is the densest metal, is 22.57g/cm3. What is the
mass of a block of osmium that measures 4.30 cm x 7.89 cm x 3.5 cm. (sig. fig.)
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28. The formulas CaCl2 and CuCl2 look very similar. What is the name for each
compound? Why do we name them differently?
29. If a 1 kg block of ice at -28C is heated until it is water at 23C, how much
energy (in Joules) is required?
30. What type of reactions are the following?
a) Na2O + CO2
 Na2CO3
b) 3 Pb(NO3)2 + 2 (NH4)3PO4  6 NH4NO3 + Pb3(PO4)2
c) 2 C4H10 + 13 O2  8 CO2 + 10 H2O
d) 2 NaClO3  2 NaCl + 3 O2
e) 3 Mg + 2 FeCl3  3 MgCl2 + 2 Fe
31. Find the empirical formula of each compound from its % composition.
a) 65.2% Sc and 34.8% O
b) 52.8% Sn, 12.4% Fe, 16.0% C, and 18.8% N.
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32. Balance this equation.
Ag2SO4 + AlCl3  AgCl + Al2(SO4)3
33. What is the volume of a 0.4 M solution containing 256.8 g of glucose
(C6H12O6)?
34. If 8.69 L propane burns in excess oxygen, how many moles of carbon dioxide
will be produced? Assume STP.
C3H8 + O2  H2O + CO2
(unbalanced)
35. Calculate the molar mass of the following compounds
a) Na2CrO4
b) Al(NO3)3
36. Predict the product, complete and balance the equation, then write the net
ionic equation for this reaction.
Aqueous barium chloride is added to aqueous potassium sulfate.
37. If a clear saturated solution of sodium nitrate is cooled, what change(s) might
you observe?
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38. The unbalanced equation for the reaction of sodium oxide and water is
Na2O s) + H2O (l)
NaOH (aq)
18.7 g of sodium oxide (Na2O) reacts with 32.4g of water.
a) Balance the equation.
b) Which is the limiting reagent?
c) When the reaction is complete, how much of the excess reagent is
remaining?
d) What is the theoretical yield of sodium hydroxide?
39. When 84.8g of iron (III) oxide reacts with an excess of carbon monoxide, 54.3g
of iron is produced. What is the percent yield of this reaction?
Fe2O3 (s) + 3CO (g)  2Fe (s) + 3CO2 (g)
40. How many grams of K2CO3 are needed to prepare 225 mL of a 0.45 M solution?
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41. Calculate the number of grams of solute required to make 150 mL of 4% MgCl2
(m/v).
42. 15.0mL of 0.6M Mg(OH)2 neutralized 65.0mL of HNO3. Determine the
concentration of the acid.
43. Write the complete electron configuration, the shorthand configuration, and
the orbital notation for arsenic.
44. In an experiment, 367g of metal at 100°C is dropped into 150g of water at
14°C. If the temperature of the water rises to 23°C, what is the specific heat
capacity of the metal?
45. A company producing ammonia did a trial reaction using 10.0 L of nitrogen.
The reaction produced 11.23 g of ammonia, NH3. Do you think these reaction
conditions produced a high enough percent yield to make the new process
economically acceptable? Show all work.
N2 (g) + 3H2 (g)  2NH3 (g)
46. You have the following stock solution available: 4.0 M KNO3. Calculate the
volume you must dilute to make 125 mL of 0.65 M KNO3.
15
47. A vial contains 0.500g of an unknown monoprotic acid. How would you
determine the molar mass of the acid using a solution of 0.120 M sodium
hydroxide and the technique of titration?
a) Lab equipment
b) Procedure
c) Measurements
d) Calculations
48. Draw a molecular level diagram showing a solid, a liquid, and a gas.
49. Draw a molecular level diagram to illustrate the difference between an atomic
element, a molecular element, and a compound.
50. Draw a molecular level diagram to illustrate vapor pressure.
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51. Draw a molecular level diagram to illustrate an ionic compound dissolving in
water.
52. Draw atom diagrams to illustrate the difference between a fluorine atom, a
neon atom, a sodium atom, a fluoride ion and a sodium ion.
53. A solution of hydrochloric acid reacts with a solution of potassium hydroxide.
a) Predict the products and write a balanced equation for this reaction.
b) Write a balanced net ionic equation for this reaction.
c) Draw a molecular level diagram to illustrate the net ionic equation for
this reaction.
54. Sodium hydrogen carbonate is often used in baking. When it decomposes it
produces water vapor, carbon dioxide and sodium carbonate. Write a balanced
equation for this reaction and then draw a molecular level diagram to illustrate
the reaction.
55. Make a list of all the questions in this review that you had difficulty with.
17
Chemical Reactions Review
Part 1: Write and balance the equations for the following reactions:
Oxidation-Reduction Reactions.
