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AP Chemistry Summer Assignment 2017-2018
Greetings! Welcome to AP Chemistry!
Dear student and parents/guardians of student,
You are receiving this letter because you have signed up for Advanced Placement Chemistry for
the 2017-2018 school year. In order to be successful in this course it is highly recommended that you have
had successful completion of a first-year high school chemistry course and also had successful completion
of a second-year algebra course.
Why Take AP Chemistry?
There are several reasons why a student might want to take AP Chemistry, including (but not limited to) the following.
1. AP Chemistry will challenge you to the limits of your academic ability. In the past you may have found classes
“too easy”, and therefore not stimulated you do your very best. This will not be the case in AP Chemistry.
2. AP Chemistry should allow you to earn college credit while still enrolled in high school. This will save time and money. Some students who
passed the AP Chemistry exam elect to take first year college chemistry anyway, where they find the material easy review and achieve top grades while other
students around them are frustrated and struggling in a class which is too large and/or the instructor is unavailable for help!
3. Being a “straight A” student no longer carries the weight it once did when applying for college. Many 4.0 grade average students are finding
themselves denied entry at the college of their choice. Taking AP Chemistry is a way to distinguish yourself in high school.
4. AP Chemistry is an intense course where students really get to know each other. It is to a student’s advantage for the teacher to know them well
when they need a letter of recommendation.
The AP Chemistry class is a yearlong college level chemistry course, at the end of which you will take an exam to see your
proficiency in college level Chemistry. The AP Chemistry test is in early May 2018 for all students world-wide. We start school later
then many students (up to a month in some cases!), so we are behind from day 1. Because of this, I require a summer assignment
that assures students are proficient in areas that will help them to be successful throughout the year.  Much of this will be review of
1st year Chemistry, but there will be some “add ons” (for example, naming acid rules). Because of this, you will need to use your
chemistry notebook and access to online chemistry resources. If you do not have online access at home, see me. Summer topics:
1. Math skills: significant figures, metric system, conversions, basic algebra skills
2. Atomic structure: counting subatomic particles, isotopes
3. Nomenclature: naming molecules and compounds (including acids), naming polyatomic ions
4. Balancing equations and identifying types of reactions
5. Solubility rules
6. Stoichiometry: g mol calculations, predicting the mass of product formed, limiting reactants
Your assignment:
1. Complete all practice questions/tasks
2. Self grade your work in a second color (checking the ones correct and marking/second attempt to those incorrect)
Online resources: (If you do not have online access over the summer, please see/email me)
1. My website (this will be a work in progress through the summer- see it for updates!):
https://sites.google.com/a/k12.shorelineschools.org/ap-chemistry/
2. Textbook (for quick help on definitions and topics): https://open.umn.edu/opentextbooks/BookDetail.aspx?bookId=69.
3. Bozeman Science videos (I will make you watch them later anyways!): http://www.bozemanscience.com/ap-chemistry/
4. Khan Academy videos (excellent resource): https://www.khanacademy.org/science/chemistry
5. Crash course videos: https://www.youtube.com/playlist?list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr
6. Sciencegeek website for AP chem students (has lots of good info and resources linked):
http://www.sciencegeek.net/APchemistry/index.shtml
7. AP chemistry college board website: https://apstudent.collegeboard.org/apcourse/ap-chemistry
The summer assignment will be due on the first day of school next fall. During the first week of school, we will have a
proficiency test over what you have done over the summer so that we can use our time as best as possible during the school year.
Since this is a college level course taught in high school, it is very demanding, both in time and effort required. Students
who are heavily involved in after school activities and/or jobs will have to learn to budget their time very carefully. We move at an
incredibly fast pace as there is much to cover before the AP Exam.
Parents/Guardians: This is a class that truly depends on the learning. Not only do students have to do the work but they need
to understand and be able to process what is being done. Since AP Chemistry class is the same world-wide it is easy to find answers to almost
every problem we assign online via search engines. This gives the student the right answer, but does not show them how to do the problem. Please
encourage your student to try things on their own and get help when they need it. Remember, it is not about the grade, it is about the learning.
Recommended Text
Cracking the AP Chemistry Exam by Princeton Review 2017 edition (can be purchased via Amazon)- has lots of practice
problems that we will work from. I have a personal copy that students can reference, but it cannot leave my classroom.
Thank you! I will be online via email periodically (Ha!) throughout the summer if you have questions. I look forward to
exploring deeper about chemistry with you next year!
