Sophomore AP
Name: ______________________________________________________ Chemistry
Sophomore Student
Golder College Prep Class of 2018
Dear AP Chemistry Student,
First, congratulations on successfully completing your freshman year at Golder. You
should be proud of all that you have accomplished! Next year, you are enrolled to be part of
Golder’s first ever Sophomore AP Chemistry course. Its going to be an amazing year and below
you will find the information you need to get you started with the course.
AP Chemistry will be a very challenging course. You will read pages and pages of your
science textbook, take hundreds of pages of notes, study for quizzes, prepare for exams, perform
laboratory experiments, write papers/lab reports, keep an organized portfolio, explore the world
around you, listen to and question current scientists, and more. We have confidence that the
class of 2018 is ready for the challenge and will have historic growth on the science section of
the PLAN. In addition, we are confident that you are ready to raise the bar for AP Chemistry
here at Golder College Prep.
Due to the large amount of material that we will need to cover next year, you will be
responsible for learning the material in this packet by the first day of school. Pace yourself and
spread it out throughout the summer. Memorization takes a while and should be done every day
for 10-15. Stay organized and on track. There is a checklist on the last page of this packet to
help you keep track of your responsibilities. Please be aware, that as an AP student, you will
need to hold yourself to a high standard. The first part of this will be doing your ABSOLUTE
best work on your summer homework. Not doing the assignment, is not an option. It will leave
you far behind and you will have so much to make up in the first few days off school. We are
confident, no student will choose to put themselves in that situation!
Get ready for a great year in AP Chemistry! Have a great (and productive) summer! J
1
Sophomore AP
Name: ______________________________________________________ Chemistry
AP Chemistry Summer Assignment
1. MEMORIZE the symbols and names for the following elements. If you are given the symbol,
you should be able to write the name. If you are given the name, you should be able to write the
symbol. (*Notice the symbols are one capital letter or one capital with one lower case letter) On
the AP test, you are given a periodic table with NO element names so this is very
important for your success in the course/on the test. YOU SHOULD MAKE
FLASHCARDS WITH THE NAME ON ONE SIDE AND SYMBOL ON THE
OTHER TO HELP YOU MEMORIZE! DO THESE 10-15 MINUTES EVERY
DAY!
Name
Symbol
Name
Symbol
Name
Symbol
Hydrogen
H
Titanium
Ti
Molybdenum
Mo
Helium
He
Vanadium
V
Technetium
Tc
Lithium
Li
Chromium
Cr
Ruthenium
Ru
Beryllium
Be
Manganese
Mn
Rhodium
Rh
Boron
B
Iron
Fe
Palladium
Pd
Carbon
C
Cobalt
Co
Silver
Ag
Nitrogen
N
Nickel
Ni
Cadmium
Cd
Oxygen
O
Copper
Cu
Indium
In
Fluorine
F
Zinc
Zn
Tin
Sn
Neon
Ne
Gallium
Ga
Antimony
Sb
Sodium
Na
Germanium
Ge
Tellurium
Te
Magnesium
Mg
Arsenic
As
Iodine
I
Aluminum
Al
Selenium
Se
Xenon
Xe
Silicon
Si
Bromine
Br
Cesium
Cs
Phosphorus
P
Krypton
Kr
Barium
Ba
Sulfur
S
Rubidium
Rb
Platinum
Pt
Chlorine
Cl
Strontium
Sr
Gold
Au
Argon
Ar
Yttrium
Y
Mercury
Hg
Potassium
K
Zirconium
Zr
Lead
Pb
Calcium
Ca
Niobium
Nb
Uranium
U
Scandium
Sc
2
Sophomore AP
Name: ______________________________________________________ Chemistry
2. MEMORIZE the symbols, charges and names of the ions on the ion list. If you are given the ion
formula, you should be able to write the name. If you are given the name, you should be able to
write the formula with charge. YOU SHOULD MAKE FLASHCARDS WITH THE
NAME ON ONE SIDE AND FORMULA WITH CHARGE ON THE OTHER TO
HELP YOU MEMORIZE! DO THESE 10-15 MINUTES EVERY DAY!
