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Advanced Placement (AP) Chemistry Summer Assignment
June 2015
To the AP Chemistry Student:
Welcome to my AP Chemistry class! I am looking forward to helping you gain a deeper appreciation for the science of
chemistry and how it impacts our lives. I hope you are looking forward to an exciting and challenging year. Since you
have elected to take this course, I assume you have the intelligence and motivation needed to be successful. Your hard
work will pay off, and you will find AP Chemistry to be a very rewarding experience.
The Advance Placement Chemistry experience is designed to provide a full year of college-level chemistry, so it places
heavy demands on the student, especially in terms of the time commitment required. In fact, the College Board
suggests that students devote a minimum of five hours per week for individual study outside of the classroom. The
ultimate objective, of course, is to prepare you to take the AP Chemistry test in May 2016, and in order to accomplish
this, topics are covered very quickly. For this reason, most students take AP Chemistry after they already completed a
year of high school chemistry, since that provides them with a solid foundation. In order to ensure the best start for you
next fall, I prepared a Summer Assignment that reviews many basic chemistry concepts. You will find much of the
material in the summer assignment to be very familiar. This is a required assignment, and your first assessment in MP1
will be drawn from topics in the Summer Assignment.
The problems in the Summer Assignment will help you build a foundation in chemistry and contribute to your success.
It is important that everyone come to the first day of class well prepared! Extensive remediation is not an option as we
work towards our goal of becoming completely prepared for the AP Exam in early May, so seek help early if you are
floundering.
There is a vast amount of chemistry help available on the Internet. With ready access to these websites in your home,
school or at the local library, I am confident that you will have everything you need to learn chemistry at the AP level.
Finally, I recommend that you spread out the Summer Assignment, rather than trying to complete it in the final week of
the summer! It takes time for a student to process, practice and subsequently learn chemistry at the level necessary for
success in AP Chemistry. Remember, AP Chemistry is an equivalent course to an Introductory Chemistry college
course, a full year program. Taking a college level course in high school is difficult, and it requires commitment,
hard work and time, but completion of a class like this is a great investment in your education. Prepare yourself and
arrive ready to learn!
You may contact me by email over the summer, and I will do my best to respond quickly. ([email protected])
Have a great summer and enjoy the chemistry.
Mrs. Johnson 
Mountain View High School
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Some Tips on How to Survive AP Chemistry:
So you have embarked on a journey to prevent yourself from taking the first semester of General Chemistry
in college. Your less ambitious friends are going to call you crazy, but even if you fail to succeed in getting
college credit, you have much to gain from this course. The key is keeping awake and thinking outside the
box.
1.
Review all of your old notes from chemistry class. If you don't have those, ask somebody who has taken neat notes from a prior class
and study those. The main point here is to simply refresh your memory: you're not going to remember it all or even be close.
2.
3.
Walk into AP Chemistry with some confidence. Don't be intimidated: just do it.
Take notes and make flashcards of ideas and formulas. Try to synthesize your own flashcards and not just copy from the book and
your notes.
Read the chapter at least three times before the test. Sounds like overkill, but it’s not.
4.

"How should you study? Study like there's going to be an exam on the material the next morning. If you study like that, you
won't have to worry about cramming for the exam later." - Unknown professor.
5.
Keep in mind your fundamental properties of everything chemistry related. Start with the basic states of matter and end with the
chemical properties such as pH and electronegativity. Cover the bases.
6.
7.
Don't be afraid of pH. Will it hurt you to do outside practice problems from the Internet? Of course not.
Use the Internet often for extra practice. There are countless resources out there on the Internet, and the problems are all different. You
won't get just a narrow mental work out.
8.
9.
10.
11.
Watch your stoichiometry. A lot of problems will be set up perfectly within the problem itself, so keep your eyes peeled.
Memorize strong acids and bases. They ionize 100%, and are therefore very important.
It's okay if you don't get something right the first time. Try again and again, until you can do it perfectly.