~Gloria Horne
[email protected]
Summer Homework Assignment:
YOUR JOB: Work through the concepts and practice problems provided. You will use the answer key at the end to check
your work in a second color! If you get a problem wrong, try it again until you get it right! I want to see your work the first day
of school. It is important that you do this work. Some time during the first week of school, you will have a proficiency test
on the concepts in this assignment, so I want you to be prepared when you arrive.
Part I: MATH review! Practice conversion calculations, scientific notation and significant figures! (essential skills in Ch 1
and 3 of online textbook)
1. How many SF in each number?
a. 1234
f. 90210
b. 0.023
g. 1090.0010
c. 890
h. 0.00120
d. 91010
i. 780
e. 9010.0
j. 1000.
2. Convert the following to scientific notation:
a. 1,200,000 ______________
b. 345,450,000 _____________
3. Round the following to 2 sig figs:
a. 0.436 ________
b. 27.2 _________
c. 0.000354 _______________
d. 0.000000045801 _________
c. 9.000 _________
d. 10000.0 _______
Calculations: Perform the following calculations and give the answer with the correct number of sig figs:
4) 628 * 342 = ___________________
5) (5.63 x 102) * (7.4 x 103) = ____________________
6) 2734/28.0 = ______________________
7) 14.98 + 27.340 + 84.7539 = __________________
8) 44.5 – 33.57 = ___________________
9) 8119 x 0.000023 = _____________________
Metric conversions- convert these quantities to the requested units- don’t forget sig figs!
10) 4.32 x 10-2 mL to L
11) 0.0655 kg to g
12) 4.62 x 103 cm to km
Dimensional analysis: Use the conversion factors and common metric conversions to perform the following calculations.
Don’t forget sig figs!
1 lb = 0.454 kg
1 m = 1.09 yd
1 hr = 60 min
1 mile = 1760 yd
1 km = 0.621 mi
1 min = 60 sec.
13) A dog is 28.7 pounds. What is his weight in kg? What is his weight in grams?
14) A marathon is 26.2 miles. What is this distance in yards? What is the distance in meters? (Hint: use your
answer in yards to convert to meters!)
15) Racing cars travel at a speed of 225 miles/hour. What is this speed in km/minute? (Hint: you will need two sets
of conversions- one for time and one for distrance!)
Part II: Atomic structure
Fill in the chart with the chemical name, symbol and number of subatomic particles. The first one has been done for you.
Chemical name
Chlorine
Chemical
symbol
35
131
# of protons
# of
neutrons
# of electrons
Mass number
17
16
18
17
16
35
32
Cl
17
Xe
131
54
13
2
14
N
20
14
40
4
7
7
Phosphorus
31
30
P
15
16) Isotopes: Explain why atoms have different isotopes. In other words, how is it that carbon can exist in three
different forms (carbon-12, carbon-13 and carbon-14)? 15
Part III: Reviewing Nomenclature (Ch 2 of online textbook)
Polyatomic Ions: Please memorize and be able to name compounds using all of the following ions! Making flash cards could help!
1. Table of Polyatomic Ions for AP Chemistry
Symbol
Name
Symbol
Name
BO33–
B4O72
C2H3O2
C2O42
ClO
ClO2
ClO3
ClO4
CN
CO32
CrO42
Cr2O72
Fe(CN)63
Fe(CN)64
HCO3
HC2O4
HPO42
H2PO4
HSO3
HSO4
H3O+
Hg22+
borate
tetraborate
acetate
oxalate
hypochlorite
chlorite
chlorate
perchlorate
cyanide
carbonate
chromate
dichromate
ferricyanide
ferrocyanide
hydrogen carbonate
hydrogen oxalate
hydrogen phosphate
dihydrogen phosphate
hydrogen sulfite
hydrogen sulfate
hydronium
mercury (I)
MnO4
MoO42
N3
NH2
NH4+
NO2
NO3
OH
PO33
PO43
P2O74
SO32
SO42
S2O32
S2O42
S2O62
S2O72
S2O82
SeO42
SiO32
VO3
permanganate
molybdate
azide
amide
ammonium
nitrite
nitrate
hydroxide
phosphite
phosphate
diphosphate
sulfite
sulfate
thiosulfate
dithionite
dithionate
disulfate
peroxydisulfate
selenate
silicate
vanadate
17) Name these binary compounds of two nonmetals.
IF7__________________ N2O5_______________ XeF2 _________________
N2O4_______________ As4O10_______________ SF6________________
PCl3________________ S2Cl2_______________
18) Name these binary compounds with a fixed charge (main group) metal.
AlCl3 _______________ MgO_______________ BaI2_________________
KI_______________ SrBr2 _______________ Na2S _______________
CaF2 _____________ Al2O3_______________
19) Name these binary compounds of cations with variable charge (transition metals).
