CHEM 5013
REVIEW SHEET
EXAM #3
Chapter Six – The Periodic Table and Atomic Structure
 [6.2] Wave Theory of Light – Know the definitions of frequency, wavelength, amplitude
of a wave
 [6.2] Electromagnetic Spectrum – Understand the relationships between frequency
and wavelength. You need to know the formula c=λν. I will provide the
value of c (Speed of light in a vacuum).
 [6.2] Energy (particle) Theory of Light – Understand the relationships between
frequency, wavelength, and energy. You need to know the formula E=hν. I
will provide the value of Planck’s Constant (h).
 [6.3] Atomic Spectra – Definitions of Continuous Spectrum and Line Spectrum,
Ground State and Excited State (Spec 20 Lab)
 (6.4) Quantum Numbers – We discussed four different ones – These are the addresses
or locations of electrons
 (6.4) Analogy: Road or street = Shell, House = Subshell, Room = Orbital
 (6.4) Limitations on number of subshells in a shell or on number of orbitals in a
subshell or number of electrons in an orbital
 (6.5) Pauli Exclusion Principle – Understand and be able to apply to a given orbital
diagram or electron configuration
 (6.5) Write the Complete Electron Configuration for an Element using Building Up
Principle (Aufbau’s Principle) or the Periodic Table
 (6.5) Write an Electron Configuration Using the Periodic Table – What are the
different “blocks” on the table?
 (6.5) Draw an Orbital Diagram for an Element
 (6.5) Definitions of Valence Electrons vs. Core Electrons
 [6.5] Write the Shorthand Electron Configuration for an Element (Noble Gas Core)
 (6.5) Understand and Apply Hund’s Rule to Provide the Lowest Energy Level
Configuration of Electrons in an Element
 [Lab] You need to know the formula ABS = 2-log(%T) and how to use it.
 [Lab] There will be some type of question where you will have to interpret a plot of %T
vs. wavelength to determine the likely color of a material as in the Spec-20 lab.
 [Lab] There will also be some type of question where you will have to use a Beer’s Law
Plot to estimate the concentration of a solution of a chemical as you did in lab.
You WILL NOT have to perform linear regression analysis.
Chapter Seven – Chemical Bonding and Molecular Structure
 (7.2) Ionic Bonds are formed between Metals and Non-Metals (Cations and Anions)
 [7.2] Use the Periodic Table to determine the charges on ions and how they react with
one another
 [7.2] Use Lewis Diagrams of elements and ions to pictorially show the transfer of
electrons to form an Ionic bond and ions of Noble Gas configuration
 [7.3] Lewis Electron Dot Symbols of Elements and Ions
 [7.3] Covalent bonds are formed between non-metals and involve the sharing of
electrons equally between both elements
 [7.3] Definition of bonding pairs and lone pairs of electrons
 [7.3] Use Lewis Diagrams of elements to pictorially show how a covalent bond is
created in a molecule by sharing electrons between atoms
 [7.5] Draw Lewis Structures for various molecules and polyatomic ions
Chapter Five – Gases
 [5.1] Basic properties of gases (Definition of a gas)
 [5.2] Pressure
o Definition of Pressure = Force per unit area
o Converting between various units of pressure – Conversion factors will be
provided
 [5.3] History and Application of the Gas Law
o Empirical Gas Laws (KNOW THESE!!!) – Recall that all temperatures MUST
be converted to Kelvin units first!!!
 Boyle’s Law: P1 V1 = P2 V2 (at constant T and constant moles)

Charles’s Law: V1/T1 = V2/T2 (at constant P and constant moles)

Combined Gas Law: P1V1/T1 = P2V2/T2 (for a given # moles of gas)

Avogadro’s Law:
Vm=specific constant = 22.41 L/mol at STP
 [5.5] STP = Standard temperature and pressure = 1 atm and 0°C (273K)
 [5.3] The Ideal Gas Law PV=nRT (where n = Number of moles of GAS) – THIS WILL
NOT BE GIVEN TO YOU FOR THE EXAM, YOU MUST MEMORIZE IT!
 [5.5] Stoichiometry of Reactions Involving Gases
 Combining Gas Law with Stoichiometry fundamentals from Chapter 4
 Make sure you understand the calculations from the Ideal Gas Law Lab!
 Determining the density of a gas. – One approach is to assume the volume is one
liter, use Ideal gas Law to calculate the moles of gas per liter, then convert moles
to grams per liter = Density.
 [5.4] Dalton’s Law of Partial Pressures; Gas Mixtures
PT=PA+PB+…
Also understand that each gas in a mixture individually follows the Ideal Gas Law.
Chapter Thirteen – Electrochemistry
 [13.2] Definitions of Oxidation (losing electrons, oxidation number rises) and
Reduction (gaining electrons, oxidation number is lowered)
 Calculating Oxidation numbers for a species
 [13.2] Definitions of Oxidizing Agent and Reducing Agent
 [13.2] Be able to write oxidation half-reactions and reduction half-reactions
 [13.2] Understand the basic construction of a Galvanic cell including the parts (Salt
Bridge, Anode=oxidation side and Cathode=reduction side)
 [13.2] Write out cell notation for a galvanic cell given a reaction and write out a
reaction given the cell notation
 [13.3] Cell Potentials – understand how to use the provided Table of Reduction
Potentials and how to calculate a Cell Potential for a galvanic cell
(E0cell = E0red – E0ox)
Rules for Exam
1. You obviously will need your calculators.
2. You will be provided with a reference sheet identical to the one given to you in class
as well as a Periodic Table.
3. No other outside sources or information allowed.
Advice
Study the suggested problems on the website and the quizzes – many problems will
be similar to the problems on these.