Summer Chem. Review (AP Chem.)
Name: ___________________________________
Instructions: Due the first day next year. Don’t worry if you have trouble doing some of it! That
just gives us something to talk about on the first day. However, doing this to the best of your
ability will help tremendously because then you will have that much less you need to learn or
review during the year. This will make your life much easier! Therefore, this review must be
attempted to the best of your ability!
Two textbook resources are listed next to the Topic Name.
• The first set of chapters listed are from the Chemistry 1 textbook (Pearson Chemistry).
• The second set of chapters listed are from the Chemistry 2 (AP Chemistry) textbook
(Chemistry: The Central Science, 11th edition; 2009 (Brown, LeMay, etal.)).
Numerical Analysis (Chapter 2 or Chapter 3; Chapter 1)
A. Significant figures and Scientific Notation
1. Underline the significant figures in each of the following measurements.
a. 0.030500 mL
b. 134 000 g
c. 2.305 400 km
2. Write the following numbers in scientific notation.
a. 0.000 6730
_________________________
b. 80 000.0
_________________________
c. 0.000 007 020
_________________________
3. Write the following numbers in ordinary notation.
a. 8.620 x 10-5 _________________________
b. 2.0005 x 103 mg _________________________
4. Perform the following operations. Express each answer in scientific notation with the
correct number of significant figures.
a. 9.250 x 104 mg + 7.246 x 103 mg _________________________
b. 8.610 x 103 m X 7.9304 x 10-2m2 _________________________
c. 4.104 33 x 105 m3 / 7.35 x 10-2 m _________________________
B. Dimensional Analysis
A student made the 23.8 km drive to school in 20.0 minutes. How many miles did the student
drive (1 mile = 1.7 km)? If the speed limit was 55 miles per hour, was the student speeding?
Lab Analysis
1. What is the percent error of a volume measurement of 229 L if the accepted value is 225 L?
2. Comment on the differences between accuracy and precision.
3. What things should you discuss when explaining a source of error in your laboratory
experiment?
4. A student does a lab where he/she reacts different concentrations of HCl together with solid
Mg metal and then measures the pressure changes inside the flask as the reaction proceeds.
Identify the following regarding this experiment:
Independent variable __________________________________________________
Dependent variable __________________________________________________
Relevant controlled variables (make sure to list them all) _________________________
________________________________________________________________________
Chemical Formulas and Chemical Compounds
A. Number of Atoms in a Sample (1 mol = 6.022 x 1023 particles) (Chapter 11 or Chapter 10; Chapter
3)
1. How many atoms of potassium are there in 1.50 moles of potassium?
2. What is the mass in grams of 9.50 x 1012 atoms of carbon?
3. How many hydrogen atoms are there in 2.00 moles of C2H6?
B. Naming and Writing Formulas of Compounds (Chapters 8 & 9; Chapter 3)
1. Write the formulas for the binary ionic compounds formed between the following elements
and name each:
a. sodium and bromine __________________________________________________
b. aluminum and oxygen ________________________________________________
c. calcium and nitrogen _________________________________________________
2. Name the following ionic compounds:
a. CuS __________________________________________________
b. FeCl __________________________________________________
c. CoBr6 __________________________________________________
d. Ba(OH)2 __________________________________________________
e. NH4NO2 __________________________________________________
f.
PbSO4 __________________________________________________
3. Write the formulas for the following ionic compounds:
a. barium chlorate ____________
d. iron (II) chromate ____________
b. lead (II) sulfate ____________
e. sodium chlorite ____________
c. calcium sulfate ____________
f. nickel (II) oxide ____________
4. Name the following binary molecular compounds:
a. SO2 ____________________________________
b. PCl5 ____________________________________
c. N2O3 ____________________________________
5. Write the formulas or name the following acids: (Chapter 19)
a. HI ________________________
c. chloric acid ____________
b. H2SO4 ________________________
d. nitrous acid ____________
C. Using Chemical Formulas (Chapter 11 or Chapter 10; Chapter 3)
1. Determine the molar mass of calcium hydroxide ________________________________
2. What is the mass of 2.50 moles of calcium hydroxide?
3. How many moles of calcium hydroxide are contained in 345 g?
4. Find the percentage composition of calcium hydroxide.
5. Analysis of a 10.150 g sample of a compound known to contain only phosphorus and
oxygen indicates a phosphorus content of 4.433 g. What is the empirical formula
(simplest ratio) for this compound?
6. What is the molecular formula of the molecule that has a simplest ratio of CH2O and a
molar mass of 120.12 g/mol?
7. Analysis of a chemical containing C, H, & O indicates a chemical composition of 65.45%
C and 5.45% H. The molar mass is found to be 110.0 g/mol. Determine the molecular
formula.
Chemical Equations and Reactions (Chapter 10 or Chapter 11)
Complete and then write balanced formula equations for the following reactions. Identify the type of
reaction each represents.
1. sodium sulfide(aq) + zinc bromide(aq) → __________________________________
Type of Reaction: ________________________________________________
2. calcium(s) + copper (II) nitrate(aq) → ______________________________________
Type of Reaction: ________________________________________________
3. chlorine(g) + potassium iodide(aq) → _____________________________________
Type of Reaction: ________________________________________________
4. ethane (C2H6)(g) + oxygen(g) → ____________________________________________
Type of Reaction: ________________________________________________
5. barium(s) + water(steam) → __________________________________________
Type of Reaction: ________________________________________________
Hopefully this assignment has not been too difficult yet. If you’re paying attention, here’s an opportunity for a
bonus assignment. Email me ([email protected]) from your personal email by Thursday,
August 13th with your name and 2 comments/questions from the above questions. Title the email “AP
Chemistry Summer” and make sure you include your first and last name in the email.
