WHS • AP Chemistry
Welcome to AP Chemistry
EXPECTATIONS
Congratulations! As an AP Chemistry student, you are about to embark on an exciting adventure into the world of
Chemistry. It will be a challenging year. You already have a background in chemistry from your Chemistry I class, but AP
Chem is very different. Rather than memorizing how to do particular types of problems, you must really understand the
chemistry and be able to apply it. AP Chemistry is a difficult course because it covers two semesters of college chemistry
AND lab work. To succeed, you must keep up with the assignments and be willing to spend time working through the
material outside of class.
In order to make sure you are prepared and everyone is on the same page when we start school in August, AP Chem
comes with a summer assignment. Your assignment involves completing three packets of work by watching the videos that
accompany each packet. You also have information you need to memorize by the start of school. The completed packets
are due the first day of class and we will have a quiz on the material that is to be memorized the first week of school. The
assignment packets will count as one test grade. I check my e-mail frequently, so feel free to contact me if you are having
problems doing the summer assignment ([email protected]). In order to assist you in this important endeavor, I
have scheduled time to meet with you as a group at the Panera on Huffman Mill. I will be there on the following dates and
times to answer questions and help you through your assignments. These meetings are not mandatory or required; they
are merely to help you as you work through the assignments - think of them as study sessions. You can show up to ask one
question or show up to ask 100. You can not show up at all. But please keep in mind, a strong understanding and mastery
of the basic skills covered in these packets will make your life as an AP Chem Student so much easier.
Date
July 16, 2013
July 30, 2013
August 13, 2013
Time
3:00 – 5:00
3:00 – 5:00
3:00 – 5:00
I am looking forward to getting to know all of you! Have a great summer!
Ms. Curtis
Topics Covered
Chemical Foundations
Atoms, Molecules and Ions
Stoichiometry I
WHS • AP Chemistry
Welcome to AP Chemistry
SUMMER
ASSIGNMENT
You will have a quiz on the second day of class on the solubility rules and common ions. You MUST memorize
these. Get an early start!!!
Solubility Rules:
1. All
common compounds of Group
I (alkali
metals) and
ammonium
ions
are
soluble.
2. All
nitrates, acetates, and chlorates
are
soluble.
3. All
binary
compounds
of
the
halogens (other
than
F)
with
metals
are
soluble,
except
those
of
Ag,
Hg(I),
and
Pb.
(Pb
halides
are
soluble
in
hot
water.)
4. All
sulfates
are
soluble,
except
those
of
barium,
strontium,
calcium,
lead,
silver,
and
mercury(I).
The
latter
three
are
slightly
soluble.
5. Except
for
rule
1,
carbonates,
hydroxides,
oxides,
silicates,
and
phosphates
are
insoluble.
6. Sulfides
are
insoluble
except
for
calcium,
barium,
strontium,
magnesium,
sodium,
potassium,
and
ammonium.
Common Ions:
aluminum
Al3+
strontium
Sr2+
ammonium
NH4+
stannous
Sn2+
barium
Ba2+
stannic
Sn4+
calcium
Ca2+
zinc
Zn2+
cuprous
Cu+
acetate
C2H3O2- or CH3COO-
cupric
Cu2+
bromide
Br-
ferrous
Fe2+
carbonate
CO32-
ferric
Fe3+
chlorate
ClO3-
hydrogen
H+
chloride
Cl-
hydronium
H3O+
chromate
CrO42-
lead
Pb2+
dichromate
Cr2O7-
lithium
Li+
fluoride
F-
magnesium
Mg2+
hydroxide
OH-
manganese
Mn2+
iodide
I-
mercurous
Hg22+
nitrate
NO3-
mercuric
Hg2+
oxide
O2-
nickel
Ni2+
permanganate
MnO4-
potassium
K+
phosphate
PO43-
silver
Ag+
sulfate
SO42-
sodium
Na+
sulfide
S2-
WHS • AP Chemistry
1 • Chemical Foundations
SUMMER ASSIGNMENT
Watch the Chemical Foundations Video found at http://vimeo.com/14216778. The questions below will
reinforce the reviewed topics.
1.
Identify the following changes as physical or chemical changes:
a.
b.
c.
Baking soda reacts with vinegar to produce carbon dioxide.
The copper sheath on the Statue of Liberty turns green.