a. Example: NO3- is nitrate. NO3- is the formula containing a -1 charge. The ion is
called nitrate.
b. Helpful Hint #1- Any positively charged ions are called cations and any
negatively charged ions are called anions.
c. Helpful Hint #2- Trends in charge on the periodic table.
i. Any element in the first group/column on the periodic table (H, Li, Na, K,
Rb, Cs, Fr) have a +1 charge.
ii. Any element in the second group/column on the periodic table (Be, Mg,
Ca, Sr, Ba, Ra) have a +2 charge.
iii. This elements in the third group/column on the periodic table (Al) has a
+3 charge.
th
iv. These elements in the 15 group/column on the periodic table (N, P) have
a -3 charge.
th
v. These elements in the 16 group/column on the periodic table (O, S) have
a -2 charge.
th
vi. Any element in the 17 group/column on the periodic table (F, Cl, Br, I)
have a -1 charge.
th
vii. Any elements in the 18 group/column on the periodic table (He, Ne, Ar,
Kr, Xe, Rn) have NO charge or a charge of zero.
d. Helpful Hint #3- Any ion with ONE element (monoatomic anions/cations)
containing a charge (Li+, N3-, etc) are named just like the elements are named. Li
is lithium and Li+ is also lithium. N is nitrogen and N3- is also nitrogen.
e. Helpful Hint #4- Memorize the –ate ions first (sulfate, nitrate, chlorate, etc).
i. Once you memorize the –ate ions, the –ite ions have ONE LESS
OXYGEN. Example sulfate is SO42- and sulfite is SO32-.
ii. Once you memorize the –ate ions, the per- ions have ONE MORE
OXYGEN. Example chlorate is ClO3- and perchlorate is ClO4-.
iii. Once you memorize the –ate ions, the hydrogen _____ ions have ONE
HYDROGEN and +1 charge added. Example sulfate is SO42- and
hydrogen sulfate is HSO4-.
f. Helpful Hint #5- “Metals with more than one ion” charges just need to be
memorized. No shortcuts on these guys J Please note the charge corresponds to
the written name (stock system). Example: Fe3+ is Iron (III) and Fe2+ is Iron (II).
3
Sophomore AP
Name: ______________________________________________________ Chemistry
3. SKILL of figuring out what formulas/compounds are created between different ions. Positively
charged ions are attracted to negatively charged ions (think of a magnet! J). Due to different
numbers of charges (+1, -3, +2, -1, etc), different formulas will be created. The key is that all
compounds formed have an overall charge of ZERO. Using the ion puzzle, attached. Complete
the follow up questions
a. For example, Li+ and N3- forming a compound (puzzle) would involve the following
thought process…
i. Each Li+ puzzle piece has one “key” and each N3- has 3 “locks”. If you have an
unlimited amount of each puzzle piece, 3 Li+ “keys” would be needed to fill the
N3- “locks”. Your formula becomes Li3N meaning you used 3 Li and 1 N.
•
•
Notice in your final answer, Li3N, there are no longer + or – signs. You
would write Li3N on the line for the formula and move on to the
next chemical combination.
Notice if you have one of something (like one N in the previous
example), you do not write Li3N1, but rather Li3N.
Directions: Cut out each of the puzzle pieces. Use the “puzzle pieces” to show how the
various compounds bond together.
1. Use your puzzle pieces to combine the following ions to show how they make a
compound. Write down the chemical formula for the final compound.
Remember: Positive ion is written first, negative ion is second! Include subscripts (small
numbers written below the symbol) to show the number of atoms! For example H + O
would use 2 H+ ions and 1 O2- ion, so you would write H2O.
