To all potential AP Chemistry Students:
Welcome to AP Chemistry! At the end of this class, you will have covered material which is the equivalent
of a college introductory Chemistry class. As I am sure you can imagine, there is a great deal of work that
will be involved in this course. In order to insure that we have enough time to thoroughly cover the more
difficult topics, I am asking that all of you complete some of the early work during the summer. I know
that doesn’t sound like a lot of fun, but all of the work I am assigning should be review for you, and, as a
result, fairly easy to complete. Here is what I would like you to do:
1) Complete the Unit I packet. I have included a set of notes, HW assignments, review sheet, and the Unit
Answer Key. The HW assignments are not required for credit, but they should help you practice the
concepts. The review sheet will be due on the day of the first test, which will be the 4th or 5th day of school.
2) Memorize the names and symbols of the elements on the periodic table. I want you to know the
elements with the atomic numbers 1-56, 72-88, and 92. You DO NOT need to know the atomic masses or
atomic numbers. There will be a quiz with 50 of these elements during the 2nd week of school.
3) Begin memorizing the ions on the table provided. There will be a series of quizzes on these beginning
the 3rd week of school.
4) Prepare lab reports for the labs listed in the “Chemistry I” column of the AP Chemistry Lab Outline
included in this packet.
These reports may either be done on MSWord, Apple Works, or written by hand in a quadrille-ruled (graph
paper) composition book. Make sure to get a set of blue lab sheets from me, so you have your data and
calculations handy. If you are writing them by hand, be sure to write ONLY on the front side of each page,
and use blue or black ink. The format is as follows:
Title of Lab
Date: Date the lab was performed
Purpose: A short description of what the lab is meant to demonstrate
Equipment: list all lab equipment to be used
Materials: list all chemicals to be consumed in the lab
Procedure: this should be a DETAILED, STEP-BY-STEP, description of what was done in the lab. It
must be written in 1ST PERSON PAST TENSE. For example: “I put 250 mL of water in the 400 mL
beaker, and place the beaker on the hot plate.”
Data/Observations: All measurements taken in the lab and observations made should be recorded here.
Make sure all data is presented neatly (tables and charts are nice). NO CALCULATIONS HERE.
Calculations: Make sure all work is shown and answers are circled.
Conclusions: Answer all the questions in this section on the blue sheet. Make sure all of your answers are
complete sentences. There is no need to recopy the question.
A copy of a good lab report is included at the end of the packet for you. You may cut and paste procedures
from my MSWord files. See me if you would like a CD with those files. Make sure to change the wording
so it is 1st person past tense.
I hope you all have a great summer, and I look forward to seeing you in September! If you have any
questions this summer as you go through these assignments, feel free to contact me at home.
Carl Van Faasen
335-3071
[email protected]
Honors/AP Chem Labs
AP Requirement
1. Determination of the Formula
of a Compound
2. Determination of the Percent
water in a Hydrate
3. Determination of molar mass by
vapor density
4. Determination of molar mass
by freezing-point depression
5. Determination of the molar
volume of a gas
6. Standardization of a solution
using a primary standard
7. Determination of Concentration
by Acid/Base Titration
8. Determination of Concentration by
oxidation-reduction titration
9. Determination of mass and mole
relationship in a chemical reaction
10. Determination of the equilibrium
constant for a chemical reaction
11. Determination of appropriate
indicators for various acid-base
titrations; pH determination
12. Determination of the rate of a
reaction and its order
13. Determination of enthalpy change
associated with a reaction
14. Separation and qualitative
analysis of cations and anions
15. Synthesis of a coordination
compound and its chemical analysis
16. Analytical gravimetric
determination
Chemistry I
Empirical Formula of Silver
Oxide
Percent Water in a Hydrate
17. Colorimetric or
spectrophotometric analysis
Determination of the
Concentration of a Solution:
Beer’s Law
Formula Mass of Butane
Determination of the freezing
point of lauric acid by fp dep.
Identity of a Volatile Liquid by
Molar Mass
Solution Making
Concentration of a Weak Acid
Solution
Redox Titration of Peroxide and
Potassium permanganate
Stoichiometry; Formation of a
Precipitate
An Acid/Base Titration Curve
Kc of Fe(SCN)+2
OR Ksp of Ca(OH)2
An Acid/Base Titration Curve
(Weak Acid / Strong Base)
Rate Law
Heat of Reaction I
18. Separation by Chromatography
19. Preparation and Properties of
buffer solutions
20. Determination of electrochemical
series
21. Measurements using electrochemical cells and electroplating
22. Synthesis, purification, and
analysis of an organic compound
AP Chem
Heat of a Reaction II (Hess’
Law)
Qualitative Analysis of Cations
Qualitative Analysis of Anions
Synthesis of Alum
Analysis of Alum
Gravimetric Analysis:
Phosphorus Concentration in
Fertilizer
Introduction to Spectroscopy
Liquid Chromatography of a
Beverage Solution
Properties of Buffer Solutions
Activity Series of the Metals
Establishing a Table of
Reduction Potentials
Nernst Equation
Synthesis of Esters
Stoichiometry: Formation of Calcium Carbonate
Name: Carl Van Faasen
Date: February 25, 2003
Purpose: To form a precipitate of calcium carbonate using a precipitation (doublereplacement) reaction. Using a limiting reactant calculation, we will be able to predict
the mass of the precipitate. We will then measure that mass and calculate a percent error
for our prediction.
