Bladensburg High School
Advanced Placement
Chemistry
Summer Packet
2012
What is covered in Advanced Placement Chemistry
The Advanced Placement course is intended to be equal to the general
chemistry course usually taken during the first year of college. The topics
covered in this course are listed below.
•
•
•
•
•
Structure of Matter
States of Matter
Reactions
Descriptive Chemistry
Laboratory
In order to be successful in Advanced Placement Chemistry, it is critical to review
concepts learned in chemistry. The activities included in this packet will help with
your review preparation prior to taking the AP Chemistry course during the 20122013 school year.
Bring your completed packet on the first day of class to address concerns and or
questions regarding the activities. Remember to review the online resources and
take the practice quizzes when available.
Good luck and have a wonderful summer!
=
Worksheet 1 - Calculations
Significant Figures - the number of significant figures (sig. fig.) is a measure of
the degree of uncertainty in a measurement. There is experimental uncertainty
in the last significant figure of a measurement. The rules for sig. fig. are given in
Chapter 1.5. All non-zero numbers are significant. Zeros between numbers are
significant. Zeros to the left of numbers are not significant. Zeros to the right of
numbers may be significant (in presence of a decimal point).
1. Express each of the following numbers in scientific notation and decide the
number of significant figures:
Scientific notation
409.10
______________
4091.00
______________
0.004091
______________
308,000
______________
30,860.
______________
0.00056030 ______________
sig.fig.
_____
_____
_____
_____
_____
_____
Calculations with significant figures - In multiplication or division, the
number of sig. fig. in the answer has only as many sig. fig. as the factor with the
smallest number of sig. fig.
which rounds to .0040 or 4.0 x 10-3 (2 sig. fig.)
In addition and subtraction, the answer should be reported to the same number
of decimal places as the term with the least number of decimal places.
which rounds to 0.84 or 8.4 x 10-1
Do addition and subtraction first. When rounding, numbers ≥ 5 are rounded up.
Do not round until the end of the calculations.
2. Do the following calculations and express the answers to the
correct number of sig. fig.
29.837-29.241 =
32.064
752.12 + 26.3 =
760.00
Dimensional Analysis - This technique can be used to change units (K → oC)
and also as an aid in solving problems, by carefully keeping track of units. SI
Units and conversion factors are listed in Appendix 6 (A26) in the textbook. A
table of metric to English conversion factors is on page 16 of the textbook.
A certain process yields 4.85 x 10-2 g of a chemical product per second.
How many kilograms will be produced in five days of continuous reaction?
Start with what you know on the left and what you are trying to find on the right.
4.85 x 10-2 g
s
=
kg
Then find conversion factors, which allow you to change your units.
Finally, determine the number of sig. fig. The first term has 3 sig. fig. All of the
other factors are definitions, and have ∞ sig. fig. So, the answer will be limited to
3 sig. fig., 21.0 kg.
In the conversion factors the value of the numerator and denominator are the
same; 60 seconds = 1 minute, 24 hours = 1 day. The final conversion unit
illustrates the use of metric prefixes; 1000 grams = 1 kilogram. It is important to
know these commonly used prefixes.
3. Fill in the missing information in the following chart.
Metric prefix Symbol Exponent
M
10-9
deci
10-6
p
kilo
m
10-2
4. A volume of 520. cm3 is equivalent to:
_____ mL
_____ dL
______ L
5. Make the following conversions (Express your answer in scientific notation.)
a.
0.0024 km to nm
b.
3.5 g/dm3 to mg/mm3
c.
95 yards to cm ( 3 feet in a yard; 2.54 cm in 1 inch)
6. You feel a bit feverish and take your temperature with a lab thermometer,
marked in degrees kelvin. It reads 310 K. What is your Fahrenheit temperature?
[Remember (oF) = 1.8 (oC) + 32o and K = oC +273]
Work on the following problems, paying attention to sig. fig.
7. Write down your height. Convert it to meters (m.)
___ft. ___in.
= ____ m.
8. A child's sandbox is 4.0 ft. wide, 4.0 ft. long and 9.0 in deep. If there are, on
the average, 55 grains of sand per mm3, how many grains of sand are there in
the sandbox?
Answer all Problems.
Significant Digits
1. How many significant digits are there in each of the following quantities?
a. 20 kg
b. 0.0051 g
c. 11 cm
d. 0.010 s
e. 90.4 C
f. 0.004 cm
g. 0.089 kg
h. 100.0 C
i. 20 cars
2. List the number of significant digits for each of the following.
a. 1 km
b. 1.5 mL
c. C. 2.15 000 cm 2
d. 5.380 00 0 s
Density
3. What is the density of piece of concrete that has a mass of 8.76 g and a volume
of 3.07 cm3?
