Download Intermolecular Forces (Chapter 16)

List of Topics to Review for the Final Exam*
Covalent Bonding: Orbitals (Chapter 14, sections 1-6)
 Lewis structures, shapes, hybridization
 Molecular orbital diagrams (with and without s-p mixing; diatomic molecules and ions)
 Bond order (calculate it and use it to determine relative bond strength and length)
 Magnetism (paramagnetic vs. diamagnetic)
 Lab 1
Kinetics (Chapter 15, all sections)
 Rate expressions
 Method of initial rates
 Differential rate laws
 Integrated rate laws and half-lives
 Pseudo-rate laws and pseudo-rate constants
 Mechanisms; intermediates; steady-state approximation
 Temperature dependence of rate constant - Arrhenius equation (activation energy)
 Catalysis
 Lab 2
Intermolecular Forces (Chapter 16, sections 1, 2, 10, and 11)
 Given a series of molecules, know how to predict which will have the highest/lowest boiling point,
vapor pressure, etc. by taking into account the dominant intermolecular forces involved (H-bond,
dipole-dipole, ion charge-dipole charge, dispersion).
 Given a molecular formula, know how to determine what type of bonding/intermolecular forces
will be important in determining solution or solid state properties.
 Vapor Pressure & Hvap of pure liquids
 Obtaining Hvap from Pvap vs Temp data (Clausius-Clapeyron equation)
 Changes of state, phase diagrams, and enthalpies of phase changes
 Lab 3
Solid State Structures (Chapter 16, sections 3-9)
 Given a series of elements, compounds, or molecules, be able to predict which will have the
highest/lowest boiling point, melting point, etc. based on what you know about bonding in liquids
and solids
 Know the differences between ccp/fcc, hcp, bcc, and sc
 Given a solid state packing structure (fcc, bcc, sc, hcp), know how many atoms or formula units
are contained in the unit cell.
 Density – radius – edge length – packing efficiency – number of atoms in a unit cell (be able to
work with these measurements)
 Ionic Solids (tetrahedral/octahedral holes and molecular formula)
 Alloys, semiconductors, doped semiconductors, conductors, and p-n junctions
Properties of Solutions (Chapter 17)
 Concentration measurements: molality, molarity, mole fraction, % by mass, % by volume
 Thermodynamics of solution formation (Hsoln, Hhyd, Hlattice)
 Predicting relative solubilities of substances
 Henry’s Law & solubility of gases
* While this a very full list, it’s always possible that I’ve overlooked something when putting this
together. I suggest that you carefully review your class notes, HWs, quizzes, and labs, and be sure you
have read the chapters as well.
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Effect of temperature on solubility
Vapor pressure lowering & Raoult’s Law (including calculations involving volatile substances)
Boiling Point Elevation, Tb
Freezing Point Depression, Tf
Osmotic Pressure, 
Determining MM from Osmotic Pressure, Tb, or Tf
Colligative Properties of Ionic and Non-Ideal Solutions
Lab 4
The Representative Elements of the Periodic Table (Chapter 18)
 Periodic trends in atomic size, ionization energies, electronegativities, metallic properties, melting
points, reducing/oxidizing abilities, etc. and the reasons for any anomalies in the trends
 Location of metals vs nonmetals vs metalloids
 Typical structures/hybridization of molecules containing elements from the various groups
 Oxidation states of elements in various compounds
 Chemistry, properties, characteristic reactions of, and important uses/roles of
o Hydrogen, Alkali Metals, and Alkaline Earth Metals (Groups 1 and 2)
o Boron, Carbon, and Nitrogen families/groups (Groups 3, 4, and 5)
o Oxygen and Halogen families/groups (Groups 6 and 7)
 Lab 5
Transition Metals and Coordination Chemistry (Chapter 19)
 Electron configurations and periodic trends within the first-row transition metal elements and their
ions
 Coordination compounds (naming/formulas, electron configuration of metal ions, coordination
numbers, ligands)
 Isomerism (classes of isomers; recognizing cis/trans or chiral isomers)
 Crystal Field Model (d-orbital splitting patterns and calculation of E; colors (absorbed and
observed) and magnetism)
 Biological importance of TMs and coordination complexes
 Lab 6
Organic and Biochemical Molecules (Chapter 21)
 Naming/drawing: alkanes, cyclic alkanes, alkenes, alkynes, and aromatic hydrocarbons, as well
as the alkyl substituents (know the systematic naming rules; for the alkyl substituents in Table
21.2, also know the common names)
 Isomers among organic molecules, both structural and stereoisomers
 Primary, secondary, and tertiary (know what these tell you about the atom(s) they are describing)
 Types of organic reactions (the three kinds we discussed)
 Recognizing, identifying, drawing, and naming functional groups within organic molecules
 Polymers (types of polymers and types reactions that create polymers)
* While this a very full list, it’s always possible that I’ve overlooked something when putting this
together. I suggest that you carefully review your class notes, HWs, quizzes, and labs, and be sure you
have read the chapters as well.