This document provides an overview and review of topics for the CHEM 111 exam. It outlines basic concepts from CHEM 101 like moles, molarity, and Lewis structures that will be important. Example problems are provided for calculating moles and experimental techniques like acid-base titrations, determining cations and anions, gas laws, and drawing Lewis structures are reviewed. The document concludes by advising students on effective exam preparation strategies.

1. CHEM 111
REVIEW SESSION
FALL 2011
STELLA KRITIKOU
SECTIONS 480, 517, 556

2. BASIC THINGS YOU NEED
TO KNOW FOR MOST
EXPERIMENTS
MAKE SURE YOU STUDY &
REVIEW
BASIC THINGS FROM CHEM 101
SUCH AS
Moles / Molarity / Molecular
Weight
Bond types / Valence Electrons
Electronegativity / Lewis
Structures

3. HOW TO CALCULATE THE NUMBER OF
MOLES
If you have a solution (therefore the volume and the
molarity/concentration of the solution is known)
n n
C n CV V
V C
Where C: the molarity/concentration of you solution (mol/L)
n: the number of moles (mol)
V: the volume of the solution in L (L)
If you have a solid compound (therefore the mass and the
molecular weight is known)
m
n m MW n
MW
Where n: the number of moles (mol)
m: the mass of your solid
Mw: the molecular weight of your solid

4. They might as well ask you something
more complicated:
Calculate the number of moles in 50g of HCl
solution, if d=1.048 kg/L and C=6M.
From the density I know that I have 1.048 kg HCl
per Liter. Notice that kg/L is the same as g/mL
Hence I can calculate the volume of my solution:
m m 50gHCl
d V V V 47.71mLHCl
V d gHCl
1.048
mLHCl

5. Now you have the Volume and the Molarity and
you can calculate the number of moles.
DON’T FORGET TO CHANGE THE VOLUME IN L!
47.71mLHCl
47.71mLHCl LHCl 0.04771LHCl
1000mLHCl
n molHCl
C n CV N 6 0.04771LHCl 0.28626molHCl
V LHCl

6. Calculate the number of moles in 50g of
10% w/w HCl solution.
Step 1:
The HCl solution is 10% w/w,
meaning that in 100 kg (or g) of the solution
I have 10 kg (or g) of HCl acid.
Therefore my solution contains:
10gHCl
50gSolution 5gHCl
100gSolution

7. Step 2:
Now you have the mass of the HCl acid (5g) and
you can easily calculate the Molecular weight:
gHCl
MW AW (H ) AW (Cl) 1 35.45 36.45
molHCl
Step 3:
Now you are ready to calculate the number of
moles:
m 5gHCl
n n n 0.137molHCl
MW gHCl
36.45
molHCl

8. Now.. Let’s move on to the
main subject!

9. Experiments / Exercises
The chemistry of recycling
The graphical depiction of Scientific Data
Acid Base Chemistry
Project 2 (cations, anions and unknown)
Enthalpy determination
Gas Laws
Scientific Literature
From Atoms to molecules

10. Chemistry of Recycling
Balance chemical equations
Write net ionic equations
Write total ionic equations
Figure out the type of the
reaction
Calculate the theoretical yield
Calculate the percent yield

11. Graphical Depiction of Scientific
Data
You should be able to determine what type of
chart you should use every time
Remember:
in chemistry, we don’t use pie charts and bar/column charts
often, because it is common to have correlation between the
quantities measured.
You should be able to tell if the trendline given
represents the data accurately or not (and how
this reflects on the R-squared value)
You should be able to tell the relationship
between two quantities, when the graph (with or
without the trendline) is given

12. Acid-Base Chemistry
You should know the most common acids and bases
that we used in the Lab. (eg you should know that
NaOH is a base and HNO3 is an acid etc)
Different types of titration
The importance of the indicator and the difference
between the final and the equivalence point
Review the mustard experiment

13. Project 2 : Determination of
an unknown ionic
compound
FROM PART I (CATIONS)
You should remember the most obvious (and easy)
things in the lab. For example that K+ didn’t precipitate
at any point, or that Cu2+ had the easiest flame test or
that Zn+ is the only amphoteric one.
Remember that the tests are based on the differences
in solubility between the cations
You should remember the two different elimination tests
that we performed & the confirmation test (flame test)

14. FROM PART II (ANIONS)
You should remember the most obvious (and easy)
things in the lab. For example that Cl- didn’t dissolve at
any point.
Remember that the confirmation tests are different for
each anion this time
You should remember the two distinct branches of the
logic tree

15. FROM PART III (UNKNOWN)
You should remember that the first thing you had
to do was to dissolve your compound
You should be able to figure at least one reason
for getting a false positive or negative result in
ANY case.

16. IN GENERAL
They might give you a logic tree and
observations and ask you to follow down the
tree.
They might give you a list with observations and
ask YOU to draw the logic tree
You should be able to go from data to logic tree
and back

17. Enthalpy Determination
Energy neither created or destroyed
Closed or open system
Heat flow of a system
Enthalpy of a chemical reaction
Memorize the basic relationships
MAKE SURE YOU KNOW HOW YOU DEFINE THE
SYSTEM AND HOW YOU DEFINE THE
SURROUNDINGS EVERY TIME

18. Heat flow & Molar enthalpy change
q mc
0 qP
n
First Law of Thermodynamics
quniverse qsystem qsurroundings 0
qsurroundings qsystem

19. Gas Laws: P, V, T
Ideal Gas Law
PV nRT
P = Pressure
V = Volume
n = number of moles
T = Temperature
R = ideal or universal Gas Constant
MAKE SURE YOU USE THE SAME UNITS
EVERYWHERE AND YOU USE THE CORRECT
VALUE FOR R (ACCORDING TO THE UNITS)

20. From the Ideal Gas Law you can determine
EVERYTHING! (REALLY E V E R Y T H I N G!!!)
Therefore you should know the relationship between
Pressure and Volume
Pressure and Temperature
Volume and Temperature
What happens to a system when you heat it up?
(Consider the kinetic energy of the system)
How can you calculate one of them when you are given
the rest of them?
How can you calculate one of them GRAPHICLY?

21.  It is possible that they will combine this
experiment with exercise 2.
 You might be given different graphs and asked
to calculate something or to determine the
relationship between the two quantities.
 You might be asked whether a given graph can
accurately describe the relationship between
two quantities.

22. Scientific Literature
Make sure you know what Peer-Reviewed
Sources are.
Make sure you know how to read a reference
Author(s)
Title
Year or date of the publication
Title of the journal where it was published
Volume and number (or issue) where the article was
printed
Page number

24. From Atoms to Molecules
Find the number of Valence electrons each time
Consider the charge of the molecule (if any)
Draw a “draft” Lewis structure
Consider the electronegativity of each one of the atoms
Assign partial charges accordingly
Figure out the molecular geometry
Draw a final Lewis structure (don’t forget the total
charge!)
Consider if there is an overall dipole or not
Remember if a molecule is more likely to intercalate or
bind to DNA

27. A word of advice! 
Don’t pull an all-nighter the day BEFORE the exam. It’s
not helpful if you’re sleepy!
Don’t assume that your exam will be the same as the
day before, because it WON’T
If you have absolutely NO CLUE about a problem don’t
try to guess; however if you know how to approach the
problem but you don’t know how to get to the final
answer go for it!
Eat something sweet before taking your exam (you
think it’s not working but .. It’s chemistry!)
Good luck !!