4. Illegal ivory is sometimes detected on the basis of density. What is the density of
a sample of ivory whose volume is 14.5 cm3 and whose mass is 26.8g?
5. An archeologist finds that a piece of ancient pottery has a mass of 0.61 g and a
volume of 0.26 cm3. What is the density of the pottery?
6. 5. Limestone has density of 2.72 g/cm3. What is the mass of 24.9 cm3 of
limestone?
7. Calcium chloride is used as a deicer on roads in winter. It has a density of 2.50
g/cm3. What is the volume of 7.91 g of this substance?
8. Determine the density if a pine board whose dimensions are 4.05 cm by 8.85 cm
by 164 cm and whose mass is 2580 g.
9. Find the density of a 51.6 g cylindrical steel rod of diameter 0.622 cm and length
22.1 cm.
Name____________________________ Date_____________ Period____
Periodic Table Worksheet
Use a Periodic table to find the information asked for below:
1.What is the atomic number of:
Calcium____
Iron _____
Gold_____
Uranium_____
2. What is the Atomic mass of:
Calcium___
Iron_____
Uranium_____
Copper_____
3. How many protons do the following have?
4. How many electrons do the following have?
Calcium have____
Gold have____
Gold_______
Iron_____
Copper______
Copper_____
Iron______
Uranium_____
5. Does mercury have more protons and electrons than tin?
6. Is mercury a heavier element than tin?
7. Does potassium have more electrons than neon?
8. Does hydrogen have more electrons than Uranium?
9. Which has more protons, sulfur or iodine?
10. Which has more protons, iodine or silver?
11. In the boxes below make Bohr models for each of the elements.
a. Determine how many electrons, protons, and neutrons there are in each atom.
b. Draw a Bohr model of each element using the number of electrons, protons, and neutrons
c. NOTE: The first energy level can only hold up to 2 electrons. The second energy level can hold
up to 8 electrons.
_________ Electrons
_________ Protons
_________ Neutrons
_________Electrons
HELIUM
_________ Protons
_________ Neutrons
OXYGEN
12. Study the following model of an atom and answer the following questions:
-
+
-
+
+
+
+
-
-
+
+
+
+
-
+
-
Key:
Particles with no charge
+
a.
b.
c.
d.
e.
Particles with negative charge
Particles with positive charge
How many electrons does this atom have? _________________
How many protons? _________________
How many neutrons? ________________
What is the atomic number? ______________
Find the name of this element by referring to the periodic chart. _______________________
13. Write the symbols or the names for each of these elements:
Chlorine __________________
_______________________ Zn
Copper ___________________
Helium _____________
Potassium _________________
Iron ________________
Silver ____________________
_______________________ P
_____________________ Na
_______________________ Ne
_____________________ Sn
Mercury ______________
50 Ways to Name Your Compound
All of the compounds that you will be asked to name consist of two parts…
Part 1
Metal (single valent)
Part 2
Non-metal
Polyatomic ion
Non-metal
Example
NaCl,
CaCO3
CuCl,
sodium chloride
calcium carbonate
copper(I) chloride
Polyatomic ion
Fe2(CO3)3
iron(III) carbonate
(Latin/old) Non-metal or
Polyatomic ion
Non-metal
Non-metal
Fe2(CO3)3,
CuCl
CO2
ferric carbonate,
cuprous chloride
carbon dioxide
Hydrogen
HCl
hydrogen chloride
HCl(aq)
hydrochloric acid
H2SO4
sulphuric acid
(or ammonium)
Metal (multivalent)
Hydrogen
Non-metal
Polyatomic ion
Rule
Name both parts, ends in -ide
Name both parts
Name both parts, ends in -ide, add
valence after metal
Name both parts, add valence after
metal
Metal has Latin name (ic for higher
valence, ous for lower)
Use Greek prefix system (mono- not
used for 1st element)
If not aqueous, name hydrogen and
non-metal (ending in -ide)
If aqueous,
“hydro” + non-metal + “ic acid”
Name polyatomic ion (ending is -ic
instead of -ate or -ous instead of -ite),
add “acid”
−
Note: no special naming is given for bases. These are considered as a metal + polyatomic ion (OH being a polyatomic ion)
Assignment: write the corresponding name or formula for each of the following:
1. lead(II) sulfide
18. N2O3
35. barium sulfite
2. perchloric acid
19. H2SO3
36. SnCl2
3. hydrogen fluoride
20. HgO(aq)
37. CaHPO3(s)
4. zinc hydroxide
21. iron(II) nitride
38. H2S(g)
5. hydrobromic acid
22. tetraphosphorus decaoxide
39. Li2O2
6. SF6(l)
23. copper(I) oxide
40. Mn(NO2)2
7. HNO2(aq)
24. hypochlorous acid
41. mercuric phosphate
8. HCl(g)
25. potassium peroxide
42. sodium hydrogen carbonate
9. PbCl2
26. CuSO3
43. copper(I) hydrogen sulfate
10. ZnSO4
27. CO
44. carbon tetrachloride
11. ammonium carbonate
28. MgS
45. ammonium phosphate
12. chromium(III) sulfite
29. KClO2
46. SO2(aq)
13. nickel(II) sulfate hexahydrate
30. HI(aq)
47. MgSO4·9H2O
14. hydrosulfuric acid
31. nitrogen trichloride
48. HC2H3O2
15. sulfur trioxide
32. plumbic carbonate
49. P2O3
16. H2CrO4
33. potassium hydrogen sulfite
50. H3PO3
17. A12O3
34. boric acid
Balancing Chemical Equations Worksheet
1.