Equipment: 2 x 250 mL beakers, glass funnel, squeeze bottle, funnel stand, ring stand,
electronic balance, stir rod
Materials: calcium chloride ( CaCl 2 • 2 H 2 O ), anhydrous sodium carbonate (Na2CO3),
distilled water, filter paper
Procedure:
1. I measured out approximately 2 grams of each of the two salts. I recorded their
exact masses on the table below.
2. I put the salts in separate beakers and added enough water to dissolve them
(approximately 50 mL). I stirred with the stir rod to speed up this process.
3. I slowly poured the solution from one beaker into the other so the 2 solutions
mixed. I noticed a cloudy, white precipitate form in the beaker. I rinsed the
empty beaker with small amounts of distilled water, pouring the rinse into the
beaker with the precipitate.
4. I weighed a piece of filter paper and folded it twice to form a filter for my glass
funnel. I placed the filter/funnel setup in a funnel stand, and put the empty beaker
under the funnel.
5. I slowly poured the slurry with the precipitate through the funnel. I noticed that
the filtrate was very clear, a good indication that the filter works well.
6. When the filtration was complete, I gently removed the wet filter from the funnel
and placed it on a metal pan. The instructor placed it in a drying oven to dry
overnight.
7. The next day, I weighed the filter paper with the dry precipitate and recorded its
mass. I disposed of the calcium carbonate as instructed.
Data:
mass of calcium chloride salt
mass of sodium carbonate salt
mass of filter paper
mass of filter paper and precipitate after drying
2.03g
1.99g
1.43g
2.75g
Calculations:
1. Predicted mass of precipitate (see reaction in conclusions #1):
2.03g CaCl 2 • 2 H 2 O ∗
(a )
1mol CaCl 2 • 2 H 2 O 1mol Ca +2 1mol CaCO 3
∗
∗
= 0.0138mol CaCO 3 → LR
147 g CaCl 2 • 2 H 2 O 1mol CaCl 2
1mol Ca + 2
−2
1.99 g Na 2 CO 3 ∗
1mol Na 2 CO 3
1mol CO 3
1mol CaCO 3
∗
∗
= 0.0188mol CaCO 3
106 g Na 2 CO 3 1mol Na 2 CO 3 1mol CO 3 − 2
(b) 0.0138mol CaCO 3 ∗
100 g CaCO 3
= 1.38 g CaCO 3
1mol CaCO 3
2. Actual mass of precipitate: (mass of filter paper & ppt – mass of paper)
•
2.75g – 1.43g = 1.32g of CaCO3
3. Percent yield:
1.32 g
x100% = 95.7%
1.38 g
Conclusions:
1. Net Ionic Equation for the reaction performed:
• Note that the spectator ions (Cl-1 and Na+1) are removed. Also the water of
hydration for the CaCl2 salt contributes to the mass, but does not enter the
chemical equation.
Ca+2(aq) + CO3-2(aq) CaCO3(s)
2. Sources of error:
Our percent yield was 95.7%, so I would consider the lab a success overall. The yield
was below the ideal of 100%, indicating that some precipitate had most likely been lost. I
noticed that some precipitate was stuck to the beaker after the filtration which could
account for this. I would also suspect that smaller grains of the precipitate may have
leaked through the filter paper. My filtrate was very clear, so I doubt this would be a
significant factor. These results could be improved by using a finer grade of filter paper,
or perhaps using a spatula-like device to remove more precipitate from the beaker.
Cations
Cu+1
Transition Metals
copper (I) or cuprous
Cu+2
Ni+2
Fe+2
Sn+2
Mn+2
Co+2
Hg+2
Pb+2
Cr+3
Fe+3
Mn+3
Co+3
copper(II) or cupric
nickel(II) or nickelous
iron(II) or ferrous
tin(II) or stannous
manganese(II)
cobalt(II)
mercury(II) or mercuric
lead(II)
chromium(III) or chromic
iron(III) or ferric
manganese(III)
cobalt(III)
Sn+4
tin(IV) or stannic
H+1
Li+1
Na+1
K+1
Rb+1
Cs+1
Representative Metals
hydrogen
lithium
sodium
potassium
rubidium
cesium
Be+2
Mg+2
Ca+2
Sr+2
Ba+2
beryllium
magnesium
calcium
strontium
barium
Al+3
aluminum
Pb+4
lead(IV)
Ag+1
Others
silver
Zn+2
zinc
Cd+2
cadmium
NH4+
Hg2+2
ammonium
mercury(I) or mercurous
Anions
ClO-1
ClO2-1
ClO3-1
ClO4-1
NO2-1
NO3-1
HSO4-1
ITE/ATE
hypochlorite
chlorite
chlorate
perchlorate
nitrite
nitrate
bisulfate or hydrogen
sulfate
SO3-2
SO4-2
sulfite
sulfate
PO3-3
PO4-3
phosphite
phosphate
F-1
Cl-1
Br-1
I-1
H-
Nonmetals
fluoride
chloride
bromide
iodide
hydride
O-2
oxide
C2H3O2-1
OH-1
CN-1
SCN-1
HPO4-2
H2PO4MnO4-
Others
acetate
hydroxide
cyanide
thiocyanate
hydrogen phosphate
dihydrogen phosphate
permanganate
S-2
sulfide
HCO3-
bicarbonate or hydrogen
carbonate
N-3
P-3
nitride
phosphide
CO3-2
O2-2
C2O4-2
CrO4-2
Cr2O7-2
carbonate
peroxide
oxalate
chromate
dichromate
I. Chemistry Today
* chemistry – the study of the materials that make up the universe and the changes they undergo
II. Scientific Method – a systematic approach to research which all scientists follow
A) Stating a problem
B) Researching the nature of the problem - assign variables