Addition of salt melts ice on the highway.
d.
e.
f.
Steam condenses on the windowpane.
Epoxy resin cures and hardens.
Sugar dissolves in a cup of coffee.
g.
Natural gas burns in a furnace.
2.
a.
b.
c.
Calculate the density of lead if a 10 kg block has a volume of 885 cm3.
What is the volume of a 100 g bar of aluminum if its density is 2.70 g·cm-3?
Calculate the mass of 100 cm3 of uranium (density 19.07 g·cm-3).
4.
Convert:
c. 25°C to K
6.
Which of the following physical properties are extensive?
a. heat of fusion
d. viscosity
b. melting point
e. conductivity
c.
7.
9.
f. density
Write the names of the following elements:
a.
8.
color
N
b. Ca
c.
K
Write the symbols for the following elements:
a. silicon
b. chlorine
c. iron
Convert:
a. 1342 mL into L
b.
3.26 x 10-6 km into mm
d.
P
d. sodium
e.
V
e. silver
c.
d.
8,768 mg into g
400 cm3 into m3
e.
3600 sq. in. into sq. ft.
f. sulfur
10. Write the following numbers in scientific notation with the correct number of significant figures:
a.
1,327
b. 0.00562
c. 2.76
d. 0.166
e. 0.09911
11, Measurements of the boiling point of a liquid were taken by two laboratory technicians (A and B). The
actual boiling point was 92.3. Which technician achieved the most accurate result and which technician
was the most precise?
A: 92.0 92.1 92.4
B: 91.9 92.5 92.6
92.2
92.0
12. Match the prefix with the correct multiplier:
milli
mega
Kilo
micro
centi
Pico
10-6
103
10-2
106
10-12
10-3
13. Evaluate the following expressions. Express the answers in scientific notation with the correct number of
significant figures and the correct units.
a. 0.0045 in + 1.0098 in + 0.987 in + 23.08 in
b. (3.45 cm3 x 2.70 g·cm-3) + (7.433 cm3 x 1.677 g·cm-3)
c.
2.703 g/(1.376 cm x 2.45 cm x 3.78 cm)
14. A 12.3 g block of an unknown metal is immersed in water in a graduated cylinder. The level of water in
the cylinder rose. The level of water in the cylinder rose exactly the same distance when 17.4 grams of
aluminum (density 2.70 g·cm-3) was added to the same cylinder. What is the unknown metal’s density?
15. Use the outline described in Section 1.8 to plan your approach to solving the following problem. Describe
the strategy you use.
The level of water in a graduated cylinder is at the 100 mL mark. When a platinum crucible floats on the
surface of the water, the level reads 157.9 mL. When the crucible is totally immersed in the same cylinder,
the level reads 102.70 mL. What is the density of platinum? The density of water is 0.997 g/mL at 25°C.
16. If one pound is 453.59 grams, how many grams are there in one ounce? How many ounces are there in one
kilogram?
17. A sample of gold alloy contains 5.6% silver by mass. How many grams of silver are there in 1 kilogram of
the alloy?
WHS • AP Chemistry
1 • Chemical Foundations
SUMMER ASSIGNMENT PRACTICE TEST
e)
1.
How many
significant digits are
present in the
4.
is
a) 1
b) 2
c) 3
temperature read
from the
thermometer
illustrated to the
right?
a) 1
b) 2
2.
5.
c) 3
d) 4
d) 4
e) 5
A box measures 3.50 cm x 2.915 cm. The
product of these numbers = 10.2025 cm2. What
is the proper way to report the area of the box?
a) 10.20 cm2
c) 10 cm2
b) 10.2 cm2
d) 10. cm2
The dimensions of a rectangular solid are 8.00
cm long, 4.00 cm wide, and 2.00 cm high. If
the density of the solid is 10.0 g/cm3, what is its
mass?
a) 10/64 grams
b) 10.0 grams
30.9232
24.85 + 23.26
The number of significant digits in 0.30500
6.
The result of 2.350 x (4.0 + 6.311) is,
a) 24
c) 24.21
b) 24.2
d) 24.205
7.
A student does a calculation using her
calculator and the number 280.27163 is shown
on the display. If there are actually three
significant figures, how should she show the
final answer?
d) 320 grams
e) 640 grams
c) 64.0 grams
3.
