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FINAL EXAM REVIEW PACKET
Metric System:
1. List the metric prefixes on the line (name & symbol). Then identify the numerical value for the prefix.
2. Convert the following:
2.65 mg = __________ g
0.0642 kL = _________ cL
3. What are the metric base units for the following? What instruments are used to measure these?
Mass = __________________
Length = _________________
Volume = _________________
4. Record the following measurements. Don’t forget the units!
5. Calculate the density of a piece of gold with a mass of 45.65 g and a volume of 24.5 mL.
Matter:
6. Fill in the following flow chart about matter classification:
7. What’s the difference between an element and a compound?
8. What’s the difference between a physical and chemical change?
The Atom:
9. What is the smallest part of an element that still retains the properties of that element? ________________
10. Label the parts of the nuclear symbol:
𝐴
𝑍𝑋
11. Complete the table for each element:
element
calcium
krypton
Nuclear symbol
#protons
40
20𝐶𝑎
31
___𝑃
___
36_____
15
# neutrons
# electrons
50
12. What kind of an ion is O-2? ________________ Has it gained or lost electrons? __________________
Periodic Table
13. What group on the periodic table is the most reactive metals? Most reactive nonmetals?
14. Above the columns of the main group elements below, identify the number of valence electrons and the
expected charges.
15. What is it important to know the number of valence electrons in an atom?
Chemical Bonding:
16. What is the definition of an ionic bond? What type of atoms make ionic bonds?
17. What is the definition of a covalent bond? What type of atoms make covalent bonds?
18. What is the general formula for alkanes?
19. What are the prefixes for naming organic compounds?
# C’s
1
2
3
4
5
Prefix
# C’s
6
7
8
9
10
Prefix
Reactions
20. In the equation:
A.
B.
C.
D.
2 HCl(aq) + Na2CO3(aq)  2 NaCl(aq) + H2O(l) + CO2(g)
circle the subscripts
underline the coefficients
box the yield sign
Fill in the phases for each compound in the chart.
Compound
Phase
HCl
H2O
CO2
E. What phase of matter is not included in the reaction above? (Name it.) What is the symbol? ______________
F. How does the following equation demonstrate the “Law of Conservation of Matter”?
21. Identify the number of atoms in each of the following formulas:
KNO3
K = ____
N = ____
O = ____
(NH4)3P
N = ____
H = ____
P = ____
22. What are the 5 evidences of chemical change?
1.
4.
2.
5.
3.
23. Name 2 examples of chemical reactions in your everyday life.
24. For each of the following reactions:
A. Identify the type of reaction and write it in the box.
B. Balance the equation. You may create an atom inventory in the space provided to help you balance.
___ FeS2(s) + ___ O2 (g) ___ Fe2O3(s) + ___ S8(s)
___ Na(NO3) (aq) + ___ PbO(s) ___ Pb(NO3)2(aq) +___ Na2O(aq)
___ C3H8 (g) + ___ O2(g)  ___ CO2(g) + ___ H2O(g)
___ SiCl4(s)  ___ Si(s) + ____ Cl2(g)
___ H2(g) + ___ O2 (g)  ___ H2O(l)
Reaction Type:
Reaction Type:
Reaction Type:
Reaction Type:
Reaction Type:
The Mole
25. The mole is a measurement of: ___________________
26. The molar mass of an element is equal to an element’s _____________ _____________ from the periodic table.
Calculate the molar mass for the following compounds, using a periodic table.
Ba(OH)2
SO2
Ba:
S:
O:
O:
H:
_________ g/mol
27. Calculate the percent composition of Ba, O, and H in Ba(OH)2. Show all work.
__________ g/mol
% Comp = part x100
total
28. Know how to convert between moles and grams using the molar mass as a conversion factor.
Mass to Mole: _________________ by molar mass
Mole to Mass: __________________by molar mass
A.
Convert 2.53 mol KCl to grams of KCl
=
B. Convert 36.2 grams CO2 to mol of CO2
=
29. True or False: To use a mole ratio, you always need a balanced chemical equation. ________
30. Balance the following equation and answer the question:
____Mg + ____ O2  _____ MgO
Starting with 6.8 mol Mg, how many mol MgO will be produced?