1. independent variable – the pre-determined variable in an experiment; x-axis
2. dependent variable – the measured variable in the experiment; y-axis
C) Forming a hypothesis
D) Designing an experiment
E) Collecting data
1) qualitative data – general observations
2) quantitative data – data containing numerical measurement
F) Using data to decide validity of hypothesis - forming a theory
III. Basic Definitions of Matter
A) Matter – anything that has mass and occupies space
B) Mass – a measure of the amount of matter in an object
* weight – the reaction of gravity to mass; varies with location
C) Substances – a form of matter with constant composition; 2 groups of pure substances:
1) compound – a chemical combination of 2 or more elements with a fixed proportion
of atoms in it; requires chemical process to separate
2) element – substances that can not be broken down by any chemical means
* represented by a one or two-lettered symbol
D) Mixtures – non-chemical combinations of 2 or more substances; composition can vary
* can be easily separated without changing the components
1) homogeneous mixture – one that appears the same throughout
2) heterogeneous mixture – one in which the separate components are visible
E) Physical Change – can be observed without modifying the substance
F) Chemical Change – observed as a result of a chemical change
Matter
Mixtures
Homogeneous
Heterogeneous
Substances
Compounds
Elements
IV. Graphing. A visual way to see patterns in data. In this class we will always use a standard
Cartesian graph (squares of equal value)
* x-axis – horizontal axis; represents the independent variable
* y-axis – vertical axis; represents the dependent variable
directly proportional – as “x” increases, “y”
increases
x
=K
y
inversely proportional – as “x” increases, “y”
decreases
xy = K OR
OR y = Kx
y=
K
x
S. After doing an experiment on the effect of temperature on the time for dissolving a sugar cube, you
obtain the following data:
Temp (oC) Time (s) Temp (oC) Time (s) Temp (oC) Time (s) Temp (oC) Time (s)
20
25
30
35
68.1
64.9
61.7
58.5
40
45
50
55
55.3
52.1
48.9
45.7
60
65
70
75
42.5
39.3
36.1
32.9
80
85
90
95
29.7
26.5
23.3
20.1
1. Graph the data on the sheet of graph paper below. Be sure to properly title the graph and label your
axes.
2. Is this directly proportional, inversely proportional, or neither?
Neither
3. Draw a best-fit
fit line through your data. Choose two points which fall on the line and use them to find the
slope.
slope =
y 2 − y1 61.7 − 68.1
=
= −0.64
x 2 − x1
30 − 20
4. Choose one of the two points you used and find the equation for the line. Be sure to express your
equation in the form: y = mx+b. Rewrite this equation substituting “T” for x, and “t” for y.
y = mx + b → 68.1 = (−0.64)(20) + b
68.1 = −12.8 + b → b = 68.1 + 12.8 = 80.9
t = −0.64T + 80.9
o
5. What should the dissolving time be at a temperature of 5 C?
y = −0.64 x + 80.9 = ( −0.64)(5) + 80.9 = 77.7 sec
6. Estimate the time required to dissolve a sugar cube in boiling water (100oC).
y = −0.64 x + 80.9 = ( −0.64)(100 ) + 80.9 = 16.9 sec
7. Describe what you think would happen to the data (and therefore the graph) if there were already 3
sugar cubes dissolved in the beaker before performing the experiment.
The dissolving times would mo
most
st likely all increase by the same amount. This would cause the
graph to have the same slope, but a higher yy-intercept.
V. The Laboratory
A. Equipment with which you should be familiar:
B. Symbols you should know:
SYMBOL
MEANING
SYMBOL
MEANING
Flammable
Solid
RED - Flammable Gas or
Liquid
BLUE – Dangerous when
wet
Poisonous
Strong Oxidizer
Radioactive
Corrosive
Strong Irritant
Biohazard
C. Important Safety Rules to know:
1. Never directly smell or taste anything in the lab – learn to waft if smell is needed.
2. When diluting an acid, always add acid to the water, especially with H2SO4.
3. Always READ THE DIRECTIONS FIRST!!!!!
4. Stick to the lab directions. Unauthorized experiments = trouble.
5. Always work with good ventilation.
6. Always heat substances slowly.
7. Always weigh objects using a weigh boat, beaker, or other container.
8. Always use the maximum number of significant digits allowed by your measuring
device.
VI. Handling Numbers
A) Significant Figures
1) Basic Rules:
a. All digits 1-9 are significant
b. All zeros in a “sandwich” are significant
c. All zeros that end a decimal fraction are significant
d. All zeros in front of a fraction and not in a sandwich are not significant
e. All zeros at the end of a number greater than 10 not in a sandwich are not
significant.
f. A “lined” zero (θ) is significant.
