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Name ________________________
Honors Chemistry Final Exam
Tuesday June 16, 2015 at 9:30 am
Room ___________
The exam consists of 100 points and 2 major sections: multiple choice and free response:
 70 points multiple choice @ 1 point each
 30 points free-response problems (3 problems @ 10 points each)
Note the following important points as you prepare for the exam:
 You will be provided a reference booklet, exam, and opscan sheet for m/c
responses.
 You will not be permitted to bring additional reference materials to the test
room.
 You will need to bring YOUR OWN CALCULATOR and pencil.
 You will not be permitted to share or borrow calculators during the exam
period.
The attached review packet is meant to assist you in preparing for your exam. The
review packet is intended to be a supplement to your notes, lab reports and class work
completed during the 2nd semester .
The following is a list of the possible problem/question topics in both the multiple
choice and free-response sections:
-Summation Equation calculations for free
energy, enthalpy & entropy
-Hess’s Law
-Specific Heat calculations
-Phase change problems
-Temperature change problems
-Basic gas law problems: Charles’s, Boyle’s,
Graham’s, etc
-Ideal gas law with stoichiometry
-Molarity, molality, and dilution of solutions
-Boiling point elevation/freezing point
depression
-Determining rate law from rate data & the
value of k
- Free Energy Calculations
-Prediction of shift based on Le Chatelier’s
principle
-Reading solubility curves
-Reading vapor phase curves
-Reading heating/cooling curves
-Reading potential energy diagrams
-Molecular shape, polarity, bond angle and
hybridization type determinations
-Periodic Properties
-Bonding systems and their general properties
-Electron configurations and light
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Unit 5: Thermodynamics – Entropy and Free Energy
1. Distinguish between an exothermic and an endothermic reaction in the following:
a) Sign of ΔH
b) Comparative enthalpies of the reactants and products
c) Direction of heat flow between system and surroundings
2. If it takes 258 J of heat to raise the temperature of 4.50 g of substance X from 24.0oC
to 26.9oC, what is the specific heat of substance X?
3. Given the equation:
Ca3N2 (s) + 6H2O (l)  3 Ca(OH)2 (s) + 2NH3 (g); ΔH = -905 kJ
How much heat is produced if 2.85 g of Ca3N2 reacts with an excess of water?
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4. Use the heats of formation in your reference booklet to calculate ΔH for the following
equation:
2HCl (aq) + Ca(OH)2 (s)  CaCl2 (s) + 2 H2O (l)
5. Determine the enthalpy of formation of Ca(OH)2 (s) by using Hess’s Law and the
following data: Ca(s) + O2(g) + H2(g)  Ca(OH)2(s) ΔH = ?
H2 (g) + ½ O2 (g)

H2O (l)
ΔH = -285.8 kJ
Ca (s) + ½ O2 (g)

CaO (s)
ΔH = -635.5 kJ
Ca(OH)2 (s)

CaO (s) + H2O (l)
ΔH = 65.3 kJ
6. Determine which of the following results in increased entropy:
a) Taking random chess pieces and setting up the board to begin the game.
b) Taking a jigsaw puzzle apart.
c) Humpty Dumpty being put together again.
d) Boiling water on a stove.
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7. For the following reaction, ΔHo is -74.8 kJ and ΔSo is -80.7 J/K.
C (s)
+ 2H2 (g)