A metal sample weighing 30.9232 grams was
added to a graduated cylinder containing 23.26
mL of water. The volume of water plus the
sample was 24.85 mL. Which setup will result
in the density of this metal?
a) 30.9232 x (24.85-23.26)
b)
30.9232
24.85 − 23.26
24.85 − 23.26
c)
30.9232
d) 30.9232 x
a) 280
b) 280.3
c) 280.27
d) 2.80 x 10-2
e) 2.80 x 102
8.
The term that refers to the reproducibility of a
laboratory measurement is
a) precision
c) accuracy
b) repeatability
d) exactness
9.
Which measurement below is NOT written
24.85
23.26
with three significant digits?
a) 2.00 cm
c) 0.003 L
13.
b) 550. grams
the
d) 12.7 mm
10. The number 6.33 x 102 equals,
a) 6.33
c) 633
b) 0.633
d) 0.0633
11. All the following are characteristic properties
Chromatography is a good way to separate
a) elements in a compound
b) the components in a mixture
c) the atoms in an element
d) the phases of a pure substance
14. When a pure solid substance was heated, a
of phosphorus. Which one is a chemical
property?
a) Both red phosphorus and white phosphorus
student obtained another solid and a gas, each
of which was a pure substance. From this
information which of the following statements
exist in solid allotropic forms.
b) The red form melts at about 600°C and the
white form melts at 44°C.
c) The white form is soluble in liquid carbon
is ALWAYS a correct conclusion?
a) The original solid is not an element.
b) Both products are elements.
c) The original solid is a compound and the
disulfide, but is insoluble in water.
d) When exposed to air, white phosphorus will
burn spontaneously, but red phosphorus
will not.
gas is an element.
d) The original solid is an element and the gas
is a compound.
e) Both products are compounds.
12. Classify each observation as a physical or a
chemical property and tally them.
Observation 1: Bubbles form on a piece of
metal when it is dropped into acid.
Observation 2: The color of a crystalline
substance is yellow.
Observation 3: A shiny metal melts at 650°C.
Observation 4: The density of a solution is 1.84
g/cm3
a) 2 chemical properties and 2 physical
properties
b) 3 chemical properties and 1 physical
properties.
c) 1 chemical properties and 3 physical
properties
d) 4 chemical properties
e) 4 physical properties
15. The prefix “milli-” corresponds to what
multiplication factor?
a) 10-6
d) 103
b) 10-3
c) 101
e) 106
16. A solution of sugar water may be defined as a
a) heterogeneous mixture
b) homogeneous mixture
c) heterogeneous compound
d) homogeneous compound
e) homogeneous element
17. “Wafting” is the proper technique for
a) neutralizing a spilled acid.
b)
c)
d)
e)
putting out burning clothing.
washing chemicals from the eye.
smelling a chemical substance.
observing the color of a chemical.
18. You measure the density of a slab of lead as
11.10 g/mL. The accepted value is 11.34
g/mL. The percent error for your measurement
is
a) 2.1 %
c) 3.7 %
b) 2.4 %
d) 5.1 %
19. Which one of the following elements is
correctly matched with its symbol?
a)
b)
c)
d)
Ag, gold
Ni, nickel
Fl, fluorine
Mg, manganese
e) H, helium
20. The marks on the following target represent
someone who is:
a) accurate, but not precise.
b) precise, but not accurate.
c) both accurate and precise.
d) neither accurate nor precise.
Answers: (Please use CAPITAL letters)
1.
11.
2.
12.
3.
13.
4.
14.
5.
15.
6.
16.
7.
17.
8.
18.
9.
19.
10.
20.
WHS • AP Chemistry
2 • Atoms, Molecules and Ions
SUMMER ASSIGNMENT
Watch the Atoms, Molecules and Ions video at http://vimeo.com/14217141. The questions below will
reinforce the reviewed topics.
For questions 7-9, you may need to refer to the Stoichiometry I Video in packet 3.
1. Give the mass number of each of the following atoms:
(a) an iron atom with 30 neutrons
(b) an americium atom with 148 neutrons
(c) a tungsten atom with 110 neutrons
2.
Give the complete symbol ( AZ X ) for each of the following atoms:
(a) nitrogen with 8 neutrons
(b) zinc with 34 neutrons
(c) xenon with 75 neutrons
3.