Synthesis
1. Ammonia gas (NH3) reacts with carbonic acid to form solid ammonium
carbonate.
2. Calcium metal reacts with chlorine gas.
3. Lithium metal reacts with oxygen gas.
4. Barium metal reacts with sulfur.
Decomposition
1. Solid potassium chlorate decomposes to give solid potassium chloride and
oxygen gas.
2. Solid calcium carbonate decomposes to give solid calcium oxide and carbon
dioxide gas.
3. Solid iron (III) oxide decomposes.
4. Solid nitrogen triiodide decomposes.
Combustion
1. Methane gas (CH4) burns in excess oxygen.
2. Liquid heptane (C7H14) burns in excess oxygen.
18
Single displacement
1. Potassium metal reacts with water to form potassium hydroxide solution and
hydrogen gas.
2. Strontium metal reacts with aqueous chromium (III) chloride.
3. Fluorine gas reacts with aluminum chloride solution.
4. Zinc metal reacts with phosphoric acid.
Double Displacement Reactions
Precipitation
1. Aqueous sodium sulfate reacts with aqueous calcium bromide.
2. Aqueous lead (IV) nitrate reacts with aqueous potassium sulfide.
3. Aqueous silver acetate reacts with aqueous iron (III) iodide.
4. Aqueous sodium phosphate reacts with aqueous lead (II) chloride
Acid-Base
1. Nitric acid reacts with aqueous barium hydroxide.
2. Phosphoric acid reacts with aqueous sodium hydroxide.
3. Sulfuric acid reacts with aqueous ammonium hydroxide.
4. Hydrochloric acid reacts with aqueous potassium carbonate
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Part 2: Identify the type of reaction for the following reactions.
1. 2Li (s) + 2 H2O (l)  2 LiOH (aq) + H2 (g)
2. 2 H2 (g) + O2 (g)  2 H2O (l)
3. 3 Ag2SO4(aq) + 2AlCl3 (aq)  6 AgCl (s) + Al2(SO4)3 (aq)
4. 2 C2H6 (g) + 7 O2 (g)  6 H2O (g) + 4 CO2 (g)
5. Zn (s) + 2AgNO3 (aq)  Zn(NO3)2 (aq) + 2 Ag (s)
6. 2 AgO (s)  4 Ag (s) + O2 (g)
7. 2 HCl (aq) + Ca(OH)2 (aq)  CaCl2 (aq) + 2 H2O (l)
8. Cl2 (g) + 2 KI (aq)  2 KCl (aq) + I2 (g)
Part 3: Predict the products of these reactions and then write and balance the
equations.
5. Liquid hexane (C6H14) burns in excess oxygen.
6. Lithium metal reacts with oxygen gas.
7. Aqueous lead (IV) nitrate reacts with aqueous potassium sulfide.
8. Chromium metal reacts with phosphoric acid.
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9. Sulfuric acid reacts with ammonium hydroxide.
10. Solid nitrogen triiodide decomposes.
Part 4: Determine whether a reaction will take place or not. If the reaction will not
take place, write “No Reaction”. If it will, write “Yes”. You do not need to write a
balanced equation. Hint use solubility rules and an activity chart.
1. cobalt metal + nitric acid 
2. Gold metal + copper (II) chloride solution 
3. Copper (II) bromide + Iron (III) nitrate 
4. potassium acetate solution and silver nitrate solution
5. Aluminum + zinc sulfate 
6. Barium chloride + lithium hydroxide 
7. Magnesium sulfate + silver nitrate 
8. Bromine + sodium chloride solution 
21
Part 4: Classify the following reactions then write a balanced equation for each one. If
the reaction will not take place, write “No Reaction”.
1. Magnesium metal + nitric acid 
2. Strontium metal + liquid bromine 
3. Calcium metal + water 
4. Aluminum oxide 
5. Copper metal + zinc chlorate solution 
6. Barium hydroxide solution + hydrochloric acid 
7. Butane gas (C4H10) +oxygen gas 
8. Copper (II) bromide + ammonium hydroxide 
9. Sodium iodide 
10. Magnesium + oxygen 
11. Sodium acetate solution and lead (II) sulfate solution
12. Aluminum + lead (II) nitrate 
13. Sulfuric acid + lithium hydroxide 
14. Magnesium sulfate + silver nitrate 
22
Part 5: For the following reactions determine the products, if any, by using the
solubility rules. Then write the formula equation, the complete ionic equation, and
the net ionic equation.
1. Aqueous potassium hydroxide is mixed with aqueous iron (III) nitrate
2. Aqueous silver nitrate is added to aqueous sodium chromate
3. Aqueous nickel nitrate is added to aqueous potassium carbonate
4. Aqueous copper nitrate is added to aqueous sodium chloride
5. Acetic acid is added to aqueous sodium hydrogen carbonate
6. Hydrochloric acid is added to aqueous sodium sulfite
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