CuCl2 _____________ Fe2O3______________ SnO_________________
PbCl4______________ Cu2S_______________ HgS_________________
AuI3_______________ CoP________________
20) Name these compounds with polyatomic ions.
Fe(NO3)3_____________ NaOH_____________ Cu2SO4_______________
Ca(ClO3)2_____________ KNO2_____________ NaHCO3______________
NH4NO2______________ Cu2Cr2O7 ___________
21) Name these binary acids – look up acid naming rules!
HCl ________________ HOCl ________________ HI ________________
22) Name these acids with polyatomic ions.
HClO4________________ H2SO4_______________ HC2H3O2____________
H3PO4________________ HNO2_______________ H2CrO4_____________
23) mixed bag: Name these compounds appropriately.
CO________________ NH4CN ___________ HIO3_______________ NI3_______________
AlP _______________ OF2_____________ LiMnO4____________ HClO _____________
NaH2PO4_____________ SO2_______________ CuCr2O7____________ K2O______________
FeF3______________ KC2H3O2__________ MnS______________
24) Write the formulas.
Tin (IV) phosphide__________
copper (II) cyanide_____________
Magnesium hydroxide____________
sodium peroxide_____________
Sulfurous acid____________
lithium silicate __________
Potassium nitride ____________
chromium (III) carbonate____________
Gallium arsenide______________
cobalt (II) chromate____________
Zinc fluoride________________
dichromic acid________________
Part IV: Solubility rules
25) Review the solubility rules found in your notes from last year, or in Chapter 4: precipitation reactions of the online text book,
Identify each of the following compounds as soluble or insoluble in water.
Na2CO3___________
CoCO3_______________
Pb(NO3)2___________
K2S______________
BaSO4________________
(NH4)2S ___________
AgI______________
Ni(NO3)2______________
KI________________
FeS______________
PbCl2_________________
CuSO4_____________
Li2O_____________
Mn(C2H3O2)2___________
Cr(OH)3______________________________
AgClO3 __________
SnS2 _______________
FeF2______________
26) Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the products. If yes,
identify the precipitate. (Hint: it may help to look up the definitions of a double replacement reaction and of a precipitate).
a) silver nitrate and potassium chloride _________
b) strontium bromide and potassium sulfate ________
c) cobalt (III) bromide and potassium sulfide __________
d) ammonium hydroxide and copper (II) acetate __________
e) lithium nitrate and chromium (III) fluoride ___________
Part IV: Balancing Equations
27) Balance the following equations with the lowest whole number coefficients.
a) S8 + O2  SO3
b)
C10H16 + Cl2  C + HCl
e)
KClO3  KCl + O2
f) H3AsO4  As2O5 + H2O
c) Fe + O2  Fe2O3
g) V2O5 + HCl  VOCl3 + H2O
d) C7H6O2 + O2  CO2 + H2O
h) Hg(OH)2 + H3PO4  Hg3(PO4)2 + H2O
Part V: Stoichiometry and Limiting Reactants (Khan Academy is best for this)
28) Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide?
Na2O + H2O  2NaOH
29) What mass of sodium chloride is formed if 45.0g of oxygen gas is also formed?
2NaClO3  2NaCl + 3O2
30) What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen?
4NH3 + 5O2  4NO + 6 H2O
31) If the reaction in #30 is done with 25.0g of each reactant, which would be the limiting reactant (also called limiting
reagent)? How many moles of each product would form?
32) Na2S + 2AgNO3  Ag2S + 2NaNO3
a) If the above reaction is carried out with 35.0g of sodium sulfide and 50.0g of silver nitrate, which is the limiting
reactant?
b) What mass of silver sulfide would precipitate?
c) challenge- try it!! What mass of the excess reactant remains?
33) What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium hydroxide with 50.0g of
aluminum?
6NaOH + 2Al  2Na3AlO3 + 3H2
END OF ASSIGNMENT
Answers:
1.
a.
b.
2.
a.
b.
3.
a.
b.