Work through old tests and practice tests on the Internet. These will help you get used to the type of questions you'll be asked in the
exam. Plenty of practice could mean the difference between passing and failing the exam.
12.
13.
14.
Make mnemonic devices for everything. It especially helps with cations and anions.
Do all of your homework assignments. Some teachers look simply for effort.
Practice makes perfect test scores. By doing problems related to your current material, you can be fully readied for that material's test or
quiz.
15.
If you don't understand then learn chemistry in a funny way by renaming concepts which you like.
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Summer Assignment June 2015
Part 1:
Memorize the four sheets given (polyatomic ions, strong acids and bases, solubility rules and nomenclature of acids and
their salts). You may use the sheets given here or the sheets you are familiar with from last year.
a.
A quiz will be given within the first two days of school on these four items. (25 points)
Part 2:
Complete the attached questions to the best of your ability.
b.
The complete questions packet will be worth 100 points and is due the first day of school. You will
be graded partially on completion and correct answers.
The problems are a constant review so it is important to be working on the problems all summer. Some of the questions
are similar but are spread out throughout the packet in order to give you the best review.
Use Internet resources, textbooks (your own textbook) and my own reference material as you complete these
problems. The URLs represent a fraction of the available chemistry addresses available. Please feel free to expand the
list and find other web sites that help prepare you for the coming year. I recommend that you complete as many online
quizzes as possible, take detailed notes, and practice the items indicated in the packet.
A completed packet and all work, showing all calculations, must be submitted the first day of school. Late work
will not be accepted. A list of College Board-approved textbooks has been provided for your reference. You
certainly do not need all the books to complete the assignment; any basic chemistry textbook will suffice.
Useful links:
http://highschoolhub.org/hub/chemistry.cfm ; http://www.chemistrycoach.com/home.htm
http://www.collegeboard.com/ap/students/chemistry/index.html
www.chemmybear.com
Part 3:
Familiarize yourself with your new AP Chemistry textbook. The first two weeks of school we will be reviewing the
first five chapters while spending a little more time in chapter 5 (Gases) and will also discuss organic compounds on a
deeper level. We will then begin working through the chapters that deal more heavily with math. Which are:

6-Thermochemistry
 17-Free Energy and Thermodynamics
 18-Electrochemistry
 12-Solutions
 13-Chemical Kinetics
 14-Chemical Equilibrium
 15-Acids and Bases
 16-Aqueous Ionic Equilibrium
To finish the course, we will work through the chapters that deal with more memorization and understanding patters.
These chapters are:
 7-The Quantum Mechanical Model of the Atom
 8-Periodic Properties of the Elements
 9-Chemical Bonding I
 10-Chemical Bonding II
 11- Liquids, Solids, and Intermolecular Forces
We will then review for your exam, which is in early May, and finish the year discussing organic chemistry and
biochemistry (chapters 20 and 21).
Part 4: Review Problems by Topic (36 points)
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To start, you will need to read chapters 1-5 and complete at least three pages of three column notes for each
chapter. These will also be due the first day of school. (75 pts) Be sure to look through the rest of the text also.
Part 1: Memorization
Strong Acids and Bases
Strong acids dissociate completely in water, so the reaction goes to completion and they never reach
equilibrium with their conjugate bases. Because there is no equilibrium, there is no equilibrium constant, so there is no
dissociation constant for strong acids and bases.
Strong Acids: HCl, HBr, HI, HNO3, HClO4, and H2SO4
Strong Bases: LiOH, NaOH, KOH, Ba(OH)2 and Sr(OH)2
Solubility Rules for Ionic Compounds in Water
The following cations are considered:
1)
2)
3)
4)
5)
6)
7)
alkali metals and NH4+ (similar reactivity), alkaline earth metals
Al3+
Sn2+, Pb2+
Cr3+
Mn2+
Fe2+, Fe3+, Co2+, Ni2+
Cu2+, Ag+, Zn2+, Cd2+, Hg22+ (= "Hg+"), Hg2+
There is no completely insoluble compound; they are often classified as "mostly soluble" or "mostly (nearly)
insoluble." For brevity I will use “soluble” and “insoluble.”
