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2015 Summer Packet
for AP Chemistry
Students
Covenant Day School
Dear adventurers,
Welcome to AP chemistry at CDS. I am really excited that we are offering this course to you. You will
definitely be challenged but hopefully you come out with a thorough understanding of the intricate
design of God at a level so small it is hard to comprehend.
There will be a few differences that you need to be aware of in order to make an informed decision as to
whether this class is a good fit for you. First, being very lab intensive class, there will be a sizable portion
of the class given to labs. However, due to the involved nature of the labs and the shorter class periods,
there will be a designated lab day. On the day that we do labs, you will be required to be at school early
to insure that there is time to finish the lab. We will start at 7:30 on lab days. This will be mandatory for
the entire class.
In addition, I have assigned and posted some summer assignments to be completed before school
begins. These assignments can be found at http://therustychemist.yolasite.com . Click on the AP
Chemistry tab at the top. Please make sure you visit the site soon and begin the work ASAP. This is not
something you want to attempt the last couple of days before school starts as some of it requires some
memorization and there are quite a few questions to answer. There should not be anything you did not
learn in your chemistry 1 class but if you are stuck on a particular question or type of question feel free
to email me at [email protected] . Also on the site there are some notes that will help with the
material that you can download to help you refresh.
Again, I am really excited about this and am looking forward to walking through this with you.
Sincerely,
Rusty Randles
CDS Chemistry
Chapter 1 Questions
1. The difference between a law and a theory is the difference between what and why. Explain.
2. To determine the volume of a cube, a student measured one of the dimensions of the cube several
times. If the true dimension of the cube is 10.62cm, give an example of four sets of measurements
that would illustrate the following:
a. imprecise and inaccurate data
b. precise but inaccurate data
c. precise and accurate data
3. Evaluate and write the answer to the appropriate number of significant figures
a.
b.
c.
d.
212.2+26.7+402.09
1.0028+.221+.10337
.14 x 6.022 x1023
2.00x106
3.00x10-7
e. 2.01x102 + 3.014x103
4. Perform the following mathematical operations and express the result to the correct number of
significant figures
a. 2.526 + 0.470 + 80.705
3.1
0.623 0.4326
b. (6.404 x 2.91)/(18.7-17.1)
c. 6.071x10-5 – 8.2x10-6 - 0.521x10-4
d. (3.8x10-12 + 4.0x10-13)/(4x1012+6.3x1013)
e. (8.925-8.905)/8.925 x 100 (assume this is a percent question so the 100 is exact)
5. Use the following exact conversion factors to perform the stated calculations
i. 5 ½ yards=1rod
ii. 40rods=1furlong
iii. 8 furlongs=1mile
iv. 1meter=1.094 yards (not exact)
v. 1L=1.06qt (not exact)
vi. 1gal=4qt
a. The Kentucky Derby race is 1.25 miles. How long is the race in rods, furlongs, meters, and
kilometers?
b. A marathon race is 26 miles and 385 yards. What is this distance in yards, furlongs, meters and
kilometers?
6. You pass a road sign saying “New York 112km”. If you drive a constant speed of 65 mi/h, how long
would it take you to reach New York? If you car gets 28 miles to the gallon, how many liters of
gasoline are necessary to travel 112km?
7. Convert the following Celsius temperatures to Kelvin and to Fahrenheit degrees.
a. the temperature of someone with a fever, 39.2°C
b. A cold, wintery day, -25°C
c. The lowest possible temperature, -273°C
d. the melting point temperature of sodium chloride, 801°C
8. For a material to float on the surface of water, the material must have a density less than that of
water (1.0g/mL) and must not react with the water or dissolve in it. A spherical ball has a radius of
0.50cm and weighs 2.0g. Will this ball float or sink when placed in water?
9. In each of the following pairs, which has the greater volume?
a. 1.0kg of feathers or 1.0kg of lead
b. 100g of gold or 100g of water
c. 1.0L of copper or 1.0L of mercury
10. A 25.00g sample of a solid is placed in a graduated cylinder and the the cylinder is filled to the
50.0mL mark with benzene. The mass of the benzene and solid together is 58.80g. Assuming that
the solid is insoluble in benzene and that the density of benzene is 0.880g/cm3, calculate the density
of the solid.
11. The density of osmium (the densest metal) is 22.57g/cm3. If a 1.00kg rectangular block of osmium
has two dimensions of 4.00cm x 4.00cm, calculate the third dimension of the block.