How many electrons, protons, and neutrons are there in an atom of:
(a) carbon-13, 13 C
(b) copper-63, 63 Cu
(c) bismuth-205, 205 Bi
4.
Fill in the blanks in the table (one column per element).
65
86
Symbol
Cu
Kr
Number of protons
Number of neutrons
Number of electrons
in the neutral atom
Name of element
78
117
46
36
5.
Radioactive americium-241 is used in household smoke detectors and in bone mineral analysis. Give
the number of electrons, protons, and neutrons in an atom of americium-241.
6.
Which of the following are isotopes of element X, with atomic number of 9:
7.
Verify that the atomic mass of magnesium is 24.31 amu, given the following information:
24
Mg , mass = 23.985042 amu; percent abundance = 78.99%
25
Mg , mass = 24.985837 amu; percent abundance = 10.00%
26
Mg , mass = 25.982593 amu; percent abundance = 11.01%
19
9
X , 209 X , 189 X , and
21
9
X.
8.
Copper has two stable isotopes, 63 Cu and 65 Cu , with masses of 62.939598 amu and 64.927793 amu,
respectively. Calculate the percent abundances of these isotopes of copper.
9.
Strontium has four stable isotopes, Strontium-84 has a very low natural abundance, but
and
88
86
Sr , 87 Sr ,
Sr are all reasonably abundant. Which of these more abundant isotopes predominates?
10. Name the following ionic compounds. Be sure to check for Roman Numerals!
Na3P
MgBr2
Ag2Se
AlCl3
Ca3P2
Ba3N2
Li2O
ZnF2
K2S
SrI2
(NH4)2S
Ca3(PO3)2
Li2CO3
Al(C2H3O2)3
KCN
AgNO3
Sb(NO3)5
NiS
Cu(NO3)2
FeCl2
Au(CN)3
Pb(SO4)2
11. Write the correct formulas for each of the ionic compounds.
silver iodide
lithium sulfide
magnesium nitride
cadmium bromide
zinc chloride
barium phosphide
aluminum fluoride
strontium oxide
potassium permanganate
strontium sulfate
cesium bromate
magnesium cyanide
aluminum hypoiodite
cadmium periodate
tin (IV) chlorate
bismuth (III) carbonate
copper (I) sulfide
iron (III) oxide
12. Name the following acids and bases:
1)
NaOH _______________________________________
2)
H2SO3 _______________________________________
3)
H2S _______________________________________
4)
H3PO4 _______________________________________
5)
NH3 _______________________________________
6)
HCN _______________________________________
7)
Ca(OH)2 _______________________________________
8)
Fe(OH)3 _______________________________________
9)
H3P_______________________________________
13. Write the formulas of the following acids and bases:
10)
hydrofluoric acid _______________________________________
11)
hydroselenic acid _______________________________________
12)
carbonic acid _______________________________________
13)
lithium hydroxide _______________________________________
14)
nitrous acid _______________________________________
15)
cobalt (II) hydroxide _______________________________________
16)
sulfuric acid _______________________________________
17)
beryllium hydroxide _______________________________________
18)
hydrobromic acid _______________________________________
WHS • AP Chemistry
2 • Atoms and Elements
S U M M E R
1.
A S S I G N M E N T
P R A C T I C E
T E S T
Certain properties are characteristic of metals.
least in a mass spectrometer?
Which property means that you can pound the
a) +2, 2 amu
c) +1, 1 amu
substance into a foil?
b) +4, 4 amu
d) +1, 4 amu
a) ductility
c) sectility
b) conductivity
d) malleability
10. In a Millikan oil drop type experiment, the
charge on four oil drops (in Coulombs) was
found to be:
2.
Which of the following is a metalloid?
a) As
b) Ag
c) S
d) Pb
3.33
8.88
6.66
11.10
e)
He
Coulombs
Coulombs
Coulombs
Coulombs
What is the charge on the electron according to
3.
4.
Which of the following is a transition metal?
this experiment?
a) Cl
a) 1.11 Coulomb
c) 4.44 Coulomb
b) 2.22 Coulomb
d) 11.10 Coulomb
b) Ni
c) P
d) Ca
e) C
Which of the following is an alkali metal?
a) Mg
b) Kr
c) K
d) Al
e)
H
11. Pictured below is a schematic of the Rutherford
experiment. Which scattered α-particle gives
the best evidence for the nuclear atom?
