Chemistry Review
Station 1: Significance in Measure
1. Name these measurements:
mL milliliters
L Liters
g grams
Kg kilograms
kPa kilopascals
Atm atmospheres
°K Kelvin
°C Celsius
2. Identify the number of significant figures for the following numbers:
100 mL 1
12, 005 g 5
230 kPa 2
0.0100020 °K 6
105 L 3
0.0000534 kg
3
2
1.00 x 10 dots
infinite
0.0030090 °C
5
Convert the following units:
3.
4.
5.
6.
7.
4.35 kg  g
5.86m  mm
486.5mL  L
47.3 °C  °K
1,538 J  Calories
4350g
5860mm
.4865L
320.3 °K
367.94 Cal
Answer to the correct number of significant figures:
8. 1.543 + 45.8
9. 38.9 + 56.001 + 32.05
10. 100.0 – 99 + 1.01
11. 4.32 x 5.052
12. 7.2 x 80.01 / 100.1
13. 394.2 / 10.0 x 5.264
47.3
127.0
2
21.8
5.8
208
Answer the following problems:
14. What is the difference between pure and applied chemistry?
Pure chemistry is based on curiosity with no anticipated outcome while applied chemistry is working
towards a predetermined outcome.
15. Describe precision and explain how it differs from accuracy.
Precision needs multiple attempts while accuracy can be one attempt. If you are precisely accurate
then you have hit a target multiple times (3 darts all hit the bullseye)
16. How would I make a quantitative measurement? How is a quantitative measurement different than a
qualitative measurement?
A quantitative measurement requires some mathematical or numerical result. This defers from a
qualitative measurement because a qualitative measurement is not exact or it is biased based on the
individual making the qualitative measurement (Colors, descriptions, approximations, etc…)
17. What is the density of a cube that has a mass of 152g and a length of a side of 2.1 cm?
16.4 g/cm3
18. What is the mass of an object that has a density of 2.5 g/mL and a volume of 23 mL?
57.5 g
Chemistry Review
19. What is the volume of an object that has a density of 19.3 g/mL and a mass of 96.50 g?
5.00 mL
20. What is the difference between a physical and chemical change?
A physical change effects the appearance of a substance where as a chemical change effects the
atomic composition of the substance. Physical: Weathering, dissolving, phase change, color change
(as in painting or coloring) Chemical: Gas formation, precipitate, oxidized (rusted, burned), color
change (bleaching, new substance)
Station 2: Atom Anatomy and Radiation
21. Create a timeline including dates and discoveries related to the atom
22. Complete the following chart:
Name
Be
F
O
Re
Protons
4
9
8
75
Electrons
4
9
8
75
Neutrons
5
10
8
111
23. Complete an electron configuration for one element in each row
24. Complete a Bohr model for an element in the range of 31-36
25. Complete the following table:
Location
IA
IIA
IIIA
IVA
VA
VIA
VIIA
VIIIA
IB-XB
57-71
89-103
Name
Alkali Metals
Alkaline Earth Metals
Transition Metals
Lanthanides
Actinides
Charge
+1
+2
+3
+/-4
-3
-2
-1
0
Varies, at least__+1___
Varies, at least__+1___
Varies, at least___+1__
26. Draw an EMS and label all major types of radiation
27. The relationship between wavelength and frequency is (inverse/direct).
28. The relationship between energy and frequency is (inverse/direct).
29. If an electron jumps from energy level 2 to energy level 1 then what kind of radiation is emitted?
30. If an electron jumps from energy level 4 to energy level 2 then what kind of radiation is emitted?
31. Complete the following chart:
Chemistry Review
Particle
Symbol
Alpha
Beta
Gamma
Complete the following reactions.
Mass
Charge
4
1x10^-8
0
+2
-1
0
Penetrating
ability
Low
Medium
High
32. 23492U  42He + _23090Th______
33. 188O +0-1e  _______+ 10n
33. 11H + 21H  _3He______
34. 146C  0-1e + _______
35. What is the half-life of a radioactive isotope? The time it takes for half of the atoms of the element to
decompose into something else
36. How much of a 25.0g sample of 146C remains after 103,140 yrs.? The half-life of 146C is 5730 yrs.
37. Determine the half-life of a radioactive isotope that decays from 100.0mg to 12.5mg in 24.0 hours.
Station 3: Bonding and Periodic Trends
38. Complete the following table:
Compound
Name
Phosphorus trichloride
Bond Type
Polarity (yes or no)
SO2
BH3
Dihydrogen Monoxide
Carbon Tetrafluoride
NaBr
Ca(NO3)2
Lithium Sulfate
Iron (III) Carbonate
Pb3(PO4)4
39. Identify the 5 trends and their directions
40. Which combination of elements would most likely form an ionic compound?
a. hydrogen and oxygen
b. carbon and chlorine
c. sodium and fluorine
d. silicon and sulfur
41. Which is an accurate comparison of the bonds that can occur between carbon atoms in terms of bond
length and strength?
a. Double bonds are shorter than single bonds, but single bonds are stronger than triple bonds.
b. Triple bonds are shorter than double bonds, and double bonds are stronger than single bonds.
c. Double bonds are both shorter and stronger than triple bonds.
d. Triple bonds are the longest and strongest.