_____ H2 + _____ O2 Æ _____ H2O
2.
_____ N2 +_____ H2 Æ_____ NH3
3.
_____ S8 + _____ O2 Æ _____ SO3
4.
_____ N2 + _____ O2 Æ _____ N2O
5.
_____ HgO Æ _____ Hg + _____ O2
6.
_____ CO2 + _____ H2O Æ _____ C6H12O6 + _____ O2
7.
_____ Zn + _____ HCl Æ _____ ZnCl2 + _____ H2
8.
_____ SiCl4 + _____ H2O Æ _____ H4SiO4 + _____ HCl
9.
_____ Na + _____ H2O Æ _____ NaOH + _____ H2
10.
_____ H3PO4 Æ _____ H4P2O7 + _____ H2O
11.
_____ C10H16 + _____ Cl2 Æ _____ C + _____ HCl
12.
_____ CO2 + _____ NH3 Æ _____ OC(NH2)2 + _____ H2O
13.
_____ Si2H3 + _____ O2 Æ _____ SiO2 + _____ H2O3
14.
_____ Al(OH)3 + _____ H2SO4 Æ _____ Al2(SO4)3 + _____ H2O
15.
_____ Fe + _____ O2 Æ _____ Fe2O3
16.
_____ Fe2(SO4)3 + _____ KOH Æ _____ K2SO4 + _____ Fe(OH)3
17.
_____ C7H6O2 + _____ O2 Æ _____ CO2 + _____ H2O
18.
_____ H2SO4 + _____ HI Æ _____ H2S + _____ I2 + _____ H2O
19.
_____ FeS2 + _____ O2 Æ _____ Fe2O3 + _____ SO2
20.
_____ Al + _____ FeO Æ _____ Al2O3 + _____ Fe
21.
_____ Fe2O3 + _____ H2 Æ _____ Fe + _____ H2O
22.
_____ Na2CO3 + _____ HCl Æ _____ NaCl + _____ H2O + _____ CO2
23.
_____ K + _____ Br2 Æ _____ KBr
24.
_____ C7H16 +
25.
_____ P4 + _____ O2 Æ _____ P2O5
_____ O2 Æ _____ CO2
+ _____ H2O
26.
Dicarbon dihydride + Oxygen Æ Carbon dioxide + Water
27.
Potassium oxide + Water Æ Potassium hydroxide
28.
Hydrogen peroxide Æ Water + Oxygen
29.
Aluminum + Oxygen Æ Aluminum oxide
30.
Sodium peroxide + Water Æ Sodium hydroxide + oxygen
31.
Silicon dioxide + Hydrogen fluoride Æ Silicon tetrafluoride
32.
Carbon + water Æ Carbon monoxide + Hydrogen
33.
Potassium chlorate Æ Potassium chloride
34.
Potassium chlorate Æ Potassium perchlorate + Potassium chloride
35.
Aluminum sulfate + Calcium hydroxide Æ Aluminum hydroxide + Calcium sulfate
36.
Tetraphosphorus decoxide
37.
Iron III chloride + Ammonium hydroxide Æ Iron III hydroxide + Ammonium chloride
38.
Antimony + Oxygen Æ Tetrantimony Hexoxide
39.
Tricarbon octahydride + Oxygen Æ Carbon dioxide + water
40.
Dinitrogen pentoxide + Water Æ Hydrogen nitrate
41.
