AP Chemistry
Westford Academy
Summer Assignment 2013
This assignment should allow the class to quickly move through the first 6 chapters of the text in the first
days of school and allow us to cover all of the material on the AP chemistry exam. You are expected to
cover and understand this material on your own as it will not be covered in class. Note most of this
material should be review. There will be an exam Friday September 13, worth 200 pts. The first 6
chapters will comprise 350 points early in the first quarter, before the issuance of progress reports, so be
sure that you thoroughly understand these concepts. Show all work, provide all units and circle your final
answer(s) for calculations.
1.
2.
3.
Read the first 6 chapters of the textbook provided.
Answer the questions on the sheets provided (no additional sheets please!!)
Be familiar with and understand the following concepts:
Different types of properties and changes (pp 7, 9)
The metric system and prefixes (Appendix pg A-9, pp 17)
Types of matter (pp 15)
Significant figures (pp 21-25)
Dimensional analysis (pp 29)
Density and the q= msΔT equation (pp 35)
Laws governing compounds, basics of chemical formulas (pp52)
Names, symbols and charges of ions (pp 55, 142)
The mole, mole conversions, avogadro’s # (pp 57-66)
Empirical and molecular formulas, % composition (pp 70-74)
Combustion analysis (pp 75)
Balancing chemical equations (pp 90)
Stoichiometry (pp 92-100) and percent yield
Solution concentration: mass % and molarity; Dilution of solutions (pp 102-110)
Strong/weak electrolytes and acids (pp 130)
Nomenclature of compounds (pg 131)
Solubility rules of compounds in water (pp 134-135)
Writing balanced molecular and net ionic equations (pp 135-136)
Redox reactions (pp 137, 146)
Types of chemical reactions and reaction prediction(pp 146-164)
Subatomic particles and their discovery (pp 175-183)
Isotopes (pp 182-189)
EM spectrum, wavelength and frequency (pp 190-194)
Bohr model, electron transitions and energy (pp 194-200)
Quantum model (pp 201-204)
Quantum numbers and electron configurations (pp 205-221)
Periodic table basics (pp 123-127 and pp 231-235)
Major periodic trends (pp 236-246)
Patterns of reactivity in specific families (pp 247 – 260)
This assignment will count for 150 points and is due on the first day of class. It will be reviewed before
being collected so that a few questions may be asked.
Have a nice summer!
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1. You are given a bottle that contains 4.59 cm3 of a metallic solid. The total mass of the bottle
and solid is 35.66 g. The empty bottle weighs 14.23 g. What is the density of the solid?
2. Mercury is traded by the “flask, a unit that has a mass of 34.5 kg. What is the volume of the
flask of mercury if the density of mercury is 13.6 g/mL?
3. A sample of ascorbic acid (vitamin C) is synthesized in the laboratory. It contains 1.50 g of
carbon and 2.00 g of oxygen. Another sample of ascorbic acid is isolated from citrus fruits
contains 6.35 g of carbon. How many grams of oxygen does it contain? Which law are you
assuming in answering this question?
4. The annual production of sodium hydroxide in the United States in 1994 was 25.83 billion
pounds.
a.) How many grams of sodium hydroxide were produced in that year?
b.) The density of sodium hydroxide is 2.130 g/cm3. How many cubic kilometers were
produced?
5. Name the following compounds (you are not given a chart of ions in this class)
a. KClO4
k. HI (aq)
b. Ca3(PO4)2
l. HNO2 (aq)
c. Al2(SO4)3
m. HIO (aq)
d. Pb(NO3)2
n. CS2
e. BaSO3
o. Zn(CN)2
f. KMnO4
p. LiH2PO3
g. K2Cr2O7
q. (NH4)2SO3
h. AuCl3
r. BF3
i. HIO2
s. Ag2O
j. NiS
t. MnO2
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6. Write formulas for the following compounds (note: you are not given ion sheets in this class
and are expected to know these and the 20 most common ions – questions 5 and 6 give a good
indication of which ions are important).
