Download AP Chemistry - West Bloomfield School District

May 11, 2014
Dear Prospective AP Chemistry Students and Parents,
Advanced Placement Chemistry is a course designed to be the equivalent of the general chemistry course
taken during the first year of college by science majors. For some students, this course enables them to undertake, as
freshmen, second year work in the chemistry sequence or to register for courses in other fields where general
chemistry is a prerequisite. For other students, the AP Chemistry course fulfills the laboratory science
requirement and frees time for other courses.
AP Chemistry is a rigorous math-based course, with a strong laboratory component. It is intended
for students who have demonstrated a willingness to commit considerable time to studying and
completing assignments outside of class, and who have successfully completed a prior course in
chemistry, preferably Honors Chemistry. Since passing the AP exam may qualify the student to
by-pass a first-year college chemistry course, AP Chemistry should not be considered "college
prep." Rather, this is a college class, with college level expectations for behavior, participation,
and effort.
REQUIRED materials:
 Scientific calculator or graphing calculator (must have LOG key)
 TEXTBOOK: You will be required to pick up your textbook from the school WHEN THERE ARE NO
LONG LINES in the bookroom (during classes, after busses leave, or week after school ends). The book we
will be using is:
Chemistry, 10th edition by Brown, Lemay, & Bursten
 Summer Packet Assignment: The AP Chemistry exam is offered in the beginning of June, so we require
that students complete summer review requirements prior to the start of school. This is vital in assuring that our
students are guided in the best way possible.
*Note: We will be utilizing the WebAssign Online Homework and the billing is applied per class.
RECOMMENDED material:
 AP Chemistry Study Guide: “Princeton Review’s Cracking the AP: Chemistry” has been most notable
(May be purchased from: Barnes and Nobles, Borders, or Amazon.com)
The SUMMER ASSIGNMENT checklist is typed on the first page of the Basics of Chemistry Packet. This
material should be a review of material learned in your prior chemistry course. Please follow those directions
carefully. An exam over the material will occur the first week of class. The assignment will be collected and
you will be held accountable for the chapter notes and memorization of charts.
Please be sure to spend the time to read through the entire packet very carefully! We hope you are excited to be
enrolled in this class. We look forward to meeting all of you in the fall. Have a wonderful summer!
Sincerely,
Mrs. Matynowski & Mrs. Ismail
West Bloomfield High School
For questions or problems, please e-mail at:
[email protected] or [email protected]
1
AP Chemistry
Name__________________________________
Basics of Chemistry Packet
The material included in this packet covers approximately the first 3 chapters of AP Chemistry. You may use your
textbook to help you review the material. The following material should be review for most of you and we
recommend that you begin this a few weeks before school resumes. (Not too early - so it stays fresh)!
Please initial and check off the following before the first day of school:
 Complete Summer Packet
Initials_______
Outline in PEN/PENCIL the first three chapters of the textbook (not typed!)
 Chapter 1 Introduction: Matter and Measurement
Initials ________
 Chapter 2 Atoms, Molecules, and Ions
Initials ________
 Chapter 3 Stoichiometry
Initials ________
 Memorize Polyatomic Ion Sheet (tips on back)
Initials _______
There are plenty of games online: http://www.sporcle.com/games/RyanWitchey/Chem_Anions
 Memorize Solubility Chart
Initials _______
The chapter outlines must be hand written! The objective of the outlines is for you to read and become familiar with
the content material. Focus on key vocabulary, equations, and processes. We recommend that you look at and understand
each sample exercise while outlining each chapter. DO NOT TAKE NOTES ON THE CHAPTER SUMMARY!!
A. Significant Figures. Review Significant Figures in the textbook, as needed. Complete the following questions.
1. How many significant figures are in each of the following measurements?
a. 35.409 grams _________
b. 100.0 ml ___________
c. 0.044 grams _________
d. 4.260 x 1023 molecules ___________
2. Compute the correct answer using significant figures.
a. 23.01 grams + 7.7 grams + 9.110 grams = ___________________
b. 23. 1 grams x 7.71 grams x 9.100 grams = ___________________
3. Compute the correct answer using significant figures.
a. What is the density of a hydrochloric acid solution that has a mass of 17.84 grams and occupies 14.0
milliliters? (density is g/ml)
b. What is the volume, in L, required of nitric acid if the mass of the acid is 32.0 grams? (The density of nitric
acid is 1.251 g/ml).
