Final Exam Review 2015 HONORS Chemistry Name ______________________________
For problems, you must show all work INCLUDING a formula, filling in the formula, the answer and
unit for full credit.
Unit 1: Math and Moles: There will be 20 questions on your final from this section.
Define and give an example of each
Word
Define
Example
1. Accuracy
How close your data is to correct
A bullseye
2. Precision
How close your set data is together
A cluster
3. Qualitative
Word description
Very fast
4. Quantitative
Number and Unit
10 m/s
5. Physical
Can use to describe matter using your
Color, mass, volume, density
Properties
6. Extrinsic
senses
Depends on amt
Mass, volume,
Independent of the amt
Density
Properties
7. Intrinsic
Properties
8. Chemical
Ability to react
Properties
9. Chemical changes Atoms rearrange
10. Physical changes
May look different but atoms don’t
Sodium has the ability to react
explosively with water
2Na + H2O  2NaOH + H2
chemical change indicators
Phase changes
rearrange
11. Density
Ratio of mass:volume; D=m/v
12. Mole
SI unit for amount
13. Molar mass
H2O = 18.02 g/mol
14. Molar Volume
Mass of 1 mole: Add up masses from
periodic table
Volume of 1 mole of a gas at STP
15. Avogadro’s
(word definition) number of particles in
Number = 6.02X 10 23
Number
16. Particles (in mole
conversions)
1 mole
Atoms, ions, molecules or formula units
1 mol=22.4L
17. Atom (in mole
conversions)
18. Molecule (in mole
conversions)
19. Formula Unit (in
mole conversions)
20. Ion (in mole
conversions)
21. Molecular
An atom without a charge
Zn
A covalent Compound
CO2
An ionic compound
ZnCl2
An atom or group of atoms with a
charge
How a compound appears in nature
Zn2+
The lowest ratio
CH2O
C6H12O6
Formula
22. Empirical
Formula
23. List the metric conversions for your class. ( ___ m= ____ km; etc.)
Convert the following:
