Spring 2017 Review
Name __________________________
You have made it!!! We have covered a lot of material this
year, and your understanding of chemistry has grown. Be sure
to review each section. Use resource such as notes, quizzes,
labs, the textbook and ask questions along the way!
Unit 1: Matter, Change and the Atom
1. Fill in each blank in the table below.
Symbol of
Name
Mass
atom or ion
number
Mg2+
Br181
gold(III) ion
lead
190
206
“Tomorrow’s victory is today’s practice.”
― Chris Bradford, The Way of the Warrior
Number of
protons
Number of
electrons
Number of
neutrons
14
82
82
76
82
122
124
2. Are there any isotopes in the chart above? If so, which ones? ____________________________
3. What is the general name for ions that have a negative charge? ______________ A positive charge? _____
4. List three physical properties of mercury at room temperature.
________________________________________________________________________________
5.
Identify each of the following as either a chemical change or a physical change:
a. leaves produce oxygen _________________
b. oil and vinegar separate _________________
c. compost pit turns into mulch _________________
d. a pencil is sharpened ___________________
6. Define the following terms:
a. mass: ____________________________________________________________________
b. volume: __________________________________________________________________
c. pressure: _________________________________________________________________
d. temperature: _____________________________________________________________
e. density: __________________________________________________________________
Unit 2: The Periodic Table
7. List 5 characteristics of metals.
8. Metals tend to gain/lose (circle one) electrons to form an ion whereas nonmetals tend to gain/lose (circle one)
electrons to form an ion.
9. List the formulas for the diatomic elements: ____ ____ ____ ____ ____ ____ ____
10. What is the electron configuration for a selenium atom? _______________________________
How many unpaired electrons does a selenium atom have? ________
11. What is the electron configuration for a phosphide ion? ________________________________
How many unpaired electrons does a phosphide ion have? ________
12. Label the different groups on the periodic table (alkali metals, alkaline earth metals, transition metals, inner transition
metals, halogens, noble gases.) Also, be able to identify the s-block, p-block, d-block, and f-block.
Unit 3: Bonding
13. Give the charge on the ions from group I, II, V, VI, VII, and VIII.
14. Classify each of the following as ionic or covalent, then name the following compounds.
a. K2O
b. N2O4
c. (NH4)2SO4
d. Hg(NO3)2
e. SO3
15. Classify each of the following as ionic or covalent, then write the formulas for the compounds
a. Sulfur hexafluoride
b. Calcium fluoride
c. Magnesium sulfide
d. Carbon tetrachloride
e. Copper (II) hydroxide
f. Iron (III) oxide
16. Draw Lewis Dot diagrams for the following
a. CH4
b. CO2
The four following compounds do not exist. Explain why not.
17. FeCl _____________________________________________
18. CuCl3_____________________________________________
19. CaXe_____________________________________________
20. NH4O _____________________________________________
21. What is the ionic charge for chemistryrocksium, Ch, in the compound Ch2S3? ______
22. Compare and contrast physical properties of ionic and covalent compounds.
Unit 4: Chemical Reactions
23. List the 5 types of reactions we covered in class.
24. Balance the following equations:
___ Al + ___ Fe2O3 à ___ Fe + ___ Al2O3
___ F2 + ___ H2O à ___ HF + ___ O2
c. NH3
___ C2H4O2 + ___ O2 à ___ CO2 + ___H2O
___ PbO + ___ NH3 à ___ Pb + ___ N2 + ___H2O
25. Write the balanced chemical equation for the following: When hydrochloric acid (HCl) reacts with sodium hydroxide
it is neutralized to form water and salt.
26. Solid lithium metal is dropped into water. Hydrogen gas and aqueous lithium hydroxide are produced. Write the
complete balanced equation.
27. Write and balance the complete chemical equation for the reaction between sodium carbonate and magnesium
chloride reacting when heated.
Which of the five types of reactions is this? ____________________________
How should the mass of the reactants compare to the mass of the products after the reaction is complete?