* Try the “Atlantic-Pacific” rule to remember:
- If the decimal point is Present, count from the Pacific side
- If the decimal point is Absent, count from the Atlantic side
2) Multiplying and Dividing
* When multiplying and dividing measurements, the answer should have a
number of significant figures equal to the multiplicant with the least
number of sig figs
For example:
36.2 x
4.3 = 155.66
3 sig figs
2 sig figs
Calculator
answer;
needs to be
rounded to
2 sig figs
155.66
Keep
these
2
digits
160
Drop
these
digits
Final
Rounded
Answer
3) Adding and Subtracting
* When adding and subtracting measurements, round your answer to the
decimal place represented by the least precise number – round it to the
“worst” decimal place
For example:
Nearest 1’s digit
Nearest 0.01
Nearest 10’s digit
123
40.55
+ 270
433.55
123
40.55
+ 270
433.55
Keep this
drop this
Perform the following:
1) 11,254.1 + 0.1983
2) 66.59 – 3.113
11,254.3
63.48
3) 8.16 x 5.1355
41.9
4) 0.0154 / 883
1.74 x 10-5
430
B) Scientific Notation
base - must be greater than
or equal to 1 and less than 10
4.56 x 10
power
5
* the number of sig figs in a number expressed in scientific notation
corresponds to the number of sig figs in the base number
Express the following in scientific notation:
1) 568.672
2) 0.00000772
5.68672 x 102
7.72 x 10-6
Express the following as decimal numbers:
1) 3.54 x 10-8
2) 9.010 x 107
0.000 000 0354
90,1θ0,000
Perform the following calculations. Make sure your answers are rounded to the correct number of sig figs.
1)
(5.444 x108 )(1.0001x10−23 )
=
(2.43x10−10 )(5.3063x1030 )
(5.0404 x10−22 )(3.2 x105 )
=
2)
(7.020 x10 −10 )(6 x10 40 )
4.22 x 10-36
4 x 10-48
C) Accuracy vs. Precision – look at the following measurements:
* accuracy - how close a measurement is to the actual value
* precision – how close a set of measurements are to each other
Actual Value: 3.532 m
Trial 1
3.539m
Trial 2
3.530m
Trial 3
3.529m
These measurements are
both accurate (close to the
actual value) and precise
(close to each other)
Actual Value: 3.532 m
Trial 1
4.192m
Trial 2
0.035m
Trial 3
10.112m
These measurements are
neither accurate nor precise
Actual Value: 3.532 m
Trial 1
4.523m
Trial 2
4.520m
Trial 3
4.529m
These measurements are not
accurate, but they are
precise. Perhaps the
measuring device is
uncalibrated or the
procedure is faulty.
AP Chemistry Summer Work
VII. Measurement – gives quantities in a way that all can understand
A) Units – scientists use the SI system (Systeme’ Internationale)
Unit
meter
gram
second
mole
Kelvin
Abbreviation
m
g
s
mol
K
Quantity Measured
length
mass
time
number of items
temperature
* When a base unit is too big or too small for the measurement you are performing,
a prefix can be added to change the unit:
Which unit would be appropriate to measure the:
Tera-
1) distance from Holland to Detroit?
(T-)
kilometers (km)
Giga- (G-)
2) volume of vaccine administered in a shot?
mL (cm3 or cc)
Mega- (M-)
3) mass of an atom?
kilo- (k-)
picograms (pg) or smaller?
(base)
deci- (d-)
centi- (c-)
milli- (m-)
4) width of a proton?
nanometers (nm)
5) volume of a tank of gasoline?
micro- (µ-)
liters (L)
nano- (n-)
6) number of bytes of memory on your computer’s hard drive?
Gigabytes (GB)
pico- (p-)
* there are also base units for charge and light intensity (Coulomb and Candela)
* there are combined units for:
1) Volume
* 1 mL = 1 cm3
= 1 dm3
1L
4) Pressure
Pascals (Pa)
kg
m• s
2
= N m 2 = Pa
2) Density
g
mL
=
3) Velocity
m
g
cm 3
5) Energy
Joules (J)
kg •m2
s2
Page 13 of 28
s
6) Force
Newtons (N)
=J
kg • m
s2
=N
AP Chemistry Summer Work
VIII. The Factor-Label Method of Solving Problems – Dimensional Analysis
* requires a known value and an equivalency
* example: I know 1m = 1000mm. How many meters are equivalent to 2430mm?
1. Write down the known value.
2430mm
2. Set up your conversion factor.
2430mm x _________
3. Match units on the bottom of the conversion
factor with the known value.