CH4 (g)
Calculate ΔGo at 25oC. Is this reaction spontaneous at this temperature?
Unit 6: Electron Configuration and Light
8. Show the three light equations discussed in class. State the relationship between
frequency, wavelength and the speed of light.
9. Determine the number of:
a) electrons occupying the p orbitals in the arsenic atom?
b) orbitals in the third energy level?
c) d orbitals in a d sublevel?
d) valence electrons in an atom of sulfur?
10. Define the term isoelectronic.
11. What ion with a charge of -2 is isoelectronic with an argon atom?
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12. Write both the complete and the abbreviated (noble gas) electron configuration of:
a) an aluminum atom
b) a sulfide ion
c) an atom of uranium
13. Draw an orbital diagram (orbital configuration or notation) of the following. DO
NOT use abbreviated (short-hand) notation.
a) a phosphorus atom
b) a strontium ion
14. Distinguish between ground and excited state for an atom.
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15. The laser in a CD player uses light with a wavelength of 780 nm. Calculate the
energy of this radiation, in joules per photon.
Periodic Properties & Trends
16. Fill in the periodic table below with the locations of :
actinides
alkaline earth metals
lanthanides
metals
halogens
alkali metals
nonmetals
transition metals
metalloids
noble gases
17. Rank the following elements from smallest to largest atomic radius:
Rb I Te Sr
-----------------------------------------------------------------------------------------------------------18. Rank the elements from lowest to highest ionization energy:
Be Ba Ca
Sr Mg
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Unit 7 – Molecular Geometry
Fill in the following table.
Lewis Structure
Molecular Geometry
(Name, Shape, & Bond
Angles)
19. CO2
20. BF3
21. CHCl3
22. BeF2
23. XeF4
(bond angles not needed
here)
24. [H3O]+
25. NO2-
Polar or
nonpolar?
Hybridization
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Unit 8 – Gas Laws
26. What is the volume of 4.50 g of N2 at STP?
27. Put the following gases in order from fastest to slowest rate of diffusion or molecular
velocity: SO2, He, N2, O2
28. Put the same four gases in order of smallest to largest density if all are measured at
the same T and P.
29. Put the same gases in order of smallest to largest volume of 1 mole of each gas at
STP.
30. If a sample of H2 occupies 2.50 L at a pressure of 500. mmHg, what volume will the
same sample occupy at 1.40 atm if there is no change in temperature?
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Unit 9 – Liquids, Solids, & IMF
31. Name the dominant type of intermolecular or intramolecular force in each of the
following substances:
a. BH3
b. CBr4
c. CH3OH
d. PCl3
e. NaCl
f. SiO2
g. Mg
h. HF
32. Discuss the differences between different types of intermolecular forces in terms of:
a. strength of forces
b. boiling point and melting point
33. Complete the following table regarding properties of compounds:
Metallic
Description of
bonding system
Conductivity
Solubility in water
Hardness
Malleability
Ductility
Molecular (Network
Covalent)
Ionic
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34. Use the chart below to answer questions a – c.
a) At what temperature does CCl4 have a
vapor pressure of 60kPa?_________
b) What temperature is the normal boiling
point of CCl4?_____________
c) At what pressure does CHCl3 have a
boiling point of 30OC?___________
35. Calculate the amount of energy required to raise the temperature of 5.00 grams of ice
at -4.0° C to steam at 110° C.
cice = 2.09 J/g °C
cwater = 4.184 J/g °C
csteam = 1.84 J/g °C
ΔHfus = 6.01 kJ/mol
ΔHvap = 40.67 kJ/mol
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36. Sketch a heating curve for water and label all phases and energy changes.
Unit 10 – Solutions
37. What mass of Al(NO3)3 is needed to make 250. mL of a 0.500 M solution?
38. What would be the concentration of the nitrate ions in the solution from problem
#37 above?
39. If 350. mL of 4.50 M KNO3 is diluted to a total volume of 1750 mL, what is the
molarity of the resulting solution?
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40. Which will boil at the highest temperature: pure water, 1.0m sugar water, or 1.0m
NaCl?
41. What is a colligative property? List examples.
For the next two questions, use the solubility curve on p.12 of your reference booklet:
42. Is a solution of 10 g of KClO3 in 50 g of water at 20°C saturated, unsaturated, or
supersaturated?
43. What is the mass percent of a saturated solution of KNO3 at 50°C?
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Unit 11 – Chemical Kinetics & Equilibrium
44. Consider the following data for the reaction: 2 A + 3 B  4 C
[A], mol/L
0.100
0.300
0.300
[B], mol/L
0.300
0.300
0.600
rate (mol/L*sec)
2.50 x 10-3
2.25 x10-2
2.25 x 10-2
a) What is the rate expression/law and the value of k for the above reaction?
b) What would the rate be if [A] = 0.800 M and [B] = 1.00 M?
45. Define the following:
a) Intermediate:
b) Catalyst:
c) Rate determining step:
d) Reaction mechanism:
e) Activation energy:
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46. Use the potential energy diagram below to answer the following questions:
120 kJ
Z
100 kJ
40 kJ
X + Y
a) potential energy of the reactants is ____________
b) potential energy of the products is _____________
c) activation energy (forward reaction) is _________________
d) potential energy of the activated complex is ______________
e) heat of reaction (∆H) of the forward reaction is ______________
f) Is the forward reaction exo- or endothermic?
Equilibrium
47. In what direction would the system shift if the following stresses were applied to
the following system at equilibrium?
Mg (s) + 2 HCl (aq)  MgCl2 (aq) + H2 (g)
a) Increase temperature
b) Add Mg
c) Remove H2
d) Add a catalyst
e) Decrease the volume of the container
f) Decrease the pressure
ΔH = -250 kJ