_________________
28. What is the percent composition of PbCrO4? _______ Show your work below.
Unit 5: Math Tools
29. A student lab group conducted three trials to experimentally determine the molar volume of a gas at STP. Their results
are as follows: Trial 1: 42.8 L/mol, Trial 2: 43.0 L/mol, and Trial 3: 42.9 L/mol. What does this mean in terms of
good/poor precision AND accuracy? Explain.
______________________________________________________________________________________________
______________________________________________________________________________________________
______________________________________________________________________________________________
30. Using the example in the problem above. Use the average of their three trials to calculate this lab group’s percent
error. Show your work below.
31. How many seconds old is your 73 year old grandma? (Use dimensional analysis to solve)
Unit 6: The Mole
Name
32.
33.
34.
35.
36.
37.
38.
39.
Compound formula
CO
K4Fe(CN)6
CCl4
Al2(SO4)3
V 2O 5
Au(C2H3O2)3
PbCrO4
CO2
Molar mass (g/mole)
40. (honors) What is the empirical formula of a compound that is 40.7% carbon, 54.2% oxygen, and the rest hydrogen?
41. (honors) If the molar mass of the compound in #40 above is 177.0 g/mol, what is the molecular formula?
42. Show all work using dimensional analysis. All numbers need a label. Mind your sig figs.
a. How many molecules of oxygen are in 0.567 moles of oxygen gas? _______________________
b. How many atoms are in 54.7 grams of chlorine gas? _______________________
c. How many moles are in 4.45 L of nitrogen monoxide gas at STP? ______________________
d. How many atoms are in a 33.66 g sample of copper metal? _____________________
For the following questions use the balanced equation below. Show all work using dimensional analysis. All numbers
need a label. Mind your sig figs.
CH4 (g) + 2 O2 (g) à CO2 (g) + 2 H2O (g)
43. Of the five reaction types we learned, which type is this? ________________________________
44. If one mole of methane (CH4) is burned, how many moles of O2 are consumed? _________
45. If 20.0 grams of CH4 is burned, how many molecules of CO2 are produced? _______
46. How many moles of methane (CH4) would be needed to produce 0.81 moles of water? _________
47. honors: If you are given 45.0 g of oxygen and 38.0 g of methane, what is your limiting reactant? __________
48. honors: Given the quantities of reactants in #46, how many grams of H2O could you produce? ____________
49. honors: Given the quantities above, how many liters of carbon dioxide could be produced at STP? ____________
Unit 7: Phases of matter and Gas Laws
The following questions deal with gases. Fill in the blanks with the words “increase” or “decrease” (or up or down
arrows) and the words “inversely” or “directly.” Also, put the scientist’s name that is credited with each relationship.
50. If pressure increases, then the volume will __________, so these variables are ___________ proportional. This is
known as ______________ Law.
51. If pressure increases, then the temperature will __________, so these variables are ___________ proportional. This is
known as ______________ Law.
52. If volume increases, then the temperature will _____, so these variables are ___________ proportional. This is known
as ______________ Law.
53. To convert a temperature in degrees Celsius to a Kelvin temperature, one must add _______ to the Celsius
temperature.
54. 23 degrees Celsius is how many Kelvin? _______
55. 333 K is how many degrees Celsius? _______
56. If a balloon at 23 degrees Celsius drops to a temperature of 0 degrees Celsius, will the volume go up or down?
57. If a balloon at 1 atm doubles in pressure, will the volume go up or will it go down? _______
58. If a balloon with a volume of 1 L at 33 oC and 1 atm changes to 0 oC and 2 atm, what will the new volume be?
_______ Show your work below.
59. If a balloon with a volume of 3.3 L at 45 oC has its temperature decreased to -45 oC, what will be the new volume?
________ Show your work below.
60. A balloon at a pressure of 718 mm Hg occupies a volume of 12.3 L. What volume will this balloon occupy at 659 mm
Hg? ________ Show your work below.