12. Classify each of the following as homogeneous or heterogeneous:
a. a door
b. the air you breathe
c. a cup of coffee (black)
d. the water you drink
e. salsa
f. your lab partner
13. Classify each of the following as a mixture or a pure substance
a. water
b. blood
c. the ocean
d. iron
e. brass
f. uranium
g. wine
h. leather
i. table salt (NaCl)
Of the pure substances which are elements and which are compounds
14. Classify the following as physical or chemical changes:
a. Moth balls gradually vaporize in a closet
b. Hydrofluoric acid attacks glass, and is used to etch calibration marks on glass laboratory
utensils.
c. A French chef making a sauce with brandy is able to burn off the alcohol from the
brandy leaving just the brandy flavoring.
d. Chemistry majors sometime get holes in the cotton jeans they wear to lab because of
acid spills (Chemistry teachers too)
15. The properties of a mixture are typically averages of the properties of its components. The
properties of a compound may differ dramatically from the properties of the elements that combine
to produce the compound. For each process described below, state whether the material being
discussed is most likely a mixture or a compound, and state whether the process is a chemical
change or a physical change
a. An orange liquid is distilled, resulting in the collection of a yellow liquid and red solid
b. A colorless, crystalline solid is decomposed, yielding a pale yellow-green gas and a soft,
shiny metal.
c. a cup of tea becomes sweeter as sugar is added to it
Chapter 2 Questions
1. With some modifications the postulates of Dalton’s theory hold up very well. Answer the
following questions concerning Dalton’s atomic theory and the modifications made today.
a. The atom can be broken down into smaller parts. What are the smaller parts?
b. How are atoms of hydrogen identical to each other and how can they be different from
one another?
c. How are atoms of hydrogen different from atoms of helium? How can atoms of
hydrogen and helium be similar?
d. How is water different from hydrogen peroxide (H2O2) even though both compounds
are composed only of hydrogen and oxygen?
e. What happens in a chemical reaction and why is mass conserved in a chemical reaction?
2. The number of protons in an atom determines the identity of the atom. What does the number
and arrangement of electrons determine? What does the number of neutrons determine?
3. When mixtures of gaseous H2 and Cl2 react, a product forms that has the same properties
regardless of the relative amounts of hydrogen and chlorine used.
a. How is this result interpreted in terms of the law of definite proportion?
b. When a volume of H2 reacts with an equal volume of Cl2, what volume of product having
the formula HCl is formed?
4. The mass of a proton is 1.67x10-27kg and the mass of an electron is 9.11x10-31kg. Using this
information and the relative size of the atom from the notes, calculate the density of a hydrogen
atom and of a hydrogen nucleus.
5. Distinguish between the following terms:
a. molecule vs. ion
b. covalent bonding vs. ionic bonding
c. molecule vs. compound
d. anion vs. cation
6. In the periodic table, how many elements are found:
a. in the halogen group?
b. in the alkali family?
c. in the lanthanide series?
d. classified as transition metals?
7. What is the symbol for an ion with 63 protons, 60 electrons, and 88 neutrons? What is the
symbol for an ion that has 50 protons, 68 neutrons, and 48 electrons?
8. Write the formula for each of the following compounds
a. Zinc chloride
b. tin (IV) fluoride
c. calcium nitride
d. aluminum sulfide
e. mercury (I) selenide
f. silver iodide
9. Name the following compounds
a. HC2H3O2
b. NH4NO2
c. Co2S3
d. ICl
e. Pb3(PO4)2
f. KIO3
g. H2SO4
h. Sr3N2
i. Al2(SO4)3
j. SnO2
k. Na2CrO4
l. HClO3
10.Write the formula for each of the following compounds
a. chromium (VI) oxide
b. disulfur dichloride
c. nickel (II) fluoride
d. potassium hydrogen phosphate
e. aluminum nitride
f. ammonia
g. manganese (IV) sulfide
h. sodium dichromate
i. ammonium sulfite
j. carbon tetraiodide
11.Write the formula
a. ammonium hydrogen phosphate
b. mercury (I) sulfide
c. silicon dioxide
d. sodium sulfite
e. aluminum hydrogen sulfate
f. nitrogen trichloride
g. hydrobromic acid
h. bromous acid
i. perbromic acid
j. potassium hydrogen sulfide
k. calcium iodide
l. cesium perchlorate
12. Each of the following compounds is incorrectly named. What is wrong with
each name and what is the correct name for each compound?
a. FeCl3, iron chloride
b. NO2, nitrogen (IV) oxide
c. CaO, calcium (II) monoxide
d. Al2S3, dialuminum trisulfide
e. Mg(C2H3O2)2, manganese diacetate
f. FePO4, iron (II) phosphide
g. P2S5, phosphorus sulfide
h. Na2O2, sodium oxide
i. HNO3, nitrate acid
j. H2S, sulfuric acid
Chapter 3 Assignment:
1. If you had a mole of US dollar bills equally distributed to each person in the world, how wealthy
would each person be? Assume a world population of 6 billion.
