Type:
Solution Manual
Resource:
General Chemistry Atoms First Plus MasteringChemistry
Edition:
2nd Edition
Author(s):
John E. McMurry
To the Instructor: When looking through the instructor versions of the other laboratory manuals currently available, my first thought was that I wouldn’t have time to wade through even 10 percent of the material contained within them. The instructor versions often contained detailed discussions of concepts I didn’t need (I have a degree in chemistry too) and redundant materials already available in the student manual. The instructor versions also seemed to lack the kind of information that I would really like to have, e.g., potential problems that can occur when the students performed the experiments or notes on points to stress that I could give to my teaching assistants. So when designing this instructor manual, I tried to include all of the information and materials I would like to have and left out those materials that seemed unnecessary. For each experiment in the lab manual you will find the following in the instructor version:
A list of chemicals, equipment, and supplies Preparation instructions for chemicals and reagents as needed A discussion of points to stress and potential problems to be aware of when performing the experiments A key for the pre-laboratory assignments A key for the post-laboratory assignments
The keys provided do not include a grading scale as I believe that different instructors will want to emphasize different portions of the assignments and reports. The reports in the manual are already delineated as to what the students should be including and will be based on their experimental data so there is no key provided for them beyond the identity of unknowns etc. It is my hope that you find this instructor manual concise, to the point, and above all, useful. If I have been remiss in including anything that you feel would help, please let me know. If you need any further assistance or have suggestions or comments regarding the use of the manual, the performance of the experiments, or the use of the keys please do not hesitate to contact me. Stephanie R. Dillon Coordinator General Chemistry Laboratories Florida State University sdillon@chem.fsu.edu
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Table of Contents To The Instructor 0)
Part A. Measurement and Expression of Experimental Data Part B. Graphing and Statistical Analysis A math review, including practice with significant figures, rounding rules, graphing techniques, and statistical analysis.
1)
Conservation of Matter A reaction of copper nitrate and zinc is observed to determine if mass is conserved.
2)
Atomic Spectra Several unknown light sources are identified by use of spectrometry.
3)
Halogen Reactions Hexane and water are used to determine the solubility of the halogens and halides.
4)
Paper Chromatography: An M&M’s® True Colors Paper chromatography is used to analyze the food colorings used in M&M’s candy shells.
5)
Molecular Models Lewis structures are presented in model form and investigated.
6)
Limiting and Excess Reagents Copper nitrate and potassium iodide are reacted at different concentrations to determine which is the limiting reagent and which is in excess.
7)
Redox Reactions in Voltaic Cells: Construction of a Potential Series Micro-scale unit cells of several metals are created and their potentials are measured in order to create a potential series.
8)
Reactions in Aqueous Solutions: Strong Acids and Bases The pH and concentration relationships for the reaction of HCl and NaOH are investigated.
9)
Calorimetry & Hess’s Law The enthalpies of reaction are determined for both magnesium metal and magnesium oxide in water. These enthalpies are then used in conjuction with Hess's Law to determine the enthalpy of reaction for magnesium burning in oxygen. .
10)
Gas Laws and Air Bags Ideal gas law and stoichiometry are used to construct a working mock-up of an automobile airbag.
11)
Intermolecular Forces and the Triple Point of CO2 Intermolecular forces are investigated by observing the temperature depression created when different solvents evaporate. The triple point of CO2 is observed and measured.
12)
The Purification of Water Fresh water samples are tested for phosphate before and after purification.
13)
Kinetics: The Iodine Clock The Iodine Clock Reaction is measured at room, high, and low temperatures, and its rate constant is determined.
14)
Photometric Determination of an Equilibrium Constant The equilibrium constant for the reaction of iron(III) thiocyanate is determined by photometric methods.
15)
Titration of 7-Up® Monoprotic and polyprotic acids are titrated using NaOH.
16)
Hydrogen Phosphate Buffer Systems Students create and then test the buffering capacity of a hydrogen phosphate buffer.
17)
Entropy, Free Energy, and Chemical Equilibrium The thermodynamics of the solubility of Ca(OH)2 are determined using titration.
18)
Electrochemistry: The Nernst Equation Unit cells are built from various metals and then tested at several temperatures. The free energy is determined using the Nernst equation.
19)
Analysis of a Hydrate The formula and percentage of water is determined in an unknown hydrate.
20)
Qualitative Analysis: Cations, Anions, and Complex Ions A single-day, microscale qualitative analysis is used to determine the cations and anions in an unknown mixture.
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21)
Isomerism in Coordination Chemistry A study of the three-dimensional structures of octahedral complexes is performed.
22)
Light Emitting Diode Students will identify the components of a complex ion and predict if that complex ion has a large or small crystal-field splitting energy while constructing an organic diode.
23)
Amino Acid Analysis by Ninhydrin Students identify the amino acids in an unknown mixture using a combination of ninhydrin and TLC.
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