B. Nomenclature
1. Naming binary molecular compounds: Do not reduce molecular compounds.
Remember that these are compounds made of 2 or more NON-METALS.
1. Use prefixes (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-)
2. If there is one atom of the first element, you do not need the “mono-“
3. Name ends in –ide.
Example: N2F4 dinitrogen tetrafluoride
CO carbon monoxide
2. Naming binary ionic compounds or ternary compounds: You should reduce ionic compounds.
Remember that these are compounds made of at least 1 METAL.
 Write the name of the metal (it is always written first.) as it appears on the periodic table.
 Check on the periodic table to see if the METAL has a variable-charge. If it has more than one charge,
you must use ROMAN numerals. (I, II, III, IV, V, VI, VII, VIII, IX, X) Memorize these now if you do
not know them.
Binary: Write down the non-metal, ending with –ide.
Ternary: Write down the polyatomic ion, ending with –ite, -ate, or –ide. CUT OUT POLYATOMIC ION SHEET
2
3. Names and Formulas of Acids and Bases
Acid - a compound that produces hydrogen ions when it is dissolved in water.
Usually seen as H+ X- (H+ is the hydrogen ion; X- is the anion)
Table 1. Chart for Naming Acids
Anion Ending
**Example
Acid Name
-ide
sulfide : S2hydro - (stem)- ic acid
2-ite
sulfite : SO3
(stem) - ous acid
-ate
sulfate : SO42(stem) - ic acid
**Example
hydrosulfuric acid
sulfurous acid
sulfuric acid
Base - a compound that produces hydroxide ions when it is dissolved in water.
Naming Rules : These are named the same as ionic compounds, cation + anion
Example: NaOH Sodium hydroxide
4. Review the rules above and name the following compounds.
a. BO3
b. Ca3P2
c. SeO4
d. Cl3O2
e. TeI5
f. Se2N4
g. OF8
h. As4Te7
i. Ba(CH3COO)2
j. Ti(CN)3
k. K2S
l. CoCO3
m. Co3N2
n. NaClO3
o. LiNO3
p. MgSO4
q. Mn(PO4)2
r. RbMnO4
s. CsOH
t. Pd(ClO4)4
u. Fe2S3
v. Sn(OH)2
w. Ni(NO2)2
x. K2Cr2O7
y. In(NO3)3
z. YI3
5. Name the following Acids
a. H2S
b. H2CrO4
c. HCl
d. H3P
e. HMnO4
f. HBr
g. H2SO4
h. HClO4
i. HC2H3O2
j. HNO2
3
6. Write the formulas for these names.
a. tetrasilicon triarsenide
b. diselenium hexabromide
c. diphosphorus monoxide
d. octasulfur trioxide
e. carbon monoxide
f. phosphorus hexachloride
g. silicon heptaiodide
h. pentaboron triselenide
i. nickel II nitrite
j. aluminum perchlorate
k. copper II carbonate
l. cadmium sulfate
m. mercury I nitrite
n. hafnium selenide
o. ruthenium III sulfate
p. yttrium carbonate
q. gallium III selenide
r. osmium IV chromate
s. niobium V sulfate
t. ruthenium IV phosphate
u. hexaoxygen difluoride
v. magnesium sulfide
w. calcium phosphide
x. tetrarsenic hexaoxide
y. lead IV chloride
z. ruthenium VI sulfate
Write the formulas for the following acids.
a. phosphorous acid
b. nitric acid
c. sulfuric acid
d. oxalic acid
e. hydrofluoric acid
f. boric acid
g. hydrocyanic acid
h. hypochlorous acid
i. carbonic acid
j. chlorous acid
C. Balance the following equations and identify the type of reaction.
Tip on balancing: If there is the same polyatomic ion on both sides of the equation, balance that compound first! If not,
begin with the most complex compound and work from there. This usually helps. You may use fractions, but be sure
your final answer is in whole numbers.
____N2 
____Ca3N2 (s)
____Fe2O3 (s) 
____Fe(s)
+
12.
____C3H8
+
____O2 
____CO2
13.
____NaCl
+
____Br2

10.
____Ca(s)
11.
+
____O2 (g)
+
____NaBr
____H2O
+
____Cl2
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D.Predicting Products of a Chemical Reaction REFER to PREDICTING PRODUCTS GUIDE at end
Predict the products for the following chemical equations. Classify each reaction as (C) Combustion, (SD) Single
Displacement, (DD) Double displacement, (D1-6) Decomposition, or (S) Synthesis. Then, write the balanced chemical
equation. Indicate the type of reaction on the line to the left of the equation. REFER TO GUIDE AT END OF PK.
14. __DD___ aluminum sulfate + calcium phosphate 
Al2(SO4)3 + Ca3(PO4)2

15. ________
2Al(PO4)
+
3CaSO4
magnesium chloride + silver nitrate 
16. ________ potassium chlorate 
17. ________ hydrogen gas + oxygen gas 
18. ________ silver metal + copper (II) nitrate 
19. ________ sulfurous acid 
20. ________ copper (I) oxide + sulfuric acid 
21. ________ nitrogen gas + hydrogen gas  ammonia gas
22. ________ sodium iodide + chlorine gas 
23. ________ copper (II) hydroxide 
24. ________ ammonia gas (NH3) + hydrochloric acid  (Single product)
25. ________ potassium metal + water (H+OH-)
26. _______ iron + oxygen gas  (will form Fe+3)
27. ________ aluminum metal + sodium acetate 
28. ________ gallium hydroxide + calcium sulfate 
29. ________ calcium chlorate 
30. ________ tungsten (V) chlorate + silver nitride 
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31. ________ barium chloride + sodium hydroxide 
32. ________ tin metal + fluorine gas (Sn4+)
33. ________ potassium iodide + bromine gas 
34. ________ octane(C8H18) + oxygen gas  (remember octane is a hydrocarbon)
35. ________ sodium chloride + sulfuric acid 
36. ________ glucose(C6H12O6) + O2  (glucose reacts as a hydrocarbon)
37. ________ potassium hydroxide + phosphoric acid 
38. ________ iron (II) sulfide + hydrochloric acid 
39. ________ magnesium + nitrogen gas 
D. Stoichiometry
Throughout the year, you will see problems involving compounds made primarily of C and H. These are called
hydrocarbons, or alkanes. You should become familiar with the first 10 normal alkanes.
Methane
CH4
Hexane
C6H14
Ethane
C2H6
Heptane
C7H16
Propane
C3H8
Octane
C8H18
Butane
C4H10
Nonane
C9H20
Pentane
C5H12
Decane
C10H22
A handy way to remember the top 4 is with “Me Eat Peanut Butter!”
You may use the “times 2, plus 2” rule to remember the ratio of C to H.
e.g. octane: I know “octa-“ refers to 8 carbons, so 8 x 2 = 16 + 2 = 18 H
Another interesting fact about hydrocarbons: When you burn (combustion) compounds with H and C (generally with O
also), you always produce CO2 + H2O. ex: CH4(g) + 2O2 (g)

CO2 (g) +
2H2O (g)
40. Write the balanced equation for the combustion of:
a) propane
b) butane
41. If 510.0 grams of propane were combusted in oxygen, how many grams of CO2 were produced? (Use the balanced
equation above, then use stoichiometry.)
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ANSWER ALL OF THE FOLLOWING, # 42 – 72 ON SEPARATE PAPER!! YOU MUST SHOW
WORK FOR FULL CREDIT!!
E. Limiting Reagents
When one chemical is used up, the reaction stops. The limiting reagent is the reactant that is used up in the
reaction. The excess reagent is the reactant that you have in excess after the reaction is complete.
“Grilled Cheese Party” Recipe for a plain grilled cheese sandwich:
1 Cheese +
2 Bread

1 Grilled Cheese Sandwich
Your dad went to Costco and bought one of those 100 singles of American Cheese (he also stocked up on the
pretzels, chips, nachos, dip, and beverages). It was party time, so the party is hopping, and people are ready for
what they came for…the Grilled Cheese Sandwiches!! So, you’re all going to get it started and you notice that
dad FORGOT TO BUY LOAVES OF BREAD. You only have a pack of bread with 6 slices of bread.
a) How many grilled sandwiches can you make?_________ (3)
b) In a sense, 100 moles of cheese were allowed to react with 6 moles of bread, so how many moles of
grilled cheese sandwiches could you produce?________________ (3 moles)
c) What is the limiting reagent? ________________. (bread)
42. If I began with 11.0 g AgNO3 and 10.0 g Na2SO4, how many grams of Ag2SO4 can I make?
Na2SO4
+
2AgNO3

2NaNO3
+
Ag2SO4
F. Molecular Weight, % Composition, Empirical Formulas
43. Find the molecular weight (molar mass) of each of these compounds.
a. RbOH
b. Na2Cr2O7
c. AlBr3
d. Ba3(PO4)2 e. Fe(NO3)2  4H2O
44. Determine the molecular weight of each of the following. [Round to tenths place (0.1)]
a. Ga(NO3)3
b. Y2(CO3)3
c. CoCl2  6H2O (do not multiply)
45. Determine the % of chlorine in each of these compounds.
a. LiCl
b. HClO4
c. AlBr3
d. Mg(ClO2)2
46. Determine the mass percent (% composition)
a. % C in Al2(CO3)3
b. % O in Na2Cr2O7
47. How many moles are represented in each of these samples?
a. 150. molecules of H2O
b. 200.0 grams of H2O
c. 500. atoms of Cu
d. 500.00 grams of Fe
48. a. How many moles are in 58.6 g of AgNO3?
b) How many formula units is this?
49. Determine the mass in grams of each of the following.
a. 3.00 x 1020 molecules of O2
b. 4.66 moles of O2
c. a single molecule of O2
d. 4.50 x 1021 formula units of KOH
e. 0.00255 moles of KOH
50. Ascorbic acid (vitamin C), C6H8O6, is an essential vitamin. It cannot be stored by the body and therefore
must be present in the diet.
a. What is the molecular weight of ascorbic acid?
b. If you were to take a vitamin C tablet everyday, with 1500. g of ascorbic acid, how many moles would
you ingest?
c. How many molecules of C6H8O6 are you taking?
7
51. Aspartame is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when it dissolves in
water. It is marketed as “Nutra-Sweet”. The molecular formula of aspartame is C14H18N2O5.
a. What is the molecular weight of aspartame?
b. How many molecules of aspartame are present in 15.0 grams of the compound?
c. Calculate the mass of 3.56 moles of aspartame.
d. How many molecules are in 5.900 mg of aspartame?
e. What is the mass in grams of 21.66 x 1015 molecules of aspartame?
f. What is the mass in grams of one molecule of aspartame?
52. A compound contains 22.1% Al, 25.4 % P, and 52.4 % O. What is the empirical formula for this
compound?
53. A particular compound contains 25.93% N and 74.07 % O. What is the empirical formula?
54. An organic compound containing 8.28 g C and 1.72 g H is analyzed. What is the empirical formula? If the
molecular weight is 58.0 g/mol, what is the molecular formula?
55. A compound that contains only carbon, hydrogen, and oxygen is 48.38% C, 8.12 % H, and 43.50 % O.
What is the empirical formula for this compound?
56. The active ingredient in photographic fixer solution contains sodium, sulfur, and oxygen. Analysis of this
sample shows that the sample contains 0.979 g Na, 1.365 g S, and 1.021 g O. What is the empirical formula for
this compound?
57. A compound that contains only nitrogen and oxygen is 30.4% by mass of nitrogen. The molar mass of the
compound is 92 grams/mole. What is the empirical formula? What is the molecular formula?
58. A sample of urea contains 1.1211 g N, 0.161 g H, 0.480 g C, and 0.640 g O. What is the empirical formula
for this compound? If the compound is found to have a molecular weight of 180. g/mol, what is the molecular
formula?
59. A compound containing only sulfur and nitrogen is 69.6% S by mass. It also has a molar mass of 184
g/mol. What are the empirical and molecular formulas?
60. Acrylic acid, used in the manufacture of plastic has a composition of 50.0% C, 5.60% H, and 44.4% O.
The molar mass of the compound is 288 g/mol. What are the empirical and molecular formulas of this
compound?
61. Over the years, the thermite reaction has been used for welding railroad rails, for incendiary (combustible)
bombs, and to ignite solid fuel rocket motors. The reaction is:
Fe2O3 (s)
+
2 Al (s)
 2 Fe (s)
+ Al2O3 (s)
What mass of iron III oxide must be used to produce 515.0 g of iron?
62. The reusable booster rocket of the U.S. space shuttle employs a mixture of aluminum and ammonium
perchlorate for fuel. A possible equation for the reaction is:
3 Al (s) + 3 NH4ClO4 (s)
 Al2O3 (s)
+ AlCl3 (s) + 3 NO (g) + 6 H2O
What mass of aluminum must be used to produce 67 grams of AlCl3?
63. Alka-Seltzer uses the reaction of sodium bicarbonate with citric acid to produce a fizz. The reaction is:
3 NaHCO3 (aq) + C6H8O7 (aq)  3CO2 (g)
+ 3 H2O (l) + Na3C6H5O7 (aq)
What mass of C6H8O7 must be used in the tablet to produce 1.558 g of CO2?
8
64. White phosphorus, P4, burned in excess oxygen forms diphosphorus pentaoxide, P 2O5.
a. Write a balanced equation for the reaction that occurs (remember oxygen is O 2).
b. How many grams of P2O5 are formed if 3.40 g of P4 react?
c. How many grams of oxygen would be consumed using 16.00 g of P 4?
65. When a mixture of silver metal and sulfur is heated, silver sulfide is formed:
16 Ag (s)
+ S8 (s)  8 Ag2S (s)
How many grams of Ag2S are produced if 2.00 g of silver reacts with 2.00 g of sulfur?
66. Aluminum burns in bromine to produce aluminum bromide:
2 Al (s)
+ 3 Br2 (l)

2 AlBr3 (s)
In a certain experiment, 6.00 g of aluminum is burned in 24.0 g of bromine. What is the maximum amount of aluminum bromide
that can be produced?
67. Acid-base neutralization reactions are very common in industrial processes. This is the reaction of sulfuric acid with sodium
hydroxide:
H2SO4 (aq) +
2 NaOH (aq)

Na2SO4 (aq)
+ 2H2O (l)
What is the maximum amount of Na2SO4 that can be produced if you use 26.5 g of H2SO4 and 25.4 g of NaOH?
Some higher thinking problems…
68. Impure nickel can be purified by first forming the compound Ni(CO) 4, which is then decomposed by heating to yield very pure
nickel. The metallic nickel in the sample reacts with carbon monoxide as follows:
Ni (s) + 4 CO (g) 
Ni(CO)4 (s)
The other metals in the ore do not react with carbon monoxide. If 94.2 g of a metal mixture produced 98.4 g of Ni(CO) 4 , what is the
mass percent of nickel in the original sample?
**The following are new problems. ☺ (SEE “Unknown CH/CHO Assistance Sheet”, and Sample Problem at end of packet)
69. Alcohols burn rapidly in oxygen. A chemist is burning an alcohol in an attempt to determine its identity. She knows the
possibilities are: CH3OH, C2H5OH, C3H7OH, C4H9OH, or C5H11OH. In the combustion of 5.00 grams of an alcohol the chemist
produced 11.89 grams of CO2 and 6.09 grams of H2O. What is the identity of the alcohol?
70. Many people take a little ascorbic acid every day to keep from getting sick (remember it’s vitamin C). The compound contains C,
H, and O. During the combustion of 2.00 g of ascorbic acid, 3.09 g CO 2 and 0.818 g H2O are produced. What is the empirical
formula for the compound? What is the molecular formula if the molar mass is found to be 176 g/mol?
71. Menthol, a strong smelling substance used in cough drops is a compound of carbon, hydrogen, and oxygen. When 15.96 grams
menthol was subjected to combustion analysis, it produced 44.9 g CO 2 and 18.4 g H2O. The molecular weight of the compound is 156
g/mol. What is the molecular formula?
72. Hydrocarbons are compounds that contain only H and C. Most of these compounds are used as organic solvents or the building
blocks of larger molecules. 7.00 g of one such hydrocarbon undergoes combustion and produces 23.69 g CO2 and 4.846 g H2O. What
is the empirical formula for this hydrocarbon? What is the molecular formula if the molar mass is found to be 78 g/mol? (Remember
only C and H).
73. The combustion of 10.0 g of a compound containing C, H, and O produced 20.0 g CO2 and 8.18 g H2O. What is the empirical
formula? If the MW = 176 g/mol, what is the molecular formula?
ACT Practice: The new AP Chemistry Exam is organized around six big ideas in chemistry. There is a focus on Inquiry-based
learning. To better prepare yourself for this, it may be helpful to practice ACT passages. Please go to the following site and write your
answers down on the paper. When you are done, check your answers and write down the corrected answer. You may “PRINT
SCREEN” or “SNAPSHOT” and print the page instead. The more practice you get, the better you will perform on these questions.
74. http://www.highschooltestprep.com/act/science/practice-test-3/
75. http://www.actstudent.org/sampletest/science/sci_06.html
Below is a fabulous resource that you may want to set to as a “favorite”. There are many different practice problems for each
chapter that we do.
http://www.sciencegeek.net/APchemistry/APtaters/directory.shtml
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Name____________________________
(DETACH FROM PACKET)
1- Charged Ions
dihydrogen phosphate
H2PO41hydrogen sulfite
HSO31hydrogen sulfate
HSO41bicarbonate
HCO31(hydrogen carbonate)
nitrite
NO21nitrate
NO31hypochlorite
ClO1chlorite
ClO21chlorate
ClO31perchlorate
ClO41cyanide
CN1thiocyanate
SCN1hydroxide
OH11acetate
C2H3O2 / CH3COO1permanganate
MnO41bromate
BrO3azide
N3-
POLYATOMIC IONS TO MEMORIZE
2- Charged Ions
3- Charged Ions
hydrogen phosphate
sulfite
sulfate
carbonate
HPO42SO32SO42CO32-
chromate
dichromate
silicate
oxalate
CrO42Cr2O72SiO32C2O42-
phosphate
phosphite
borate
PO43PO33BO33-
ammonium
NH4+
--------------------------------------------------------CUT HERE---------------------------------------------------------------
Solubility Rules for Common Ionic Compounds in Water
ALL 1A elements, the ALKALI METALS, in compounds are soluble!!!
*1
NO3All nitrates are soluble.
C2H3O2-
*2
All acetates are soluble.
-
*3
All chlorides are soluble. Exceptions: AgCl
PbClX
Hg2Cl2
Br -
*3
All bromides are soluble. Exceptions: AgBr
PbBrX
HgBr2
-
*3
All iodides are soluble.
Exceptions: AgI
PbIX
HgI2
*4
All sulfates are soluble.
Exceptions: Ag2SO4 PbSO4 Hg2SO4 BaSO4 CaSO4 SrSO4
Cl
I
SO4
2-
Hg2Br2
Hg2I2
S2-
All sulfides are insoluble. Soluble: Those of *61A, 2A elements and *5(NH4)2S
CO32-
All carbonates are insoluble. Soluble: Those of *61A elements and *5 (NH4)2CO3
PO43-
All phosphates are insoluble. Soluble: Those of *61A elements and *5 (NH4)3PO4
OH -
All hydroxides are insoluble. Soluble: Those of *61A elements and Ba(OH)2 Ca(OH)2 Sr(OH)2
Some tips on remembering some of these: (You’re on your own for the rest!)
*1: “Knights can take on anything.”
*2: “Aces can take on anything.”
*3: “I ClobBer” can take on anything except silver, lead, and mercury.
*4: Fat Sol or “Solfat” will eat anything except silver, lead, mercury, just BaCause Sir.
*5: Got “Ammo”(ammonium), than you can take on just about anything!
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A Nomenclature Tip Sheet
Diatomics: H2 N2 O2 F2 Cl2 Br2 I2 Use the “Triple 7 Rule” or “H-I O-N F-Cl-Br”
Molecular: The prefixes tell you how many, just write the formula and do not reduce.
Ionic: If there is a metal, you must CRISS-CROSS ABSOLUTE-VALUE & REDUCE. Remember to put
polyatomic ions in parentheses.
Some of the polyatomic ion tips:
1. First of all, notice the bolded borders. These ions have been grouped according to similarities.
2. Compare PO4-3 to HPO4-2 to H2PO41-. Notice that each time you add a H+, the overall charge increases. (that’s what
happens when you add + charges.) This works for others on the list.
3. Choosing –ite versus –ate: “After I –ate, I gained an O”. Notice that the –ate version contains an extra oxygen atom
compared to the –ite.
**Please also note, -ite and –ate do not tell how many O atoms, just whether there are more or less.
4. “Silly Kate rides a tricycle, not a bicycle”. Don’t ask!! Silicate has -O3. Many people incorrectly write SiO4. The
charge is –2.
5. “A COw (or an OX) has 2 eyes and 4 legs.” Again, don’t ask. Oxalate is C2O42- (all evens.)
6. Have some “carbonated” COke in your car(3 letters); it’s better with 2 people: CO327. Night is the 3rd part of the day and there is one moon, so NO31- is nitrate.
8. Chromate: Chrome wheels come in 4’s and then think “24’s” CrO429. Nick the Camel ATE a Clam Supper in Phoenix
**Use number of consonants & vowels
Nitrate
Carbonate
Chlorate Sulfate
Phosphate
to determine
#O
& charge
NO3CO32ClO3- SO42PO43- Example: Nick has 3 consonants and 1 vowel, so NO3- The –ite version is just one less oxygen, with the same charge
I hope some of these help. You are on your own otherwise. ☺
11
(DETACH FROM PACKET)
Predicting Chemical Reactions Notes
The products of a chemical reaction may often be predicted by applying known facts about common reaction types.
While there are hundreds of different kinds of chemical reactions, only 5 general types of reactions will be considered:
Combustion, Single Displacement, Double Displacement, Synthesis, and Decomposition (Analysis).
Balancing Equations and Identifying Reactions
Synthesis / Combination
2> smaller compounds/elements
Decomposition (see below)
1 larger compound
Combustion
any reaction with O2 as a reactant
Single Replacement “Football Substitution”
AB
+
Double Replacement
“Double Dating”
AB
+
 1 larger compound
 >2 smaller compounds / elements
B 
CD 
AC
AD
+
+
B
CB
A COMBUSTION REACTION occurs when an element/compound reacts with oxygen(O2), often producing energy in
the form of heat/light.
Ex: CH4 + 2 O2  CO2 + 2 H2O + heat/light
**Hydrocarbons are compounds made up mainly of carbon and hydrogen (they also may contain oxygen or
nitrogen). When hydrocarbons react with oxygen gas, they from CO2 + H2O
**A rhyme to help you remember: “Reacting O2 with “CH or CHO” always produces “CO and HO”!
A SINGLE DISPLACEMENT REACTION occurs when one element displaces another in a compound. The general
form is: element + compound 
element + compound
A
+ BC

B
+ AC
ex:
Zn
+ 2HCl

H2
+
ZnCl2
We call this: “FOOTBALL SUBSTITUTION”
A DOUBLE DISPLACEMENT REACTION occurs when the cations and anions of the two reactants are interchanged.
The general form is:
compound + compound  compound + compound
AB
+ CD

AD
+
CB
Ex:
FeS
+ 2HCl

FeCl2
+
H2S
We call this: “DOUBLE DATING”
A SYNTHESIS REACTION occurs when two or more elements or compounds are combined to form ONE more
complex substance.
The general form is: element/compound + element/compound  compound
ex:
Fe
+
S
 FeS
A DECOMPOSITION (ANALYSIS) REACTION occurs when energy in the form of heat, light, electricity, or
mechanical shock is supplied. A compound may decompose to form simpler compounds and/or elements.
The general form is: compound  two or more substance. There are six general types:
1. Some oxy-acids, when heated, decompose to form water and the non-metal oxide.
Ex: H2CO3  H2O + CO2
2. Some metallic hydroxides, when heated, decompose to form the metal oxide and water.
Ex: Ca(OH)2  CaO + H2O
3. Some metallic carbonates, when heated, decompose to form the metal oxide and carbon dioxide.
Ex: Li2CO3  Li2O + CO2
4. Some metallic chlorates, when heated, decompose to form the metal chloride and oxygen gas.
Ex: 2KClO3  2KCl + 3O2
5. Most metallic oxides are stable, but a few decompose when heated to form the metal and oxygen gas. Ex:
2HgO  2Hg + O2
6. Some compounds may be decomposed by electricity, called electrolysis, into their elements.
Ex: 2NaCl
 2Na + Cl2
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Unknown CH/CHO Assistance Sheet
Before you begin the problem, analyze that you are solving for an EMPIRICAL and MOLECULAR FOR”MOL”A. So,
you need to find “MOLES” of C, H, and O to get the answer.
1. Write the equation for the combustion reaction. Then, write the values given below each substance.
2.  Find the %C in the CO2 and multiply this constant value (using the decimal form of the percent) by the total
grams of CO2. Underline this value, #g C.
 Change #g C #moles C and underline your answer.
 Repeat this for the H in H2O.
3. Now, you have to deal with the oxygen. The problem is that the O appears in both of the reactants, making it hard
to find exactly how much is only in the {CHO}, not in the O2. But, you know by the Law of Conservation of Mass
how much C and H are in {CHO}, because the amount present in the products must be equal to what is present in the
reactants and each of these only appear in one place on either side. You also were given the amount of {CHO} that
you started with; the C+H+O = {CHO}!
 #grams of {CHO} - #grams C - #grams H = #grams O
 change #grams O  #moles O
4. Write the for”MOL”a. Divide by the lowest number to get whole numbers greater than 1. This whole number,
reduced ratio between the atoms is called the EMPIRICAL for”mol”a.
5. For the molecular for”mol”a, use the “ME” equation to find your “multiplier”:
Molar mass of MOLECULAR FORMULA =
Molar mass of EMPIRICAL FORMULA
Multiply the empirical formula by this value to find the molecular formula. YOU ARE DONE!!
Sample problem: Vanillin (methyl vanillin) is used in flavorings, fragrances, pharmaceuticals, and perfumes is made of
carbon, hydrogen, and oxygen. If 3.00g of the substance is combusted and 6.93 grams of CO2 and 1.42 grams of water are
produced, what is the empirical formula for the substance? The molar mass of the molecular formula is 456 g/mol. Find
the molecular formula.
AP Chemistry *may detach
Name_______________________________
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Equations Guide Part 1
The following are optional ways to solve particular types of problems. Some are simple rules we will follow when
solving problems.
Molecular Weights
Mass %
(a.k.a. % composition or
% by weight)
Empirical Formula or
“forMOLa”
Empirical Formula
-when masses of products
are given (combustion
process)
**NEW
Molecular Formula
-when mass of compound
and Empirical Formula are
given
Grams  Moles
Round atomic weights from the periodic table to the tenth's place.
(units: g/mol)
%X=
grams of element X
total molecular weight of compound
Use the following steps. Start at the point of units that you are given.
a. Change % to grams out of 100 grams
b. Change grams  moles (use periodic table)
c. Write the chemical formula with moles (rounded to .01 place) as subscripts.
d. Divide each mole value by the lowest number to achieve estimated whole
number values.
a. Calculate grams of each element:
#g of product
mole
(MW) #g of element
(MW) #g
mole
of product
b. If the compound given contains oxygen, you need to subtract grams of
each element from the total mass to find how much oxygen there is.
c. Now you know grams of each element. Follow b-d under “Empirical
Formula”.
a. Calculate the total MW of the empirical formula.
b. Divide the given mass of the compound by the MW of the empirical
formula.
c. Multiply the subscripts in the empirical formula by the unit calculated in b).
# grams
mole
(Use P.T to find molecular weight in g/mol)
(MW)# grams
Moles  Grams
# moles
Moles  Molecules
# moles
6.02 x 1023 molecules
mole
Molecules  Moles
# molecules
mole
6.02 x 1023 molecules
Stoichiometry
There are three bridges (ratios) you can use when going from one chemical to
another. They are M L M (not M & M ). These stand for:
Moles
Liters
Molecules
(MW)# grams
mole
(Use P.T to find molecular weight in g/mol)
Example: Find molecules of A when you know grams of B
# grams B
mole
# mol A 6.02 x 1023 molecules
(MW)# grams B
# mol B
mol A
(Note: in bold is the ratio of the formulas from the chemical equation.)
Remember, the only time you can use 22.4 liters = 1 mole is for a gas at STP.
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