Name (IN INK!)____________________________________________ Date ___________ Class ___________
HONORS CHEM 1st SEMESTER EXAM STUDY GUIDE FALL 2010
STRATEGY: Start by reading through your notes to refresh your memory on these topics. Then, use this review sheet as a starting
point to identify the areas on which you need to spend more study time. For those areas, go back to homework assignments, quizzes,
and reviews to practice more problems. I would also recommend going through all of your tests since these questions are only samples
and do not include specific examples of how vocabulary and other conceptual information might appear in a multiple-choice or other
format. Remember you can access notes and reviews on my website.
IMPORTANT INFORMATION:
 This must be handed in BEFORE taking your final exam
 If entirely complete, 5 points will be added to your exam grade
 All work must be shown in DETAIL on lined paper
Introduction to Chemistry – Chapter 1
1. Identify safe/unsafe lab practices.
2. List pieces and uses of lab equipment.
3. List the requirements for tables and graphs.
4. What is plotted on the x-axis and on the y-axis?
5. Make a density graph.
6. What is water displacement?
Matter and Change – Chapter 2
7. Classify the following substances as solid, liquid, gas, or plasma based on their properties.
a. flexible volume, high KE, particles can disperse freely.
b. flexible volume, very high KE, particles are charged.
c. fixed volume, very low KE, orderly particles.
d. fixed volume, low KE, particles can move past each other.
8. Classify the following as element, compound, heterogeneous mixture, or solution.
a. graphite (carbon)
b. grape juice
c. table salt (NaCl)
d. pepper
9. Classify the following as chemical or physical changes.
a. cutting wire
b. ripening tomato
c. apple slices turning brown
d. compressing a gas
10. Classify the following properties as physical or chemical.
a. melts at 68.0C
b. corrosive
c. reacts violently with water
d. decomposes in air
e. magnetic
11. Classify the following properties as intensive or extensive.
a. melting point
b. volume
c. mass
d. reactivity
e. density
VOCAB:kinetic molecular theory
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Scientific Measurement – Chapter 3
12. In a lab, the average measured density for Pre-1982 pennies was 7.98 g/cm3. Given that the
accepted value for the density is 8.92 g/cm3, calculate the percent error.
13. How many sig figs are in the following numbers?
a. 2.35
_______
c. 89.70 _______
b. 34,000 _______
d. 0.0052 _______
14. Convert the following numbers into or out of scientific notation.
a. 548,000
__________________
c. 1.200 × 10-3 __________________
b. 0.0000770 __________________
d. 9.25 × 107
__________________
3
15. Osmium is the densest element with a density of 22.57 g/cm . Find the mass of a 56.2 cm3
sample of osmium.
16. Perform the following SI prefix conversions.
a. 65.2 mm = _____ dm
c. 65,000 mL = _____ L
b. 2.3 kg = _____g
d. 0.502 km = _____ cm
17. Perform the following temperature conversions.
a. 25oC = _____ K
c. 29.8oC = _____ oF
o
b. 398 K = _____ C
d. 75.5oF = _____ K
18. How many milliliters are in a 2.0 quart jug of milk?
19. I will spend next weekend grading lab reports. If each lab report averages 4.12 pages and it takes
me an average of 2.50 min per page, how many hours will it take me to grade all 39 papers?
20. Record the appropriate # of SigFigs when measuring with equipment. (look back at test)
VOCAB: accuracy vs. precision
Periodic Table, Bonding & Chemical Formulas and Names– Chapters 7, 8 & 9
21. What are the names of Groups 1, 2, 17 and 18 on the periodic table?
22. Which of the following is a representative/main group element? Fe, Be, Ce, Re
23. Are the bonds in the following substances IONIC or COVALENT?
a. MgO
c.
LiCl
b. H2O
d.
Br2
24. Are the following properties characteristics of ionic or covalent bonding?
a. These bonds involve a transfer of electrons.
b. Substances containing these bonds do not conduct electricity and have low melting points.
c. Compounds containing these bonds have a crystal lattice structure.
d. These bonds are formed by sharing electrons.
25. Which metalloid is in the 4th period and the same group as phosphorus?
26. Write formulas for the following compounds (HINT: First determine ionic/acid/covalent).
a. hydrosulfuric acid
e.
sulfur trioxide
b. calcium chloride
f.
ammonium dichromate
c. iron(III) nitrate
g.
dinitrogen pentoxide
d. hydrobromic acid
h.
sulfurous acid
27. Write names for the following compounds (HINT: First determine ionic/acid/covalent).
a. CrCl2
e.
