Dr. Ron Briggs CHM 113
Exam 4 Study Guide
The exam will cover Chapters 10, 11 and 13 and all material covered in lecture. Specific material from your lab
experiments will not be tested on this exam, but the concepts presented during your lab sessions tie in closely with the
lecture material. At least a few questions will be taken directly from your online HW and recitation activities.
A practice exam is attached. As stated in the syllabus, you should use practice exams as practices of real exams. In
other words, study as you would for a real exam, sit down with nothing but a pencil and a calculator, and give yourself 75
minutes to complete it. This should be a good indicator of how you will do on the real thing and give you clues on what
to brush up on. These questions are also different from doing problems in the book in that they are not
“compartmentalized” in such a way that you know exactly what section of the book to look at to solve them. The practice
exam includes a Periodic Table and Equation sheet, which are identical to what will be included on the actual exam.
In addition to the attached practice exam, your lecture notes, lecture quizzes, handouts, recitation activities, and assigned
homework questions are valuable study aids. As always, copies of all quizzes and handouts are available in the
‘Content/Handouts’ section of Blackboard.
Need help? Take advantage of TA and instructor office hours. Chad (our former LRC Manager) has some helpful review
sessions posted online at http://www.chadsreview.org. The site is free, but does require registration. Once you're logged
in, the review sessions are posted by chapter in the "Videos" section. Review sessions are also being planned by Dr. Timo
Park (one of our lead recitation instructors) and the University Academic Success Program (UASP) at the following times:
Timo’s Exam 4 Review: Monday (12/1) from 4:30-6:30 PM in PS H-135
Lin’s Exam 4 Review: Wednesday (12/3) from 7:00-8:00 PM in PS A-203
UASP Exam 4 Review: Tuesday (12/2) from 7:00-8:00 PM in PS H-153
Your SI leader may also be planning additional review sessions. They will send email announcements as appropriate.
* DISCLAIMER: Dr. Briggs does not prepare or run these sessions (he has already prepared a practice exam and study
guide for you). Any material presented is the responsibility of the person running the session. If you have any questions
about this material, please ask them. Supplemental materials from other sessions will not necessarily be posted on
Blackboard.
Exam 4 is Thursday, December 4th (the last day of lecture) in the normal lecture room (PS H-150) at the normal lecture
time. The exam will begin promptly at the start of class and you will have the entire period to complete it. Please
show up on time and do not sit next to a lab or recitation partner or someone you’re used to working with in class.
If you do, a proctor may ask you to move.
You will need to bring a #2 pencil, a scientific calculator, and your student ID. NO OTHER DEVICES OR MATERIALS
WILL BE PERMITTED--THIS INCLUDES CELL PHONES, TABLETS, HEADPHONES, TEXTBOOKS, AND
HANDOUTS (INCLUDING ANY FREE EXAM QUESTIONS). If your calculator has any
notes programmed into it, you will need to delete them. If you need a device to keep track of time, bring a watch since
cell phones will not be allowed. If you do not know what your Affiliate ID is, ask your TA or instructor well in advance
of the exam. During the exam, please help the proctors avoid all suspicion by not leaving your Scantron and test
booklet within site of your neighbors.
Early exams are only possible for those with a very good, documented reason for missing the regular time. If you feel that
you fall in this category, you must make arrangements with Dr. Briggs at least 5 days in advance and be prepared to
present appropriate documentation (such as an official university letter) to support your absence at the normal time.
Keep in mind that those taking an early exam are putting themselves at a disadvantage, as they will not benefit from the
latest lecture material or review sessions. Late exams are not possible under any circumstances.