5.
Which of the following is an lanthanide?
a) Xe
b) Eu
c) Cd
d) P
a
α
W
6.
b) Au
c) Os
d) W
e
e) Hg
a) a
c)
positive
c) c
d) d
e) e
b) power source
12. Which of the following is an isotope of the
element with 20 protons (p=20) and 22
electrode
d) gas inside the tube
In a cathode ray tube, electrons are bent toward
a) a positively charged plate.
b) a negatively charged plate.
9.
b) b
d
Cathode rays start at the
a) negative electrode
8.
c
Which element has the highest melting point?
a) Pb
7.
b
e)
Listed below are the charges and masses of
four particles. Which one will be deflected the
neutrons (n=22)?
a) titanium-22
c) calcium-40
b) zirconium-40
d) titanium-48
13. The imaginary element X has the following
natural abundances and isotopic masses. What
22. He added to the atomic theory the idea that
atoms had positive and negative parts.
is the atomic mass of X?
24
12
26
12
X
24.02 amu
40.0%
X
26.10 amu
60.0%
Show your work:
23. What is the formula of the ionic compound
formed between Mg and Br?
a) MgBr
d) Mg2Br2
b) Mg2Br
For questions 14 - 17, use the following key:
e) Mg2Br3
c) MgBr2
(each answer may be used once, more than
once,
or not at all)
24. What is the formula of the ionic compound
a) alpha
formed between Ca and P?
a) Ca2P3
d) Ca2P
b) beta
b) CaP
c) gamma
c) Ca5P10
e) Ca3P2
d) alpha and beta, but not gamma
25. What is the name of the SO32– ion?
14. A high energy form of light
a) sulfate
d) sulfur trioxide
15. Two protons & two neutrons
b) nitrate
e) hydrogen sulfate
16. A high speed electron
c) sulfite
17. Used by Ernest Rutherford as a “probe”
26. What is the correct formula and charge for the
For questions 18 - 22, use the following key:
(each answer may be used once, more than
chromate ion?
a) CrO42–
d) Cr2O7–
once,
b) CrO4–
e) Cr3+
or not at all.)
c) Cr2O72–
a) John Dalton
b) Ernest Rutherford
27. Which one of the following elements forms
c) J.J. Thomson
ions with two different valences?
d) Democritus
a) calcium
c) iron
b) arsenic
d) fluorine
18. His model of the atom has been called the
“plum pudding” Model.
28. The correct name for CCl4 is
a) carbon(I) chloride
19. His model of the atom has been called the
“billiard ball” model.
b) carbon chloride
c) carbon tetrachloride
20. He studied matter in cathode ray tubes.
d) monocarbon chloride(IV)
21. His philosophical idea included the term
e) carbochlorinate
“atomos”.
29. The correct formula for hydrogen telluride is
a) HTe
c) H3Te
b) H2Te
d) HTe2
30. The correct formula for dinitrogen tetroxide is
a) NO2
d) NO3–
b) N2O4
e) (N2O)4
c) N2O5
31. The correct name for S2Cl2 is
a) sulfur dichloride
b) sulfur(I) chloride
c) sulfur(II) chloride
d) disulfur dichloride
e) sulfur chloride
32. The correct name for NO2 is
a) nitrogen dioxide
b) nitrite
c) nitrogen oxide
d) nitrogen(II) oxide
e) nitrate
33.
Consider the following notation:
220
86
Rn
Which statement below is correct?
a) This particle contains 86 protons
b) This particle has a mass number of 86
c) This particle has an atomic number of 220
d) This particle contains 220 neutrons
34. Which elements did Mendeleev leave spaces
for in his periodic table?
_____
_____
Just For Fun:
Element names finish these sentences.
• A ridiculous inmate is a ___.
• I bumped my ___ the car door.
• I am sad when all the flowers ____.
• What the police officer does to the crook.
___
• What the doctor does to the patient. ___
•
_____
•
35. If copper metal is a mixture two isotopes, Cu63, mass = 62.9298 u and Cu-65, mass =
•
•
64.9278 u. The molar mass of copper is 64.546
g/mole. Calculate the % abundances of the two
isotopes of copper. Show your work.