Given:
Unknown:
=
31. You are making ice cream in chemistry class and there are 20 students.
For one serving of ice cream:
Supplies you have for the whole class:
½ tsp of vanilla
1 tbsp sugar
½ cup heavy cream
A. Is there enough supplies for the whole class?
8 tsp of vanilla
25 tbsp sugar
10 cups heavy cream
B. What is the limiting ingredient (reactant)? If you were able to make 20 batches, what would be in excess?
32. What is the difference between expected yield and actual yield?
33. An experiment produced 9.50 grams of MgCl2. The scientist expected to produce
10.25 grams. What is the % yield?
% Yield = actual x100
expected
Why is the percent yield less than 100%? What does it mean if it is over 100%?
Solutions
34. What is a solution? What are the two parts of a solution?
35. When a student dissolves salt in water, the salt acts as the ________________ because is it dissolved. The water
in the solution acts like the ______________ because it does that dissolving.
36. Salt dissolves in water; salt is (circle one): soluble / insoluble.
37. Lead Phosphate does not dissolve in water; lead phosphate is (circle one): soluble / insoluble.
38. How do you know if something will dissolve? Fill in the blanks.
“________________ dissolves _________________,” which means that polar molecules dissolve in
______________ solvents , and nonpolar molecules dissolve in ________________ solvents.
39. List three things which will increase the speed at which a substance dissolves.
1.
2.
3.
40. Compare the following types of electrolytes:
Type
Nonelectrolyte
Weak Electrolyte
Strong Electryolyte
Light Bulb Brightness
Amount of Ions
41. When a substance dissolves in water:
A. The solution’s ___________________ point is higher. (when you cook pasta)
B. The solution’s ___________________ point is lower. (when you add salt to roads in winter)
C. These properties are called __________________properties because they depend on the concentration
of solute but not the nature of the particle.
D. Please explain, using scientific terms, why adding salt to water raises it’s boiling point.
42. The concentration of a solution can be calculated by solving for M, which stands for __________________ .
A. You have 39.2 L of solution that contains 49.21 mol of sodium chloride, NaCl.
What is the molarity of that solution?
Mol
B. What is the Molarity of a solution that has 2.18 mol of solute and 0.85 L of solution?
M
L
Acids and Bases
43. Identify the following as acid or base:
HCl
Na(OH)
H2SO4
_______________
_______________
_______________
44. Give an example of a Monoprotic Acid:____________
Ca(OH)2
K(OH)
H3PO4
_______________
_______________
_______________
Give an example of a Polyprotic Acid: __________
45. What is the formula of Hydronium? _______ What is the formula of Hydroxide? _______
46. What ion does pH measure the concentration of?
47. Fill in the pH scale below with the appropriate numbers. Label what ranges are acidic, basic, and neutral.
48. Write Acidic, Basic, or Neutral in the box:
Hydronium > Hydroxide
H3O+ > OH-
Hydronium = Hydroxide
H3O+ = OH-
Hydronium < Hydroxide
H3O+ < OH-
49. Do all solutions contain hydronium and hydroxide? How does water prove this?
50. Put an A for “Acid” or B for “Base”:
Hand soap: _____
Lemon juice: ____
Hand sanitizer: ____
Distilled Water:______
51. What does a buffer do?
52. What is acid rain? Why is it a problem?
53. Neutralization Reactions:
A. Fill in the formula for the missing product.
B. Underneath each formula, identify the: salt, water, acid, and base.
Mg(OH)2
+
__________
H3PO4
 _________ +
__________
Mg3(PO4)2
_________
___________
54. Fill in the properties of acids and bases below:
Acids
Bases
55. Complete the following table using your knowledge of the pH equation:
[H3O+] Concentration
[H3O+]
Concentration
0.001
10-3
pH
0.000000001
9
0.0001
4
0.01
Acid, Base, or Neutral?
10-2
56. A student prepares an acidic solution at a pH of 4. Another student prepares an acidic solution at a pH of 3.
A. Which solution is more acidic? pH of 3 / pH of 4 (circle one)
B. How many times more H3O+ ions does a solution of a pH of 3 have compared to a solution of a pH of 4.
(Hint: Use the chart above to help you).