H + F____________
Be + O ___________
Be + I _____________
Al + N ___________
Al + P ____________
Li + P _____________
Li + F ___________
Li + Br ___________
Ca + O ____________
Ca + S ___________
H + O ____________
Al + N _____________
Al + Br __________
K + Cl ____________
K + I ______________
Mg + S __________
K + S ____________
Rb + I _____________
Rb + Br __________
H + Cl ___________
Be + N _____________
4
Sophomore AP
Name: ______________________________________________________ Chemistry
2. What happens to the total charge of the compound after the ions bond together? (Hint:
add together the charges of the ions in the compound).
3. How many lithium ions are required to bond with one nitrogen ion? Why?
4. How many chlorine ions are required to bond with one aluminum ion? Why?
b. Follow Up Questions when you are finished completing your puzzle activity…
i. What do you notice about the formula created when a positive ion and
negative ion join together and have the same, but opposite charge? For
example, Be2+ and O2- or Li+ and Br-.
ii. What do you notice about the formula created when a positive ion and
negative ion join together and have different, but opposite charge? For
example, Be2+ and N3- or K+ and S2-.
4. KNOWLEDGE of comparing and contrasting ionic and covalent bonding. You MUST complete
this section before moving onto nomenclature.
a. Watch and take outline notes on the following ionic/covalent bonding videos.
i. https://www.youtube.com/watch?v=CGA8sRwqIFg
ii. https://www.youtube.com/watch?v=QqjcCvzWwww
b. IONIC BONDING
i. Between a metal and a nonmetal OR a metal with a polyatomic ion
• Ex: NaCl (metal + nonmetal) or Mg3(PO4)2 (metal + polyatomic ion)
ii. Transfer of electrons
• Metals lose electrons and have positive charges
• Nonmetals gain electrons and have negative charges
• Positive and negative charges attract causing a compound to form
c. COVALENT/MOLECULAR BONDING
i. Between 2 or more nonmetals
• Ex: HCl (nonmetal + nonmetal) or CO2 (nonmetal + nonmetal)
ii. Sharing of electrons
• No charges, just sharing of electrons
5
Sophomore AP
Name: ______________________________________________________ Chemistry
iii. Follow Up Question Are the following compounds ionic or covalent?
•
CaSO4
_______________________________________
•
FeCl3
_______________________________________
•
P2 O5
_______________________________________
•
N2 O
_______________________________________
•
NH4Cl
_______________________________________
•
MgCl2
_______________________________________
•
HNO3
_______________________________________
•
SiO2
_______________________________________
•
H2 O
_______________________________________
•
Al(NO3)3
_______________________________________
6
Sophomore AP
Name: ______________________________________________________ Chemistry
5. SKILL of naming ionic and covalent compounds. This process is called Nomenclature. There
are different rules for naming ionic and covalent compounds. Ionic is much more
challenging and diverse so we will start with those.
a. Naming Monoatomic Ionic Compounds (Example: CaBr2)
i. The first element is a metal and will just be called by its element name.
Example: In CaBr2, Ca is pronounced “Calcium”
ii. The second element is a nonmetal and will be called by its element name
ending in –ide (also found on ION LIST in googledocs). Example: In
CaBr2, Br2 is Bromine pronounced à “Bromide”
iii. Try the following compounds
•
NaF
______________________________________
•
CaCl2 ______________________________________
•
AlF3
______________________________________
•
BaI2
______________________________________
•
KCl
______________________________________
b. Naming Polyatomic Ionic Compounds (Example: Al(NO3)3)
i. The first element is a metal and will just be called by its element name.
Example: In Al(NO3)3, Al is pronounced “Aluminum”
ii. The second element is a nonmetal and will be called by its ion name
(found on ION LIST in googledocs that you should have memorized).
