CHEM 117 - General Chemistry 2 and Qualitative Analysis

Credits: 5
Lecture Contact Hours: 4
Lab Contact Hours: 4
Description: This course is the second course in a traditional one-year general college chemistry program and includes the study of kinetics, solution equilibria, solubility equilibria, hydrolysis, electrochemistry, coordination compounds, thermodynamics and qualitative analysis. A brief introduction to organic chemistry and quantitative analysis is also included. Laboratory work correlates with lecture and stresses the identification of common cations and anions by semi-micro methods.

Prerequisites: CHEM 111 with a minimum grade of 2.0.
Corequisites: None.
Recommended: None.

Course Category: Liberal Arts | Science with Lab
This course counts toward Schoolcraft’s General Education Requirements.
This course counts toward a Michigan Transfer Agreement General Education Requirement.

This Course is Typically Offered: Winter, Spring, Fall
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Course Competencies

Calculate equilibrium constants and reactant/product concentrations relating to various chemical equilibria.
Differentiate between Arrhenius, Bronsted/Lowry and Lewis definitions of acids and bases.
Measure the pH of a solution using a pH meter and acid/base indicators.
Write balanced equations for acids, bases and insoluble solids dissolved in water.
Write balanced equations for reactions between acids and bases.
Calculate the hydrogen ion, hydroxide ion, pH and pOH of strong and weak acids and bases, salt solutions, buffer solutions and mixtures of acids and bases.
Interpret titration curves.
Calculate Ksp and molar solubility for slightly soluble solids.
Calculate molar solubility for slightly soluble solids in the presence of common ions or complexing agents.
Determine the effect of pH on the solubility of a solid.
Determine concentration, reaction stoichiometry and chemical formulas from titration data.
Calculate reaction rate and reaction order from kinetic data.
Determine the rate law for a reaction mechanism.
Explain the relationship between a reaction mechanism and a balanced equation.
Explain the ways in which concentration, temperature, surface area and catalysts affect reaction rates.
Identify by experiment, cations and anions present in various unknown compounds or mixtures.
Compare properties of transition metals and main group elements.
Explain trends of size, melting point, density, magnetism and electron configuration of transition metals.
Relate Crystal Field Theory to the reactivity, magnetic properties, electron configuration and color of transition metal compounds.
Write names and formulas for transition metal complexes.
Classify groups of substances as geometric isomers, constitutional isomers, optical isomers, identical compounds or unrelated substances.
Draw constitutional, geometric and/or optical isomers for a given chemical formula.
Calculate delta H, delta S and delta G values for chemical changes given a table of standard values.
Relate delta H, delta S and delta G values to the equilibrium constant and spontaneity of a chemical reaction.
Determine reaction enthalpies using a calorimeter to collect the necessary data.
Apply the concepts of oxidation reduction chemistry to various systems including electrolytic and galvanic cells.
Determine the concentration of a solution using spectroscopic data.
Apply a working knowledge of laboratory safety, including proper use of safety equipment (e.g. protective eyewear) and safe work habits.
Utilize laboratory equipment in the performance of laboratory experiments.
Organize laboratory data, calculations and analyses in an accurate and detailed fashion.
Execute appropriate disposal procedures for the various compounds used in the laboratory.
Demonstrate interpersonal communication and group work skills while cooperating with other students to complete laboratory experiments.