24. 456 m to cm A: 4.56 X104 cm
25. 90.8 mm to m A: 9.08 X10-2 m
26. 459 km to m A: 4.59 X105 m
27. 0.158 um to Gm A: 1.58X10 -16 Gm
28. List and define the parts of the scientific method.
29. Describe how to solve a density problem when you are given mass and volume and want density.
30. A box has a mass of 15.0 g and a volume of 45.0 mL. What is the density? 15/45= 3.3X10-1g/mL
31. Describe how to solve a density problem when you want mass and are given density and volume.
32. A box has a density of 25.0 g/mL and a volume of 5.0 mL. What is the mass? 25(5)= 1.25X102 g
33. Describe how to solve a density problem when you want volume and are given mass and density.
34. A box has a density of 50.0 g/mL and a mass of 10.0 g. What is the volume? 10/50 = 2.00X10-1 mL
35. Describe how to find the molar mass and what unit you would use.
36. Find the molar mass of: H2O, Zn3(PO4)2, C6H12O6 A: 18.02 g/mol; 386.11 g/mol; 180.16g/mol
37. Describe how to find the % by mass given the formula.
38. Find the % by mass for each element in H2O, Zn3(PO4)2, C6H12O6 A: A: %H= 11.19% & % O =
88.79%; %Zn= 50.81%, % P 16.04%, %O = 33.15%; %C= 40.00%, %H= 6.71%, %O = 53.28%
39. Describe how to convert from grams to moles.
40. Convert 16.0 g of helium to moles. A. 16.0/4.00= 4.00 mole
41. Convert 9.01 g of water to moles. A. 9.01/18.02= 5.00X10-1 moles
42. Describe how to convert from moles to grams.
43. Convert 5.6 moles of ZnCl2 to grams. A: 5.6*136.30= 7.6 X102g
44. Convert .086 moles of lead (II) chloride to grams. A= 0.086*278.11= 2.4X101 g
45. Describe how to convert from moles to particles. A: multiply by 6.02 X 1023
46. Convert 1.5 moles of zinc acetate to particles (make sure to specify the particle!). A: 1.5 X
6.02X1023= 9.0X1023 formula units
47. Convert 0.52 moles of carbon dioxide to particles. A: 0.52 X 6.02X1023 =3.1X1023 molecules
48. Describe how to convert from particles to moles. A: divide by 6.02X 1023
49. Convert 5 atoms of lithium to moles. A: 5/6.02X1023 =8X10-24moles
50. Convert 0.75 atoms of vanadium to moles. A: 0.75 /6.02X1023 =1.2X10-24moles
51. Describe how to convert from moles to volume. A: multiply 22.4L/1mol
52. Convert 75 moles of helium to volume. A: 75*22.4= 1.7X103 L
53. Convert 0.412 moles of hydrochloric acid (g) to volume. A: 0.412*22.4= 9.23 L
54. Describe how to convert from volume to moles. A: divide by 22.4
55. Convert 44.8 L of oxygen gas to moles A: 44.8/22.4= 2.00 mol
56. Convert 0.75 L iodine gas to moles A:0.75/22.4= 3.3 X10-2moles
57. Describe how to convert from molar mass to molar volume. A: divide by molar mass X 22.4
58. Convert 100.0g hydrogen gas to liters. A: 100.0/2.02*22.4= 1.109X103 L
59. Convert 0.89 g astatine gas to liters. A: 0.89/420*22.4= 8.4 X103 L
60. Describe how to convert from molar volume to molar mass. A: divide by 22.4 X molar mass
61. Describe how to find empirical formula. A: change % to g, change g to mol, divide by smallest
(becomes subscript)
62. A compound is 94.1 % oxygen & the rest hydrogen. Find the empirical formula. A: HO
63. A compound if 53.0% aluminum & the rest oxygen. Find the empirical formula. A: Al2O3
64. Describe how to find molecular formula. A: Molecular mass/empirical mass= ratio
65. A compound has a molar mass of 100. The mystery compound has the formula X2Z4. If the
empirical formula mass is found to be 20, what is the molecular formula? (The most important
person in the room is …) A: X10Z20
66. A compound has a molar mass of 150. The mystery compound has the formula X4Z6. If the
empirical formula mass is found to be 50, what is the molecular formula? (The most important
person in the room is …) A: X12Z18
Unit 2: Thermo There will be 10 questions on your final from this section.
Define the following words and give an example of each.
Word
Definition
Example
67. Endothermic
Takes in heat
Ice melting
68. Exothermic
Removes heat
Ice freezing
69. Phase Diagram
Shows state of matter at T and P
70. Heating Curve
12 3
5
4
Shows state of matter at T and
time
For each of the following phase changes, define it and tell if the process is endothermic or exothermic.
Phase change
Definition
Endothermic or exothermic
71. Deposition
Gas solid
Exo
72. Fusion
solid liquid
Endo
73. Condensation
Gas  liquid
Exo
74. Sublimation
Solid gas
Endo
75. Solidification
Liquid  solid
Exo
76. Vaporization
Liquid  gas
Endo
77. Label 1-5 of the phase diagram. A: solid, liquid, critical point, triple pt, gas
1 2
4
3
5
78. At 0C and 8 atm, what is the phase of matter? A: gas
79. In a thermo-chemical equation, the heat is on the right in a
_exothermic__ reaction and the left in a _endothermic___ reaction.
80. In a thermo-chemical equation, the delta H is positive in a
__endothermic_ reaction and negative in a __exothermic__ reaction.
81. 500 g of a metal is heated to 150C. When transferred to 200 g of
water, the water T rises from 20C to 50C. Assume no heat is lost.
The specific heat of water is 4.184 J/gC.
Find the specific heat of the metal. A: 5X10-1J/gC
82. Draw graphs of endothermic reaction and an exothermic
reaction. In each graph, label the both axis, products, reactants,
& activation energy.
83. If the temperature of 600 g of ethanol (CH3CH2OH) decreases
to 50 C from 150 C, how much energy was released? The
specific heat of ethanol is 2.44 J/gC. A: -146400 J= - 1 X105 J
84. Find the specific heat of an object with a mass of 250g that had
a decrease of 10 C when 150 J of energy was removed. A: 6 X
10 -2 J/gC
85. Describe in words what happens when you add a catalyst to a reaction. A: lowers activation
energy
86. Label the heating curve below. Make sure to label the axes, the states of matter, the phase
changes, endo and exo thermic and the boiling point and freezing point of water.
87. Explain why the temperature doesn’t change during a phase change on a heating curve. A: all
extra E used for phase change
88. Calculate the heat required to change 75.0 g of ice at -15.8 C to steam at 145 C. A: 2.35X105J
(cwater=4.184 J/gC; cice = 2.06 J/gC; csteam= 2.06 J/gC;  Hvap = 40.7kJ/mol;  Hfus = 6.01 kJ/mol)
89. Find the H of the reaction below using: TYPO 3rd equation should be 2 water; A: -226.9 kJ
C(s) + O2(g) CO2 (g) H = -393.5 kJ
H2 (g) + ½ O2 (g)  H2O (l)H= - 285.5kJ
2C2H2(g) + 5O2(g)  4CO2(g) + 2H2O(l)
H = -2598.8 kJ
Target: C2H2 (g)  2 C(s) + H2 (g) H = ?