CaSO4
b. H3PO3
f.
P5O8
c. As2Cl3
g.
Fe2CO3
d. Na2C2O4
h.
HClO4
VOCAB: octet rule
Chemical Quantities – Chapter 10
28. How many magnesium sulfate molecules are in 25.0 g?
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29. Find the number of moles in 346 g of potassium nitrate.
30. Calculate the number of grams in of 6.12 moles of NaOH.
31. Find the % composition of copper (II) chloride.
32. The percent composition of a compound is 40.91% C, 4.58% H, and 54.51% O. The molar mass
of the compound is 176.12 g/mol. Find its empirical and molecular formulas.
33. Find the percent composition of a sample of amoxicillin which has the formula C16H19N3O5S• 3H2O.
34. List these in order of decreasing hydrogen, by mass: water, methane, glucose, and hydrochloric
acid.
35. How many grams of lead are in a 41.2-gram sample of lead (II) oxide?
36. What is the percent of H2O in magesium sulfate pentahydrate?
VOCAB:
Avogadro’s number
empirical formula percent composition
molecular formula
Chemical Reactions – Chapter 11
37. Write a word equation for the following reaction (incl. how many? of what? what state?).

Ba(ClO3)2(s) 
BaCl2(s) + 3O2(g)
38. Rewrite and balance the following word equation using chemical formulas, physical states, and
energy. – When solid sodium chlorate absorbs energy, it produces solid sodium chloride and
oxygen gas.
39. Balance this equation:
Fe2(SO4)3 + KSCN  K3Fe(SCN)6 + K2SO4
40. Predict the products and balance (48 – 51). Write N.R. if no reaction will occur. Include physical
states. For each of the reactions, specify whether it is combustion, synthesis, decomposition,
single replacement, or double replacement.
41. Cu(s) + MgSO4(aq) 
42. C5H12(l) + O2(g) 
43. NH4Cl(aq) + Pb(NO3)2(aq) 
44. Fe2O3(s) 
VOCAB:
Aqueous
Combustion
Synthesis
Decomposition
Precipitate
Complete ionic equation
Net ionic equation Spectator ion
Stoichiometry – Chapter 12
45. How many grams of copper would be produced from 49.48 g of chromium?
Cr + CuSO4  Cu + Cr2(SO4)3
46. How many grams of chromium are required to react with 125 g CuSO4. (same reaction as above)
47. How many grams of ZnS are required to react with 12.6 g of oxygen gas?
ZnS + O2  ZnO + SO2
48. 6.45 g of lithium reacts with 9.20 g of oxygen gas to produce lithium oxide. How many grams of
Li2O are formed?
49. What are the limiting and excess reactants in #38?
50. The actual yield of the reaction in #39 is 12.5 g. What is the percent yield of this reaction?
51. Dimethlylhydrazine has a molar mass of 60.10g/mol. It is made up of carbon, hydrogen,
nitrogen atoms. The combustion of 2.859g of Dimethyhydrazine in excess oxygen yields
nitrogen, 4.190 g of CO2 and 3.428 g water, what are its empirical and molecular formulas?
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VOCAB:
theoretical yield
percent yield
limiting reactant
excess reactant
Extra Practice with Ionic Names & Formulas and Predicting Products
For the following compounds, give the names:
Name
52. Na2CO3 _______________________________________
53. KCl
_______________________________________
54. FeCl2
_______________________________________
55. FeCl3
_______________________________________
56. Zn(OH)2 _______________________________________
57. Be2SO4 _______________________________________
58. Li3PO4
_______________________________________
59. TiI4
_______________________________________
For the following compounds, give the formulas:
Formula
60. sodium phosphide
____________________________
61. lead (II) sulfite
____________________________
62. gallium nitride
____________________________
63. iron (II) bromide
____________________________
64. vanadium (V) phosphate
____________________________
65. silver bromide
____________________________
66. lead (IV) nitrite
____________________________
Predict the products of the following reactions, if applicable, write complete and net ionic equations:
67. ____ Na + ____ FeBr3 
68. ____ NaOH + ____ H2SO4 
69. ____ Cl2 + ____ Al 
70. ____ Na2SO4 + ____ AgNO3 
71. ____ PBr3 
72. ____ HBr + ____ Fe 
73. ____ K2CO3 + ____ ZnCl2 
74. ____ Na + ____ H2O 
75. ____ Na2SO4 + ____ Ca(OH)2 
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HONORS CHEMISTRY – 1st SEMESTER EXAM REVIEW – FALL 2010
ANSWER KEY
common sense – safe: wear goggles, tie back hair, no horseplay, Bunsen burner safety; unsafe: running, eating, drinking, pouring
down the drain, cleaning spills
2. volume – graduated cylinder, mass – triple-beam balance, all metric measurements
3. make sure they have a title, both axes are labeled, both have correct units; line graph for change over time, bar graph for
comparing counts, pie chart for percentages
4. x-axis = independent variable, y-axis = dependent variable
5. mass versus volume
6. using water to find the volume of irregularly shaped objects
7. a. gas, b. plasma, c. solid , d. liquid
8. a. element, b. solution, c. compound, d. heterogeneous mixture
9. a. physical, b. chemical, c. chemical, d. physical
10. a. physical, b. chemical, c. chemical, d. chemical, e. physical
11. a. intentensive, b. extensive, c. extensive, d. intensive, e. intensive
12. 10.5%
13. a. 3, b. 2, c. 4, d. 2
14. a. 5.48 × 105, b. 7.70 × 10-5, c. 0.001200, d. 92,500,000
15. 1270 g
16. a. 0.652 dm, b. 2,300 kg, c. 65 mL, d. 50,200 cm
17. a. 298K, b. 125oC, c. 85.6oF, d. 297K
18. 1900 mL
19. 6.70 hours
20. look back at your tests!!
