Chemistry 162:  Final Exam Study Guide

Instructor: Ken Marr
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Final Exam.  The final exam is comprehensive, covering chapters 7-13 and all labs performed during the quarter. However, almost half of the questions will be on material covered in lecture and lab since exam 2. If it helps your grade, your lowest exam score will be replaced with the percentage that you earn on the final exam. 

 

Bring the following with you to the final exam: 

  • Portfolio (due at the start of the exam): only include ALE's since exam #2 Portfolio Contents Sheet

  • Scantron card, #2 pencil and a good eraser. 

  • You may find a 3 x 5 inch "cheat sheet" helpful--bring one if you want.

Note: a periodic table and a sheet of equations, constants and other useful information will be provided (click here to see it)

Stuff to concentrate on while reviewing for the final exam:

Study Guide for Chapters 12-13 (Silberberg 4ed)

You might find the following study guide useful. It is adapted/stolen (with permission of course!!) from my colleague at GRCC, Roger Knutsen

  1. Terms/Concepts
    1. The Kinetic Molecular view of the three states of matter
    2. Vaporization, condensation, freezing, melting, fusion, and sublimation
    3. Phase diagram, triple point, critical point
    4. Simple cubic, body–centered and face–centered unit cells in crystal lattices
    5. Molarity, molality, percent by weight, percent by volume
    6. Colligative properties
    7. Entropy
  2. Skills/Background Knowledge
    1. Use phase diagrams to determine the conditions under which phase changes will occur
    2. Construct phase diagrams from the appropriate physical data
    3. Describe the nature of the intermolecular forces ion–dipole, dipole–dipole, hydrogen bonds, ion–induced dipole, dipole–induced dipole, and London
    4. Discuss the relationship between DHvap, DHfus, and DHsubl and the processes involved in phase changes
    5. Describe the forces that hold atomic, molecular, ionic, metallic and network covalent solids together
    6. Describe our model for how water dissolves ionic substances, and use simple drawings to depict the process as well as our molecular view of ions in solution
    7. Perform calculations involving the concentration of solutions, using molarity, molality, percent by weight, percent by volume, mole fraction
    8. Discuss the relationship between DHsoln and the solubility of a compound, and the importance of entropy in understanding why substances dissolve even when the process is endothermic
    9. Describe solubility as an equilibrium process
    10. Perform calculations involving freezing point depression and boiling point elevation
  3. Problem Solving Abilities & Application of Principles
    1. Apply concepts related to intermolecular attractions to explain the processes involved in changes of state, as well as surface tension, viscosity and the formation of solutions
    2. Apply concepts of hybridization and bonding, polarity, and hydrogen bonds to explain the unique properties of water
    3. Calculate the properties of unit cells, such as cell size, number of atoms, atomic mass, empirical formula and density
    4. Apply concepts related to intermolecular interactions to predict/explain why a solute would be soluble, or insoluble, in a solvent
    5. Apply concepts related to intermolecular interactions to explain the effect solutes have on the solvent properties of vapor pressure, boiling point, melting point, and osmotic pressure
    6. Calculate the freezing point and boiling point of solutions containing a molecular or ionic solute. 
    7. Calculate the molar mass of a solute from freezing point depression data.

© Kenneth R. Marr 2001