Nitrogen trihydride + Nitrogen monoxide Æ Nitrogen + Water
42.
Aluminum + Hydrogen chloride Æ Aluminum chloride + Hydrogen
43.
Phosphorus pentachloride + water Æ Hydrogen chloride + Hydrogen phosphate
44.
Magnesium + Nitrogen Æ Magnesium nitride
45.
Iron + Water Æ Iron III oxide + Hydrogen
46.
Sodium hydroxide + Chlorine Æ Sodium chloride + Sodium hypochlorite + water
47.
Lithium oxide + Water Æ Lithium hydroxide
48.
Ammonium nitrate Æ Dinitrogen monoxide + water
49.
Lead II nitrate Æ Lead II oxide + Nitrogen dioxide + Oxygen
50.
Calcium chlorate Æ Calcium chloride + Oxygen
+
Water
+ Oxygen
+ Water Æ Hydrogen phosphate
Balancing Chemical Equations Worksheet
1.
_____ H2 + _____ O2 Æ _____ H2O
2.
_____ N2 +_____ H2 Æ_____ NH3
3.
_____ S8 + _____ O2 Æ _____ SO3
4.
_____ N2 + _____ O2 Æ _____ N2O
5.
_____ HgO Æ _____ Hg + _____ O2
6.
_____ CO2 + _____ H2O Æ _____ C6H12O6 + _____ O2
7.
_____ Zn + _____ HCl Æ _____ ZnCl2 + _____ H2
8.
_____ SiCl4 + _____ H2O Æ _____ H4SiO4 + _____ HCl
9.
_____ Na + _____ H2O Æ _____ NaOH + _____ H2
10.
_____ H3PO4 Æ _____ H4P2O7 + _____ H2O
11.
_____ C10H16 + _____ Cl2 Æ _____ C + _____ HCl
12.
_____ CO2 + _____ NH3 Æ _____ OC(NH2)2 + _____ H2O
13.
_____ Si2H3 + _____ O2 Æ _____ SiO2 + _____ H2O3
14.
_____ Al(OH)3 + _____ H2SO4 Æ _____ Al2(SO4)3 + _____ H2O
15.
_____ Fe + _____ O2 Æ _____ Fe2O3
16.
_____ Fe2(SO4)3 + _____ KOH Æ _____ K2SO4 + _____ Fe(OH)3
17.
_____ C7H6O2 + _____ O2 Æ _____ CO2 + _____ H2O
18.
_____ H2SO4 + _____ HI Æ _____ H2S + _____ I2 + _____ H2O
19.
_____ FeS2 + _____ O2 Æ _____ Fe2O3 + _____ SO2
20.
_____ Al + _____ FeO Æ _____ Al2O3 + _____ Fe
21.
_____ Fe2O3 + _____ H2 Æ _____ Fe + _____ H2O
22.
_____ Na2CO3 + _____ HCl Æ _____ NaCl + _____ H2O + _____ CO2
23.
_____ K + _____ Br2 Æ _____ KBr
24.
_____ C7H16 +
25.
_____ P4 + _____ O2 Æ _____ P2O5
_____ O2 Æ _____ CO2
+ _____ H2O
26.
Dicarbon dihydride + Oxygen Æ Carbon dioxide + Water
27.
Potassium oxide + Water Æ Potassium hydroxide
28.
Hydrogen peroxide Æ Water + Oxygen
29.
Aluminum + Oxygen Æ Aluminum oxide
30.
Sodium peroxide + Water Æ Sodium hydroxide + oxygen
31.
Silicon dioxide + Hydrogen fluoride Æ Silicon tetrafluoride
32.
Carbon + water Æ Carbon monoxide + Hydrogen
33.
Potassium chlorate Æ Potassium chloride
34.
Potassium chlorate Æ Potassium perchlorate + Potassium chloride
35.
Aluminum sulfate + Calcium hydroxide Æ Aluminum hydroxide + Calcium sulfate
36.
Tetraphosphorus decoxide
37.
Iron III chloride + Ammonium hydroxide Æ Iron III hydroxide + Ammonium chloride
38.
Antimony + Oxygen Æ Tetrantimony Hexoxide
39.
Tricarbon octahydride + Oxygen Æ Carbon dioxide + water
40.
Dinitrogen pentoxide + Water Æ Hydrogen nitrate
41.
Nitrogen trihydride + Nitrogen monoxide Æ Nitrogen + Water
42.
Aluminum + Hydrogen chloride Æ Aluminum chloride + Hydrogen
43.
Phosphorus pentachloride + water Æ Hydrogen chloride + Hydrogen phosphate
44.