Soluble salts with the following anions:
NO3-, C2H3O2-, ClO3-, ClO4-, FCl-
(except: Ag+, Hg22+, Pb2+)
Br-
(except: Ag+, Hg22+, Hg2+, Pb2+)
I-
(except: Ag+, Hg22+, Hg2+, Pb2+)
SO42-
(except: Ca2+, Sr2+, Ba2+, Hg22+, Hg2+, Pb2+)
Insoluble salts with the following anions
S2-
(except: alkali and alkaline earth , NH4+)
CO32-
(except: alkali, NH4+)
SO32-
(except: alkali, NH4+)
PO43-
(except: alkali, NH4+)
OH-
(except: alkali, Ba2+, Sr2+, Ca2+)
O2-
(except: alkali, Ba2+, Sr2+, Ca2+;  reacts with H2O to form OH-)
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Polyatomic Ions
Name
ammonium
acetate
bromate
chlorate
chlorite
cyanide
dihydrogen phosphate
hypochlorite
hydrogencarbonate(bicarbonate)
hydrogen sulfate (bisulfate)
hydrogen sulfite (bisulfite)
hydroxide
iodate
nitrate
nitrite
perchlorate
permanganate
thiocyanate
carbonate
chromate
dichromate
oxalate
selenate
silicate
sulfate
sulfite
phosphate
phosphite
Symbol
NH4
C2H3O2
BrO3
ClO3
ClO2
CN
H2PO4
ClO
HCO3
HSO4
HSO3
OH
IO3
NO3
NO2
ClO4
MnO4
SCN
CO3
CrO4
Cr2O7
C2O4
SeO4
SiO3
SO4
SO3
PO4
PO3
Charge
+1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-2
-2
-2
-2
-2
-2
-2
-2
-3
-3
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Nomenclature of Acids and Their Salts
1)
Binary Acids:
Binary acids contain only one hydrogen and one more element. The names of acids and corresponding ions are
derived from the element name.
Acid: “hydro” + (element) + “ic” Anion: (element) + “ide”
Formula
HCl
hydrochloric acid
Cl-
chloride
HBr
hydrobromic acid
Br-
bromide
H 2S
hydrosulfuric acid
S2(HS-
sulfide
hydrogensulfide)
analogous names: F- fluoride, N3- nitride, P3- phosphide, O2- oxide, etc.
2)
Ternary Acids:
Ternary acids contain hydrogen and two more elements, one of them usually being oxygen ( oxyacids). The
amount of oxygen present (i.e., the oxidation state of the third element) is denoted by various pre- and suffixes.
Group 17
Formula
Name
HClO4
HClO3
HClO2
HClO
Formula
perchloric
chloric
chlorous
hypochlorous
acid
acid
acid
acid
Name
ClO4ClO3ClO2ClO-
perchlorate
chlorate
chlorite
hypochlorite
(analogous: Br, I)
Fluorine forms only hypofluorous acid HOF.
Group 16
Formula
Name
Formula
Name
H2SO4
sulfuric acid
SO42(HSO4-
sulfate
hydrogensulfate)
H2SO3
sulfurous acid
SO32(HSO3-
sulfite
hydrogensulfite)
analogous: Se, Te
Group 15
Formula
Name
Formula
Name
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H3PO4
H3PO3
PO43PO33-
phosphoric acid
phosphorous acid
H3AsO5 perarsenic acid
H3AsO4 arsenic acid
AsO53AsO53-
phosphate
phosphite
perarsenate
arsenate
Some elements form only one type of oxyacid:
H2CO3
H3BO3
H4SiO4
CO32BO33SiO44-
carbonic acid
boric acid
silicic acid
carbonate
borate
silicate
In general, salts of elements in the same group follow the same pattern (formula and name). This is not true for carbon
(no H4CO4) and nitrogen (no H3NO4).
