Hayfield Secondary AP Summer Assignment Cover Sheet
Course
Teacher Names & Email Addresses
Assignment Title
Date Assigned
Date Due
Objective/Purpose of Assignment
Description of how Assignment
will be Assessed
Grade Value of Assignment
Tools/Resources Needed to
Complete Assignment
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Complete Assignment
Sara Hubbart (szhubbart@fcps.edu)
Chemistry 1 Review
May, 2013
2nd class of AP Chemistry
To review important concepts of Chemistry 1 which
are essential to success in AP Chemistry.
Assignment will be assessed based on completion.
Please do not leave any questions blank. Contact
me over the summer if you need help. I will make
every effort to respond to your questions within 1
week.
5% of first quarter grade
Chemistry 1 notes. Internet if needed.
4-5 hours
Name:
Date:
AP Chemistry: Summer Assignment
Section 1: Naming, Formula and Equation Writing
1. Please fill in this grid on naming and formula writing:
Formula
Name
Bonding Type (Ionic, Covalent or Both)
Aluminum Sulfide
P2O5
Manganese (IV) Oxide
Magnesium Phosphate
Ti(SO4)2
Diboron Tetrabromide
K3N
Iron(III) Hydroxide
2. Write balanced molecular equations and identify the type of reaction (decomposition, etc) for
the following reactions:
Silicon Tetrachloride and Magnesium react to form Magnesium Chloride and Silicon
Hydrochloric acid and Ammonia react to form Ammonium Chloride
Methane (CH4) combusts
Aluminum Nitrate and Barium Hydroxide react to form Aluminum Hydroxide and Barium Nitrate
3. Write and balance the following reactions. You must predict the products. Also identify the
type of reaction.
Al + HCl ?
CoCl2 + Na2CO3 ?
C3H8 + O2 ?
Na + N2 
4. Write balanced equations for the following reactions. Use a solubility chart (see last page) to
determine the aqueous species and the precipitate. Then, write a net ionic equation.
A) Potassium Oxide + Iron (III) Chloride 
Molecular:
Net Ionic:
B) Tin (IV) Bromide + Sodium Sulfide ?
Molecular:
Net Ionic:
C) Barium Hydroxide + Potassium Phosphate 
Molecular:
Net Ionic:
5. Adrenaline is 56.79% C, 6.56% H 28.37% O and 8.28% N by mass. What is the empirical formula?
Section 2: Elements and Compounds
6. Write Lewis Structures and identify the shape for the following molecules:
OCl2
NF3
CF4
CO32-
SO3
HCN
7. Write Lewis Structures for the following molecules:
C2H4
C5H12
CH3CH2OH
CH2BrCH2CH2Cl
8. Identify the number of protons, neutrons and electrons in each species
Species
14
C
P358
Fe2+
Protons
Neutrons
Electrons
Section 3: Moles and Stoichiometry
9. Answer the following questions about this reaction: __C2H4 + __O2  __ CO2 + __H2O
A) .495 moles of oxygen produces how many moles of water?
B) 2.25g C2H4 produces how many moles of carbon dioxide?
C) 12.5 moles of O2 produces how many molecules of carbon dioxide?
D) 49g of ethylene (C2H4) produces how many grams of water?
10. Answer the following questions about this reaction: __ Fe2O3 (s) + __ C(s)  __Fe (s) + __ CO (g)
A) If 13.25g C react, how many grams of Fe are produced?
B) If you perform the experiment in 10A and 4.25g Fe form, what is the percent yield?
C) 225g of Fe2O3 react. How many molecules of CO are produced?
D) If .445 moles C and .229 Fe2O3 moles react, what is the limiting reactant?
E) What is the maximum mass of CO that may be produced in 10D?
F) How many moles of excess reactant are consumed in 10D?
G) If 12.45g C and 25.29g Fe2O3 react, what is the limiting reactant?
H) How many grams of Fe may be produced in 10G?
I)
If 44.0g C and 22.0g Fe2O3 react, how many grams of CO may be produced?
J)
How many grams of excess reactant are consumed and left over in 10I?
11. The percentage by mass of calcium carbonate (CaCO3) in eggshell was determined by adding
excess hydrochloric acid (HCl) to ensure that all the calcium carbonate had reacted. The excess
acid left was then reacted with aqueous sodium hydroxide (NaOH).
A) A student added 27.20mL of 0.200M HCl to 0.188 g of eggshell. Calculate the amount, in mol, of
HCl added.
B) The excess acid requires 23.80mL of 0.100M NaOH for neutralization. Calculate the amount, in
mol, of acid that reacts with the NaOH.
C) Using the amount of excess acid in part B and the original amount in part A, determine the
amount, in mol, of HCl that reacted with the calcium carbonate in the eggshell.
D) Write the equation for the reaction of HCl with the calcium carbonate in the eggshell.
E) Determine the amount, in mol, of calcium carbonate in the sample of the eggshell.
F) Calculate the mass and the percentage by mass of calcium carbonate in the eggshell sample.
Section 4: Thermochemistry
12. The specific heat capacity of silver is .24 J/goC
A) Calculate the energy required to raise the temperature of 150.0g Ag from 0oC to 25oC.
B) Calculate the energy required to raise the temperature of 1.25 moles Ag by 2.0oC.
C) What is the mass of a sample of Ag if it takes 1.25kJ of energy to heat it from 12.0oC to 15.2oC?
13. An experiment requires the preparation of a water bath at 37.0oC. The temperature of the cold
tap water is 22.0oC and the temperature of the hot tap water is 55.0oC. If a student starts with
90.0g of cold water, what mass of hot water must be added to reach 37.0oC? Cwater is 4.18 J/goC
14. Consider this reaction: 2H2 + O2  2H2O
∆H = -572kJ
A) What is the energy change if 1.00 moles of H2O are produced?
B) What is the energy change when 4.03g hydrogen reacts in excess oxygen?
C) What is the energy change when 186g oxygen reacts in excess hydrogen?
D) What is the maximum energy change if 25.0g hydrogen reacts with 14.0g oxygen? (Hint: find
the limiting reactant first!)
15. Consider the following reaction: C2H6 + Cl2  CH3CH2Cl + HCl
A) Write Lewis Structures for each molecule.
B) Using the list of bond energies below, calculate ∆H for the reaction.
C-C 347kJ
C-H 413kJ
Cl-Cl 239kJ
H-Cl 427kJ
C-Cl 339kJ
Section 5: Gas Laws and STP
16. What is the pressure of 85.0g argon gas that is held at 45.2oC and 775mL?
17. A sample of gas is held at 1.25atm, .25L and 45.2oC. The volume is changed to .75L and the
temperature to 75.2oC. What is the final pressure?
18. A sample of gas is held at 2.25atm and 1.25L. What is the final volume if the pressure is changed
to 912mmHg? Assume the temperature remains constant.
19. Consider the following reaction at STP: 2SO2(g) + O2(g)  2SO3
A) 25.2g oxygen occupies what volume at STP?
B) 2.95L O2 produces what volume of SO3 at STP?
C) 3.5L SO2 produces what mass of SO3 at STP?
D) What is the maximum volume of SO3 that may be produced if 24.0g SO2 and 25.0g O2 react at
STP?