Chemistry 111: Final Exam Topics
The final exam is comprehensive – covering the whole quarter. An approximate
breakdown is as follows:
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Multiple Choice (160 points):
o Roughly 2/3 based on older material (Topics from Exams 1–3)
o Rest based on new material – Chapters 16, 17, 18
Lab – related question (short answer= 40 points):
o ½ (20 points) based on lab questions from Exams 1-3.
o ½ (20 points) based on the Titration & Beer’s Law labs.
Chapter 17: Net Ionic Equations
Chapter 18: Acid – Base Reactions
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“Electrolyte,” how these solutions conduct
electricity.
Write total ionic equation, then cancel the
“spectator ions” to get a net ionic equation
Solubility Rules & precipitation reactions
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Definition – Arrhenius & Bronsted (Not Lewis)
Recognize Acids & Bases (from formula)
Water as an acid/base (amphoteric)
Water, Kw, and calculating [H+] & [OH-]
Calculate pH, pOH & relationship between them.
Weak Acids & Bases, Conjugate Acids & Bases.
Chapter 2
Chapter 10
This is mostly science vocabulary!
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Scales in Science – Fig 2.1
States (s/l/g)
Review Goals – Page 36
Review Vocabulary – Page 37
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Electromagnetic spectrum (understand):
Continuous spectrum vs. line spectrum
“Quantized”
Quantum Model – slides from Monday are
good…
Valence electrons. ns2np6 notation
Ionization Energy
Vocabulary from end of chapter.
Chapter 3
Chapter 11
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Scientific Notation
Scientific Notation & the EE/EXP button on your
calculator.
Given factors (the table I gave you or given in the
problem), find a unit path & do a conversion.
NOTE: you don’t get the metric prefixes –
memorize them.
Metric Units for mass, volume, length
Significant Figures
o understand concept
o Do the math (rules for + & -,  & )
o Know how to round
Density = Mass  Volume
Convert °F  °C  K (equations might be
given)
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Monatomic Ions
Ionic Bonds
Covalent Bonds
Covalent Bond Polarity
Multiple Bonds
Octet Rule Exceptions.
Chapter 5
Chapter 12
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Dalton’s Rules
Protons, neutrons, electrons.
Plum Pudding & Nuclear Model,
Rutherford Experiment & it’s conclusions
Isotopes, Nuclear Symbols
Average Atomic Mass (weighted sum)
AMU vs. g/mol
Periodic Table Trends
Chapter 6
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Names of Cations for elements (metals)
Names of Anions for element (nonmetals)
Names of covalent compounds from formula
Formulas of covalent compounds from name.
Names of ionic compounds  Formula of ionic
compounds.
Transition metal ions:
o Formula from Stock system name for any
element
o ion from stock system name for any element
o know charges of selected elements (see class
notes)
o Common names (ferric ion = Fe3+, ferrous =
Fe2+)
o Understand Hg2+ = mercury(II) ion, Hg22+ =
mercury(I) ion
Polyatomic Ions
o Oxyanions
o CN-, CH3COO-, …
o H3O+, NH4+
o HPO42-, HCO3-, …
Some common names: NH3, H2O
Oxyacids – HNO3 = nitric acid (-ate-ic, …)
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Be able to draw a Lewis structure.
Molecular Geometry
o How many VSEPR pairs (electron domains
are there?)
o What is the VSEPR shape?
o What is the angle?
o What is the molecular shape (when there
are lone pairs)
o What is the angle when there are lone pairs?
Bond Polarity (applied to next item)
Molecular Polarity
o Sum up the bond dipoles to decide if a
molecule is polar.
o Good examples: CH4, CH2F2, CO2, H2S, CH3F
Chapter 4
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Understand kinetic theory – explain
pressure/temp/volume based on molecular
collisions
Understand how to read a barometer
Understand how to read a manometer
Be able to convert pressure units
Remember to use Kelvin!
Understand what’s held constant in Boyle’s Law,
Charles’ Law
Use combined gas law (P1V1/T1=P2V2/T2 is
given).
Chapter 13: Ideal Gas Law (PV=nRT)
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Recognize that you have to solve this type of
problem – should have 4 out of 5 gas variables.
Set up a table to solve the problem!
Be able to use equation for gas density.
Use n=PV/RT for stoichoimetry (ugh)
Sometimes cheat - @ STP have 22.4 L/mol of any
gas
Chapter 7
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Calculate molecular weight
Understand moles.
Determine % composition
Determine empirical formula from %
composition
(for above 2, use my table method!)
Chapter 15: Gases, Liquids & Solids
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Chapter 8
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Balance chemical equations
Write chemical equations from descriptions.
Get mole ratios from balanced equations
Partial Pressure
Intermolecular Forces (IMF)
o Dipole-Dipole
o London Dispersion (Induced Dipole)
o Hydrogen Bond
o Figure 15.9!
Know viscosity, boiling point, Hvap, surface
tension, vapor pressure.
Relate the above to IMF
Types of solids – what holds them together
(ionic bond, covalent bond, or IMF?)
Calculate heat for temperature
changes.
Know reactions from in class
Chapter 9
Chapter 16: Solutions
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Mass calculations (massmolesmolesmass)
You will have the map on the exam cover sheet!
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Find % yield
Use % yield as a conversion factor
Vocabulary
Formation of a solution – NaCl  hydrated Na+ &
Cl IMF & Solubility
 Concentration Units
o % (g/100g)
o ppm (mg/L)
o Molarity (mol/L)
 Dilution (M1V1=M2V2)
 Solution Stoichiometry – Conc (M)  Volume (L) =
moles
 Titration (2 cases only):
o Easy – 1:1 stoichiometry, M1V1=M2V2
Lab: 1:1 stoich, find MW