YOU WILL FIND THIS LETTER ON MY WEBSITE UNDER “WORKSHEETS”
MY WEBSITE ADDRESS IS: http://info.conroeisd.net/~bsieber/
June1, 2015
PLEASE READ CAREFULLY – IMPORTANT INFORMATION ON PAGE 3!
Dear Prospective ASHP AP Chemistry Student:
Greetings! I hope you are as ready as I am to have an enjoyable and relaxing summer. This is
the summer assignment for AP Chemistry. The assignment is to answer questions from
the first three chapters in your text (Zumdahl Chemistry, 5th ed.). This is the text we use
for AP Chemistry. Since it was not possible to issue you this book over the summer, I have
included a set of notes and a list of websites to help you answer those questions
The rationale is this: we will be losing approximately eight school days due to clinical rotations
and the AP exam dates will remain the same. In order to adjust for this, I have given you the
first unit in advance. The notes that accompany the first unit are a review of a few concepts
covered in first year chemistry. The PowerPoint notes are aligned with the first three chapters
of the Zumdahl text. Copies of them are included in this packet.
The following websites can also help you with the summer assignment:
Scientific method:
http://www.sciencebuddies.org/mentoring/project_scientific_method.shtml
Units of measurement:
http://lamar.colostate.edu/~hillger/common.html
Significant Figures:
http://www.chem.tamu.edu/class/fyp/mathrev/mr-sigfg.html
Dimensional Analysis:
http://www.ncsu.edu/felder-public/kenny/papers/units.html
Temperature:
http://abyss.uoregon.edu/~js/glossary/temperature_scale.html
http://chemunder.chemistry.ohio-state.edu/under/chemed/qbank/1/1-29/index.htm
Density:
http://www.elmhurst.edu/~chm/vchembook/120Adensity.html
Classification of matter:
http://www.emsb.qc.ca/laurenhill/science/classification.html
http://www.fordhamprep.org/gcurran/sho/sho/lessons/lesson14.htm
Law of Definite Proportions
http://www.iscid.org/encyclopedia/Law_of_Definite_Proportions
Law of Multiple Proportions
http://www.factmonster.com/ce6/sci/A0829092.html
Early Atomic Experiments
Thomson’s Cathode Ray tube
http://www.aip.org/history/electron/jjhome.htm
Rutherford’ Atomic model
http://www.daviddarling.info/encyclopedia/R/Rutherfords_experiment_and_atomic_model.html
Nuclear structure
http://web.jjay.cuny.edu/~acarpi/NSC/3-atoms.html
Ionic and Molecular substances
http://chemistry.twu.edu/tutorial/IonForSum.html
http://chemistry.twu.edu/tutorial/molforsum.html
Ball and stick models vs. space filling models
http://dl.clackamas.cc.or.us/ch106-03/structur1.htm
Periodic table
http://www.dayah.com/periodic/
Chemical nomenclature – writing chemical formulas
http://science.widener.edu/svb/pset/nomen_b.html
Isotopes
http://www.chemteam.info/Mole/AvgAtomicWt-Reverse.html
http://www.chemteam.info/Mole/AverageAtomicWeight.html
Molar mass and mole conversions
http://www.fordhamprep.org/gcurran/sho/sho/lessons/lesson92.htm
Percent composition
http://pages.towson.edu/ladon/empiric.html
Even though you won’t have your AP text, I don’t anticipate you should have much difficulty in
answering these questions. Don’t forget that I can help you if you have any questions
regarding your summer assignment or the course in general. My email address is
bsieber@conroeisd.net.
IMPORTANT:
THE ASSIGNMENT WILL BE DUE ON THE SECOND DAY OF CLASS: AUGUST 25, 2015.
PLACE ANSWERS ON SEPARATE PAPER. IFA CALCULATION IS REQUIRED, SHOW
WORK FOR THE CALCULATION. WRITE IN COMPLETE SENTENCES WHERE
APPROPRIATE.
ENJOY YOUR SUMMER!
Thank you,
Mr. Sieber
ZUMDAHL – CHAPTER ONE QUESTIONS
16. Define and explain the differences between the following terms.
a. law and theory
b. theory and experiment
c. qualitative and quantitative
d. hypothesis and theory
17. Is the scientific method suitable for solving problems only in the sciences? Explain.
19. Explain why the uncertainty of measurement depends on the precision of the measuring
of the measure device. Give an example to illustrate.