Example: In Al(NO3)3, (NO3)3 is “Nitrate”
iii. Try the following compounds
•
NaNO2
______________________________________
•
CaSO4
______________________________________
•
Al(OH)3
______________________________________
•
Ba3(PO4)2
______________________________________
•
KNO3
______________________________________
7
Sophomore AP
Name: ______________________________________________________ Chemistry
c. Naming Covalent Compounds (Example: N2O3)
i. Covalent compounds use prefixes to tell us how many atoms of each
element are present in the compound. In N2O3 there are 2 nitrogen atoms
and 3 oxygen atoms. Using the prefix list below, the compound would be
named “dinitrogen trioxide” to represent 2N and 3O.
• Note that the first word is simply the element name with the prefix
added on and the second is the element ending in –ide (similar to
ionic naming) with the prefix added on.
• HELPFUL HINT- Do NOT add mono- to the first element’s
name. For example CO2 is NOT monocarbon dioxide. It is
carbon dioxide.
ii. 1- mono
2- di
3- tri
4- tetra
5- penta
6- hexa
7- hepta
8- octa
9- nona
10- deca
iii. Try the following compounds
•
P2O5
______________________________________
•
SiO2
______________________________________
•
PCl5
______________________________________
•
CO
______________________________________
•
S2Cl4
______________________________________
6. Balancing Chemical Equations (Note: This may be tricky at first. KEEP TRYING!
It is really fun once you get the hang of it. )
a. Watch and take outline notes on the following balancing chemical equations videos.
i. https://www.youtube.com/watch?v=RnGu3xO2h74
ii. https://www.youtube.com/watch?v=UGf60kq_ZDI
b. Practice balancing on this website (start with beginner and move to
intermediate and advanced. The more practice the better!!! J)
http://education.jlab.org/elementbalancing/
8
Sophomore AP
Name: ______________________________________________________ Chemistry
c. Balance the following equations
•
____S8 + ____O2 → ____SO3
•
____N2 + ____O2 → ____N2O
•
____Zn + ____HCl → ____ZnCl2 + ____H2
•
____CO2 + ____H2O → ____C6H12O6 + ____O2
•
____Al + ____FeO → ____Al2O3 + ____Fe
7. Dimensional Analysis (You should have learned the basics of unit conversions
Freshman year in math. You may use the factor-label method [road maps, etc] or you
may solve these with whatever method you choose) If you need extra help, use resources
such as youtube to find videos to help you J
DIMENSIONAL ANALYSIS PROBLEMS
Conversions Factors
1 hr = 60 min
1 min = 60 sec
1 ton = 2000 lbs
7 days = 1 week
24 hrs = 1 day
1 kg = 2.2 lbs
1 gal = 3.79 L
264.2 gal = 1 cubic meter
1 mi = 5,280 ft
1 kg = 1000 g
1 lb = 16 oz
20 drops = 1 mL
365 days = 1 yr
52 weeks = 1 yr
2.54 cm = 1 in
1 L = 1000 mL
0.621 mi = 1.00 km 1 yd = 36 inches
3
1 cc is 1 cm
1 mL = 1 cm3
DIRECTIONS: Solve each problem using dimensional analysis. Every number must have a
unit. Work must be shown. Conversion factors are given below
1.) How many miles will a person run during a 10 kilometer race?
2.) The moon is 250,000 miles away. How many feet is it from earth?
9
Sophomore AP
Name: ______________________________________________________ Chemistry
3.) A family pool holds 10,000 gallons of water. How many cubic meters is this?
4.) The average American student is in class 330 minutes/day. How many hours/day is this?
How many seconds is this?
5) How many seconds are there in 1 year?
6) Lake Michigan holds 1.3 x 1015 gallons of water. How many liters is this?
7) Pepsi puts 355 ml of pop in a can. How many drops is this?
How many cubic meters is this?
8) Chicago uses 1.2 x 109 gallons of water /day. How many gallons per second must be pumped
from the lake every second to supply the city?
9) Sixty miles/ hour is how many ft/sec?