a. sulfur difluoride
b. sulfur hexafluoride
c. sodium hydrogen phosphate
d. lithium nitride
e. chromium(III) carbonate
f. tin(II) fluoride
g. ammonium acetate
h. ammonium hydrogen sulfate
i. cobalt(III) nitrate
j. mercury(I) chloride
k. potassium chlorate
l. sodium hydride
m. carbonic acid
7. Identify each of the following elements:
a. a noble gas with 54 protons in the nucleus
b. a member of the same family as oxygen. The anion with a 2- charge and 36 electrons
c. a member of the alkaline earth metal family. The 2+ cation contains 18 electrons
d. a transition metal with 42 protons in the nucleus
e. a radioactive element with 94 protons and 94 electrons in the neutral atom
8. The molecular formula of acetylsalicylic acid (aspirin), one of the most commonly used pain
relievers, is C9H8O4.
a. Calculate the molecular weight of aspirin
b. A typical aspirin tablet contains 500 mg of C9H8O4. How many moles of C9H8O4 and
how many molecules are in a 500 mg tablet?
9. Calculate the percent composition by mass of the following compounds that are important
starting materials for synthetic polymers.
a. C3H4O2 (acrylic acid, from which acrylic plastics are made)
b. C4H6O2 (methyl acrylate, from which plexiglass is made)
10. A sample of urea contains only 1.21 g of nitrogen, 0.161 g of hydrogen, 0.480 g of carbon and
0.640 g of oxygen. What is the empirical formula of urea?
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11. A compound that contains only nitrogen and oxygen is found to be 30.4 % nitrogen by mass.
The molecular weight of the compound is 92 g/mol. What are the empirical and molecular
formulas for this compound?
12. a. Write the balanced chemical equation for the combustion of isooctane (C8H18) to produce
water vapor and carbon dioxide gas.
b. Assuming that gasoline is 100% isooctane, with a density of 0.692 g/mL, what mass of carbon
dioxide is produced by the combustion of 1.2 x1010 gal of gasoline?
13. An automobile has a gas mileage of 36.1 mi/gal. How many kilometers can it travel on 1.0 L
of gasoline?
14. Ammonia is produced from the reaction of nitrogen gas with hydrogen gas according to the
following chemical equation:
N2 + H2  NH3
a. What mass of ammonia is produced from a mixture of 1.00 x103 g of nitrogen and 5.00
x102 g of hydrogen?
b. What mass of which starting material remains unreacted?
c. If 15.0 grams of ammonia are actually produced, what is the percent yield of the
reaction?
15. Determine the number of significant figures in the following:
a. 0.0007
f. 1000.000
b. 2000
g. 2.00
c. 1m = 100 cm
h. 0.0009
d. 7.00010
i. 0.00070
e. 0.000100
j. 32
f. 1000.000
k. 5 apples
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16. Convert the following
a. 1.35 kg into mg
b. 1.5 miles into mm
c. 5.0 cubic meters into kL
d. 9,000. nJ into MJ
17. For the following reactions:
Determine the type of reaction (even if it does not occur)
If the reaction occurs, predict the products ( if there is no reaction state this)
If the reaction occurs, balance the molecular equation and provide the net ionic equation.
(assume moderately soluble means it will precipitate)
a. Solutions of copper(II) sulfate and strontium nitrate are mixed
b. Solutions of nitric acid and calcium hydroxide are mixed
c. Solutions of iron(III) chloride and silver nitrate are mixed
d. A piece of iron metal is placed into a solution of copper(II) chloride
e. A piece of silver metal is placed into some nitric acid
f.
A piece of aluminum metal is placed into some sulfuric acid
g. Some chlorine gas is bubbled through a solution of potassium iodide
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h. Some bromine gas is bubbled through a solution of sodium fluoride
i.
Solutions of chromic acid and sodium hydroxide are mixed
j.
Solutions of ammonium acetate and calcium nitrate are mixed
k. Some solid magnesium carbonate is heated
l.
Zinc metal is reacted with chlorine gas
m. Sulfur trioxide gas is bubbled through water
18. For the following redox (reduction-oxidation) reactions, determine which substances are
reduced and oxidized. Determine the oxidation states of each element in each reaction.
a. Zn + CoCl3  ZnCl2 + Co
b. NH3 + O2  N2 + H2O
c. sulfuric acid reacts with hydrogen iodide to produce sulfur dioxide, iodine and water
19. When 75.0 grams of metal at 75.0°C is added to 150. grams of water at 15.0 °C, the
temperature of the water rises to 18.3°C. Assuming no heat is lost to the surroundings, what is
the specific heat of the metal?