Gases
57. Describe what it means for a gas to be compressible:
58. Fill in the word that best describes the property of gases
A. Gases experience _________________ meaning they mix evenly and completely.
B. Gases take the ________________ and _________________ of their container.
C. Gases exert __________________ .
D. Gases have ___________________ that shows when you place a filled balloon on a balance.
E. Gases have very low _______________________ in comparison to solids and liquids.
59. What two variables are related to each other in Boyle’s Law: _______________ __________________
A. When pressure is increased, volume ___________________
B. When pressure is decreased, volume __________________
C. This law illustrates a direct / inverse relationship between pressure and volume.
60. What two variables are related to each other in Charles’ Law: _________________ ____________________
A. When temperature is increased, volume ___________________
B. When temperature is decreased, volume ___________________
C. This law illustrates a direct / inverse relationship between temperature and volume.
61. How do you convert from °C to K?
62. Complete the chart:
Temperature
Freezing point of water
Celsius (°C)
Kelvin (K)
Boiling point of water
Room temperature
25 °C
436 K
63. What does STP stand for?
What are the values for STP? ______oC or ________ K
and
_________ atm
64. On the lines next to picture, rank pressure lowest to highest with 1 being lowest.
Flying in an airplane
Climbing the Mountain
Sailing
Explain your ranking of this pressure:
Scuba diving
Rates and Thermochemistry
65. What is activation energy?
66. What is the difference between endothermic and exothermic reactions?
67. What is the sign ( + or - ) for ∆H, the enthalpy of reaction, when the reaction is
Exothermic: ______
Endothermic: ______
68. What must happen for molecules to react?
69. List several ways the rate of a reaction can be increased:
70. Draw a heating and cooling curve and label each phase of matter and each phase change.
Heating:
Cooling:
71. What happens to the temperature of a substance when it is freezing or melting?
72. How much heat is absorbed when a 25.0 g sample of water (c = 4.184 J/g oC ) has a temp change of 23oC ?
Formula : Q = m c ∆T
Q
=
m
c
Equilibrium and Redox
73. Which reaction below is reversible?
NH4OH  H2O + NH3
H2O2  H2 + O2
∆T
74. What happens when a reaction reaches equilibrium?
75. Identify which way the reaction will shift in the given scenarios:
NaCl(s)  Na+(aq) + Cl-(aq) + energy
Change
Shift
Remove ClAdd NaCl
Increase the Temperature
Add Na+
76. If a scientist wanted to use this reaction to produce a lot of sodium ions, what change could be used to keep the
reaction going forward? Why?
77. REDOX is an abbreviation for _________________________ _______________________ reactions.
78. What is reduction?
79. What is oxidation?
80. Identify the type of half reaction as reduction or oxidation.
Ca  Ca2+ + 2 e-
___________________________
Cl2 + 2 e-  2 Cl-
___________________________
2 Br-  Br2 + 2 e-
___________________________
81. List three practical applications of Electrochemistry:
1.
2.
3.
Nuclear
82. All types of radiation from low to high energy are organized on the _______________________ spectrum.
83. What part of the atom “decays?”
84. What is background radiation?
85. What makes a nuclear reaction different from a chemical reaction?
86.
_______________ Energy
_______________ Energy
87. Circle the type of electromagnetic wave that is the highest energy.
gamma ray
visible
or
microwave
or
ultraviolet
x-ray
or
radio
x-ray
or
visible
88. Complete the following table about nuclear decay particles.
Type of
Nuclear Decay
Symbol
Charge
Reaction
Particle
89. What is the difference between nuclear FISSION and nuclear FUSION?
Fission:
Where are fission reactions used?
Fusion:
Where are fusion reactions used?
Strength
Stopped by…
90. What is critical mass?
91. Write a nuclear equation for the following decay reactions:
A. Beta decay of
43
20Ca.
B. Alpha decay of 24395Am.
92. Define Half-Life:
93. The half-life of potassium is 2 hrs. If you start with a sample of 60.0g, how much of it will still be left after 10 hrs?
94. Why is nuclear waste so dangerous? How do we get rid of it?
95. What does radiation do to people who are exposed to high doses of it?
96. What are 2 beneficial uses of radiation?