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 4 th or 5 th 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 2 nd week of school.
3) Begin memorizing the ions on the table provided. There will be a series of quizzes on these beginning the 3 rd 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 gray 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 1 ST 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 gray 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 1 st 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 cvanfaas@att.net

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
17. Colorimetric or spectrophotometric analysis
18. Separation by Chromatography
Honors/AP Chem Labs
Chemistry I
Empirical Formula of Silver
Oxide
Percent Water in a Hydrate
Formula Mass of Butane
Solution Making
AP Chem
Determination of the freezing point of lauric acid by fp dep.
Identity of a Volatile Liquid by
Molar Mass
Concentration of a Weak Acid
Solution
Redox Titration of Peroxide and
Potassium permanganate
Stoichiometry; Formation of a
Precipitate
K c
of Fe(SCN) +2
OR K sp
of Ca(OH)
2
An Acid/Base Titration Curve An Acid/Base Titration Curve
(Weak Acid / Strong Base)
Rate Law
Heat of Reaction I 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
Determination of the
Concentration of a Solution:
Beer’s Law
Introduction to Spectroscopy
Properties of Buffer Solutions
Liquid Chromatography of a
Beverage Solution
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
Activity Series of the Metals
Establishing a Table of
Reduction Potentials
Nernst Equation
Synthesis of Esters

: Carl Van Faasen
: February 25, 2003
: 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.
: 2 x 250 mL beakers, glass funnel, squeeze bottle, funnel stand, ring stand, electronic balance, stir rod
: calcium chloride ( distilled water, filter paper
CaCl
2

2 H
2
O ), anhydrous sodium carbonate (Na
2
CO
3
),
:
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.
: mass of calcium chloride salt 2.03g mass of sodium carbonate salt mass of filter paper mass of filter paper and precipitate after drying
1.99g
1.43g
2.75g

:
1. Predicted mass of precipitate (see reaction in conclusions #1):
( a )
2 .
03 g CaCl
2

1 .
99 g Na
2
CO
3
2 H
2
O


1 mol
1 mol
Na
2
CaCl
CO
3
106 g Na
2
CO
3
2
147 g CaCl
2


2 H
2 H
2
O
2
O
1 mol Ca

2

1 mol CaCl
2

1 mol CO
1 mol Na
2
3

2
CO
3


1 mol CaCO
1
1 mol CaCO
3
1 mol CO
3

2 mol

Ca

2
0 .
0188
3 
0 .
0138 mol CaCO
3 mol CaCO
3

LR
( b ) 0 .
0138 mol CaCO
3

100 g CaCO
3
1 mol CaCO
3

1 .
38 g CaCO
3
2. Actual mass of precipitate: (mass of filter paper & ppt – mass of paper)
 2.75g – 1.43g = 1.32g of CaCO
3
3. Percent yield:
1 .
32 g
1 .
38 g x 100 %

95 .
7 %
:
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 CaCl
2
salt contributes to the mass, but does not enter the chemical equation.
Ca +2
(aq)
+ CO
3
-2
(aq)

CaCO
3(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.

SO
3
-2
SO
4
-2
PO
3
-3
PO
4
-3
ClO -1
ClO
2
-1
ClO
3
-1
ClO
4
-1
NO
2
-1
NO
3
-1
HSO
4
-1
Cu +1
Cu +2
Ni +2
Fe +2
Transition Metals copper (I) or cuprous copper(II) or cupric nickel(II) or nickelous iron(II) or ferrous
H +1
Li
Na
+1
+1
Representative Metals hydrogen Ag +1 lithium sodium
K +1 potassium
Rb +1 rubidium
Sn +2 tin(II) or stannous
Mn +2 manganese(II)
Co +2 cobalt(II)
Cs
Be
+1
+2 cesium beryllium
Hg +2 mercury(II) or mercuric Mg +2 magnesium
Zn +2
Cd +2
NH
4
+
Hg
2
+2
Pb
Cr
+2
+3
Fe +3 lead(II) Ca +2 calcium chromium(III) or chromic Sr +2 strontium iron(III) or ferric
Mn +3 manganese(III)
Ba +2 barium
Co +3 cobalt(III) Al +3 aluminum
Sn +4 tin(IV) or stannic Pb +4 lead(IV)
ITE/ATE hypochlorite chlorite chlorate perchlorate nitrite nitrate bisulfate or hydrogen sulfate
F -1
Nonmetals fluoride
Cl -1 chloride
Br -1
I -1
H - bromide iodide hydride
O -2 oxide
S -2 sulfide
C
2
H
3
O
2
-1
OH -1
CN -1
SCN -1
HPO
4
-2
H
2
PO
4
-
MnO
4
-
HCO
3
- sulfite sulfate phosphite phosphate
N -3
P -3 nitride phosphide
CO
3
-2
O
2
-2
C
2
O
4
-2
CrO
4
-2
Cr
2
O
7
-2
Others silver zinc cadmium ammonium mercury(I) or mercurous
Others acetate hydroxide cyanide thiocyanate hydrogen phosphate dihydrogen phosphate permanganate bicarbonate or hydrogen carbonate 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
E) Collecting experiment 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 Defenitions 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
* can be easily separated without changing the components
1) homogeneous mixture – one that appears the same throughout
E) Physical Change – can be observed without modifying the substance
F) Chemical Change – observed as a result of a chemical change 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
2) heterogeneous mixture – one in which the separate components are visible
Matter
Mixtures Substances
Homogeneous Heterogeneous 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 y-axis
– horizontal axis; represents the
– vertical axis; represents the independent variable dependent variable directly proportional – as “x” increases, “y” increases inversely proportional – as “x” increases, “y” decreases x y

