Name___________________________________________Date___________________
Chemistry in the Community Final Exam Review Guide 2015
Unit 2.A.1 page 151 through Unit 3C up to and including page 353.
 For your exam, know all the bold-faced terms in the text.
 This study guide is not meant as a stand-alone study guide for the final exam.
 I will collect this study guide the day of the final exam. It will be graded for correctness
and completeness!
1) I suggest you go through the power point I made (link on my website and on MBC) and write down
the answers to the following questions. Have your book available to assist you with areas where
you need a more detailed explanation.
2) Go through this study guide a second time and try to answer all the questions from memory.
3) If you are still missing more than 10-20 percent of the questions I suggest you read the book and go
over your weak areas until you can master all of the concepts below. There are plenty of practice
questions at the end of each chapter to assist you with the review process.
As of May 29, 2015 there are (These numbers are not final);
1 question on 1A
12 questions on 3A
16 questions on 2A
4 questions on 3B
13 questions on 2B
14 questions on 3C
18 questions on 2C
? questions on 3D
79 Questions (So Far)
2 questions on 2D
Unit 1A (Chemistry Basics)
1) Give an example of a chemical symbol, chemical formula, and chemical equation.
2) Label the subscript and the coefficient in chemical formulas below?
2H2O
3) List the diatomic elements. What memory aid did you use?
4) How would you measure the density of:
a) A block of wood?
b) A sample of a liquid?
5) Name the different metric prefixes we have learned. What does each mean?
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Review - Unit 2A
6) Define “pressure”.
7) What are some appropriate units for pressure?
8) Name the SI unit for pressure. Is it a base or derived unit?
9) On what two factors does Pressure depend?
10) What type of relationship with Pressure does each factor (from #9) have? (inverse/direct)
11) Name the different metric prefixes we have learned. What does each mean?
12) How is a cm3 related to a mL? A cm 3 to a L ? A mL to a L?
13) A barometer at 1 atmosphere of pressure will read ________mmHg.
14) What are the names of the 3 gas laws we have studied? (PT, VT, and PV) What kind of relationship does each
describe? (direct or inverse?) Describe the simple experiments we used in class to illustrate each law. What is
the shape of a graph representing each?
15) What is the significance of the Kelvin scale of temperature?
16) How do you convert degrees Celsius to Kelvin?
17) A balloon inflated to 3.40 L at 810. Torr pressure is taken into a chamber where its volume changes to 4.40 L.
What is the pressure in the chamber? (Boyles Law)
18) A spray can contains a vapor under 9.70 atmospheres pressure at a room temperature of 22.0 oC. If the can is
left in a closed car on a hot summer day, the pressure rises to 10,100 mmHg. What is the temperature in the
car? (Gay-Lussac)
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19) A balloon occupies 8500 mL when the air surrounding it is 27 oC. If its volume shrinks to 8.2 L, what has the
temperature of the air become, in degrees Celsius? (Charles Law)
20) What happens to atoms and molecules at “absolute zero”?
Review – Unit 2B
21) Describe the motion of particles in a gas compared to those in a solid or liquid.
22) What state of matter exhibits the least attraction between particles? ________________________
23) What causes pressure on a particle level?
24) As the kinetic energy of a gas increases what happens to the temperature of the gas?
25) What is an “ideal gas”? (How does an “ideal gas” behave?)
26) Under what two conditions will a real gas NOT behave ideally?
27) How much volume does a mole of a gas occupy? (What two other properties besides the number of molecules
– a mole – have to be defined?)
28) What are standard conditions for a gas? (STP?)
29) What is the volume of a mole of an ideal gas under standard conditions?
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30) How many moles of gas would be in a 2.0 L bottle of air at 0.0 oC and 1.0 atm?
Review – Unit 2C
31) What is the name of the zone of the earth’s atmosphere which contains most of the atmosphere’s matter
contains all of our weather, and which is closest to the surface of the earth?
32) What are the two major components of the zone of the atmosphere closest to the earth, and what are their
approximate percentages?
33) Name the four main layers of the atmosphere, starting with the one closest to the surface of the earth.
34) What happens to temperature and pressure as you increase altitude in the troposphere?
35) Why is air a gas at room temperature?
36) What is the difference between a homogeneous mixture and a heterogeneous mixture?
(and how is a homogeneous mixture different from a pure substance?)
37) What is the electromagnetic spectrum? Name all the kinds of electromagnetic radiation spanned by the
spectrum.
38) Draw a diagram of a light wave and label the parts.
39) Explain the relationship between wavelength and frequency of a wave. How do these properties relate to the
energy of the wave?
40) What is constant for ALL light waves, regardless of region of the spectrum?
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41) What is a photon?
42) In what 3 regions of the electromagnetic spectrum does the sun produce almost all its light?
43) List two benefits of visible light.
44) How does the presence of our atmosphere affect the daytime and nighttime temperatures on Earth?
45) Name several greenhouse gases and explain why they are called “greenhouse gases”.
Review - 2D
46) What is an acid? Give two examples.
a) How can you recognize an acid from its formula?
47) What is a base? Give two examples.
a) How can you recognize a base from its formula?
48) Describe the pH scale. Be sure to explain the significance of a pH of 7.
Review – Unit 3A
49) Most of the substances making up the mixture we call petroleum are _________________________ because
they contain only atoms of the elements hydrogen and carbon.
50) Petroleum is an example of a _____________________ resource, meaning once it has been used, it will take
millions of years for nature to replace it. (Section 3C?)
51) Parts of mixtures can be separated by distillation processes because the different substances in those mixtures
have different ____________________________, which is a ____________ property.