21. Group 1 – Alkali Metals, Group – Alkaline Earth Metals, Group 17 – Halogens, Group 18 – Noble Gases
22. Be
32. EF = C3H4O3, MF = C6H8O6
23. a. ionic, b. covalent, c. ionic, d. covalent
33. 45.81% C, 4.57% H, 10.02% N, 19.07% O, 7.64% S,
24. a. ionic, b. covalent, c. ionic, d. covalent
11.00% H2O
25. arsenic
34. CH4, H2O, C6H12O6, HCl
26. a. H2S, b. CaCl2, c. Fe(NO3)3, d. HBr, e. SO3, f.
35. 38.2 g Pb
(NH4)2Cr2O7, g. N2O5, h. H2SO3
36. 42.81% H2O
27. a. chromium(II) chloride, b. phosphorous acid, c.
37. One unit of solid barium chlorate when heated produces
diarsenic trichloride, d. sodium oxalate, e. calcium
one unit of solid barium chloride and three molecules of
sulfate, e. pentaphosphorous octoxide, g. iron (I)
oxygen gas.

carbonate h. perchloric acid.

38. 2NaClO3(s) 
2NaCl(s) + 3O2(g)
28. 1.25 x 1023 molec MgSO4
39.
Fe
2(SO4)3 + 12KSCN  2K3Fe(SCN)6 + 3K2SO4
29. 3.42 mol KNO3
40. single replacement, combustion, double replacement,
30. 245 g NaOH
decomposition
31. 47.27%Cu, 5.73% Cl
_______________
64. V3(PO4)5
41. Cu(s) + MgSO4(aq)  N.R.
65. AgBr
42. C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(g)
66. Pb(NO2)4
43. 2NH4Cl(aq) + Pb(NO3)2(aq)  2NH4NO3(aq) + PbCl2(s)
67. 3 Na + 1 FeBr3  3 NaBr + 1 Fe
44. 2Fe2O3(s)  4Fe(s) + 3O2(g)
68. 2 NaOH + 1 H2SO4  2 H2O (l) + 1 Na2SO4 (aq)
45. 90.71 g Cu
69. 3 Cl2 + 2 Al 2 AlCl3
46. 27.1 g Cr
70. 1 Na2SO4 + 2 AgNO3  2 NaNO3 (aq) + 1 Ag2SO4 (s)
47. 25.6 g ZnS
71. 2 PBr3  2 P (s) + 3 Br2 (l)
48. 13.9 g Li2O
72. 2 HBr + 1 Fe  1 FeBr2 (s) +1 H2 (g)
49. LR: Li, XS: O2
73. K2CO3 + ZnCl2  2 KCl (aq) + ZnCO3 (s)
50. 89.9% yield
74. 2 Na + 2 H2O  2NaOH + H2
51. EF = CH4N, MF = C2H8N2
75. ____ Na2SO4 + ____ Ca(OH)2  CaSO4 + NaOH  NR
52. sodium carbonate
53. potassium chloride
54. iron (II) chloride
55. iron (III) chloride
56. zinc hydroxide
57. beryllium sulfate
58. lithium phosphate
59. titanium (IV) iodide
60. Na3P
61. PbSO3
62. GaN
63. FeBr2
1.
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