21. Distinguish between physical changes and chemical changes.
23. Which of the following are exact numbers?
a. The elevation of Breckenridge, Colorado is 9,600 feet
b. There are 12 eggs in a dozen
c. One yard is equal to 0.9144 m.
d. The announced attendance at a football game was 52,806 m
e. In 1983, 1759 Ph.D.s in chemistry were awarded in the United States
f. The budget deficit of the U.S. government in fiscal year 1990 was $269
billion.
25. How many significant figures are in each of the following:
a. 12
b. 1098
c. 2001
d. 2.001 x 10-3
e. 0.0000101
f. 1.01 x 10-5
g. 1000.
h. 22.04030
27. Round off each of the following numbers to three significant figures, and write the answer
in standard exponential notation.
a. 312.54
b. 0.00031254
c. 31254000
d. 0.31254
29. Perform the following mathematical operations, and express each result to the correct
number of significant figures.
a. 97.381 + 4.2502 + 0.99195
b. 171.5 + 72.915 – 8.23
c. 1.00914 + 0.87104 + 1.2012
d. 21.901 – 13.21 – 4.0215
31. Perform the following mathematical operations, and express each result to the correct
number of significant figures.
a. 4.184 x 100.62 x (25.27 – 24.16)
b. 8.925 – 8.904/8.925 x 100 (This type of calculation is done many times in calculating a
percentage error. Assume that this example is such a calculation: thus 100 can be considered
to be an exact number.)
c. (9.04 – 8.23 + 21.954 + 81.0) / 3.1416
d. 9.2 x 100.65 / 8.3221 + 4.026
e. 0.1654 + 2.07 – 2.114
f. 8.27(4.987 – 4.962)
g. 9.5 + 4.1 + 2.8 + 3.175 / 4 (Assume that this operation is taking the average of four
numbers. Thus 4 in the denominator is exact).
h. 9.025 – 9.024 / 9.025 x 100 (100 is exact)
33. Perform each of the following conversions.
a. 8.43 cm to millimeters
b. 2.41 x 102 cm to meters
c. 294.5 nm to centimeters
d. 1.445 x 104 m to kilometers
e. 235.3 m to millimeters
f. 903.3 nm to micrometers
35. Many atomic dimensions are expressed in angstroms. (1 Å = 1 x 10 -8 cm). What is the
angstrom equal to in terms of the SI units nanometer (nm) and picometer (pm)?
37. Perform the following unit conversions:
a. Congratulations! You and your spouse are the proud parents of a new baby, born while you
are studying in a country that uses the metric system. The nurse has informed you that the
baby weighs 3.91 kg and measures 51.4 cm. Convert your baby’s weight to pounds and
ounces and her length (rounded to the nearest quarter inch).
45. You’re planning to buy a new car. One model that you’re considering gets 32 miles to a
gallon gasoline in highway travel. The one that your spouse likes gets 14 kilometers to the
liter. Which car has the better gas mileage?
47. A person has a temperature of 102.5oF. What is the temperature on the Celsius scale? On
the Kelvin scale?
49. Many chemical quantities are specified as being measured at 25oC. What is this
temperature on the Fahrenheit scale? On the Kelvin scale?
51. A thermometer gives a reading of 20.6oC ± 0.1 oC. What is the temperature in oF? What is
the uncertainty?
53. The density of aluminum is 2.70 g/cm3. Express this value in units of kilograms per cubic
meter and pounds per cubic foot.
55. A star is estimated to have a mass of 2 x 1036 kg. Assuming it to be a sphere of average
radius 7.0 x 105 km, calculate the average density of the star in units of grams per cubic
centimeter.
63. What are some of the differences between a solid, a liquid, and a gas?
65. Classify each of the following as a mixture or a pure substance.
a. water
b. blood
c. the oceans
d. iron
e. brass
f. uranium
g. wine
h. leather
i. table salt (NaCl)
Of the substances, which are elements and which are compounds?
83. A rule of thumb in designing experiments is to avoid using a result that is the small
difference between two large measured quantities. In terms of uncertainties in measurement,
why is this good advice?
ZUMDAHL – CHAPTER TWO QUESTIONS
15. Use Dalton’s atomic theory to account for each of the following:
a. The law of conservation of mass
b. The law of definite proportion
c. The law of multiple proportions
16. What refinements had to be made in Dalton’s atomic theory to account for Gay-Lussac’s
results on the combining volumes of gases?
17. What evidence led to the conclusion that cathode rays had a negative charge?
18. What discoveries were made by J. J. Thomson, Henri Bequerel, and Lord Rutherford?
How did Dalton’s model of the atom have to be modified to account for these discoveries?