Specific exam topics (broken down by chapter) are listed below:
1
,Dr. Ron Briggs CHM 113
Chapter 10 (Gases)
What you should know for this test:
Properties of a gas
The 4 variables that describe a gas (P, V, T, and n) including their meanings, most common units, and how
to interconvert between units
The meaning of Standard Temperature, Standard Pressure, and STP
Conceptual relationships between P, V, T, and n according to Boyle’s Law, Charles’ Law, and Avogadro’s
Law (i.e. which variables are inversely and directly proportional)
How to use the Ideal Gas Law to solve numerical problems
How to use the Ideal Gas Law to solve for mass, initial/final values when a gas undergoes a change in P,
V, T, and gas density
The differences between a Real and an Ideal Gas
Limitations of the Ideal Gas Law and the assumptions made
How to use the Van der Waals equation to calculate gas variables and the significant differences from the
Ideal Gas Law
When and how to use Dalton’s Law of Partial Pressure
How to solve stoichiometry problems in the gas phase
Definition and five key points of the Kinetic-Molecular Theory (KMT)
The relationship between pressure and collisions
The relationship between temperature and average speed and kinetic energy
The meanings of effusion and diffusion and what factors affect each
What will not be on this test:
N/A
Chapter 11 (Intermolecular Forces)
What you should know for this test:
Meaning of intermolecular forces (and the difference from intramolecular forces)
What a dipole-dipole interaction is and how to predict the relative strengths of such an interaction
What London Dispersion Forces are and how to predict the relative strengths of such interactions
What a hydrogen bond is and when they can occur
Unique properties of water as a result of hydrogen bonding and geometry
Relative strengths of different intermolecular forces
Properties of the three phases of matter and how they relate to intermolecular forces
The relationship between heat, kinetic energy, and phases at the molecular level
Meaning of boiling point, melting point, vapor pressure, freezing point, surface tension, viscosity, and
critical temperature and pressure and how they can be predicted with intermolecular forces
How to interpret a simple phase diagram—what each region is and where the critical and triple points lie
Some of the interesting properties of H2O and CO2 and how they relate to IM forces and phase diagrams
What will not be on this test:
Section 11.7 (Liquid Crystals)
Chapter 13 (Solutions) – Selected Topics
What you should know for this test:
What a solution is
How to recognize the solute and solvent in a solution and the special name given to a solution in water
The three steps involved in forming a solution and that they occur simultaneously
How energy input/release is related to solvation and how to predict if an solution will form based on
energy considerations
The meaning of entropy and how it changes when a solutions is formed
How to predict solubility based on the type of solvent and solute
2
, Dr. Ron Briggs CHM 113
Review Qualitative (dilute, saturated, etc.) and Quantitative (volume %, molality, etc.) representations of
solubility from Ch. 4 Lecture Notes. Molality (m) is important in the colligative property equations
The effect of temperature and pressure on solubility in a gas and liquid
The meaning of a “Colligative Property”
Vapor Pressure Lowering, Boiling Point Elevation, Freezing Point Depression and Osmotic Pressure
What will not be on this test:
Section 13.6 (Colloids)
3
Exam 4 Study Guide
The exam will cover Chapters 10, 11 and 13 and all material covered in lecture. Specific material from your lab
experiments will not be tested on this exam, but the concepts presented during your lab sessions tie in closely with the
lecture material. At least a few questions will be taken directly from your online HW and recitation activities.
A practice exam is attached. As stated in the syllabus, you should use practice exams as practices of real exams. In
other words, study as you would for a real exam, sit down with nothing but a pencil and a calculator, and give yourself 75
minutes to complete it. This should be a good indicator of how you will do on the real thing and give you clues on what
to brush up on. These questions are also different from doing problems in the book in that they are not
“compartmentalized” in such a way that you know exactly what section of the book to look at to solve them. The practice
exam includes a Periodic Table and Equation sheet, which are identical to what will be included on the actual exam.
In addition to the attached practice exam, your lecture notes, lecture quizzes, handouts, recitation activities, and assigned
homework questions are valuable study aids. As always, copies of all quizzes and handouts are available in the
‘Content/Handouts’ section of Blackboard.
Need help? Take advantage of TA and instructor office hours. Chad (our former LRC Manager) has some helpful review
sessions posted online at http://www.chadsreview.org. The site is free, but does require registration. Once you're logged
in, the review sessions are posted by chapter in the "Videos" section. Review sessions are also being planned by Dr. Timo
Park (one of our lead recitation instructors) and the University Academic Success Program (UASP) at the following times:
Timo’s Exam 4 Review: Monday (12/1) from 4:30-6:30 PM in PS H-135
Lin’s Exam 4 Review: Wednesday (12/3) from 7:00-8:00 PM in PS A-203
UASP Exam 4 Review: Tuesday (12/2) from 7:00-8:00 PM in PS H-153
Your SI leader may also be planning additional review sessions. They will send email announcements as appropriate.
* DISCLAIMER: Dr. Briggs does not prepare or run these sessions (he has already prepared a practice exam and study
guide for you). Any material presented is the responsibility of the person running the session. If you have any questions
about this material, please ask them. Supplemental materials from other sessions will not necessarily be posted on
Blackboard.