42. What kind of bond forms CO2? double
43. Which pair of elements is both malleable and able to conduct heat?
a. bromine and silver
Chemistry Review
b. iodine and neon
c. iron and bromine
d. silver and iron
44. When aluminum and sulfur react, which compound is produced? Aluminum sulfide
45. Create a vin diagram for ionic and covalent bonds
Station 4: Chemical Reactions and Stoichiometry
Identify and Balance the following reactions:
46. 4Fe + 3O2  2Fe2O3
47. 2P2O5  2P2 + 5O2
48. K2SO4 + BaCl2  2KCl + BaSO4
49. C12H24 + 18O2  12CO2 + 12H2O
Identify, Finish, and Balance the following reactions:
50. Cu + O2  CuO2
51. H2O  2H2 + O2
52. 2Al + 2Pb(NO3)2 
3Pb + 2Al(NO3)3
53. K3PO4 + AlBr3  3KBr + AlPO4
Convert the following units:
54.
55.
56.
57.
58.
2.89 moles of NaCl to mass
67.32g of PbCl3 to moles
1.20x1024 atoms of U to moles 2 moles
393.94g of Gold to atoms of Gold
1.987x1024 molecules of H2O to mass
Find the empirical and/or molecular formulas based on the following questions:
59. A 170g sample of an unidentified compound contains 29.84g Na, 67.49g Cr, and 72.67g Oxygen.
What is the compound’s empirical formula? Na2Cr2O7
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60. A sample measures 1.388g C, 0.345g H, and 1.850g O (3.583g). The molar mass is 62g. What is
the molecular formula of this substance?
Find the limiting reactant and theoretical yield in the following reactions:
61. 10g of K2SO4 + 10g of BaCl2  KCl + BaSO4
62. Lead isolation using 21g of Lead (IV) Carbonate and 18g of Aluminum metal
Answer the following questions:
63. What do double replacement reactions create?
64. Which compound is soluble? CaCO3; Ba(OH)2; Fe2O3; CuSO4; PbCl2; FeF3
65. What is an exothermic reaction?
66. What is an endothermic reaction?
Station 5: Phase Changes, Gas Laws, and Energy
Create and label the following charts:
67.
Identify the shift that would occur in each scenario:
68.
H2 (g) + O2 (g)  H2O (l) ΔH= 534J
69. Increasing the amount of H2 Products
70. Increasing the amount of H2O
71. Turning up the heat
72. Decreasing the amount of O2
73. Putting the reaction on ice Reactants
74. Increasing the pressure of the reaction
Show your work for the following problems:
75. If I have 17 liters of gas at a temperature of 67 0C and a pressure of 88.89 atm, what will be the
pressure of the gas if I raise the temperature to 94 0C and decrease the volume to 12 liters?
Chemistry Review
76. I have an unknown volume of gas at a pressure of 0.5 atm and a temperature of 325 K. If I raise the
pressure to 1.2 atm, decrease the temperature to 320 K, and measure the final volume to be 48 liters,
what was the initial volume of the gas? 117L
77. What is the specific heat capacity of a metal if 55.00 g of the metal absorbs 47.3 calories of heat and
the temperature rises 15.0°C?
78. Calculate the heat capacity of a piece of wood if 1500.0 g of the wood absorbs 67,500 joules of heat,
and its temperature changes from 32°C to 57°C.
79. What would the pressure of a 4.5L container holding 2.3 moles of CO2 at 15ºC be in mmHg?
80. How many moles of N2 are in a .45L container under 16.3 kPa of pressure and 17ºC?
Station 6: Acids, Bases, and Solutions
Use the graph to answer the following questions:
81. Amount of NaNO3 at 50 C°
82. Compound where solubility decreases with increasing
temperature
83. Compound with a solubility of 70g in 90 °C solution
84. Compound with a solubility of 58g in 18 °C solution
85. Temperature of KClO3 where 36g will dissolve
86. Temperature of NaNO3 where 115g will dissolve
87. Type of NaNO3 solution with 130g at 50 °C
88. Type of NH3 solution with 68g at 10 °C
89. Type of KCl solution with 42g at 55 °C
90. Type of Ce2(SO4)3 solution with 5g at 39 °C
Use the graph to answer the following questions:
91. Which indicator is best suited for a strong
acid?
92. Which indicator is best suited for a strong
base?
93. Which indicator would be best for a
neutral solution?
94. If a solution has a hydroxide concentration of 4.38 x 10-7 then what color would each indicator
show?
95. Complete the chart:
[H+]
[OH-]
5.4x10-3
8.9x10-12
pH
pOH
Classification
Chemistry Review
3.2
.0316
3.16E-13
12.5
Acid
1.5
Base
Show work for the following problems:
96. What is the molarity of 35g NaCl in 500mL of solvent?
97. What is the volume of a 4M MgCO3 solution with 85g of solute? 248 mL
98. What is the mass of AlPO4 in 225mL of 1.5M solution?
99. What is the concentration of an unknown acid if 450mL of 3.5M base neutralizes 255mL of the
acid?
100.
Name the following acids and bases:
HCl
H2SO3
Hydrochloric Acid
Sulfurous Acid
HNO3
NaOH
Nitric Acid
Sodium Hydroxide
Al(OH)3
Aluminum Hydroxide