WELCOME TO AP CHEMISTRY!
Mrs. Tolentino
Summer Assignment 2017
This course is designed to give you the equivalent of a general chemistry course that is typically
taken during the first year of college. The text, Chemistry by Zumdahl contains 22 chapters,
seven of which were topics already covered in Chemistry R.
Due Date
This assignment is due in full on Wednesday, September 6, 2017.
Ten points per day will be deducted for late assignments.
Grading
This assignment will be equivalent to one major test. Woodbridge Board of Education Policy states that marking
period grades for Advanced Placement courses are determined using the following formulas:
 75% Major Assessments
Tests, Major Laboratory Reports, Summer Assignment
 25% Minor Assessments
Quizzes, Weekly Participation grade/minor labs
Assignment
The assignment is divided into four parts:
I. Writing Names and Formulas
Memorize the names, symbols, and charges of the ions by making flashcards (or other
memorization learning devices). You should be able to name and write formulas of ionic
compounds, covalent compounds and acids.
II. Stoichiometry/Problems and Short Answer Questions
Read Chapters 1 to 4 of the textbook. These problems were taken from the End-of-Chapter
section of the textbook. Check out the answers to the odd-numbered problems at the back. The
Solubility Rules (page 144 Zumdahl) and the list of strong acids and bases (page 131 Zumdahl)
should be memorized.
III. Chemical Equations and Predicting Products
Predict the products and balance the equations. For each type of reaction, use as your guide the
examples given.
IV. AP Insight Performance Tasks: Geometry, Nonpolar, Dipole Forces, and IMF's
(Get from me the Part IV Hard copy together with your books by June 19. Copyright laws
prevent me from posting these online.)
Suggestions:
 Complete this assignment as soon as possible! Complete Parts 1 and 2 by end of July and submit
scanned answers and solutions/work via email or google classroom.
 You may email me for any concerns or questions at [email protected]
 Join and check google classroom periodically Class Code: g8wnof
 Looking forward to seeing you in September!
Part I. Writing Names and Formulas
Write the chemical formula for the following:
1. sodium sulfate
____________________
2. manganese dioxide
____________________
3. potassium carbonate
____________________
4.
____________________
calcium phosphate
5. ammonium chloride
____________________
6. sodium hydroxide
____________________
7. iron (III) chloride
____________________
8. dinitrogen monoxide
____________________
9. lead (II) sulfide
____________________
10. potassium chlorate
____________________
11. hydrochloric acid
____________________
12. nitric acid
____________________
13. sulfuric acid
____________________
14. perchloric acid
____________________
15. potassium dichromate
____________________
16. potassium permanganate ____________________
17. carbon tetrachloride
____________________
18. acetic acid
____________________
19. zinc nitrate
____________________
20. chromium(II) oxide
____________________
Write the chemical name for the following
1. NaHCO3
____________________
2. PCl3
____________________
3. BaSO4
____________________
4. AgCl
____________________
5. H2S
____________________
6. CuCl
____________________
7. Li3N
____________________
8. Na2SO3
____________________
9. HF
____________________
10. NaCN
____________________
11. NaH
____________________
12. P4O10
____________________
13. KOH
____________________
14. NH3
____________________
15. CaCO3
____________________
16. SnCl4
____________________
17. Fe2O3
____________________
18. H2CO3
____________________
19. H3PO4
____________________
20. (NH4)2SO4
____________________
Part II. Stoichiometry / Conversions / Problems
Solve the following problems. Encircle your final answer. All solutions should be shown.
The AP College Board gives partial points for correct solutions.
Cham R Chapter 3 Measurements and Dimensional Analysis
1. Gasoline has a density of 0.73 g/cm3. How many liters of gasoline would be required to
increase the mass of an automobile from 1271 kg to 1305 kg?
(Note: 1 cm3 = 1 mL )
2. Pure gold can be made into extremely thin sheets called gold leaf. Suppose that 50 kg of
gold is made into gold leaf having an area of 3620 m2. The density of gold is 19.3 g/cm3.
a) How thick in micrometers is the gold leaf? (106 micrometers = 1 meter)
b) A gold atom has a radius of 1.44 x 10-10 m. How many atoms thick is the gold leaf?