Exam 4 is Thursday, December 4th (the last day of lecture) in the normal lecture room (PS H-150) at the normal lecture
time. The exam will begin promptly at the start of class and you will have the entire period to complete it. Please
show up on time and do not sit next to a lab or recitation partner or someone you’re used to working with in class.
If you do, a proctor may ask you to move.
You will need to bring a #2 pencil, a scientific calculator, and your student ID. NO OTHER DEVICES OR MATERIALS
WILL BE PERMITTED--THIS INCLUDES CELL PHONES, TABLETS, HEADPHONES, TEXTBOOKS, AND
HANDOUTS (INCLUDING ANY FREE EXAM QUESTIONS). If your calculator has any
notes programmed into it, you will need to delete them. If you need a device to keep track of time, bring a watch since
cell phones will not be allowed. If you do not know what your Affiliate ID is, ask your TA or instructor well in advance
of the exam. During the exam, please help the proctors avoid all suspicion by not leaving your Scantron and test
booklet within site of your neighbors.
Early exams are only possible for those with a very good, documented reason for missing the regular time. If you feel that
you fall in this category, you must make arrangements with Dr. Briggs at least 5 days in advance and be prepared to
present appropriate documentation (such as an official university letter) to support your absence at the normal time.
Keep in mind that those taking an early exam are putting themselves at a disadvantage, as they will not benefit from the
latest lecture material or review sessions. Late exams are not possible under any circumstances.
Specific exam topics (broken down by chapter) are listed below:
1
,Dr. Ron Briggs CHM 113
Chapter 10 (Gases)
What you should know for this test:
Properties of a gas
The 4 variables that describe a gas (P, V, T, and n) including their meanings, most common units, and how
to interconvert between units
The meaning of Standard Temperature, Standard Pressure, and STP
Conceptual relationships between P, V, T, and n according to Boyle’s Law, Charles’ Law, and Avogadro’s
Law (i.e. which variables are inversely and directly proportional)
How to use the Ideal Gas Law to solve numerical problems
How to use the Ideal Gas Law to solve for mass, initial/final values when a gas undergoes a change in P,
V, T, and gas density
The differences between a Real and an Ideal Gas
Limitations of the Ideal Gas Law and the assumptions made
How to use the Van der Waals equation to calculate gas variables and the significant differences from the
Ideal Gas Law
When and how to use Dalton’s Law of Partial Pressure
How to solve stoichiometry problems in the gas phase
Definition and five key points of the Kinetic-Molecular Theory (KMT)
The relationship between pressure and collisions
The relationship between temperature and average speed and kinetic energy
The meanings of effusion and diffusion and what factors affect each
What will not be on this test:
N/A
Chapter 11 (Intermolecular Forces)
What you should know for this test:
Meaning of intermolecular forces (and the difference from intramolecular forces)
What a dipole-dipole interaction is and how to predict the relative strengths of such an interaction
What London Dispersion Forces are and how to predict the relative strengths of such interactions
What a hydrogen bond is and when they can occur
Unique properties of water as a result of hydrogen bonding and geometry
Relative strengths of different intermolecular forces
Properties of the three phases of matter and how they relate to intermolecular forces
The relationship between heat, kinetic energy, and phases at the molecular level
Meaning of boiling point, melting point, vapor pressure, freezing point, surface tension, viscosity, and
critical temperature and pressure and how they can be predicted with intermolecular forces
How to interpret a simple phase diagram—what each region is and where the critical and triple points lie
Some of the interesting properties of H2O and CO2 and how they relate to IM forces and phase diagrams
What will not be on this test:
Section 11.7 (Liquid Crystals)
Chapter 13 (Solutions) – Selected Topics
What you should know for this test:
What a solution is
How to recognize the solute and solvent in a solution and the special name given to a solution in water
The three steps involved in forming a solution and that they occur simultaneously
How energy input/release is related to solvation and how to predict if an solution will form based on
energy considerations
The meaning of entropy and how it changes when a solutions is formed
How to predict solubility based on the type of solvent and solute
2
, Dr. Ron Briggs CHM 113
Review Qualitative (dilute, saturated, etc.) and Quantitative (volume %, molality, etc.) representations of
solubility from Ch. 4 Lecture Notes. Molality (m) is important in the colligative property equations
The effect of temperature and pressure on solubility in a gas and liquid
The meaning of a “Colligative Property”
Vapor Pressure Lowering, Boiling Point Elevation, Freezing Point Depression and Osmotic Pressure
What will not be on this test:
Section 13.6 (Colloids)
3