And some ions do not follow these “rules” at all:
MnO4RuO4-
permanganate
perruthenate
but
but
MnO42- manganate
RuO42ruthenate
Here are some websites about the nomenclature of oxyacids:



http://www.mpcfaculty.net/mark_bishop/acid_nomenclature.htm
http://www.ucdsb.on.ca/tiss/stretton/chem1/atomic7.html
http://dbhs.wvusd.k12.ca.us/Nomenclature/Acid-Nomenclature.html
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Part 2: Practice Problems
DIRECTIONS: Solve the problems below, showing your setup, calculations, units and correct Significant
Figures (SigFigs). Neatly-written solutions are acceptable. (Points are deducted from AP tests if correct SigFig
rules and labels are ignored, so get into the habit of using them all of the time!)
1. Demonstrate that you know the correct use of significant figures (SigFig digits) by completing the
following:
a. 738.90 m has _____ SigFgs.
b. 0.0304 g has _____ SigFigs.
c. 1.4 X 104 joules has _____SigFigs.
d. 1 dozen donuts has _____ SigFigs.
c. 40 mL has _____ SigFigs.
f. 800. m has _____ SigFigs.
2. A cylinder rod formed from silicon is 21.3 cm long and has a mass of 5.00 kg. The density of silicon is
2.33 g/cm3. What is the diameter of the cylinder? (The volume of cylinder is given by V = πr2h, where r is
the radius and h is the length.)
3. 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. 2.1m x 3.215m = _____________________
f.
200.1mi x 120 min = __________________
g. (17.6 + 2.838 + 2.3 + 110.77)g = _________________
4. 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.
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5. Write the correct formula of the following compounds:
a. Calcium sulfate
b. Ammonium phosphate
c. Lithium nitrite
d. Potassium perchlorate
e. Barium oxide
f. Zinc sulfide
g. Sodium peroxide
i. Calcium iodide
j. Aluminum carbonate
6. Determine number of protons, neutrons and electrons in each of the following.
a.
39
19 K
b. 2311Na1+
c. 20882Pb
d. 3315P3-
7. White gold is an alloy that typically contains 45.0% by mass gold and the remainder is platinum. If 154 g
of gold are available, how many grams of platinum are required to combine with the gold to form this alloy?
8. What is the empirical formula of a compound that contains 53.73% Fe and 46.27% of S ?
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9. Determine the number of molecules present in a 4.56 mol sample of methane gas (CH4) ; then determine
the number of hydrogen atoms in the sample.
10. 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
c. 12.4 x 1015 molecules of formaldehyde (CH2O)
11. In an experiment, a student gently heated a hydrated copper compound to remove the water of hydration.
The following data was recorded:
1. Mass of crucible, cover, and contents before heating = 23.4 g.
2. Mass of empty crucible and cover = 18.82 g.
3. Mass of crucible, cover, and contents after heating to constant mass = 20.94 g.
Calculate the percent by mass of water in the copper compound.
12. A hydrated compound has an analysis of 18.29% Ca, 32.37% Cl, and 49.34% water. What is its
formula?
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13. What mass of copper is required to completely replace silver from 4.00g of silver nitrate dissolved in
water by the reaction Cu(s) + 2 AgNO3 → Cu(NO3)2 + 2 Ag.
14. Write the chemical formula for the following:
a. Calcium carbonate
b. Ammonium phosphate
c. Potassium fluoride
d. Sodium oxide
e. Calcium sulfate
f. Sodium nitrite
g. Magnesium acetate
h. Potassium cyanide
i. Zinc nitrate
j. Iron(II) phosphate
k. Aluminum phosphide
15. In Nature, strontium consists of four isotopes with masses and percent abundance of 83.9134 amu
(0.50%), 85.9094 amu (9.9%) , 86.9089 amu (7.0 %) , and 87.9056 amu (82.6 %). Calculate the atomic mass
of Sr.
16. Mercury has an atomic mass of 200.59 amu. Calculate the
h. Mass of 3.0 x 1010 atoms of mercury
i.
Number of atoms in exactly one nanogram of mercury.