19. What is the distinction between atomic number and mass number? Between mass
number and atomic mass?
20. Distinguish between the terms family and period in connection with the periodic table. For
which of these terms is the term group also used?
21. When hydrogen is burned in oxygen to form water, the composition of water formed does
not depend on the amount of oxygen. Interpret this in terms of the law of definite proportions.
22. The two most reactive families of elements are the halogens and the alkali metals. How
do they differ in their reactivities?
23. When mixtures of gaseous H2 and gaseous Cl2 react, a product forms that has the same
properties regardless of the relative amounts of H2 and Cl2 used.
a. How is this result interpreted in terms of the law of definite
proportions?
b. When a volume of H2 reacts with an equal volume of Cl2 at the same
temperature and pressure, what volume of product having the formula HCl is
formed?
24. A reaction of 1 liter of chlorine gas, (Cl2) with 3 liters of fluorine gas (F2) yields 2 liters of
gaseous product. All gas volumes are at the same temperature and pressure. What is the
formula of the gaseous product?
25. Several compounds containing only sulfur (S) and fluorine (F) are known. Three of them
have the following compositions:
i. 1.188 g of F for every 1.000 g of S
ii. 2.375 g of F for every 1.000 g of S
iii. 3.56 3 g of F for every 1.000 g of S
How do these data illustrate the law of multiple proportions?
26. Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The
mass of hydrogen that combines with 1.00 g of nitrogen for each compound is 1.44 x 10 -1 g,
2.16 x 10-1 g, and 2.40 x 10-2 g, respectively. Show how these data illustrate the law of
multiple proportions.
27. Early tables of atomic weights (masses) were generated by measuring the mass of a
substance that reacts with 1.00 g of oxygen. Given the following data and taking the atomic
mass of hydrogen as 1.00, generate a table of relative atomic masses for oxygen, sodium,
and magnesium.
Element
Mass that combines with 1.00 g Oxygen Assumed formula
Hydrogen
0.126 g
HO
Sodium
2.875 g
NaO
Magnesium 1.500 g
MgO
29. After researching information on the mass of the proton, the mass of the electron, and the
sizes of the nucleus and the atom, calculate the densities of a hydrogen nucleus and
hydrogen atom.
30. If you wanted to make an accurate scale model of the hydrogen atom and decided that
the nucleus would have a diameter of 1 mm, what would be the diameter of the entire model?
39. List the noble gas elements. Which of the noble gases has only radioactive isotopes?
41. In the periodic table, how many elements are found in
a. The second period?
b. The third period?
c. The fourth period?
d. Group 5A?
43. How many protons and neutrons are contained in the nucleus of each of the following
atoms? In an atom of each element how many electrons are present?
a. Pu – 238
b. He – 4
c. Cu – 65
d. Co – 60
e. Cr – 52
f. Cr - 54
45. An atom has 9 protons and 10 neutrons in the nucleus. What is its symbol?
47. What is the symbol for an ion with 63 protons, 60 electrons, and 88 neutrons?
49. What is the symbol of an ion with 16 protons, 18 neutrons, and 18 electrons?
53 . Classify the following elements as metals or nonmetals:
a. Mg
d. Si
g. Rn
j. Ti
b. Ge
e Eu
h. Au
k. B
c Am
f. Bi
i. At
l. Br
55. Which of the following sets of elements are all in the same group in the periodic table?
a. Fe, Ru, Os
c. Sn, As, S
b. Rh, Pd, Ag
d. Se, Te, Po
57. Consider the elements of Group 4A (the “carbon family”): C, Si, Ge, Sn, and Pb. What is
the trend in metallic character as one goes down this group?
59. Would you expect each of the following atoms to gain or lose electrons when forming
ions? What ion is the most likely in each case?