90. How much heat is evolved when 50.6 g oxygen is burned according to this equation? C(s) + O2(g) CO2
(g) H = -393.5 kJ
A: 50.6/32/1*-393.5 =- 6.22X102 kJ
91. Calculate the heat required to freeze 456.36 g of liquid ethanol (C2H5OH) at its freezing point.
( Hvap = 38.6kJ/mol;  Hfus = 4.94 kJ/mol) A: 456.36*-4.94= - 4.8924X101 kJ
92. If the T of 67.00 g of gold decreases from 150.0 to 70.0C, how much heat has been released? (specific heat
of gold is 0.13 J/gC). A: q=mcT= 67.00*(70-150)*0.13= -6.968X102 J
93. 46 g of metal is heated to 190C. When transferred to 50.0g H2O in a calorimeter, the water T raises from
25.6C to 35.3C. Assume no heat is lost. Find the specific heat of the metal. A: (50.0*4.184*(35.3-25.6)= q q/46/(35.3-190) = 2.85X10-1 J/gC
94. Find the Hrxn for 2F2 (g) + 2H2O (l)  4HF (g) + O2 (g) Hrxn=?
Given: F2(g) = 0kJ/mol; H2O (l)= -571.6 kJ/mol; HF(g)= -542.2kJ/mol; O2 (g)= 0kJ/mol
A= (4*-542.2)-(2*-571.6) =-1025.6 kJ
95. Find the Hrxn for 2F2 (g) + 2H2O (l)  4HF (g) + O2 (g) Hrxn=?
Given:F2(g) = 0kJ/mol; H2O (l)= -571.6 kJ/mol; HF(g)= -542.2kJ/mol; O2 (g)= 0kJ/mol
A= -1025.6 kJ
96. Write the thermochemical equation using the following information: H2O2(l) →2H2(g)+ O2(g) Hrxn = +188
kJ/mol
A: 188 kJ + H2O2(l) →2H2(g)+ O2(g) Is this an exothermic or endothermic equation? How do you know? +
H
97. What is the specific heat of a metal with a temperature of a 50.0g sample is increased by 15.0oC when 45.8 J
of heat is added? A: 45.8/15.0/50.0= 6.11X10-2 J/gC
Unit 3: Nomenclature & Bonding There will be 10 questions on your final from this section.
Word
Define
Example
98. Ionic Bond
Oppositely charged ions attract;
metal & nonmetal, high mp, bp;
conducts electricity in water
An atom with an uneven number
of protons & electrons
A negatively charged ion; gained
an electron; nonmetal
A positively charged ion; lost an
electron; metal
Share electrons; lowest mp, bp;
does not conduct electricity;
nonmetals and metalloids
ZnCl2
99. Ion
100.
Anion
101.
Cation
102.
Covalent Bond
Zn2+ or ClClZn2+
CO2
103.
Polar
104.
Nonpolar
105.
Metallic
106.
107.
108.
109.
110.
Uneven sharing; EN difference
0.4-2.1
Even sharing; EN 0-0.4
HCl
H2
Sea of electrons overlapping,
Cu
conducts, high bp mp; ductile,
malleable
Write the rules for writing and naming ionic compounds A: see notes or flip book
Write the rules for writing and naming covalent compounds A: see notes or flip book
Write the rules for writing and naming acidic compounds A: see notes or flip book
Name the Following
Write formulas for the following:
111. sodium fluoride
NaF
112.
aluminum
AlCl3
chloride
113.
carbon dioxide
CO2
114.
silver sulfate
Ag2SO4
115.
nitrogen dioxide
NO2
116.
lithium sulfide
Li2S
117.
dinitrogen
N2S3
trisulfide
118.
Nitric acid
HNO3
119.
Phosphorous acid
H3PO3
120.
Calcium
Ca3P2
phosphide
121.
Sulfuric acid
H2SO4
Name the following compounds and molecules.
122.
PbCl4
Lead (IV) chloride
123.
P4I7
Tetraphosphorus heptaiodide
124.
AgCl
Silver chloride
125.
N6O10
Hexanitrogen decoxide
126.
H3PO4
Phosphoric acid
127.
CaS
Calcium sulfide
128.
(NH4)2SO3
Ammonium sulfite
129.
Al2(CO3)3
Aluminum carbonate
130.