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52) The fundamental difference between simple distillation and _________________________________ is that the
distillates produced in simple distillation are _____________________________, whereas in
_________________________________, the distillates produced are mixtures, which are called
_______________________.
53) In a refinery’s fractionating tower, the substances which have really low boiling points are recovered as
___________and are recovered at the __________(top/bottom)of the tower.
54) The substances which have really high boiling points are recovered from the ______________ of the
fractionating tower and are called____________or____________.
55) The temperature in the _____________ of the fractionating tower is hotter than that in the _____________ of
the tower. (where)
56) The type of hydrocarbon molecule in which each carbon is bonded to four other atoms is a(n)
____________________. In these molecules, the only kind of carbon-to-carbon bond is a ______________
bond. These molecules are also said to be __________________.
57) The atoms in hydrocarbons and most other organic compounds are held together by _____________ bonds.
(what kind?)
58) Each such bond is a ___________ of electrons. When drawing a structural formula, the bond is represented by
a _____________. In electron dot notation, a bond is represented by a ______________________.
59) In any atom, the maximum number of electrons which may occupy the first energy level is ________. The
maximum number of electrons which may occupy the second energy level of any atom is _________.
60) In any atom from carbon on, there is a special stability associated with an atom having _________ electrons in
its highest energy level. This is termed the ____________ rule. The electrons in the highest energy level are
termed the _______________ electrons and the energy level which they occupy is sometimes termed the
_____________ shell.
61) The first ten alkanes are named:
62) The more carbon atoms in a hydrocarbon, the ______________ the boiling point of the hydrocarbon. This is
because the _________________________________ between the molecules are larger for molecules which
contain more atoms. For a substance to boil, enough heat must be added to the substance (the temperature
must be raised enough) to overcome these forces so that molecules can move apart into the gaseous state.
molecular formula
structural formula
electron dot formulas
63) Write and draw the molecular formula, structural formula and the electron dot formulas for propane.
64) What is the general formula for any alkane?
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65) Draw the complete structural formulas of any two isomers of pentane.
66) If several isomers of an alkane exist, how are their boiling points related to their degree of branching?
Review – Unit 3C
67) Explain the difference between potential and kinetic energy:
68) Unburned gasoline has _______________ energy and is considered to be a kind of _______________(type of
potential/kinetic) energy.
Endothermic vs. exothermic changes:
69) Which energy type is from breaking of chemical bonds and which one is from the making of chemical bonds?
70) Sketch and Label an exothermic potential energy diagram:
71) Write the equation for the burning of methane gas. Make sure it is balanced, has the correct states of matter for
each formula, and the appropriate quantity of energy is included in the product of the reaction (look up the HOC
in section 3.C.4 of the book)
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72) How much energy would be released if 10 moles of methane were burned?
73) The molar heat of combustion for octane is 5450 kJ/mole. Calculate the KJ/g of octane. (Hint: That big chart in
the front of your classroom is not just a decoration.)
74) Heat of combustion is measured in either kJ/mole or kJ/gram. Which value increases with the number of carbon
atoms in a molecule of a hydrocarbon?___________________
75) Specific heat (“specific heat capacity”) is a physical property of a substance. In general, what does it indicate
about a substance? What is the specific heat of water? (value and units)
76) How is the specific heat capacity of water used to determine the heat of combustion of hydrocarbons? (Think
about the candle lab.)
77) What is the mathematical equation for determining the heat required to heat (or cool) a specific mass of a
substance so that its temperature changes by a specific amount?
78) Use that equation to determine how much heat must be absorbed by 2 liters of water to raise its temperature
from room temperature (25 oC) to boiling.
Review – Unit 3D
79) Homes in the 1920s primarily used__________________to heat their homes.
80) What was petroleum mostly used for in the early 1900’s?
81) What is the only emission produced by a hydrogen fuel cell vehicle?
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82) Explain what biomass is and give 3 examples of biomass.
83) Name 3 advantages and 3 disadvantages of compressed natural gas for use in transportation.
84) How is “cracking” accomplished and why is it valuable in the making of petroleum?
85) What is a catalyst and what why are catalysts used in some chemical reactions? (Such as the cracking
process)
86) What property of a hydrocarbon makes it burn more slowly in a gasoline engine, thus reducing “pinging” or
“knocking”?
87) What three substances have been added to gasoline to increase its antiknock characteristics?
88) Which two are known to cause environmental problems?
89) The use of which one has already been discontinued?
Review – Unit 3B
90) What is the simplest hydrocarbon builder molecule? Draw its structural formula.
91) To what class of compounds does ethylene belong?
92) When the double bond is broken a monomer is formed. When many of these monomers are joined together the
new molecule chain is called a________________.
93) What kind of reactions can alkenes and alkynes participate in, but alkanes can NOT participate in?
94) Draw the structural formulas for the 2-butene isomers.
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95) Draw a propyne molecule. How many propyne isomers are there?_______
96) To what class of compounds does butyne belong?
97) Draw an electron-dot formula for a propyne molecule
98) What is the general molecular formula for a cycloalkane? Draw the structural formula for a cyclohexane.
99) Draw the structural formulas for benzene.
100)
What group of hydrocarbons is benzene considered a part of?
101)
Write the functional groups for an alcohol, carboxylic acid, and an ester:
alcohol
carboxylic acid
ester
102)
Write an equation for a carboxylic acid (ethanoic acid) and an alcohol (methanol) combining to make an ester.
(Don’t forget the sulfuric acid!)
A. What is the purpose of the sulfuric acid?
B. What kind of reaction is this an example of?
Additional Notes:
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