4
2
c. 2
d. 4
e. 5
f. 4
g. 8
h. 3
1.2 x 106
3.4545 x 108
c. 3.54 x 10-4
d. 4.5801 x 10-8
0.44
27
c. 9.0
d. 1.0 x 104
4. 215000
5. 4200000
6. 97.6
7. 127.07
8. 10.9
9. 0.19
10. 4.32 x 10-5 L or 0.0000432 L
chart:
Chemical name
Chlorine
sulfur
xenon
i. 2
j. 4
11. 65.5 g
12. 0.04620 km
13. 13.0 kg, 13000g
14. 46100 yd, 42300 m
15. 6.04 km/min
Chemical
symbol
# of
protons
# of
neutrons
# of
electrons
Mass number
17
18
17
35
S
16
16
16
32
Xe
54
77
54
131
Ca
20
20
20
40
35
17
Cl
32
16
131
54
Calcium
40
20
aluminum
27
13
Al
13
14
13
27
helium
4
2
He
2
2
2
4
7
7
7
14
Nitrogen
14
7
Phosphorus
31
15
P
15
15
16
31
Phosphorus
30
15
P
15
15
15
30
N
16. They have different numbers of neutrons (and a different mass), but they all have the same number of
protons (same element)
17. IF7 Iodine heptafluoride N2O5 dinitrogen pentoxide XeF2 xenon difluoride
N2O4 dinitrogen tetraoxide As4O10 tetraarsenic decoxide SF6 sulfur hexafluoride
PCl3 phosphorus trichloride S2Cl2 disulfur dichloride
18. AlCl3 aluminum chloride MgO magnesium oxide BaI2 barium iodide
KI potassium iodide SrBr2 strontium bromide Na2S sodium sulfide
CaF2 calcium fluoride Al2O3 aluminum oxide
19. CuCl2 copper II chloride Fe2O3 iron III oxide SnO tin II oxide
PbCl4 lead IV chloride Cu2S copper I sulfide HgS mercury II sulfide
AuI3 gold III iodide CoP cobalt III phosphide
20. Fe(NO3)3 Iron III nitrate NaOH sodium hydroxide Cu2SO4 copper I sulfate
Ca(ClO3)2 calcium chlorate KNO2 potassium nitrite NaHCO3 sodium hydrogen carbonate
NH4NO2 ammonium nitrite Cu2Cr2O7 copper I dichromate
21. HCl hydrochloric acid HOCl hypochlorous acid HI hydroiodic acid
22. HClO4 perchloric acid H2SO4 sulfuric acid HC2H3O2 acetic acid
H3PO4 phosphoric acid HNO2 nitrous acid H2CrO4 chromic acid
23. COcarbon monoxide NH4CN ammonium cyanide HIO3 iodic acid NI3 nitrogen triiodide
AlP aluminum phosphide OF2oxygen difluoride LiMnO4lithium permanganate HClO hypochlorus acid
NaH2PO4 sodium dihydrogen phosphate SO2 sulfur dioxide CuCr2O7copper II dichromate K2Opotassium oxide
FeF3 Iron III fluoride KC2H3O2 potassium acetate MnS manganese II sulfide
24. Tin (IV) phosphide Sn3P4
copper (II) cyanide Cu(CN)2
Magnesium hydroxide Mg(OH)2
sodium peroxide Na2O2
Sulfurous acid H2SO3
lithium silicate Li2SiO3
Potassium nitride K3N
chromium (III) carbonate Cr2(CO3)3
Gallium arsenide GaAs
cobalt (II) chromate CoCrO4
Zinc fluoride ZnF2
dichromic acid H2Cr2O7
25. Na2CO3 soluble
K2S soluble
CoCO3 insoluble
BaSO4 insoluble
Pb(NO3)2 soluble
(NH4)2S soluble
AgI insoluble
Ni(NO3)2 soluble
KI soluble
FeS insoluble
PbCl2 insoluble
Li2O soluble
Mn(C2H3O2)2 soluble Cr(OH)3 insoluble
AgClO3 insoluble
CuSO4 soluble
SnS2 insoluble
FeF2 insoluble
26. silver nitrate and potassium chloride solid = AgCl
strontium bromide and potassium sulfate SrSO4
cobalt (III) bromide and potassium sulfide Co2S3
ammonium hydroxide and copper (II) acetate Cu(OH)2
lithium nitrate and chromium (III) fluoride none
27.
a. S8 + 12 O2  8 SO3
e. 2KClO3  2KCl +3 O2
b. C10H16 + 8Cl2  10 C + 16HCl
f. 2H3AsO4  As2O5 + 3H2O
c. 4Fe + 3O2  2Fe2O3
g. V2O5 + 6HCl  2VOCl3 + 3H2O
d. 2C7H6O2 + 15O2  14CO2 + 6H2O
h. 3Hg(OH)2 + 2H3PO4  Hg3(PO4)2 + 6H2O
28. 2.90 g
29. 54.6 g
30. 158.8 g
31. oxygen is LR, 0.625 mol NO, 0.938 mol H2O
32.
a. silver nitrate
33. 21.0 L H2 (L.R.  NaOH)
b. 36.5 g
c. 23.5 g