61. What volume exists if you have 2.87 moles of helium gas at a temperature of 347 K and a pressure of 792 mm Hg?
(Hint: Watch your units!) ___________
62. A sample of propane gas at a temperature of 23 oC is at a pressure of 1.4 atm. What Celsius temperature must this
sample be changed to if the pressure is decreased to 0.6 atm? Show your work below. __________
63. What is climate change? Describe the impact of human activity on climate change.
Unit 8: Solutions and Acids and Bases
64. In a solution, the _________________ is the substance that is being dissolved, whereas the _________________ is
the substance doing the dissolving.
65. What is the molarity of a copper(II) sulfate solution where 87.20 grams is dissolved in water and diluted to a final
volume of 500. mL? Show all work.
66. How many grams of FeCl3 would be needed to produce 500. mL of a 3.3 M solution?
67. If you took 33 mL from the stock solution in the problem above and diluted it to a final volume of 250 mL, what
would be the new molarity?
68. Define acids and bases in terms of hydrogen ion transfer (Bronsted-Lowry definition)
Acids _________________ the hydrogen ion. Bases _______________ the hydrogen ion.
69. (honors) Given the balanced equation, label the conjugate acid/base pairs.
a. HCl + NaOH à H2O + NaCl
b. NH3 + CH3COOH à NH4+ + CH3COO70. Label approximately where you would find the following household items on the pH scale below: Detergent, Lemon
Juice, Ammonia, Baking Soda, Soft Drink, Vinegar, Drain Cleaner
pH 0 ---------------------------------------------------- 7 ---------------------------------------------------------14
71. Determine the pH and the pOH of:
a. A 4.5 x 10 -3 M HBr solution. Is the solution acidic, basic or neutral?
b. A solution with hydrogen ion concentration of 1.33 x 10-4 M. Is the solution acidic, basic or neutral?
c. A solution with hydrogen ion concentration of 2.44 x 10-14 M. Is the solution acidic, basic or neutral?
d. A solution with a hydroxide ion concentration of 2.44 x 10-14 M. Is the solution acidic, basic or neutral?
e. (Honors) a 3.67 x 10-5 M potassium hydroxide solution. Is the solution acidic, basic or neutral?
72. What is the hydrogen ion concentration of a solution with a pH of 3.58?
73. What is the hydrogen ion concentration and hydroxide ion concentration of a solution with a pH of 10.5?
74. (honors) What is the difference between strong and weak acids?
75. (honors) Write the Ka expression for hydrocyanic acid.
76. (honors) Consider the acetic acid, CH3COOH. Give the concentration, in terms of x, for CH3COOH, CH3COO- and
H+ for a 0.025 M solution.
77. (Honors) What are the pH and pOH of a solution made by diluting 25 mL of a 6.0M HCl solution until the final
volume of the solution is 1.75L?
78. (Honors) What is the pH of a 5.0 L solution containing 1.0 g of HBr and 1.0 g of HNO3?
79. (honors) If it takes 54 mL of 0.10 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the
HCl?
80. (honors) if it takes 25 mL of a 0.050 M HCl solution to neutralize 345 mL of NaOH solution, what is the
concentration of the NaOH solution?
81. (honors) An acid-base titration requires 29.88 mL of 1.17 M NaOH to neutralize 5.00 mL of an H2SO4 solution.
Calculate the molarity of the H2SO4 solution.
82. Use the curve below to answer the following:
a. Which is the most soluble salt at 50oC?
b. At which temperature are the solubility of sodium nitrate and potassium nitrate the same?
c. What is the solubility of ammonia at 20oC?
d. What is the maximum amount of potassium chloride that can dissolve in 100 g of water at 75oC?
e. Is a solution containing 25 grams of potassium chlorate in 100 g of water at 60 saturated or unsaturated?
f. What is the maximum amount of ammonium chloride that can dissolve in 250 g of water at 60oC?