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17. Calculate the molar mass ( g/ mol) of
a. Ammonia ( NH3)
b. Baking soda ( NaHCO3)
c. Osmium Metal (Os)
18. The molecular formula of morphine, a pain-killing narcotic, is C17H19NO3.
j. What is its molar mass?
k. What fraction of atoms in morphine is accounted for by carbon?
l.
Which element contributes least to the molar mass?
19. Complete the list of ionic compounds. (Supply the name or formula.)
m. Cupric hydroxide
n. Strontium chromate
o. Ammonium perchlorate
p. Ca(HCO3)2
q. Fe2 (CO3)3
r. Sodium hydroxide.
s. H3PO4
20. The hormone, thyroxine is secreted by the thyroid gland, and has the formula: C15H17NO4I4. How many
milligrams of iodine can be extracted from 15.0 grams of thyroxine?
12
21. Determine the formula weight for the following:
a. N2O5
b. CuSO4
c. Ca(HCO3)2
d. CaSO4. 2 H2O
22. Calculate the percentage by mass of the following compounds:
a. SO3
b. CH3COOCH3
c. Ammonium Nitrate.
23. Determine the empirical formula of the compounds with the following compositions by mass:
t. 10. 4 % C, 27. 8% S , 61. 7 % Cl
u. 21.7 % C, 9.6 % O, and 68.7 % F
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24. Arsenic reacts with chlorine to form a chloride. If 1.587 g of arsenic reacts with 3.755 g of chlorine,
what is the empirical formula of the chloride?
25. Vanillin, a flavoring agent, is made up of carbon, hydrogen, and oxygen atoms. When a sample of
vanillin weighing 2.500g burns in pure oxygen, 5.79 g of carbon dioxide and 1.18 g of water are obtained.
Calculate the empirical formula of vanillin?
26. Washing soda is a hydrate of sodium carbonate. Its formula is Na2CO3. x H2O. A 2.714 g sample of
washing soda is heated until a constant mass of 1.006 g of Na2CO3 is reached. What is the value of x in the
formula?
27. What is the molecular formula of each of the following compounds?
v. Empirical formula CH2 , molar mass =84g/mol
w. Empirical formula NH2Cl, molar mass = 51.5 g/mol
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28. Determine the empirical and molecular formula of each of the following substances:
x. Ibufuren, a headache remedy contains 75.6 % C, 8.80 % H , and 15.5 % O by mass and
a molar mass about 206 g/mol.
y. Epinerphine (adrenaline), a hormone secreted into the bloodstream in times of danger
or stress contains 59% C, 7.1% H, 26.2% O, and 7.7% N by mass; its molar mass is
about 180 amu.
29. Write balanced chemical equations for the reaction of sodium with the following nonmetals to form
ionic solids:
a. Nitrogen
b. Oxygen
c. Sulfur
d. Bromine
30. Write a balanced chemical equation for each of the following:
z. The reaction of magnesium oxide with iron to form iron(III) oxide and magnesium.
aa. The decomposition of dinitrogen oxide gas to its elements.
bb. The reaction of solid calcium carbide with water to form calcium hydroxide and
acetylene (C2H2) gas.
cc. The reaction of solid calcium cyanamide (CaCN2) with water to form calcium
carbonate and ammonia gas.
dd. Propane (C3H8) burns in excess air (oxygen).
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ee. Nitrogen gas reacts with hydrogen to form ammonia.
ff. Hydrogen reacts with Iodine gas to form hydrogen iodide.
gg. Sodium reacts with iodine gas to form sodium iodide.
hh. Sodium oxide reacts with water to form sodium hydroxide and hydrogen.
ii. Magnesium and nitrogen gas combine to form magnesium nitride.
jj. Concentrated hydrochloric acid reacts with concentrated sodium hydroxide to form
sodium chloride and water.