10) Lake Michigan holds 1.3 x 1015 gallons of water. If just Chicago removed water from the
lake and it never rained again, how many days would the water last? Chicago uses 1.2 x 109
gallons of water /day
10
Sophomore AP
Name: ______________________________________________________ Chemistry
11
Sophomore AP
Name: ______________________________________________________ Chemistry
12
Sophomore AP
Name: ______________________________________________________ Chemistry
13
Sophomore AP
Name: ______________________________________________________ Chemistry
14
Sophomore AP
Name: ______________________________________________________ Chemistry
15
Sophomore AP
Name: ______________________________________________________ Chemistry
Checklist for Summer Assignment
You should have memorized:
o Elements
o Ion list
You should have completed:
o This packet and all questions
o Ion Puzzle
o Balancing Practice Online
o Watching all videos on this packet
You should bring with you on the first day of AP Chemistry:
o This packet
o Flashcards of elements and ions
o Puzzle pieces
o Notes that you took on videos
o Your brain and lots of excitement!!!!!
16
List of Common Ions
Monatomic Cations
+
Polyatomic Cations
H
Li+
Na+
K+
Rb+
Cs+
Ag+
hydrogen
lithium
sodium
potassium
rubidium
cesium
silver
NH4+
H3O+
OHCNO22-
hydroxide
cyanide
peroxide
2+
Mg2+
Ca2+
Sr2+
Ba2+
Zn2+
Cd2+
magnesium
calcium
strontium
barium
zinc
cadmium
3+
Al3+
Bi3+
aluminum
bismuth
CO32C2O42NO2NO3PO33PO43SO32SO42S2O32ClOClO2ClO3ClO4CH3COOor C2H3O2AsO43BO33SiO32MnO4CrO42Cr2O72CHO2-
carbonate
oxalate
nitrite
nitrate
phosphite
phosphate
sulfite
sulfate
thiosulfate
hypochlorite
chlorite
chlorate
perchlorate
1+
Monatomic Anions
HFClBrI-
hydride
fluoride
chloride
bromide
iodide
2-
O2S2-
oxide
sulfide
3-
N3P3-
nitride
phosphide
4-
4-
1-
C
(C22-)
carbide
ammonium
hydronium
Polyatomic Anions
HCO3HSO3HSO4HPO42H2PO4-
acetate
arsenate
borate
silicate
permanganate
chromate
dichromate
formate
hydrogen carbonate
or bicarbonate
hydrogen sulfite
or bisulfite
hydrogen sulfate
or bisulfate
hydrogen phosphate
dihydrogen phosphate
Metals with more than one ion
Element
Ion
Classical (ous, ic)
Stock system System
Chromium
Cr2+
Cr3+
Co2+
Co3+
Cu+
Cu2+
Fe2+
Fe3+
Pb2+
Pb4+
Mn2+
Mn3+
Mn4+
Hg22+
Hg2+
Sn2+
Sn4+
chromium(II)
chromium(III)
cobalt(II)
cobalt(III)
copper(I)
copper(II)
iron(II)
iron(III)
lead(II)
lead(IV)
manganese(II)
manganese(III)
manganese(IV)
mercury(I)
mercury(II)
tin(II)
tin(IV)
Cobalt
Copper
Iron
Lead
Manganese
Mercury
Tin
chromous
chromic
cobaltous
cobaltic
cuprous
cupric
ferrous
ferric
plumbous
plumbic
manganous
manganic
mercurous
mercuric
stannous
stannic
INFORMATION IN THE TABLE BELOW AND ON THE FOLLOWING PAGES MAY BE USEFUL IN
ANSWERING THE QUESTIONS IN THIS SECTION OF THE EXAMINATION.