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20. When an electron transitions from the 3rd energy level down to the 1st energy level, energy is
released. What is the wavelength of the light emitted?
21. Why could the Bohr model not predict line spectra for atoms other than hydrogen?
22. The first step in the formation of ozone in the upper atmosphere occurs when oxygen
molecules absorb UV radiation of wavelength greater than or equal to 242 nm. What is the
frequency and energy of this minimum wavelength?
23. Write condensed electron configurations for the following:
a. Ni
b. Lr
c.Ba2+
d. P3e. element 119
f. As
24. Determine which of the following sets of quantum numbers are incorrect and state why.
Write a correct set of numbers. For the originally correct sets, identify an atom it might represent.
a. (5,3,3,-1/2)
b. (3,2,0,+1/2)
c. (4,4,3,0)
d. (6,2,2,-1/2)
e. (2,1,0,-1/2)
25. Electric power is typically stated in units of watts (1 W = 1 J/s). About 95% of the power
output of an incandescent bulb is converted to heat and 5% to light. If 10% of the light shines on
your chemistry text, how many photons per second shine on the text from the 75 W bulb?
(assume photons have a wavelength of 550. nm)
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26. Enormous numbers of microwave photons are needed to warm macroscopic samples of
matter. A portion of soup containing 252 g of water is heated in a microwave oven from 20. °C
to 98 °C with radiation of a wavelength of 0.0155 m. How many photons are absorbed by the
water in the soup?
27. Arrange the following elements according to the following trends (smallest to largest):
a. Second ionization energy: Na, Al, Mg
b. Atomic radius: Cl,K,S
c. Electronegativity: Li,Ne,B, Zn, Ca
d. Metallic character: Ba,Ca,Na,P,Cl,F
28. Why do successive ionization energies of a given element always increase? When the
difference between successive IEs of a given element is exceptionally large, what do we learn
about its electron configuration?
29. Define shielding and effective nuclear charge. What is the relationship between these
concepts?
30. Name the following elements:
a. smallest in group 6A
b. largest in period 6
c. smallest metal in period 3
d. highest IE (ionization energy) in group 4A
e. lowest IE in period 5
f. most metallic in group 15
g. Group 3A element that forms the most basic oxide
h. Period 4A element with a filled outer level
i. Heaviest lanthanide
j. Alkaline earth metal that is isoelectronic with Kr
k. Group 5A metalloid with the most acidic oxide
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31. Distinguish among oxides, peroxides and superoxides. What is the oxidation number of
oxygen in each case?
32. Are the following basic or acidic oxides?
a. Na2O
b. CO2
c. SeO3
d. CaO
e. N2O5
f. Al2O3
33. Write reactions of the above (#32) oxides in water
a.
b.
c.
d.
e.
f.
34. Menthol (molar mass 156.3 g/mol), a strong smelling substance used in cough drops, is a
compound of carbon, hydrogen and oxygen. When 0.1595 g of menthol was combusted, it
produced 0.449 g of carbon dioxide and 0.184 g of water. What is the molecular formula of
menthol?
35. How many grams of barium sulfate precipitate are created when 25.0 mL of 0.160 M barium
chloride react with 68.0 mL of 0.055 M sodium sulfate?
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36. When 1.5173 g of an organic compound containing Fe, C, H and O was burned in excess
oxygen, 2.838 g of carbon dioxide and 0.8122 g of water were produced. In a separate
experiment, 0.3355 g of the compound yielded 0.0758 g of iron(III) oxide. What is the empirical
formula of the compound?
37. The active ingredient in Pepto-Bismol contains C, H, O and Bi.
a. When 0.22105g of it was burned in excess oxygen, 0.1422 g of bismuth(III) oxide,
0.1880 g of carbon dioxide, and 0.02750 g of water were formed. What is the empirical
formula of this compound?
b. Given a molar mass of 1086 g/mol, what is the molecular formula?
c. Complete and balance the acid-base reaction between bismuth(III) hydroxide and
salicylic acid (HC7H5O3), which is used to form this compound.
d. A dose of Pepto-Bismol contains 0.500 mg of the active ingredient. If the yield of the
reaction in part (c) is 78.0% what mass in mg of bismuth(III) hydroxide is required to
prepare one dose?
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