2. The element rhenium has two naturally occurring isotopes, Re-185 and Re-187 with an average
atomic mass of 186.207amu. Rhenium is 62.60% Re-187 which has a mass of 186.956amu.
Calculate the mass of Re-185.
3. Diamond is a natural form of pure carbon. What number of atoms of carbon are in a 1.00carat
diamond (1.00 carat=0.200g)
4. How many moles of compound are present in1.00g of:
a. NH3
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
b. N2H4
What mass of nitrogen is present in 5.00moles of each compound in question 4?
What number of atoms of nitrogen is present in 1.00g of each compound in question 4?
What is the molar mass of vitamin C (C6H8O6)? If a typical tablet contains 500.0mg of vitamin C,
what amount, in moles, and what number of molecules of vitamin C does it contain?
One anabolic steroid is fluorxymesterone (C20H29FO3). Calculate the percent composition by
mass of each element in the steroid.
Place the following in order of increasing mass percent of nitrogen
a. NO
b. NO2
c. N2O4
d. N2O
Express the composition of each of the following compounds as the mass percents of its
elements.
a. CH2O
b. C6H12O6
c. HC2H3O2
A compound containing only sulfur and nitrogen is 69.9% sulfur by mass; the molar mass is
184g/mol. what are the empirical and molecular formulas?
Adipic acid is composed of 49.31%C, 43.79%O, and the rest hydrogen. If the molar mass of
adipic acid is 146.1g/mol, what are the empirical and molecular formulas of the compound?
Maleic acid is composed of 41.39%C, 3.47%H and the rest oxygen. If 0.129moles of maleic
acidhas a mass of 15.0g, what are the empirical and molecular formulas?
Give the balanced equation for each of the following chemical reactions:
a. Glucose(C6H12O6) reacts with oxygen gas to produce gaseous carbon dioxide and water
vapor
b. Solid Iron(III) sulfide reactis with gaseous hydrogen chloride to form solid iron (III)
chloride and hydrogen sulfide gas
c. Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and
solid ammonium thiocyanate (NH4SCN)
Fe2O3 +2Al →2Fe +Al2O3
a. What masses of Iron (III) oxide and aluminum must be used to produce 15.0g of iron?
b. What is the maximum mass of aluminum oxide that could be produced?
KClO3 + P4 →P4O10 + KCl (unbalanced)
a. If you were to react 52.9g of potassium chlorate with excess red phosphorus, what mass
of tetraphosphorus decaoxide would be produced?
3Al + 3NH4ClO4→Al2O3 + AlCl3 +3NO + 6H2O
a. What mass of ammonium perchlorate should be used in the fuel mixture for every
kilogram of aluminum?
Bacterial digestion is an economical method of sewage treatment. The reaction
5CO2 + 55NH4+ + 76O2→C5H7O2N (bacterial tissue) + 54NO2- + 52H2O + 109H+
19.
20.
21.
22.
23.
a. What mass of bacterial tissue is produced in a treatment plant for every 1.0x104 kg of
wastewater containing 3.0% NH4+ ions by mass? Assume that 95% of the ammonium
ions are consumed by the bacteria.
Phosphorus can be prepared from calcium phosphate by the following reaction:
2Ca3(PO4)2 + 6SiO2 + 10C→6CaSiO3 + P4 + 10CO
a. Phosphorite is a mineral that contains about 75% calcium phosphate by mass. What is
the maximum amount of phosphorus that can be produced from 1.0kg of phosphorite?
Pg 121 (97, 101-105)
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen and
methane: 2NH3 + 3O2 +2CH4→2HCN +6H2O
a. If 5.00x103kg of each reactant react, what mass of HCN and of H2O will be produced,
assuming 100% yield?
2C3H6 +2NH3 + 3O2 →2C3H3N + 6H2O.
a. If 15.0g of C3H6, 10.0g oxygen, and 5.00g of ammonia are reacted what mass of C3H3N
can be produced, assuming 100% yield?
2C6H5Cl + C2HOCl3 →C14H9Cl5 + H2O
a. 1142g of C6H5Cl is reacted with 485g of C2HOCl3.
i. What mass of C14H9Cl5 is formed?
ii. Which reactant is limiting? Which is excess?
iii. What mass of the excess reactant is left over?
iv. If the actual yield is 200.0g, what is the percent yield?
2Cu3FeS3 + 7O2 →6Cu + 2FeO + 6SO2.
a. If 2.50metric tons (1000kg) of Cu3FeS3 is reacted with excess O2 and the process has an
86.3% yield of copper, what mass of copper is produced?