2011 Chemistry II Summer Assignment
To prepare for Chemistry II, it is important that you have mastered the skills taught in Chemistry I and have
retained them for future use. You will be expected to know and use these skills fluidly throughout the course. This
review packet has been created to ensure your smooth and successful transition from Chemistry I to Chemistry II.
An emphasis should be placed on nomenclature and problem solving skills.
1) Complete both “Tough Balancing Problems” worksheet & “Nomenclature Review” worksheet
independently. You may write directly on the worksheet. Please use a periodic table. You may consult your
textbook for reference after first attempting the problems unassisted. Use pencil or blue or black ink.
2) Complete the following Appendix D problems from the back of your Modern Chemistry textbook:
Mixed Review, Odds: 9-33, 59-75, 79-93, 109-131, 137-149, 153-163, & 177-197 (A total of 66 questions)
3) Thoroughly read and take Cornell notes on Chapter 10 in your Modern Chemistry textbook.
Enjoy your summer- we look forward to seeing you in September! 
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MATES Science Department
Tough Balancing Problems
Balance the following equations and provide the word equation.
1.
CH3CH2OH +
O2 →
2.
NH3 +
O2 →
NO +
H2O
3.
CS2 +
O2 →
CO2 +
SO2
4.
Al +
CH3OH →
5.
C6H12O6 +
O2 →
CO2
+
H2O
(CH3O)3Al +
CO2 +
H2
H2O
For the following: write the formula equation then balance.
6. Silver +
Nitrate
Potassium
Iodide
7. Nitrogen + Water
Dioxide
8. Silicon
Tetrachloride
9. Ammonium
Dichromate
10. Iron (III) +
Oxide
+
→
→
Silver
Iodide
→ Nitric
Acid
Water
Potassium
Nitrate
Nitrogen
Monoxide
→ Silicon +
Dioxide
Nitrogen +
Magnesium
+
+
Chromium
(III) Oxide
Hydrochloric
Acid
+
Water
→ Magnesium + Iron
Oxide
Nomenclature Review
For each formula, classify the compound as Ionic (I) or Molecular (M)/Covalent (C).
________ 1. CuCl2
________ 2. NaCl
________ 3. FeBr3
________ 4. H2O
________ 5. (NH4)3CO3
________ 6. HCl
________ 7. NH4OH
________ 8. CCl4
Write the chemical name for each ionic compound identified above.
9.
10.
11.
12.
13.
Write the name for each molecular compound identified above.
14.
15.
16.
Write the formula for each ionic compound listed below. (Don’t forget Roman Numerals!)
17. iron (II) nitrate
18. aluminum oxide
19. potassium iodide
20. sodium nitrate
21. copper (I) nitrate
22. iron (III) oxide
23. iron (III) hydroxide
24. ammonium sulfate
25. zinc (II) nitrate
26. hydrogen sulfide
27. lead (II) sulfate
28. potassium chlorate
Write the formula for each molecular compound listed below.
29. diphosphorus pentoxide
30. dihydrogen dioxide
31. sulfur dioxide
32. carbon tetrachloride
33. pentacarbon decoxide
34. silicon hexachloride
35. diphosphorus monobromide
36. selenium trioxide
37. tribismuth heptafluoride
38. nonacarbon decahydride
Write the common oxidation number (charge) for each element listed below.
________ 39. sodium
________ 40. potassium
________ 41. aluminum
________ 42.. bromine
________ 43. arsenic
________ 44. copper
________ 45. strontium
________ 46. silicon
________ 47. chlorine
________ 48. argon
________ 49. oxygen
________ 50. magnesium
Fill in the missing information for each compound.
Hints: Be sure to distinguish between ionic or molecular. Don’t forget roman numerals!
Name
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
Compound
Ca(OH)2
hydrogen sulfate
nitrogen trihydride
SO2
Na2O
CCl4
diphosphorus pentoxide
hydrogen chloride
mercury (II) oxide
FeBr3
For each of the following formulas, write true if the formula is correct or if it is false, correct it.
61. NACl
62. AlF3
63. K3PO4
64. CaNO3
65. BaCl2
66. Fli
67. MgSO4
68. Ca2C2H3O2
69. K2Cr2O7
70. MgI
______________
______________
______________
______________
______________
______________
______________
______________
______________
______________