a. Na
c. Ba
e. Al
b. Sr
d. I
f. S
61. Name each of the following compounds:
a. NaCl
b. Rb2O
c. CaS
d. AlI3
63. Name each of the following compounds:
a. CrO3
c. Al2O3
e. CaBr2
b. Cr2O3
d. NaH
f. ZnCl2
65. Name each of the following compounds:
a. KClO4
c. Al2(SO4)3
b. Ca3(PO4)2 d. Pb(NO3)2
67. Name each of the following compounds:
a. NI3
c. SF2
b. PCl3
d. N2F4
69. Name each of the following compounds:
a. CuI
f. S4N4
b. CuI2
g. SF6
c. CoI2
h. NaOCl
d. Na2O3
i. BaCrO4
e. NaHCO3
k. NH4NO3
71. Write the formula for each of the following compounds:
a. cesium bromide
e. silicon Tetrachloride
b. barium sulfate
f. chlorine trifluoride
c. ammonium chloride
g. beryllium oxide
d. chlorine monoxide
h. magnesium fluoride
73. Write the formula for each of the following compounds:
a. Sodium oxide
g. lead(IV) sulfide
b. Sodium peroxide
h. copper(I) chloride
c. Potassium cyanide
i. gallium arsenide
d. Copper(II) nitrate
j. cadmium selenide
e. Silicon tetrachloride
k. zinc sulfide
f. Lead(II) sulfide
ZUMDAHL – CHAPTER THREE QUESTIONS
21. The element Magnesium (Mg) has three stable isotopes with the following masses and
abundances:
Istotope
Mass (amu)
Abundance
24Mg
23.9850
78.99%
25Mg
24.9858
10.00%
26Mg
25.9826
11.01%
23. An element is a mixture of two isotopes. One isotope of an element has an atomic mass
of 34.96885 amu and has a relative abundance of 75.53%. The other isotope has an atomic
mass of 36.96590 amu. Calculate the average atomic mass and identify the element.
25. The element Europium exists in nature as two isotopes: 151Eu has a mass of 150.9196
amu, and 153Eu has a mass of 151.96 amu. Calculate the relative abundance of the two
europium isotopes.
29. Calculate the mass of 500. atoms of iron (Fe)
31. Diamond is a natural form of pure carbon. How many atoms of carbon are in a 1.00-carat
diamond (1.00 carat = 0.200 g)?
33. Aluminum metal is produced by passing an electric current through a solution of
aluminum oxide (Al2O3) dissolved in molten cryolite (Na3AlF6). Calculate the molar masses of
Al2O3 and Na3AlF6.
35. Calculate the molar mass of the following substances.
a. NH3
b. N2H2
c. (NH4)2Cr2O7
37. How many moles of compound are present in 1.00 g of each of the compounds in
Exercise 35?
39. How many grams of compound are present in 5.00 mol of each of the compounds in
Exercise 35?
41. How many grams of Nitrogen are present in 5.00 mol of each of the compounds in
Exercise 35?
43. How many molecules (or formula units) are present in 1.00 g of each of the compounds
in Exercise 35?
47. Ascorbic acid, or vitamin C (C6H8O6), is an essential vitamin. It cannot be stored by the
body and must be present in the diet. What is the molar mass of ascorbic acid? Vitamin C
tablets are taken as a dietary supplement. If a typical tablet contains 500.0 mg of vitamin C,
how many moles and how many molecules of Vitamin C does it contain?
49. How many moles are represented by each of these samples?
a. 100 molecules (exactly) of H2O
b. 100.0 g H2O
c. 150 molecules (exactly) of O2
51. Determine the mass in grams of the following:
a. 3.00 x 1020 N2 molecules
b. 3.00 x 10-3 mol N2
c. 1.5 x 102 mol N2
d. A single N2 molecule
53. Aspartame is an artificial sweetner that is 160 times sweeter than sucrose (table sugar)
when dissolved in water. It is marketed as Nutra-Sweet. The molecular formula of aspartame
is C14H18N2O5.
a. Calculate the molar mass of aspartame.
b. How many moles of molecules are present in 10.0 g aspartame?
c. Calculate the mass in grams of 1.56 mol aspartame.
d. How many molecules are in 5.0 mg aspartame?
e. How many atoms of nitrogen are in 1.2 g aspartame?
f. What is the mass in grams of 1.0 x 109 molecules of aspartame?
g. What is the mass in grams of one molecule of aspartame?
55. Photocells use a semiconducting material that produces an electric current or a change
in resistance on exposure to light. Compounds of cadmium (Cd) combined with an element
from Group 6A of the periodic table are used in many common photocells. Calculate the mass
percent of Cd in CdS, CdSe, and CdTe.
57. In 1987 the first substance to act as a superconductor at a temperature above that of
liquid nitrogen (77K) was discovered. The approximate formula fo the substance is
YBa2Cu3O7. Calculate the percent composition by mass of this material.