31. Sodium hydroxide reacts with carbon dioxide as follows:
2 NaOH(s) + CO2 (g) → Na2CO3 (s) + H2O(l)
Which reagent (reactant) is limiting when 1.85 mol of sodium hydroxide and 1.00 mol carbon
dioxide are allowed to react? How many moles of sodium carbonate can be produced? How many
moles of the excess reactant remain after the completion of the reaction?
32. When benzene (C6H6) reacts with bromine (Br2), bromobenzene (C6H5Br) is obtained:
C6H6 + Br2 → C6H5Br + HBr
kk. What is the theoretical yield of bromobenzene in this reaction when 30.0g of benzene
reacts with 65.0 g of bromine?
ll. If the actual yield of bromobenzene was 56.7 g, what was the percentage yield?
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33. One way to remove nitrogen oxide (NO) from smokestack emissions is to react it with ammonia:
4 NH3 (g) + 6 NO (g)  5 N2 (g) + 6 H2O (l). Fill in the blanks below:
mm.
12.3 mol of NO reacts with _____ mol of ammonia.
nn.
5.87 mol NO yields _______ mol nitrogen.
34. Chlorine and fluorine react to form gaseous chlorine trifluoride. You start with 1.75 mol of chlorine and
3.68 mol of fluorine.
oo. Write the balanced equation for the reaction.
pp. What is the limiting reactant?
35. To prevent a condition called the “bends”, deep sea divers breathe a mixture containing, in mole
percent, 10.0% O2, 10.0% N2 , and 80.0% He.
qq. Calculate the molar mass of this mixture.
rr. What is the ratio of the density of this gas to that of pure Oxygen?
36. A 2.0g sample of SX6 (g) has a volume of 329.5 cm3 at 1.00 atm and 20oC. Identify the element ‘X’,
and name the compound.
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37. When hydrogen sulfide gas, H2S, reacts with oxygen, sulfur dioxide gas and steam are produced.
ss. Write the balanced chemical equation for this reaction.
tt. How many liters of sulfur dioxide would be produced from 4.0 l of oxygen? Assume
100% yield and that all gases are measured at the same temperature and pressure.
38. A gaseous mixture contains 5.78 g of methane, 2.15 g of neon, and 6.8 g of sulfur dioxide. What
pressure is exerted by the mixture inside a 75.0 L cylinder at 850C and 751 mm Hg?
39. A sample of methane gas is at 500C and 20 atm. Would you expect it to behave more ideally or less
ideally if:
uu. The pressure was reduced to 1 atm.
vv. The temperature were reduced to - 500 C?
40. Define solubility. Prepare a list of solubility rules for ionic compounds in water, and learn them. (Use a
textbook or online resources.) (This is IMPORTANT for the AP test since you are expected to make
predictions!)
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41. Name the following:
a. CO2
b. P4S10
c. NI3
d. PCl5
e. CCl4
f. SF6
g. CH4
h. C2H6
i. C3H8
42. Define Oxidation and Reduction. Provide at least three examples of oxidation and reduction, and
write the balanced chemical reaction for each. (Example: Rusting of Iron: 4Fe + 3O2 → 2Fe2O3)
43. Define Oxidation number. Determine the Oxidation number of
ww. Carbon in CO2
xx.
Sulfur in H2SO4
yy.
Phosphorus in PO43zz.
Manganese in MnO42-
44. Which of the following statements are always true? Never true? Not always true?
aaa. A compound with the molecular formula C6H6 has the same simplest formula.
bbb. The mass percent of copper in CuO is less than in Cu2O.
ccc. The limiting reactant is the one present in the smallest number of grams.
ddd. Since C3H6O3 and C6H12O6 reduce to the same formula, they represent the same
compound.
45. A bedroom 11.0 ft x 12.4 ft x 8.0 ft contains 35.41 kg of air at 25˚C. Express the volume of the room
in liters, the amount of air in moles (Use the molar mass of air as 29.0 g/mol.) and the temperature in
Kelvin.