3. Precious metals are commonly measured in troy ounces. A troy ounce is equivalent to 31.1
g. How many moles are in a troy ounce of silver?
Chem R Chapter 12 Stoichiometry / Mole Ratios
4. A combustion reaction involves the reaction of a substance with oxygen gas. The complete
combustion of any hydrocarbon (binary compound of carbon and hydrogen) produces
carbon dioxide and water as the only products. Octane is a hydrocarbon that is found in
gasoline. Complete combustion of octane produces 8 moles of carbon dioxide for every 9
moles of water vapor. What is the molecular formula of octane?
Chem R Chapter 4 Atomic Structure
5. The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 amu and
153
Eu has a mass of 152.9209 amu. The average atomic mass of europium is 151.96 amu.
Calculate the relative abundance of the two europium isotopes.
Chem R Chapter 10 Chemical Quantities
6. Ascorbic acid, or vitamin C (C6H8O6), is an essential vitamin. It cannot be stored by the body
and must be present in the diet.
a) What is the molar mass of ascorbic acid?
b) Vitamin C tablets are taken as a dietary supplement. If a typical tablet contains 0.500 g
(equivalent to 500 milligrams) of vitamin C, how many moles of vitamin C does it
contain?
c) how many molecules of vitamin C does it contain?
7.A compound contains only C, H, and N. Combustion of 35.0 mg of the compound produces
33.5 mg CO2 and 41.1 mg H2O. What is the empirical formula of the compound?
8. The compound cisplatin, Pt(NH3)2Cl2, has been studied extensively as an antitumor agent.
Calculate the elemental percent composition by mass of cisplatin.
%Pt
%N
%H
%Cl
9. The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol.
What is the molecular formula of styrene?
How many H atoms are present in a 2.00g sample of styrene?
Chem R Chapter 16 Solutions pages 525-527
10. Calculate the molarity of a solution prepared by dissolving a 5.623g sample of NaHCO 3 in
enough water to make 250mL.
III. Chemical Equations and Predicting Products
Predict the products and balance the equations. ALL reactions will occur.
Make sure to write the correct formulas for the reactants and products.
Synthesis/Combination
A metal combines with a nonmetal to form a binary salt
Example: A piece of lithium metal is dropped into a container of nitrogen gas.
6Li + N2 → 2Li3N
Metallic oxides and water form bases (metallic hydroxides)
Example: Solid sodium oxide is added to water
Na2O + HOH → 2NaOH
Nonmetallic oxides and water form acids
Example: Carbon dioxide is bubbled into water
CO2 + H2O → H2CO3
Metallic oxides and nonmetallic oxides form salts
Example: Solid sodium oxide is added to carbon dioxide
Na2O + CO2 →Na2CO3
1. A strip of aluminum foil is placed in liquid bromine.
2. Magnesium metal is burned in nitrogen gas.
3. Solid magnesium oxide is added to water.
4. Powdered magnesium oxide is added to a container of carbon dioxide gas.
5. Sulfur trioxide gas is added to excess water.
6. Calcium metal heated in nitrogen gas.
7. Excess chlorine gas is passed over hot iron filings.
Decomposition
A binary compound may break down to produce two elements usually through the
of electrolysis
Example: 2NaCl → 2Na + Cl2
process
metallic carbonates metallic oxides + carbon dioxide
Example: A sample of magnesium carbonate is heated
MgCO3 → MgO + CO2
metallic chlorates metallic chlorides + oxygen gas
Example: A sample of magnesium chlorate is heated
Mg(ClO3)2 → MgCl2 + 3O2
hydrates → compound and water
1. A solution of hydrogen peroxide is decomposed catalytically.
Identify the oxidation state of oxygen in hydrogen peroxide.
2. Molten aluminum chloride is electrolyzed
3. Solid mercury(II) oxide decomposes as it is heated in an open test tube in a fume hood.
After the reaction is complete, is the mass of the material in the test tube greater than, less than,
or equal to the mass of the original sample? Explain.