HCl
Hydrochloric acid
131.
KClO4
Potassium chlorate
132.
Si4Cl10
Tetrasilicon decachloride
Unit 4 Reactions: There will be 10 questions on your final from this section.
Define the following and given an example:
Word
Definition
Generic Example:
Example
A + B  AB
133. Reactant
Start with
X
A + B  AB
134. Product
End with
X
A + B  AB
135. Yield
arrow
X

136. Synthesis
1 product
A + B  AB
2Al + 3S  Al2S3
137. Single Replacement
1 element swaps
A + BC  AC + B
2AgNO3 + Zn 
places
Zn
(NO3)2+ 2Ag
138. Decomposition
1 reactant
AB A + B
H2CO3  CO2 + H2O
139. Double displacement
2 elements swap
AB + CD AD + CB
MnCl2 +2AgNO3 
places
140. Combustion
Plus oxygen
Mn(NO3)2 +2AgCl
+ O2  oxide
4Al + 3O2  2Al2O3
X
4Al + 3O2  2Al2O3
oil
Al from 0 to 3+= Al is
makes oxide
141.Redox reaction
Reaction where
e- are lost and
gained
142.Oxidized
Lost e-
oxidized
143.Reduced
Gains e-
rig
O2 goes from 0 to 2-;
gained electrons= O2 is
reduced
144.Oxidizing agent
Is reduced
X
O2
145.Reducing agent
Is oxidized
X
Al
146. Using a balanced chemical equation, how can you tell what the state of matter is? How do you
show solid, liquid, gas & aqueous in a balanced chemical equation? Give an example of each.
147. List the seven indicators of a chemical reaction.
148.
List and give formulas of 7 Diatomic Elements
149.
Balance the following equations and give the type of reaction.
150.
______Syn_________R_____
3Sn
151.
_________SD_____R____
152.
____________Decomp________
153.
____________Comb____
2C2H6
154.
_____________Sd___R____
2Na + 2H2O
155.
_____________DD_____
156.
________________DD____ CaCO3
157.
______Comb___________
2AgNO3
2P 
+
+

Zn
H2CO3 
+


4CO2
2NaOH +
2 HCl 
2C4H10 +
Zn (NO3)2 +
2Ag
CO2 + H2O
2AgNO3 
MnCl2 +
+
7O2
Sn3P2
6H2O
H2
Mn(NO3)2 +
CaCl2
13O2 
+
2AgCl
+ H2CO3
8CO2 + 10H2O
Predict the products, write and balance the following equations. Give the type of reaction.
158.
Sodium + chlorine gas  2Na + Cl2  2NaCl ®
159.
Aluminum oxide decomposes 2Al2O3  4Al + 3O2
®
160.
copper + nickel (III) nitrite  3Cu + 2Ni (NO2)3 3Cu (NO2)2 + 2Ni ®
161.
silver nitrate + potassium acetate AgNO3 + KC2H3O2  AgC2H3O2 + KNO3
162.
Combustion of C2H6O C2H6O + 3O2  2CO2 + 3H2O
163.
Which of the questions 150-162 are redox? Identify what is being oxidized, reduced, the oxidizing
agent and the reducing agent. Ex: 159. 2Al2O3  4Al + 3O2
Al is going from +3 to 0= gaining
electrons= (rig); Al3+ is reduced and OA O is going from 2- to a 0= losing electrons= (oil); O2- is
oxidized and is RA
Note: this is the opposite reaction of the ex in the definition boxes
164.
Assign oxidation numbers
a.
KCl K+, Cl-
b. Ca(ClO4)2 Ca 2+, O2-, Cl 7+
Unit 5 Stoichiometry – there will only be 6 questions from this section because we have not completed this
unit
165. Write the balanced chemical equation for the production of water from its elements.
2H2 + O2 2H2O
Use this equation for the remaining questions.
166. How many moles of hydrogen are needed to completely react 4.5 moles of oxygen gas? A:
4.5/1*2=9.0 mol O2
167. How many grams of water are produced when 3.0 moles of hydrogen gas completely react with
excess oxygen? 3/2*2*18.02= 5.4 X 10 1 g H2O
168. How many moles of water are produced when 95 g of oxygen gas react completely? 95/32/1*2=5.75
moles H2O
169. How many grams of oxygen are needed to completely react with 800. g of hydrogen gas?
800/2.02/2*1*32= 6.34X103 g O2
170. What volume of hydrogen gas is needed to produce 450 g of water?
450/18.02/2*2*22.4=5.6X 102L