K OR y = Kx xy = K OR 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 ( o C) Time (s) Temp ( o C) Time (s) Temp ( o C) Time (s) Temp ( o C) Time (s)
20 68.1 40 55.3 60 42.5 80 29.7
25
30
35
64.9
61.7
58.5
45
50
55
52.1
48.9
45.7
65
70
75
39.3
36.1
32.9
85
90
95
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 line through your data. Choose two points which fall on the line and use them to find the slope. slope
 y x
2
2

 y x
1
1 
61 .
7
30


68
20
.
1
 
0 .
64
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 .
64 T

80 .
9
5. What should the dissolving time be at a temperature of 5 o
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 (100 o C). 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 most likely all increase by the same amount. This would cause the graph to have the same slope, but a higher y-intercept.
V. The Laboratory
A. Equipment with which you should be familiar:

B. Symbols you should know:
SYMBOL MEANING
Flammable
Solid
Poisonous
SYMBOL MEANING
RED - Flammable Gas or
Liquid
BLUE – Dangerous when wet
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 H
2
SO
4
.
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
P resent, count from the
P acific side
- If the decimal point is
A bsent, count from the
A tlantic side
For example:
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
36.2 x 4.3 = 155.66 155.66 160
3 sig figs 2 sig figs Calculator answer; needs to be rounded to
2 sig figs
Keep these
2 digits
Drop these digits
Final
Rounded
Answer
For example:
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
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
430
Perform the following:
1) 11,254.1 + 0.1983
11,254.3
3) 8.16 x 5.1355
41.9
2) 66.59 – 3.113
63.48
4) 0.0154 / 883
1.74 x 10 -5

B) Scientific Notation base - must be greater than or equal to 1 and less than 10 power
4.56 x 10
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:
2) 0.00000772 1) 568.672
5.68672 x 10 2 7.72 x 10 -6
Express the following as decimal numbers:
1) 3.54 x 10 -8 2) 9.010 x 10 7
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 x 10
8
)( 1 .
0001 x 10

23
)
( 2 .
43 x 10

10
)( 5 .
3063 x 10
30
)

2)
( 5 .
0404 x 10

22
)( 3 .
2 x 10
5
( 7 .
020 x 10

10
)( 6 x 10
40
)
)

4.22 x 10 -36 4 x 10
C) Accuracy vs. Precision – look at the following measurements:
*
* accuracy precision
- how close a measurement is to the actual value
– how close a set of measurements are to each other
-48
Actual Value: 3.532 m
Trial 1 3.539m
Trial 2
Trial 3
3.530m
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
Trial 3
0.035m
10.112m
These measurements are neither accurate nor precise
Actual Value: 3.532 m
Trial 1 4.523m
Trial 2
Trial 3
4.520m
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 Abbreviation Quantity Measured meter m length gram second g s mass time mole
Kelvin mol
K 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:
Tera- (T-)
Which unit would be appropriate to measure the:
1) distance from Holland to Detroit?
Giga- (G-)
Mega- (M-) kilo- (k-) kilometers (km)
2) volume of vaccine administered in a shot? mL (cm 3 or cc)
3) mass of an atom? picograms (pg) or smaller?
4) width of a proton?
(base) deci- (d-) centi- (c-) milli- (m-) micro- (