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46. A sample of carbon dioxide gas, CO2 (g), occupies a volume of 5.75 L at 0.890 atm. If the temperature
and the number of moles remain constant, calculate the volume when the pressure
eee. increased by a factor of 10.0
fff. decreases to 0.445 atm
47. A nitrogen sample at 30˚C has a volume of 1.75L. If the pressure and the amount of gas remain
unchanged, determine the volume when the Celsius temperature is doubled.
48. An open flask contains 0.200 mol of air. Atmospheric pressure is 745 mmHg and room temperature is
25˚C. How many moles are present in the flask when the pressure is 1.10 atm and the temperature is 33˚C?
49. On a warm day, an amusement park balloon is filled with 47.8 g He. The temperature is 33˚C and the
pressure in the balloon is 2.25 atm. Calculate the volume of the balloon.
50. A drum used to transport crude oil has a volume of 162 L. How many water molecules, as steam, are
required to fill the drum at 1.00 atm and 100˚C? What volume of liquid water (density equals 1.00 g/cm3) is
required to produce that amount of steam?
20
51. Calculate the density of carbon dioxide gas at 27˚C and 763 torr.
52. Distinguish between strong and weak electrolytes, and provide two examples of each.
53. What is the Activity Series of metals, and how does it help us in studying properties of elements?
54. A volatile liquid (one that evaporates) is put into a jar and the jar is then sealed. How does the mass of
the sealed jar and its contents change upon the vaporization of the liquid?
55. Distinguish between an Exothermic and an Endothermic reaction. In each case, how does the
temperature of the surroundings change during such reactions?
56. How much heat is required to raise the temperature of 100 grams of water from 250C to 820C?
57. A piece of unknown metal with mass 14.9 g is heated to 1000C and dropped into 75.0 g of water at 200C.
The final temperature of the system is 28 degree Celsius. What is the specific heat capacity of the metal?
21
58. Calculate the molarity of a solution that contains 0.0345 mol NH4Cl in 400. ml of solution.
59. Calculate the molarity of a solution that contains 20.0grams of sodium hydroxide in 200. ml of
solution.
59. How many grams of solute are present in 50.0 ml of 0.360 M sodium chloride?
60. What volume of 12.0 M HCl solution is needed to prepare 5.00 liters of 0.0250 M solution?
61. The compound adrenaline contains 56.7 % C, 6.56 % H, 28.37% O and 8.28 % N by mass. What is
the empirical formula for adrenaline?
22
62. DDT, an insecticide harmful to fish, birds and humans, is produced by the following reaction:
2C6H5Cl + C2HOCl3 → C14H9Cl5 + H2O
Chlorobenzene Choral
DDT
If 1142 g of chlorobenzene is reacted with 485 g of chloral.
a.
b.
c.
d.
What mass of DDT is formed?
Which reactant is limiting? Which is in excess?
What mass of excess reactant is left over?
If the actual yield of DDT is 200.0 g, what is the percent yield?
63. A 2.25 g sample of scandium metal is reacted with excess hydrochloric acid to produce 0.1502 g
hydrogen gas. Use this information to determine the formula of the scandium chloride produced in the
reaction.
64. What volume of 0.100 M HCl solution is needed to neutralize 50.0 ml of 0.350 M KOH?
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65. Describe in detail what happens when the following are dissolved in water:
a. Polar solute (CH3OH) vs. non polar solute (CH3(CH2)4CH3.)
b. KF vs. CO2
66. Balance the following REDOX reactions.
Acid Solutions
67.Mn 2+ + BiO3 - ===> MnO4 - + Bi 3+
68.
MnO4 - + S2O3 2- ===> S4O6 2- + Mn 2+
69.ClO3 - + Cl - ===> Cl2 + ClO2
70.P + Cu 2+ ===> Cu + H2PO4 -
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Basic Solutions
71.MnO4 - + C2O4 2- ===> MnO2 + CO2
72. Zn + NO3 - ===> Zn(OH)4 2- + NH3
73.Al + OH - ===> AlO2 - + H2
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Part 3:
Complete as many three column notes needed for each chapter while reading chapters 1-5. (Should
be at least 3+)
Part 4:
Part A: Review Significant Figures, Rounding and Calculator Use
1) Determine the number of significant figures in each of the following:
a) 0.00404
b) 0.00080
c) 4.50x10-4
d) 200.020
2) Perform the following calculations:
a) 5.70m x 8.4m
b) 4.05 + 3.2
Part B: Review Calculations Involving Moles, Molecules, Mass and Stoichiometry
3) Given 0.080 moles barium sulfate, how many grams?