Chemistry Practice Exam
11
Chemistry Reference Sheet
Periodic Table of the Elements
California Standards Test
1
1A
1
1
H
Hydrogen
1.01
3
2
3
Li
Beryllium
9.01
11
12
Na
6
7
Mg
Sodium
Magnesium
22.99
24.31
K
Key
20
Ca
Na
Sodium
22.99
3
3B
21
Sc
4
4B
22
5
5B
23
Ti
V
Potassium
Calcium
Scandium
Titanium
Vanadium
39.10
40.08
44.96
47.87
50.94
38
39
Rubidium
Strontium
Yttrium
Zirconium
Niobium
85.47
87.62
88.91
91.22
55
56
57
72
Rb
Cs
Sr
Y
Hf
41
Nb
7
7B
25
8
26
Mn
Fe
Iron
Cobalt
52.00
54.94
55.85
58.93
42
43
44
Mo
Tc
Ru
92.91
95.94
(98)
101.07
73
74
75
Co
45
Rh
10
28
Ni
11
1B
29
Nitrogen
Oxygen
Fluorine
Neon
12.01�
14.01
16.00
19.00�
20.18�
14
15
16
Si
P
S
F
17
Cl
10
Ne
18
Ar
12
2B
30
Aluminum
Silicon
Phosphorus
Sulfur
Chlorine
Argon
26.98
28.09�
30.97
32.07
35.45
39.95
31
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
65.39
69.72
72.61
74.92
78.96
79.90
83.80
52
53
Palladium
Silver
102.91
106.42
107.87
76
77
78
79
49
50
51
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon
112.41
114.82
118.71
121.76
127.60
126.90
131.29
80
81
82
83
84
85
86
Rhenium
Osmium
Iridium
Platinum
Pt
Au
Gold
Mercury
Thallium
Tl
Pb
Lead
Bismuth
Polonium
Astatine
Radon
132.91
137.33
138.91
178.49
180.95
183.84
186.21
190.23
192.22
195.08
196.97
200.59
204.38
207.2
208.98
(209)
(210)
(222)
87
88
89
104
105
106
107
108
109
Bh
Hs
Radium
Actinium
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
(223)
(226)
(227)
(261)
(262)
(266)
(264)
(269)
(268)
58
* If this number is in parentheses, then
it refers to the atomic mass of the
most stable isotope.
Cerium
140.12
90
59
Pr
Praseodymium
140.91
60
61
62
Nd
Pm
Sm
144.24
(145)
150.36
Neodymium Promethium Samarium
68
Er
69
Tm
70
Yb
71
Lu
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
157.25
158.93
162.50
164.93
167.26
168.93
173.04
174.97
102
103
Neptunium
Plutonium
Americium
Curium
232.04
231.04
238.03
(237)
(244)
(243)
(247)
Copyright © 2003 California Department of Education
67
Ho
Gadolinium
Uranium
Pu
66
Dy
151.96
Protactinium
Np
65
Tb
Europium
Thorium
U
94
64
Gd
92
Pa
93
63
Eu
91
Th
Rn
Mt
Francium
Ce
At
Xe
Tungsten
Sg
Po
I
54
Sn
Bi
Te
Kr
In
Hg
Sb
Br
36
63.55
48
Se
35
Copper
Cd
As
34
Nickel
47
Ge
33
58.69
46
Ga
32
Zn
Rhodium
Ir
Al
O
Cu
Ag
Os
Carbon
N
4.00�
Tantalum
Db
Re
Boron
10.81
C
Helium
Hafnium
Rf
W
17
7A
9
13
Pd
Molybdenum Technetium Ruthenium
16
6A
8
Lanthanum
Ac
Ta
9
8B
27
Cr
Chromium Manganese
15
5A
7
Barium
Ra
La
40
Zr
6
6B
24
14
4A
6
B
Average atomic mass*
He
13
3A
5
Cesium
Fr
Ba
Atomic number
Element symbol
Element name
11
Be
6.94
37
5
2
2A
4
Lithium
19
4
18
8A
2
95
Am
96
Cm
97
Bk
98
Cf
99
Es
Berkelium Californium Einsteinium
(247)
(251)
(252)
100
Fm
101
Md
Fermium
Mendelevium
(257)
(258)
No
Lr
Nobelium Lawrencium
(259)
(262)