2430mm x _________
mm
4. Put the units desired on the top.
2430mm x
5. Place the known equivalency into the conversion factor.
2430mm x
6. Simplify.
DEFINITIONS
1 ton = 2000 lbs
16 oz = 1 lb
1 gal = 4 qts
1 foot = 12 in
m
mm
1
m
1000 mm
2430 mm x
1 m = 2.43 m
1000 mm
APPROXIMATIONS
1 inch = 2.54 cm
1 liter = 1.06 qts
1 km = 0.6214 mi
1 kg = 2.2046 lbs
Perform the following operations:
1) 5.6 dm = ? m
2) 0.504 L = ? mL
103 mL
0.504 L ∗
= 504mL
1L
1m
5.6dm ∗ 1
= 0.56m
10 dm
3) 3.55 x 108 mg = ? kg
3.55 x10 8 mg ∗
4) 2.06 x 10-5 km = ? cm
1kg
= 355kg
10 6 mg
2.06 x10 −5 km ∗
5) 45.5 cm = ? in
6) 162 lbs = ? g
1kg
103 g
162lbs ∗
∗
= 73,500 g
2.2046lbs 1kg
1in
45.5cm ∗
= 17.9in
2.54cm
7) 14.3 gallons = ? L
14.3 gal ∗
10 5
= 2.06cm
1km
8) 25 miles/hr = ? km/hr
4qts
1L
∗
= 54.0 L
1gal 1.06qts
9) 3.45 x 10-5 g/mL = ? g/L
25mi
1km
∗
= 4θ km hr
hr
0.6214mi
10) 6.2 m3 = ? cm3
3.45 x10 −5 g 103 mL
∗
= 0.0345 g L
mL
1L
Page 14 of 28
(10 ) cm
∗
2 3
6.2m
3
1m
3
3
= 6.2 x106 cm3
AP Chemistry Summer Work
IX. Density - an intensive property; what does that mean? The property does not depend on the size of the
sample. Mass and volume are examples of extensive properties (they depend on sample size).
Densities of Some Common Densities of Some Common
Gases at 25oC
Liquids at 25oC
Substance
Hydrogen
Helium
Air
Oxygen
SF6
Density
(g/L)
0.0837
0.179
1.28
1.33
6.52
Substance
Ether
Ethanol
Water
Mercury
Density
(g/mL)
0.719
0.781
1.00
13.3
Densities of Some Common
Solids at 25oC
Substance
Styrofoam
Sodium
Magnesium
Aluminum
Iron
Density =
Density
(g/mL)
0.145
0.68
1.38
2.70
7.86
Substance
Copper
Silver
Lead
Gold
Osmium
Density
(g/mL)
8.96
10.50
11.34
19.30
22.6
mass
Volume
1) What is the density of a cube with sides 2.51cm in length which has a mass of 27.1g?
V = ( 2.51cm) 3 = 15.813251cm 3 → D =
m
27.1g
=
= 1.71 g cm3
V 15.8cm 3
2) What is the mass of 50.0 mL of water? ethanol?
m
m
→ 1.00 g mL =
→ m = (1.00 g mL )(50.0mL) = 50.0 g
V
50.0mL
m
m
D = → 0.781 g mL =
→ m = (0.781 g mL )(50.0mL) = 39.1g
V
50.0mL
D=
3) If the mass of the copper rectangular solid below is 154.82g, what is the length of side “x”?
x
m
154.82 g
→ 8.96 g mL =
→ (8.96 g mL )V = 154.82 g
V
V
154.82 g
V=
= 17.279mL = 17.279cm 3 = (5.4cm)(1.0cm) x → x = 3.2cm
8.96 g mL
D=
5.4 cm
4) Diamonds are measured in carats, and 1 carat = 0.200g. The density of diamond is 3.51 g/cm3. What is
the volume of a 5.0-carat diamond?
5.0carats ∗
0.200 g 1cm3
∗
= 0.28cm3
1carat 3.51g
Page 15 of 28
1.0 cm
AP Chemistry Summer Work
Introduction & Laboratory (p. 17 & 18)
I. 1) Bunsen burner 2) funnel 3) beaker 4) crucible 5) beaker tongs 6) Erlenmeyer flask
7) ring stand with a test tube clamp
II. geifhbca
III. 1) directly proportional. xy-1 = 2.22… OR yx-1 = 0.45 OR y = 0.45x
2) PC, CC, CC, PC, PC, PC 3) 1st row (LR): E,C,C; 2nd row: HetM, HomM, E
4) discuss in class
Sig Figs and Scientific Notation (p. 19)
I. 3,1,1,1,5,5,4,3,4,6,1,2,3,4,3
II. 1) 365 2) 2754 3) 20 4) 16,000 5) 0.2 6) 22.6 7) 20 8) 0.05 9) 1.00 10) 1.0 11) 1100
12) 150 13) 52.2 14) 1.3 x 1019 15) 5 x 105 16) -3.40 x 1035 17) -1.38 x 10-16 18) 7.5 x 1016
Measurement (p 20)
1) 0.02876m 2) 0.000602Gm 3) 3.4mg 4) 2 x 10-15 ML 5) 3.4565 x 1010 umol 6) 1.09 x 108mg
7) 6.25 x 10-4 g/mL 8) 6.83 x 10-5 m3 9) $11.51 10) 3.1557 x 107 s 11) 3.94 kg, 52.1 cm
12) 1.07 hrs 13) 35,000 mL 14) 8.3 min
Density I (p. 21 & 22)
1) D = 1.4 g/mL m = 19.8 g V = 3.41 mL 2) a) 1.4 g/mL b) 19 g/mL c) 9.0 g/mL d) 1.4 g/mL