4)
Given 5.4x1015 atoms of calcium, how many moles?
5) Given 3.20g of glucose, how many molecules?
6) Write a balanced chemical equation for the combustion of glucose.
7) Using the equation above, if 25.00g of glucose react, how many grams of carbon dioxide are
formed.
8)
Using the equation in problem 4…you are given 120.0g glucose and 180.0g oxygen. Who is the
limiting reactant?
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Part C: Review Formulas, Writing Balanced Equations
9) Write a balanced chemical equation when calcium nitrate reacts with sodium phosphate.
10) Determine the states in the above problem, and write the ionic and net ionic equations.
Part D: Review Atoms
11) “Draw” an neutral atom of oxygen with a mass number of 17. Indicate # protons, electrons,
neutrons, as well as their location and charge (perhaps set up a chart)
12) Explain in a few sentences why Dalton “is important”.
13) Explain in a few sentences why Rutherford “is important”.
14) Explain in a few sentences why Thompson “is important”.
15) Define a) isotopes, b) ions
16) Given n=3, generate a “chart” indicating the possible acceptable values for the three remaining
quantum numbers.
17) Define each of the four quantum numbers supporting with “facts, hints & information” to help you
in comprehending this information again, i.e. the principle quantum number, n, corresponds to the
period location in the Periodic Table.
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18)
Write the extended and Noble-gas electron configuration of a) C, b) Ca, c) Ar, d) F, e) F-1, g) Ca+2
Part E: Review Bonding
19) Define and carefully explain the most important types of bonds learned (ionic, polar covalent,
nonpolar covalent, hydrogen) such as where found, when seen, why seen.
20) Draw the Lewis Dot of: a) H2O b) CH4 c) C2H2
Part F: Review Oxidation Numbers
21) Determine the oxidation numbers in: a) H2SO4 b) N2O5 c) PCl3 d) PO4-3
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Part G: Gas Laws
22) Given a gas at 30.05K at 320. torr, what is the pressure if the temperature is doubled.
23) Given a gas at 270.00K, 275torr in 355ml, what is the new temperature if the pressure is tripled,
and the volume is halved.
24) Write the Ideal Gas Law, defining the variables and their units.
25) Write Graham’s Law. Use oxygen and methane to “prove” this Law.
Part H: Review Solutions
26) Write three facts about solutions
27) You have 34.5g of HCl dissolved in 200.0 milliliters of solution, what is the molarity.
28) You have 34.5g of HCl dissolved in 200.0 milliliters of water, what is the molality.
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Part I: Review Acids & Bases
29) Given a pOH of 3.22, find pH, [H+], [OH-]
30) Define Bronsted-Lowry Acid and Base, respectively.
Part J: Review Thermochemistry (NEW-Use Text)
31) Define and give symbols for Gibbs free energy, enthalpy, entropy.
32) Define what is meant by an exothermic reaction; locate a real-life exothermic reaction, and write
the equation.
Part K: Review Equilibrium (NEW-Use Text)
33) Define K, the equilibrium constant
34) What effect would an increase in temperature have on an exothermic reaction (think Le Chatelier).
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Part L: Review Redox
35) Define oxidation and reduction.
36) Write an oxidation half reaction.
The official AP Chemistry website is listed below so you can familiarize yourself with the exam and scope of the class.
http://apcentral.collegeboard.com/apc/public/courses/teachers_corner/2119.html
The website that we will use all year as a guide and where all assignments will be listed is:
http://twiningapchemistry.wikispaces.com/
You can look at this and gain an idea of how the class will be structured and also the work load. Just note that this year
will be a little bit different.
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