4. Solid potassium chlorate is heated in the presence of manganese dioxide catalyst
5. A solution of hydrogen peroxide is heated.
6. Solid calcium carbonate is strongly heated.
7. Solid copper(II) sulfate pentahydrate, CuSO4·5H2O is gently heated.
How many grams of water are present in 1.00 mol of copper(II) sulfate pentahydrate?
8. Electrolysis of water
Single Displacement
Active metals replace less reactive metals from their compounds in aqueous solution
Example: Magnesium turnings are added to a solution of iron(III) chloride.
3Mg + 2FeCl3 → 2Fe + 3MgCl2
Active metals replace hydrogen in water
Example: A pea-sized lithium is added to water
2Li + 2HOH → H2 + 2LiOH
Active metals replace hydrogen in acids
Example: Lithium is added to hydrochloric acid
2Li + 2HCl → H2 + 2LiCl
Active nonmetals replace less active nonmetals from their compounds in aqueous solution
Example: Chlorine gas is bubbled into a solution of potassium iodide
Cl2 + 2KI → I2 + 2KCl
1. Calcium metal is added to a dilute solution of hydrochloric acid.
2. Liquid bromine is added to a solution of potassium iodide.
3. Pellets of lead are dropped into hot sulfuric acid.
4. Chlorine gas is bubbled into a solution of sodium bromide.
What is the oxidation number of chlorine before the reaction occurs?
What is the oxidation number of chlorine after the reaction occurs?
5. Solid zinc strips are added to a solution of copper sulfate.
6. Lead foil is immersed in silver nitrate solution.
7. Hydrogen gas is passed over hot iron(III) oxide
8. Aluminum metal is added to a solution of copper(II) chloride.
9. Small chunks of solid sodium are added to water.
The reaction is exothermic, and sometimes small flames are observed as the sodium reacts with
the water. Identify the product of the reaction that burns to produce the flames.
10. Chlorine gas is bubbled into a solution of potassium iodide.
11. A strip of magnesium is added to a solution of silver nitrate.
12. A piece of cadmium metal is added to a solution of copper(II) chloride.
List two visible changes that would occur in the reaction container as the reaction is proceeding.
13. A copper wire is dipped into a solution of silver(I) nitrate.
Describe what is observed as the reaction proceeds.
14. Sulfuric acid is added to mossy zinc.
The gas generated by this reaction was tested using a glowing splint (a wooden stick with one
end that has been ignited ). Describe the result.
Double Displacement
1. Dilute sulfuric acid is added to a solution of barium acetate.
2. Ammonium chloride crystals are added to a solution of sodium hydroxide.
3. Hydrogen sulfide gas is bubbled through a solution of lead(II) nitrate.
4. Solutions of silver nitrate and sodium chromate are mixed
If the contents of the reaction mixture described above are filtered, what substance(s), if any,
would remain on the filter paper?
5. A barium nitrate solution and a potassium fluoride solution are combined and a precipitate
forms.
If equal number of moles (equimolar) of barium nitrate and potassium fluoride are combined,
which reactant, if any, is the limiting reactant? Explain.
6. A solution of ammonium sulfate is added to a saturated solution of barium hydroxide.
7. Excess nitric acid is added to solid calcium carbonate.
Briefly explain why statues made of marble (calcium carbonate) displayed outdoors in urban
areas are deteriorating.
8. Solid potassium oxide is added to water.
If a few drops of phenolphthalein indicator are added to the resulting solution, what would be
observed? Explain.
9. A piece of solid strontium carbonate is dropped into a solution of hydrochloric acid
Indicate one thing that would be observed as the reaction occurs.
Combustion
Compounds containing carbon and hydrogen (and oxygen) burn in oxygen to produce carbon
dioxide and water. If sulfur is present, SO2 is formed.
1. Ethanol (CH3CH2OH) is completely burned in the air.
2. Lithium metal is burned in air.
3. The hydrocarbon hexane (C6H14) is burned in excess oxygen.
4. Magnesium metal is strongly heated in oxygen gas.
What is the oxidation number of magnesium before the reaction occurs, and what is the oxidation number
of magnesium after the reaction is complete?