3)a) 13 cm b) 9.12 cm 4) 1.62 g/mL 5) 44.3 mL 6) 3.2 x 1015 g/cm3 7) $6,700,000
8) D = 0.848 g/mL , yes it will float
Density II (p. 23 & 24)
1) a) 0.00837g b) 100.0g c) 1930g
2) a) 11,900,000 mL b) 10θ0 mL c) 51.8 mL
3) 11.7 mL 4) 50.0 m (50θ0 cm) 5) 2.16 g/cm3 6) Dmin = 0.639 g/cm3, Dmax = 0.738 g/cm3
Review (p. 25 - 28)
I) adeh
II. 1,3,2,5,2,5,3,1,1,3
III. 1) 1.8 x 1043 2) 2.7 x 10-10 3) 1.6 x 10-52 4) 20,600 5) 1.231 x 1060 6) 0.00109 7) 1826.97
8) 3.695 9) 9.00
IV. 1) 0.00910 2) 4,0θ0,000
V. 1) 4.75 x 1039 2) 3.40 x 10-18
VI. 1) 29,000mm3 2) 24.6cm2 3) 0.000687kg 4) 8.010 x 1010 um 5) 401kJ 6) 273θcm3
7) 33.8km 8) 22.7kg 9) 1.65m 10) 0.00200m2 11) 10.0 ft 12) 1.9 oz
13) 52.8 L, $0.44/L, $23.10 14) $1.59/lb 15) 6.71 x 108 miles/hr
VII. 1) 3.6 g/mL 2) 0.471 g/mL 3) 2.30 g/cm3 4) 133 g 5) 23.5 g 6) 577 mL 7) 5.4 g/cm3
Page 16 of 28
AP Chemistry Summer Work
I. Name the following pieces of lab equipment:
1.
5.
2.
3.
6.
4.
7.
(name the two things here
besides the round-bottom flask)
II. Match the warning symbol with its correct meaning using the answers below:
a. flammable liquid or gas
b. dangerous when wet c. oxidizer
e. flammable solid
f. poisonous
g. radioactive
i. corrosive
______ 1.
______ 2.
______ 3.
_______ 4.
_______ 5.
______ 6.
______ 7.
______ 8.
(red)
Page 17 of 28
d. irritant
h. biohazard
(blue)
AP Chemistry Summer Work
III. Miscellaneous
1) Is the following data directly or inversely proportional? Give an equation (including a number for “K”)
that would properly represent this relationship.
Mass of
Cheese (g)
100
200
300
400
Satisfied
Customers
45
90
135
180
2) Label each of the following as a physical change (PC) or chemical change (CC):
_______ a. You place some liquid water in a cold
environment, and it then
becomes a solid.
_______ b. An iron nail rusts.
________ d. You place some red Kool-Aid
in water, and the powder dissolves
and the water becomes red.
________ e. You break a pencil.
_______ c. You place some baking soda in
water, and bubbles form and the
powder disappears.
________ f. When you heat an iron nail to a sufficient temperature, it melts.
3) Label the following substances as an element (E), compound (C), homogeneous mixture (HomM), or
heterogeneous mixture (HetM)
COPPER____
SAND ____
COPPER OXIDE____
WATER____
AIR ____
OXYGEN GAS ____
4) Describe any errors in (i) lab safety and (ii) scientific method you see in the following statement:
You wish to determine the effect of temperature on the volatility of gasoline. First, you enter the
lab area and make sure all the windows are closed and the vents are off so you don’t pollute the
environment. Then you set up a 250 mL, a 400 mL, and a 600 mL beaker on your lab table . You fill the
first beaker up to the 50 mL line, the second beaker to the 100 mL line, and the third beaker to the 150 mL
line with gasoline. You then smell each individual beaker, rating the strength of the odor on a scale from 1
to 5, with 5 being the strongest odor. Then you turn on the gas for your Bunsen burner and obtain a box of
matches from the lab drawer. You then light the match, and use it to light the burner. Holding the beaker
in your hand, you heat the 400 mL beaker over the flame until it is at a temperature of 40oC. You then
smell the beaker, and rate the odor. This step is repeated for the 600 mL beaker, only heating the beaker to
60oC. Your final data appears below:
Beaker Temp (oC) Odor Before Odor After
Heating
Heating
250 mL
22
1
1
400 mL
40
1
3
600 mL
60
1
5
Page 18 of 28
AP Chemistry Summer Work
I. How many significant figures?
_____ 1) 46.1
______ 6) 36.300
______ 11) 400
_____ 2) 5
______ 7) 41.00
______ 12) 4θ0
_____ 3) 30
______ 8) 4010
______ 13) 40θ
_____ 4) 0.004
______ 9) 0.005010
______ 14) 400.0
_____ 5) 10.004
______ 10) -38.3001
______ 15) 0.00400
II. Perform the following calculations. Make sure your answer has the correct number of sig figs.
______________ 1) 36.5 x 10.0
_______________ 6) 45.1 / 2.000
______________ 2) 71.15 x 38.71
_______________ 7) 45.1 / 2
______________ 3) 1 x 17
_______________ 8) 8 / 153.1
______________ 4) 4θ0 x 40.0
_______________ 9) 6.44 / 6.44
______________ 5) 0.0005 x 361.32
_______________ 10) 36 / 36
11)
500
36.11
+ 555
--------------
12)
1θ0
41.00
+ 5
------------
13)
60.0
- 7.815
------------
14) (3.0 x 10-6) ( 4.440 x 1024) =
15) (7.45 x 107) (2 x 104) (3.1056 x 10-7) =
16) (4.71 x 10-9) (-7.22 x 1043) =
(3.33x10 )
(6.02 x10 )(− 4.00x10 )
11
17)
23
3
(2.2 x10 )(3.000x10 )
(2.2 x10 )(4.0 x10 )
−7
18)
Page 19 of 28
16
32
−8
AP Chemistry Summer Work
__________________ 1) 2.876 cm = ? m
__________________ 2) 6.02 x 1014 nm = ? Gm
__________________ 3) 3.4 x 10-6 kg = ? mg
__________________ 4) 0.000002 mL = ? ML
__________________ 5) 34,565 mol = ? umol
__________________ 6) 242 lb = ? mg
__________________ 7) 0.625 g/L = ? g/mL
__________________ 8) 68.3 cm3 = ? m3
____________________ 9) If the price of gold is $327 per ounce, how much would 1.00g of gold be
worth?
____________________ 10) How many seconds are there in a year (365.24 days)?
____________________ 11) When my son, Neil was born, he weighed 8 lbs, 11 oz and had a height of
20.5 inches. What would his measurements be in kilograms and
centimeters?
____________________ 12) If you are driving to New York at a rate of 65 miles/hour, and you pass a sign
that informs you it is 112 km to New York, how long should it take you
to arrive?
____________________ 13) What is the volume of this cylinder in mL? (V = πr2h)
r = 1.4 dm
h = 5.7 dm
____________________ 14) The approximate distance from the Earth to the Sun is 93 million miles.
If the speed of light is about 3.00 x 108 m/s, how many minutes would
it take for sunlight to travel from the sun to the Earth?
Page 20 of 28
AP Chemistry Summer Work
1. Fill in the following table:
Mass
Volume
6.50 g
4.6 mL
10.5 mL
42.3 g
Density
1.89 g/mL
12.4 g/mL
2. What is the density of the following solids in g/cm3?
24.1 cm
1.6 cm
r=1.1 cm
1.03 dm
12.4 cm
0.43 dm
4.4 cm
2.5 cm
m = 1031 g
0.22 dm
(sphere)
m = 154 g
m = 323 g
m = 134 g
3. If the solids shown below are made of aluminum, what is the length of side x?
5.6 cm
a.
x
x
b.
m = 2.05 kg
8.2 cm
m = 1583.28 g
4. If you have an unusually shaped solid which weighs 45.71g and when you place it in a graduated
cylinder containing 20.0 mL of water, the volume increases to 48.3 mL, what is the density of the
solid?
Page 21 of 28
AP Chemistry Summer Work
5. If I have a blob of silver which has a mass of 0.465kg, what is its volume?
6. The diameter of a hydrogen nucleus is 1.0 x 10-6 nm and its mass is 1.67 x 10-24 g.
What is the density of the hydrogen nucleus in g/cm3? Vsphere = 4/3πr3
7. Assuming a cost of $350/oz, how much would you have to pay for a solid cubic foot of gold?
(1 oz = 28.4 g, 1 in = 2.54 cm)
8. A 10.0 cm3 piece of lead is fastened to a 150.0 cm3 piece of Styrofoam. Will the resulting object float or
sink in water?
Page 22 of 28
AP Chemistry Summer Work
1) What is the mass of 100.0 cm3 of:
a) hydrogen gas?
b) water?
c) gold?
b) water?
c) gold?
2) What is the volume (in mL) of 1.00 kg of:
a) hydrogen gas?
3) If 5.25 g of pure silver pellets were added to a graduated cylinder containing 11.2 mL of water, to
what volume level will the water in the cylinder rise?
4) A copper wire has a diameter of 0.25 mm. If a sample of this copper wire has a mass of 22.00g, how
long is the wire (assume the wire is a perfect cylinder)?
5) A 25.00g sample of a solid is placed in a graduated cylinder and then the cylinder is filled to the
50.0 mL mark with benzene. The mass of the benzene and the solid together is 58.80g. Assuming
that the solid is insoluble in benzene and that the density of benzene is 0.880 g/mL, calculate the
density of the solid.
Page 23 of 28
AP Chemistry Summer Work
6) According to the Official Rules of Baseball, a baseball must have a circumference between 9.00 and
9.25 in, and a mass between 5.00 oz and 5.25 oz. What is the maximum and minimum density for
a baseball in g/cm3? Vsphere = 4/3πr3
Page 24 of 28
AP Chemistry Summer Work
I. Good things to know:
• chemistry
• scientific method: hypothesis, data, theory, variables
• matter substances: elements, compounds; mixtures: homogeneous, heterogeneous
• graphing: x-axis, independent variable; y-axis, dependent variable
• graphing: directly proportional, inversely proportional
• commonly used lab equipment and how to use properly
• lab safety, hazard symbols
• significant figures their importance in measurement
• scientific notation: base, power where are the sig figs?
• accuracy vs. precision
• SI system: what are the base units? what units are appropriate in what situations?
• density; intensive properties
Sample Questions and Problems
_______________________ I) Which of the following would be considered proper laboratory procedure?
a. determining the odor of a substance by gently wafting the vapors
if you know the substance is not harmful
b. weighing a crucible while it is still hot
c. measuring a liquid in a graduated cylinder by taking a reading from
the top of the liquid
d. rinsing a pipet with the test solution before performing a titration
e. using a pipet bulb to draw liquid into a pipet
f. pulling your goggles up briefly to rub your eyes
g. measuring the volume of a liquid in a beaker
h. diluting sulfuric acid by measuring out the desired amount of water,
and then slowly pouring the concentrated acid to the water
II. How many sig figs in the following number?
_______ 1) 0.003
________ 2) 10.0
________ 3) 550
_________ 4) 310.01
________ 5) 0.0023
_______ 6) 0.29104
________ 7) 84.2
________ 8) 800
________ 9) 100
________ 10) 1.20
III. Calculate the following. Be sure your answer has the correct number of sig figs.
1) (4.0 x 1028) (4.4783 x 1014) =
3)
5)
.
.
.
. . 2) (5.3 x 10-26) (5.12 x 1015) =
4)
6)
.
.
,
.
.
.
Page 25 of 28
AP Chemistry Summer Work
7)
456.30 + 1107.284 + 263.388 =
9)
10.20 - 1.201 =
8)
3.200 + 0.03892 + 0.45653 =
IV. Convert the following into decimal notation:
1) 9.10 x 10-3
2) 4.00 x 106
V. Convert the following into scientific notation:
1) 4,750,000,000,000,000,000,000,000,000,000,000,000,000
2) 0.000 000 000 000 000 003 40
VI. Answer the following questions. Use the given conversion factors:
DEFINITIONS
1 ton = 2000 lbs
16 oz = 1 lb
1 gal = 4 qts
1 foot = 12 in
APPROXIMATIONS
1 inch = 2.54 cm
1 liter = 1.06 qts
1 km = 0.6214 mi
1 kg = 2.2046 lbs
1) What is the volume of this solid?
2) What is the area of this rectangle?
3.40 cm
32.0 mm
9.6 mm
7.23 cm
93.4 mm
Page 26 of 28
AP Chemistry Summer Work
3) 687 mg = ? kg
7) 21.0 mi = ? km
4) 80.10 km = ? um
8) 50.0 lbs = ? kg
Tera-
(T-)
Giga- (G-)
5) 4.01 x 105 J = ? kJ
9) 65.0 in = ? m
Mega- (M-)
kilo- (k-)
6) 2.730 dm3 = ? cm3
10) 20.0 cm2 = ? m2
(base)
deci- (d-)
centi- (c-)
milli- (m-)
micro- (µ-)
11) A condor has a wingspan of 305 cm. What is this wingspan in feet?
nano- (n-)
pico- (p-)
12) Many candy bars have 9g of fat per bar. If during a chocolate attack you ate one pack of candy
(0.6 dekabars), how many ounces of fat have you ingested?
13) In Europe, gasoline is sold by the liter. If Mr. V’s 1990 Honda Accord has a 14.0 gallon gas tank, how
many liters of gas would it require? If the price of gas at the Speedway is $1.65 per gallon, what
is the price per liter? How much will it cost to fill the tank completely?
14) You are in Paris and want to buy some peaches for lunch. The sign on the fruit stand says that peaches
cost 4.00 euros per kilogram. Assuming that there are 1.14 euros to the dollar, calculate the cost
of a pound of peaches in dollars.
15) If the speed of light is approximately 3.00x 108 m/s, what is the approximate speed in miles/hr?
Page 27 of 28
AP Chemistry Summer Work
VII. Density.
Substance
Density
(g/L)
Hydrogen
0.0837
Helium
0.179
Air
1.28
Oxygen
1.33
SF6
6.52
Substance
Ether
Ethanol
Water
Mercury
Density
(g/mL)
0.719
0.781
1.00
13.3
Substance
Styrofoam
Sodium
Magnesium
Aluminum
Iron
Density
(g/mL)
0.145
0.68
1.38
2.70
7.86
Substance
Copper
Silver
Lead
Gold
Osmium
Density
(g/mL)
8.96
10.50
11.34
19.30
22.6
1. What is the density of an object which has a mass of 4.28 g and displaces 1.2 mL of water when the
object is placed in it?
2. If you have an empty graduated cylinder with a mass of 25.64 g which has a mass of 35.06 g when filled
with 20.0 mL of a liquid, what is the liquid’s density?
3. What is the density of the solid shown below if its mass is 45.86 g?
3.06 cm
4.82 cm
1.35 cm
4. What is the mass of 10.0 mL of mercury?
5. What is the mass of 23.45 mL of water?
6. What volume of ethanol will weigh 1.00 lbs.?
7. The approximate mass of the earth is 5.94 x 1021 metric tons. If the circumference of the Earth at the
equator is approximately 25,000 miles, what is the approximate density of the earth in g/mL ?
Vsphere = 4/3 πr3
C = 2πr
1 metric ton = 1000 kg
8. A sheet of aluminum foil has a total area of 1.000 square feet and a mass of 3.636g. What is the thickness of the foil in millimeters?
Page 28 of 28