Laboratory Manual for General Chemistry Atoms First

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  • Edition: 1st
  • Format: Spiral Bound
  • Copyright: 5/29/2013
  • Publisher: Pearson

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By Stephanie Dillon with contributions from Sandra Chimon Peszek, DePaul University

Laboratory Manual for General Chemistry: Atoms First, Second Edition is organized using the atoms first approach and is written to correspond with the Second Edition of General Chemistry: Atoms First by McMurry/Fay. This manual contains twenty-four experiments with a focus on real world applications, following an intuitive logic progressing from the simplest building blocks to successively more complex concepts.


Each experiment covers one or more topics discussed within a chapter of the textbook to help students understand the underlying concepts covered in the lecture course. Additionally, each experiment contains a set of pre-laboratory questions (also assignable in MasteringChemistry®), an introduction, a background section explaining concepts that each student is expected to master for a full understanding of the experimental results,  a step-by-step procedure (including safety information), and a report section featuring post-laboratory questions.


Note: This is the standalone book (Laboratory Manual for General Chemistry: Atoms First, Second Edition) if you want the book/access card order the ISBN below: You must have the Instructor ID to access MasteringChemistry.


0321913329 / 9780321913326 General Chemistry: Atoms First Plus MasteringChemistry with eText -- Access Card Package & Laboratory Manual for General Chemistry: Atoms First Package*


Package consists of:   

032180483X / 9780321804839 General Chemistry: Atoms First Plus MasteringChemistry with eText -- Access Card Package

0321813375 / 9780321813374 Laboratory Manual for General Chemistry: Atoms First


Table of Contents

Table of Contents

Experiment 0: A. Measurement and Expression of Experimental Data; B. Graphing and Statistical Analysis

A math review including practice with significant figures, rounding rules, graphing techniques and statistical analysis.

Experiment 1: Conservation of Matter

A reaction of Copper Nitrate and Zinc is observed to determine if Mass is conserved.

Experiment 2: Atomic Spectra

Several unknown light sources are identified by use of spectrometry.

Experiment 3: Halogen Reactions

Hexane and water are used to determine the solubility of the halogens and halides.

Experiment 4: Paper Chromatography: A M&M’s® True Colors

Paper Chromatography is used to analyze the food colorings used in M&M’s® candy shells

Experiment 5: Building Molecular Models

Lewis Structures are presented in model form and investigated.

Experiment 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.

Experiment 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.

Experiment 8: Reactions in Aqueous Solutions: Strong Acids and Bases

The pH and concentration relationships for the reaction of HCl and NaOH are investigated.

Experiment 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.

Experiment 10: Gas Laws and Air Bags

Ideal gas law and stoichiometry are used to construct a working mock-up of an automobile airbag.

Experiment 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.

Experiment 12: The Purification of Water

Fresh water samples are tested for phosphate before and after purification.

Experiment 13: Kinetics: The Iodine Clock

The Iodine Clock Reaction is measured at room, high and low temperatures and is Rate Constant is Determined.

Experiment 14: Photometric Determination of an Equilibrium Constant

The equilibrium constant for the reaction of iron (III) thiocyanate is determined by photometric methods.

Experiment 15: Titration of 7-Up©

Monoprotic and polyprotic acids are titrated using NaOH.

Experiment 16: Hydrogen Phosphate Buffer Systems

Students create and then test the buffering capacity of a hydrogen phosphate buffer.

Experiment 17: Entropy, Free Energy and Chemical Equilibrium

The thermodynamics of the solubility of Ca(OH)2 are

determined using titration.

Experiment 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.

Experiment 19: Analysis of hydrates

The formula and percentage of water is determined in an hydrate unknown

Experiment 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.

Experiment 21: Isomers of Coordination Chemistry

A study of the three dimensional structures of octahedral complexes is performed.

Experiment 22: Making an Organic 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


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