-) nano- (n-) nanometers (nm)
5) volume of a tank of gasoline? liters (L)
6) number of bytes of memory on your computer’s hard drive? pico- (p-)
Gigabytes (GB)
* there are also base units for charge and light intensity ( Coulomb and Candela)
* there are combined units for:
1) Volume
* 1 mL = 1 cm 3
2) Density 3) Velocity
1 L = 1 dm 3 g mL
 g cm
3 m s
4) Pressure
Pascals (Pa) kg m
 s
2

N m
2

Pa
5) Energy
Joules (J) kg
 m
2 s
2

J
6) Force
Newtons (N) kg
 m s
2

N
Page 13 of 28

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.
3. Match units on the bottom of the conversion
factor with the known value.
4. Put the units desired on the top.
5. Place the known equivalency into the conversion factor. 2430mm x 1 m
1000 mm
6. Simplify.
2430mm x _________
2430mm x _________ mm
2430mm x m mm
2430 mm x 1 m = 2.43 m
1000 mm
DEFINITIONS APPROXIMATIONS
1 ton = 2000 lbs 1 inch = 2.54 cm
16 oz = 1 lb
1 gal = 4 qts
1 foot = 12 in
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
5 .
6 dm

1
10
1 m dm
3) 3.55 x 10 8 mg = ? kg

0 .
56 m 0 .
504 L

10
3 mL
1 L

504 mL
3 .
55 x 10 8 mg

1 kg
10
6 mg

355 kg
4) 2.06 x 10 -5 km = ? cm
2 .
06 x 10

5
10
5 km

1 km

2 .
06 cm
5) 45.5 cm = ? in 6) 162 lbs = ? g
162 lbs

1 kg
2 .
2046 lbs

10
3
1 kg g

73 , 500 g 45 .
5 cm

1 in
2 .
54 cm

17 .
9 in
7) 14.3 gallons = ? L
14 .
3 gal

4 qts
1 gal

1 L
1 .
06 qts

54 .
0 L
9) 3.45 x 10 -5 g/mL = ? g/L
3 .
45 x 10

5 g mL

10
3 mL
1 L

0 .
0345 g
L
8) 25 miles/hr = ? km/hr
25 mi
 hr
1 km
0 .
6214 mi

4
 km hr
10) 6.2 m 3 = ? cm 3
6 .
2 m
3 
 
3
1 m
3 cm
3

6 .
2 x 10
6 cm
3
Page 14 of 28

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 25 o C Liquids at 25 o C
Densities of Some Common
Solids at 25 o C
Substance Density
(g/L)
Substance Density
(g/mL)
Substance Density
(g/mL)
Substance Density
(g/mL)
Hydrogen 0.0837
Helium 0.179
Air
Oxygen
SF
6
1.28
1.33
6.52
Ether
Ethanol
Water
Mercury
0.719
0.781
1.00
13.3
Styrofoam 0.145
Sodium 0.68
Magnesium 1.38
Aluminum 2.70
Iron 7.86
Copper
Silver
Lead
Gold
Osmium
Density
 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 .
51 cm )
3 
15 .
813251 cm
3 
D
 m
V

27 .
1 g
15 .
8 cm 3

1 .
71 g cm
3
2) What is the mass of 50.0 mL of water? ethanol?
8.96
10.50
11.34
19.30
22.6
D
 m
V

1 .
00 g mL
 m
50 .
0 mL
 m

( 1 .
00 g mL
)( 50 .
0 mL )

50 .
0 g
D
 m

0 .
781 g mL
 m
 m

( 0 .
781 g mL
)( 50 .
0 mL )

39 .
1 g
V 50 .
0 mL
3) If the mass of the copper rectangular solid below is 154.82g, what is the length of side “x”?
D
 m
V

8 .
96 g mL

154 .
82 g
V

( 8 .
96 g mL
) V

154 .
82 g

( 5 .
4 cm )( 1 .
0 cm ) x
 x

3 .
2 cm V

154 .
82 g
8 .
96 g mL

17 .
279 mL

17 .
279 cm
3
5.4 cm
4) Diamonds are measured in carats, and 1 carat = 0.200g. The density of diamond is 3.51 g/cm 3 . What is the volume of a 5.0-carat diamond?
1.0 cm x
5 .
0 carats