•
What the undertaker does if the doctor
doesn’t succeed. ___
If your cattle get away, ___.
A famous London theatre is the ___.
Demonstrations help keep the lectures
from getting ___.
Linoleum, tile, and hardwood are three
types of ___.
WHS • AP Chemistry
3 • Stoichiometry I
SUMMER ASSIGNMENT
What the Stoichiometry I Video at http://vimeo.com/13588248. The questions below will reinforce the
reviewed topics.
I. Molar Masses
Given a periodic table, you should be able to calculate the molecular mass (in u’s) or the molar mass (in grams)
for any element or compound.
Examples: (give answers to two decimal places)
H2SO4
Cl2
CO2
N2O
Ca(OH)2
HC2H3O2
NaOCl
Al2S3
II. Fraction and Percent Composition
It is useful to determine how much of a compound’s mass is made up of each element. Water, H2O, for
example has a molar mass of 18.02 g. The H’s mass is 2(1.0079) = 2.02 g. The O’s mass is 16.00 g.
2.02
16.00
= 0.112 = 11.2%.
O=
= 0.888 = 88.8%.
We can set up fractions for each element: H =
18.02
18.02
This is called the percent composition. The fraction composition is a good in-between step.
Determine the fraction and percent composition of each element below (answer to one decimal place):
1. H2SO4
2. Ca(OH)2
3. HC2H3O2
4. CO2
5. N2O
6. NaOCl
7. Al2S3
Mole Calculations - Difficulty Level 1
1 mole = 6.02 x 1023 molecules = 22.4 L (@ STP)
1.
Calculate the mass of 1.58 moles CH4. [molar mass CH4 = 16.0 g/mol]
G: 1.58 moles CH4
N: ? g CH4
1.58 moles CH4
=
2.
What volume will 7.29 moles of CO2 gas occupy at STP?
G: 7.29 moles CO2
N: ? L CO2
7.29 moles CO2
=
3.
How many molecules are there in a 0.00583 mole sample of H2O?
G: 0.00583 moles H2O
N: ? molecules H2O
0.00583 moles H2O
=
4.
What mass of CO2 gas occupies a volume of 100. Liters at STP? [molar mass CO2 = 44.0 g/mol]
G: 100. Liters CO2
N: ? g CO2
100. Liters CO2
=
5.
How many molecules are in a 35.0 gram sample of H2O? [molar mass H2O = 18.0 g/mol]
G: 35.0 g H2O
N: ? molecules H2O
35.0 g H2O
=
6.
What volume will 5.25 x 1022 molecules of CH4 occupy at STP?
G: 5.25 x 1022 molecules CH4
N: ? L
22
5.25 x 10 molecules CH4
=
Mole Calculations - Difficulty Level 2
1 mole = 6.02 x 1023 molecules = 22.4 L (@ STP)
1.
Calculate the mass of 2.19 moles CH4. [molar mass CH4 = 16.0 g/mol]
G:
N:
=
2.
What volume will 2.22 moles of CO2 gas occupy at STP?
G:
N:
=
3.
How many molecules are there in a 0.127 mole sample of H2O?
G:
N:
=
4.
What mass of CO2 gas occupies a volume of 395 Liters at STP? [molar mass CO2 = 44.0 g/mol]
G:
N:
=
5.
How many molecules are in a 0.250 gram sample of H2O? [molar mass H2O = 18.0 g/mol]
G:
N:
=
6.
What volume will 3.01 x 1022 molecules of CH4 occupy at STP?
G:
N:
=
Mole Calculations - Difficulty Level 3
1 mole = 6.02 x 1023 molecules = 22.4 L (@ STP)
1.
Calculate the mass of 7.23 moles CH4. [molar mass CH4 = 16.0 g/mol]
G:
N:
2.
What volume will 9.35 moles of CO2 gas occupy at STP?
G:
N:
3.
How many molecules are there in a 0.0752 mole sample of H2O?
G:
N:
4.
What mass of CO2 gas occupies a volume of 10.8 Liters at STP? [molar mass CO2 = 44.0 g/mol]
G:
N:
5.
How many molecules are in a 1.44 gram sample of H2O? [molar mass H2O = 18.0 g/mol]
G:
N:
6.
What volume will 1.21 x 1024 molecules of CH4 occupy at STP?
G:
N: