NOTE:
1. You will need to complete the problems on the following pages prior to
the 1st day of school. This is the 1st required assignment for the AP/ECE
Chemistry course. Mastery of these problems is critical for your success
in AP/ECE Chemistry. Yes, answers are shown in parentheses for
selected problems. YOU WILL NEED TO SHOW YOUR WORK TO
RECEIVE CREDIT! Use the answers to check yours!
2. Commit to memory the selected ions required for this course. You will
be expected to know these throughout the year. Pay attention to the
hints I gave you on the sheet. It will make your memorizing much
easier.
3. Commit to memory the solubility rules required for this course. You
will be expected to know these throughout the year.
This section is a review of topics and material covered in your Honors Chemistry course.
This is to prepare you for more advance topics in the AP/ECE Chemistry course. Please
complete all work on a separate sheet of paper!
Significant Figures
Nomenclature and Solubility Rules
Dimensional Analysis
Density
Metric Quantities
Nomenclature
Understanding the Atom
The Mole Concept
Chemical Equations

For each equation below, identify the type (synthesis, decomposition, single
replacement, double replacement, or combustion), predict the products, and then
write the balanced reaction.
o Remember to use the solubility rules for double replacement reactions.

You are always given the reactants so write their formulas and try to figure out
the products. For example:
Solutions of silver nitrate and magnesium iodide are combined.
This is a double replacement precipitation reaction.
2AgNO
3(aq)
+ MgI
2(aq)
→2AgI + Mg(NO )
(s)
3 2(aq)
a. Ammonium sulfate reacts with barium nitrate.
b. Zinc metal is added to a solution of copper (II) chloride.
c. Propane gas (C3H8) is burned in excess oxygen.
d. Solid calcium chlorate is heated strongly decomposing into calcium chloride and
oxygen gas.
e. Magnesium and nitrogen gas are heated together.
f. Chlorine gas is bubbled through a solution of sodium bromide.
g. Solutions of lead nitrate and calcium iodide are combined.
h. Sulfuric acid is combined with sodium hydroxide.
i. Isopropyl alcohol (C3H7OH) is burned in oxygen.
j. Iron metal shavings are added to hydrochloric acid.
k. Solid sodium carbonate is heated in a crucible.
l. Sodium metal is added to distilled water.
Stoichiometry
Do the following stoichiometric calculations. For every problem you need to balance the
equation correctly so that you can use the right mole ratios. If you are given amounts of both
reactants, you need to find the limiting reactant. Remember than when gases are involved, there are
22.4 Liters in a mol of any gas at standard temperature and pressure (STP). If the reactions occur in
solution the concentration is used as molarity (M) recall that molarity is the number of moles of
solute in a liter of solution.
a. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon
dioxide gas.
i. Write a balanced chemical equation for this reaction.
ii. How many grams of calcium oxide will be produced after 12.25 g of calcium
carbonate is completely decomposed? (ans: 6.86 g CaO)
iii. What volume of carbon dioxide gas is produced from this amount of calcium
carbonate, at STP? (ans: 2.94 L)
b. Hydrogen gas and bromine gas react to form hydrogen bromide gas.
i. Write a balanced chemical equation for this reaction.
ii. 3.2 g of hydrogen gas and 9.5 g of bromine gas react. Which is the limiting
reagent? (ans: Br )
2
iii.
iv.
v.
How many grams of hydrogen bromide gas can be produced using the
amounts in (b)? (ans: 9.7 g HBr)
How many grams of the excess reactant are left unreacted? (ans: 3.1 g)
What volume of HBr, measured at STP, is produced in (b)? (ans: 2.7 L of
HBr)
c. When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products
are hydrogen cyanide gas and water.
i. Write a balanced chemical equation for this reaction.
ii. Calculate the mass of each product produced when 225 g of oxygen gas is
reacted with an excess of the other two reactants. (ans: 253.8 g H O and
2
iii.
127 g HCN)
If the actual yield of the experiment in (b) is 105 g of HCN, calculate the
percent yield. (ans: 82.7%)
d. When solutions of potassium iodide and lead (II) nitrate are combined, the products
are potassium nitrate and bright yellow lead (II) iodide.
i. Write a balanced equation for this reaction, including (aq) and (s).
ii. Calculate the mass of precipitate produced when 50.0mL of 0.45M
potassium iodide solution and 75mL of 0.55M lead (II) nitrate solution are
mixed. (ans: 5.2 g PbI )
2
iii.
Calculate the volume of 0.50M potassium iodide required to react
completely with 50.0mL of 0.50M lead (II) nitrate (ans: 100 mL)
Electron Configurations
23. Write the electron configurations (full or condensed) for the following elements:
a. Mg
b. Pb
c. Co
d. S
e. Cl
f. Ne
g. O
24. State the number of valence electrons each of the following elements have and draw
an electron dot structure for each:
a. Ni
b. Pb
c. Li
d. S
e. I
Periodic Trends
25. List the following elements in order of decreasing atomic size.
F, H, N, Na, O, Ga, Cs
26. Which element has the greatest electron affinity?
a. O
b. B
c. Li
d. C
e. N
27. Explain some properties of metals and explain how the metallic character of
elements changes across the periodic table.
28. What is ionization energy and how does it change as we view the periodic table?
29. List an element that is a metalloid, its atom has 4 energy levels, its atom has 5
valence electrons and its atomic size is smaller than that of calcium.
Basic pH Properties
30. A solution has a [H+] = 1 x 10-10. Is this solution acidic, basic, or neutral?
31. An aqueous solution of HCl has a molarity of 1.35 x 10-3 M. What is the
concentration of the hydrogen ion, H+ ?
32. If the pOH of a solution is 8, what is the pH?
Laboratory Safety and Equipment
33.
34.
35.
36.
BE SURE TO READ THE TOPIC REVIEW PACKET FIRST BEFORE ANSWERING
THESE QUESTIONS!
A laboratory investigation requires that you use glacial acetic acid. Upon obtaining
the bottle of glacial acetic acid, you see that the acid has crystallized. What should
you do before using it?
During a laboratory investigation, several acids are being used. What two acids are
incompatible and should be kept AP/ECEart. Why?
Explain the difference between an acid that is a strong dehydrating agent and one
that is a strong oxidizing agent?
What is the first aid procedure if an acid is splashed onto your clothing?
37. Elemental carbon can be heated to very high temperatures to combine with oxygen
to form carbon dioxide. List the AP/ECEpropriate pieces of equipment needed to
conduct this reaction in a laboratory setting.
38. A volatile liquid substance requires a slow and even heating during a lab in order to
reduce a sudden increase in temperature. Which flask should be used in this
occasion, the Erlenmeyer or Florence flask? Explain.
39. A solution of 0.30M AgNO3 needs to be prepared using a stock solution of 1.0M
AgNO3. List the pieces of equipment that are required to perform this dilution.
SKIP THE HYDROCARBON NOMENCLATURE SECTION BELOW!
Basic Hydrocarbon Nomenclature
40. How many carbon atoms would a molecule of butane have?
41. Write the chemical formula for decane.
42. Which substance does the following stick diagram represent:
43. What type of compound is represented by the following diagram? Name it!