59. Arrange the following substances in order of increasing mass percent of carbon:
a. caffeine, C8H10N4O2
b. sucrose, C12H22O11
c. ethanol, C2H5OH
63. Express the composition of each of the following compounds as the mass percents of its
elements.
a. formaldehyde, CH2O
b. glucose, C6H12O6
c. acetic acid HC2H3O2
65. Give the empirical formula for each of the following compounds for which the common
names are given.
a. vitamin C, C6H8O6
b. benzene, C6H6
c. acetylene, C2H2
d. phosphorus pentoxide, P4O10
e. glucose, C6H12O6
f. acetic acid, HC2H3O2
67. One of the most commonly used white pigments in paint is a compound of titanium and
oxygen that contains 59.9% Ti by mass. Determine the empirical formula of this compound.
71. A compound that contains only nitrogen and oxygen is 30.4$ N by mass; the molar mass
of the compound is 92 g/mol. What is the empirical formula of the compound? What is the
molecular formula of the compound?
73. Benzene contains only carbon and hydrogen and is 7.74% H by mass; the molar mass
of benzene is 78.1 g/mol. Determine the empirical and molecular formulas of benzene.
79. Write a balanced chemical equation that describes each of the following:
a. Iron metal reacts with oxygen to form rust, iron (III) oxide.
b. Calcium metal reacts with water to produce aqueous calcium hydroxide and hydrogen
gas.
c. Aqueous barium hydroxide reacts with aqueous sulfuric acid to produce solid barium
sulfate and water.
81. Balance the following equations:
a. Cu(s) + AgNO3 (aq) → Ag(s) + Cu(NO3)2 (aq)
b. Zn (s) + HCl (aq) → ZnCl2 (aq) + H2(g)
c. Au2S3(s) + H2(g) → Au (s) + H2S (g)
83. Balance the following equations representing combustion reactions:
a. C12H22O11 (s) + O2 (g) → CO2 (g) + H2O (g)
b. C6H6 (l) + O2 (g) → CO2 (g) + H2O (g)
c. Fe (s) + O2 (g) → Fe2O3 (s)
d. C4H10 (g) + O2 (g) → CO2 (g) + H2O (g)
e. FeO (s) + O2 (g) → Fe2O3 (s)
91. The reusable booster rockets of the U.S. space shuttle employ a mixture of aluminum
and ammonium perchlorate for fuel. A possible equation for this reaction is
3Al (s) + 3NH4ClO4 (s) → Al2O3 + AlCl3 (s) + 3 NO (g) + 6H2O (g)
What mass of NH4ClO4 should be used in the fuel mixture for every kilogram of Al?
93. Coke is an impure form of carbon that is often used in the industrial production of metals
from their oxides. If a sample of coke is 95% carbon by mass, determine the mass of coke
needed to react completely with 1.0 ton of copper (II) oxide.
2CuO (s) + C (s) → 2Cu (s) + CO2 (g)
95. The compound cisplatin, Pt(NH3)2C12, has been studied extensively as an antitumor
agent.
a. Calculate the elemental percent composition by mass of cisplatin.
b. Cisplatin is synthesized as follows:
K2PtCl4 (aq) + 2NH3 (aq) → Pt(NH3)2Cl2(s) + 2KCl(aq)
What mass of cisplatin can be made from 100. g of K2PtCl4 and sufficient NH3? What mass of
KCl is also produced?
97. Consider the reaction
Mg (s) + I2 (s) → MgI2 (s)
Identify the limiting reacgen in each of the reaction mixtures below:
a. 100 atoms of Mg and 100 molecules of I2
b. 150 atoms of Mg and 100 molecules of I2
c. 200 atoms of Mg and 300 molecules of I2
d. 0.16 mol Mg and 0.25 mol I2
e. 0.14 mol Mg and 0.14 mol I2
f.
0.12 mol Mg and 0.08 mol I2
g. 6.078 g Mg and 63.46 g I2
h. 1.00 g Mg and 2.00 g I2
i. 1.00 g Mg and 20.00 g I2
99. When a mixture of silver metal and sulfur is heated, silver sulfide is formed:
16Ag (s) + S8(s) → 8Ag2S (s)
a. What mass of Ag2S is produced from a mixture of 2.0 g Ag and 2.0 g S8?
b. What mass of which reactant is left unreacted?
101. Consider the following unbalanced equation:
Ca3(PO4)2 (s) + H2SO4 (aq) → CaSO4 (s) + H3PO4 (aq)
What masses of calcium sulfate and phosphoric acid can be produced from the
reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H 2SO4 by
mass)?
105. Aluminum burns in bromine, producing aluminum bromide:
2Al(s) + 3Br2 (l) → 2AlBr3 (s)
In a certain experiment, 6.0 g of aluminum was reacted with an excess of bromine to yield
50.3 g aluminum bromide. Calculate the theoretical and percent yields for this experiment.