0 .
200 g
1 carat
1 cm
3

3 .
51 g

0 .
28 cm
3
Page 15 of 28

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) 1 st row (L

R): E,C,C; 2 nd 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 10 19 15) 5 x 10 5 16) -3.40 x 10 35 17) -1.38 x 10 -16 18) 7.5 x 10 16
Measurement (p 20)
1) 0.02876m 2) 0.000602Gm 3) 3.4mg 4) 2 x 10 -15 ML 5) 3.4565 x 10 10 umol 6) 1.09 x 10 8 mg
7) 6.25 x 10 -4 g/mL 8) 6.83 x 10 -5 m 3 9) $11.51 10) 3.1557 x 10 7 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 10 15 g/cm 3
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/cm 3 6) D min
= 0.639 g/cm 3 , D max
= 0.738 g/cm 3
Review (p. 25 - 28)
I) adeh
II. 1,3,2,5,2,5,3,1,1,3
III. 1) 1.8 x 10 43 2) 2.7 x 10 -10 3) 1.6 x 10 -52 4) 20,600 5) 1.231 x 10 60 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 10 39 2) 3.40 x 10 -18
VI. 1) 29,000mm 3 2) 24.6cm
2 3) 0.000687kg 4) 8.010 x 10 10 um 5) 401kJ 6) 273θcm 3
7) 33.8km 8) 22.7kg 9) 1.65m 10) 0.00200m
2 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 10 8 miles/hr
VII. 1) 3.6 g/mL 2) 0.471 g/mL 3) 2.30 g/cm 3 4) 133 g 5) 23.5 g 6) 577 mL 7) 5.4 g/cm 3
Page 16 of 28

AP Chemistry Summer Work
I. Name the following pieces of lab equipment:
1. 2. 3. 4.
5. besides the round-bottom flask)
II. Match the warning symbol with its correct meaning using the answers below: a. flammable liquid or gas e. flammable solid i. corrosive
6. 7.
(name the two things here b. dangerous when wet c. oxidizer f. poisonous g. radioactive d. irritant h. biohazard
______ 1. ______ 2. ______ 3.
_______ 4. _______ 5. ______ 6. (blue)
______ 7. ______ 8. (red)
Page 17 of 28

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
Satisfied
Customers
45
90
300
400
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 ________ d. You place some red Kool-Aid environment, and it then in water, and the powder dissolves becomes a solid.
_______ b. An iron nail rusts. 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 suf- ficient temperature, it melts.
3) Label the following substances as an element (E), compound (C), homogeneous mixture (HomM), or heterogeneous mixture (HetM)
WATER____ COPPER____ COPPER OXIDE____
SAND ____ 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 40 o C. You then smell the beaker, and rate the odor. This step is repeated for the 600 mL beaker, only heating the beaker to
60 o C. Your final data appears below:
Beaker Temp ( o C) Odor Before Odor After
Heating Heating
250 mL
400 mL
600 mL
22
40
60
1
1
1
1
3
5
Page 18 of 28

AP Chemistry Summer Work
I. How many significant figures?
_____ 1) 46.1
_____ 2) 5
______ 6) 36.300
______ 7) 41.00
______ 11) 400
______ 12) 4θ0
_____ 3) 30
_____ 4) 0.004
______ 8) 4010
______ 9) 0.005010
______ 13) 40θ
______ 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
______________ 2) 71.15 x 38.71
______________ 3) 1 x 17
36.11
+ 555
--------------
______________ 4) 4θ0 x 40.0
______________ 5) 0.0005 x 361.32
11) 500 12) 1θ0
41.00
+ 5
------------
14) (3.0 x 10 -6 ) ( 4.440 x 10 24 ) =
15) (7.45 x 10 7 ) (2 x 10 4 ) (3.1056 x 10 -7 ) =
_______________ 6) 45.1 / 2.000
_______________ 7) 45.1 / 2
_______________ 8) 8 / 153.1
_______________ 9) 6.44 / 6.44
_______________ 10) 36 / 36
13) 60.0
- 7.815
------------
16) (4.71 x 10 -9 ) (-7.22 x 10 43 ) =
17)

6 .
02

3 .
33 x 10
11 x 10
23



4 .
00 x 10
3

18)