Stoichiometry: Limiting Reactant, Theoretical Yield (Chapter 12; Chapter 3)
What is the percent yield of CaO when 212 grams of calcium are mixed with 312 grams of
vanadium (V) oxide according to the following equation and the amount of CaO recovered at the
end of the experiment is 230.0 g
5Ca
+
V 2O 5
→
5CaO
+
2V
a. Determine the limiting reactant and the amount of excess reactant that remains after
the reaction is complete.
b. Calculate the theoretical yield for this reaction.
c. Calculate the percent yield.
Gases (Chapters 13 & 14; Chapter 10)
A. Gas Laws
1. A 55.0 cm3 sample of gas was collected over water at a temperature of 35.0 °C when the
barometric pressure reading was 762.0 mm Hg. What is the volume of the dry gas at STP?
2. Calculate the volume, in liters, occupied by 0.425 mol of NH3 at 37˚C and 0.724 atm.
3. If the density of an unknown gas is 3.20 g/dm3 at 18°C and 2.17 atm, what is the molar mass
of this gas?
4. If 2.0 L of a gas in an expandable piston is heated from 25 to 55°C, what will be the new
volume of the gas in mL?
5. How many L will 22.3 moles of an ideal gas occupy at STP?
6. Sketch the relationship on a graph between pressure and volume and then sketch the
relationship on a graph between volume and temperature.
B. Gas Stoichiometry
1. Consider the following reaction:
C2H2(g) + 2H2(g) → C2H6(g)
If 4.0 L of H2 gas reacts, how many L of C2H6 gas will be produced? Assume this
reaction occurs at constant temperature and pressure conditions.
2. A 3.25 g sample of solid calcium carbide, CaC2, reacted with water to produce acetylene gas,
C2H2, and aqueous calcium hydroxide. If the acetylene was collected at STP, how many mL
of acetylene were produced?
Solutions (Chapter 15 or Chapter 16; Chapter 4)
A. Concentration
1. How many grams of NaOH are dissolved in 500.0 mL of a 0.250 mol L-1 solution?
2. A student wishes to prepare 500 mL of 0.25 M HCl solution for an experiment. The only
HCl available is a stock solution of 3.0 M HCl. How much of the stock solution should
the student use in order to make the desired amount of 0.25 M HCl?
3. In a titration, 25.34 mL of 2.4 x 103 M Ca(OH)2 neutralized 14.62 mL of HCl solution.
What is the molarity of the HCl solution?
4. A 2.1 g sample of a pure compound, with formula M(SO4)2, was dissolved and treated
with an excess of aqueous barium chloride, resulting in the precipitation of all the sulfate
ions as barium sulfate. The precipitate was collected, dried, and found to weigh 4.71 g.
Determine the atomic mass of M, and identify M. (This problem will probably seem a
little difficult. However, try it! First, ask yourself what seems like the first thing you
should do and then do this. Next, ask yourself what seems like the second thing you
should do, and do this, etc.)
The following you will need to review for a quiz that will occur during the first 2 weeks of the
school year.
a. The formulas of polyatomic ions learned in chemistry I
b. The states of elements at room temperature
c. The basic solubility rules that are below (There are more we will review later):
a. Alkali metals and NH4+ are always soluble. (Note: compounds made of these
cations are always soluble regardless of rules b & c.)
b. Anions with -1 charge are soluble except for OH-, AgCl, & PbCl2.
c. Anions with -2 or higher are insoluble except for most sulfates.
Polyatomic ion rules:
1. Memorize these or you will be sorry. I don’t lie; you will be sorry if you don’t because they
count for test points and you will have no one to blame but yourself.
2. Most common ion is given suffix “ate”
a. Ion with one more oxygen than most common is called “per…ate”
b. Ion with one less oxygen than most common is given suffix “ite”
c. Ion with two less oxygen atoms than most common is called “hypo…ite”
Ex: perchlorate = ClO4chlorate = ClO3chlorite = ClO2hypochlorite =ClO3. When an H is added to an ion +1 is added to the charge.
Table of selected polyatomic ions:
Ions with a -1 charge
cyanide: CNthiocyanate: SCN
Ions with a -2
Ions with a -3
charge
charge
Carbonate:
-
CO3
2-
acetate: C2H3O2- or CH3COO-
Hydrogen
nitrate: NO3-
phosphate:
nitrite: NO2-
HPO42-
hydroxide: OH-
Sulfate: SO42-
hydrogen sulfate or bisulfate: HSO4-
Sulfite: SO32-
dihydrogen phosphate: H2PO4-
Chromate: CrO42-
hydrogen carbonate or bicarbonate: HCO3-
Dichromate:
perchlorate: ClO4-
Cr2O72-
chlorate: ClO3-
Peroxide: O22-
chlorite: ClO2-
Oxalate: C2O42-
hypochlorite: ClO-
Silicate: SiO32-
permanganate: MnO4azide: N3-
Phosphite: PO33Phosphate: PO4
3-
Ions with a +1
charge
Ammonium:
NH4+