Magnesium + Nitrogen Æ Magnesium nitride
45.
Iron + Water Æ Iron III oxide + Hydrogen
46.
Sodium hydroxide + Chlorine Æ Sodium chloride + Sodium hypochlorite + water
47.
Lithium oxide + Water Æ Lithium hydroxide
48.
Ammonium nitrate Æ Dinitrogen monoxide + water
49.
Lead II nitrate Æ Lead II oxide + Nitrogen dioxide + Oxygen
50.
Calcium chlorate Æ Calcium chloride + Oxygen
+
Water
+ Oxygen
+ Water Æ Hydrogen phosphate
Stoichiometry
Worksheet
1.
Na2SIO3
(s)
+
8
HF(aq)

H2SiF6
(aq)
+
2
NaF(aq)
+
3
H2O
(l)
a.
How
many
moles
of
HF
are
needed
to
react
with
0.300
mol
of
Na2SiO3?
b.
How
many
grams
of
NaF
form
when
0.500
mol
of
HF
reacts
with
excess
Na2SiO3?
c.
How
many
grams
of
Na2SiO3
can
react
with
0.800
g
of
HF?
2.
C6H12O6
(aq)

2
C2H5OH
(aq)
+
2
CO2
(g)
a.
How
many
moles
of
CO2
are
produced
when
0.400
mol
of
C6H12O6
reacts
in
this
fashion?
b.
How
many
grams
of
C6H12O6
are
needed
to
form
7.50
g
of
C2H5OH?
c.
How
many
grams
of
CO2
form
when
7.50
g
of
C2H5OH
are
produced?
3.
Fe2O3
(s)
+
CO
(g)

Fe(s)
+
CO2
(g)
(unbalanced!)
a.
Calculate
the
number
of
grams
of
CO
that
can
react
with
0.150
kg
of
Fe2O3
b.
Calculate
the
number
of
grams
of
Fe
and
the
number
of
grams
of
CO2
formed
when
0.150
kg
of
Fe2O3
reacts
4.
2
NaOH
(s)
+
CO2
(g)

Na2CO3
(s)
+
H2O
(l)
a.
Which
reagent
is
the
limiting
reactant
when
1.85
mol
NaOH
and
1.00
mol
CO2
are
allowed
to
react?
b.
How
many
moles
of
Na2CO3
can
be
produced?
5.
C6H6
+
Br2

C6H5Br
+
HBr
a.
What
is
the
theoretical
yield
of
C6H5Br
in
this
reaction
when
30.0
g
of
C6H6
reacts
with
65.0
g
or
Br2?
b.
If
the
actual
yield
of
C6H5Br
was
56.7
g,
what
is
the
percent
yield?
Solubility
Complete all activities.
Activity 1
Go to the site listed below which is a tutorial on precipitation reactions. Follow all
directions. You will be required to hand in a sheet of paper that has each of the
three chemical reactions that you will perform during this tutorial. Record the
complete molecular reaction for each combination of solutions you mix. Identify
the precipitate (name and formula) produced.
9 www.wisc-online.com/objects/index_tj.asp?objID=GCH2904
Activity 2
Go to the site below and mix two solutions at a time. Write the complete
molecular equations for each combination of solutions. Identify the precipitate
(name and formula) that is produced. (You should have three reactions when you
are finished.)
9 www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/crm3s2_3.s
wf
Advanced Placement Chemistry Online Resources
Significant Figures
http://www.chem.sc.edu/faculty/morgan/res
ources/sigfigs/index.html
Writing Formulas and Balancing
Equations
•
http://funbasedlearning.com/chemistr
y/chemBalancer/default.htm
•
http://www.chymist.com/Formulas.pdf
Stoichiometry, Empirical and Molecular
Formula review
Read chapter 10 & 12 in the textbook online
at www.phschool.com . Enter code: cae0611 to access the textbook. Answer the
following practice problems and show your
work.
•
•
•
•
•
•
•
Useful Chemistry sites
http://chemteam.info/ChemTeamInde
x.html
www.chemmybear.com
http://www.sciencegeek.net/APchemi
stry/index.shtml
http://www.chem4kids.com/
Practice problems numbers 36-39 on
pages 310-312
Practice problems numbers 11-14 on
pages 360-361
Practice problems numbers 15 - 18
on pages 365-366
Videos
(very helpful if you are having trouble
understanding the concepts)
• http://docott.com/files.141/screencast
s/
• http://www.gpb.org/chemistryphysics/chemistry/603
Quizzes
http://www.adriandingleschemistrypages.co
m/apquiz.html