2 .
2 x 10
2 .
2

7 x 10
16


3 .
000
4 .
0 x 10
32 x 10

8


Page 19 of 28

AP Chemistry Summer Work
__________________ 1) 2.876 cm = ? m
__________________ 3) 3.4 x 10 -6 kg = ? mg
__________________ 5) 34,565 mol = ? umol
__________________ 7) 0.625 g/L = ? g/mL
__________________ 2) 6.02 x 10 14 nm = ? Gm
__________________ 4) 0.000002 mL = ? ML
__________________ 6) 242 lb = ? mg
__________________ 8) 68.3 cm 3 = ? m 3
____________________ 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 =
 r 2 h) 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 10 8 m/s, how many minutes would it take for sunlight to travel from the sun to the Earth?
Page 20 of 28

1. Fill in the following table:
AP Chemistry Summer Work
Mass Volume Density
6.50 g
42.3 g
4.6 mL
10.5 mL 1.89 g/mL
12.4 g/mL
2. What is the density of the following solids in g/cm 3 ?
24.1 cm r=1.1 cm 1.6 cm
12.4 cm
4.4 cm
2.5 cm
(sphere)
m = 1031 g m = 323 g m = 154 g
3. If the solids shown below are made of aluminum, what is the length of side x?
1.03 dm m = 134 g
0.43 dm
0.22 dm
5.6 cm x a. 8.2 cm m = 1583.28 g b. x m = 2.05 kg
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/cm 3 ? V sphere
= 4/3πr 3
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 cm 3 piece of lead is fastened to a 150.0 cm 3 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 cm 3 of: a) hydrogen gas?
2) What is the volume (in mL) of 1.00 kg of: a) hydrogen gas? b) water? b) water? c) gold? c) gold?
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/cm 3 ? V sphere
= 4/3πr 3
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
 accuracy vs. precision

where are the sig figs?

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
________ 9) 100 ________ 10) 1.20
________ 7) 84.2 ________ 8) 800
III. Calculate the following. Be sure your answer has the correct number of sig figs.
1) (4.0 x 10 28 ) (4.4783 x 10 14 ) = 2) (5.3 x 10 -26 ) (5.12 x 10 15 ) =
3)
7.02×10
4.4×10
−72
−20
5.1348×10
30
5)
(6.012×10 −34 )(6.938×10 3 )
9.02×10
17
4)
4.3872×10 13
6)
(13,430)(0.0235)
(40.01)(7240.01)
Page 25 of 28

AP Chemistry Summer Work
7) 456.30 + 1107.284 + 263.388 =
9) 10.20 - 1.201 =
IV. Convert the following into decimal notation:
1) 9.10 x 10 -3
8) 3.200 + 0.03892 + 0.45653 =
2) 4.00 x 10 6
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 APPROXIMATIONS
1 ton = 2000 lbs 1 inch = 2.54 cm
16 oz = 1 lb
1 gal = 4 qts
1 liter = 1.06 qts
1 km = 0.6214 mi
1 foot = 12 in 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
93.4 mm
7.23 cm
Page 26 of 28

AP Chemistry Summer Work
3) 687 mg = ? kg 7) 21.0 mi = ? km
4) 80.10 km = ? um
5) 4.01 x 10 5 J = ? kJ
6) 2.730 dm 3 = ? cm 3
8) 50.0 lbs = ? kg
9) 65.0 in = ? m
Tera- (T-)
Giga- (G-)
Mega- (M-) kilo- (k-)
10) 20.0 cm 2 = ? m 2 (base) deci- (d-) centi- (c-) milli- (m-)
11) A condor has a wingspan of 305 cm. What is this wingspan in feet? micro- (

-) 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 10 8 m/s, what is the approximate speed in miles/hr?
Page 27 of 28

AP Chemistry Summer Work
VII. Density.
Substance Density
(g/L)
Substance Density
(g/mL)
Substance Density
(g/mL)
Substance Density
(g/mL)
Hydrogen 0.0837
Helium 0.179
Air
Oxygen
1.28
1.33
Ether
Ethanol
Water
Mercury
0.719
0.781
1.00
13.3
Styrofoam 0.145
Sodium 0.68
Magnesium 1.38
Aluminum 2.70
Copper
Silver
Lead
Gold
8.96
10.50
11.34
19.30
SF
6
6.52 Iron 7.86 Osmium 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?
4.82 cm
4. What is the mass of 10.0 mL of mercury?
3.06 cm
1.35 cm
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 10 21 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 ?
V sphere
= 4/3 πr 3 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 thick- ness of the foil in millimeters?
Page 28 of 28