CHEM 1220 Exam #3 Study Guide

The following topics are fair game for the CHEM 1220 Exam #3 for Spring 2013. Under each topic there are practice problems from the text to help you study for the exam. These questions can also be found on Mastering Chemistry in teh Exam #3 Practice Problems assignment.

The Chem 1220 Exam #3 useful Information sheet attached to the exam is the same document attached to last exam.

Section 19.1
Spontaneous Processes
Be able to distinguish between a spontaneous process, reversible process, irreversible process, and isothermal process.

Section 19.2
Entropy and the Second Law of Thermodynamics
State the second law of thermodynamics and describe the notion of entropy. Be able to justify how/why the entropy of the universe increases in a spontaneous process.

Section 19.3
Molecular Interpretation of Entropy
Explain how the entropy of a system is related to the number of possible microstates and describe the kinds of molecular motion that a molecule can possess. Be able to use the concepts of microstates and molecular motion to make qualitative predictions about entropy.

Section 19.4
Entropy Changes in Chemical Reactions
Predict the sign of the entropy change for physical and chemical processes.
19.3, 19.4, 19.43, 19.47, 19.48, 19.49

Section 19.5
Gibbs Free Energy
Be able to calculate changes in entropy, or changes in Gibbs free energy, for chemical reactions to determine if a reaction is spontaneous.
19.53, 19.54, 19.59, 19.61

Section 19.6
Free Energy and Temperature
Recognize how changing the temperature influences the spontaneity of a reaction and predict which temperatures a reaction will be spontaneous given the change in enthalpy and the change in entropy.
19.66, 19.67, 19.69, 19.71

Section 19.7
Free Energy and Temperature
Be able to calculate ΔG under non-standard conditions and recognize how ΔG changes when the partial pressures of gases are not equal to one atmosphere and the concentration of solutions are not one molar.

Relate Gibbs free energy to the equilibrium constant and understand how the magnitude of K relates to spontaneity.
19.77, 19.81, 19.99

Understand the molecular interpretation of entropy, and how it relates to the 2nd law of thermodynamics.
19.27, 19.37, 19.43

Laboratory experiment #22 Solubility and Determination of ΔG, ΔH and ΔS of Ca(OH)2
Understand calculations & concepts.

Section 20.1
Oxidation States and Oxidation-Reduction Reactions
Be able to determine the oxidation states of all species in an electrochemical reaction in order to identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent based on standard reduction potential data or reactivity.
20.6, 20.43, 20.47

Section 20.2
Balancing Redox Reactions
Complete and balance redox equations using the method of half-reactions in both acidic and basic solutions.
20.21, 20.23

Section 20.3
Voltaic Cells
Sketch a voltaic cell and identify its cathode, anode, and the directions that electrons and ions move.
Be able to visualize the change in mass at the anode/cathode and the change in concentrations in the anode/cathode compartment at the molecular level.
20.8, 20.27, 20.37, 20.39

Section 20.4
Cell Potentials Under Standard Conditions
Calculate standard cell potentials (emfs) from standard reduction potentials.

Use reduction potentials to predict whether a redox reaction is spontaneous and to determine the relative strengths of oxidizing and reducing agents.

Understand the terms standard reduction potential and the operation of a standard hydrogen electrode.
20.33, 20.34

Section 20.5
Free Energy and Redox Reactions
Related the standard cell potential to the standard free energy change and the equilibrium constant.

Section 20.6
Cell Potentials Under Nonstandard Conditions
be able to apply the Nernst equation to determine the cell potential under non-standard conditions and relate the standard cell potential to the standard free energy change and the equilibrium constant.
20.65, 20.69, 20.72

Section 20.6
Cell Potentials Under Nonstandard Conditions
Electrolysis in non-aqueous and aqueous systems.
20.89, 20.90, 20.109

Section 20.8
Be able to apply concepts of spontaneous electrochemical processes to explain how corrosion is prevented by cathodic protection.
20.84, 20.85

Section 20.9
Describe the reactions in electrolytic cells and relate amounts of products and reactants in redox reactions to electrical charge.

Laboratory experiment #23 Electrochemistry
Understand calculations & concepts.

Section 23.1-23.2
Transition Metal Complexes
Determine the oxidation number and number of d electrons for metal ions in complexes and determine the coordination number about the central atom and geometry of the transition metal complex.
23.15, 23.23, 23.25, 23.29

Section 23.4
Isomerization in Coordination Chemistry
Recognize and draw the structural and stereoisomers in a transition metal complex.
23.5, 23.6, 23.39, 23.40

Section 23.4
Isomerization in Coordination Chemistry

Section 23.6
Crystal-Field Theory
Be able to interpret crystal-field splitting diagrams for octahedral, square-planar & tetrahedral geometries, and for weak and strong field ligands. Understand the terms high spin and low spin.
23.8, 23.47, 23.59, 23.63.

Use crystal-field theory to explain color in coordination compounds.
23.51, 23.53, 23.54

One Response to CHEM 1220 Exam #3 Study Guide

  1. Lauren O'Brien says:

    Dr. Fus-
    Lauren O’Brien here. We met when you spoke at a Pearson event about a month ago. You had interest in coming to Auburn. Would love to talk with you about doing so. My email is lauren.o’ or 404-422-5501.


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