Evaluation
outcome(s)
1, 2, 4, 6, 7

· Assess a problem in kinetics to determine what information is known/unknown, relevant/extraneous, and derive the necessary equations
· Assess a problem in solution chemistry and determine the type of problem (colligative property, concentration, acid/base, equilibrium) and equations needed to solve the problem.
· Assess a problem in equilibrium to determine what type of equilibrium (acid/base, buffer, solubility, complexion), relevant information, and necessary equations to solve the problem.
· Assess a problem in electrochemistry to determine type of cell (and be able to draw cell showing all components), evaluate information given and what is needed, and determine and/or derive equations necessary to solve the problem.
· Balance REDOX equations in neutral, acidic, and basic solutions and apply to electrochemical cells.
· Draw and explain an electrochemical cell
· Evaluate Gibbs free energy using the Nernst Equation, Free energy tables, and entropyenthalpy tables.

· Assess a problem in kinetics to determine what information is known/unknown, relevant/extraneous, and choose the necessary equations
· Assess a problem in solution chemistry and determine the type of problem (3 from: colligative property, concentration, acid/base, equilibrium) and equations needed to solve the problem.
· Assess a problem in equilibrium to determine what type of equilibrium (3 from: acid/base, buffer, solubility, complexion), relevant information, and necessary equations to solve the problem.
· Assess a problem in electrochemistry to determine type of cell (and be able to draw cell showing all components), evaluate information given and what is needed, and determine the equations necessary to solve the problem.
· Balance REDOX equations in neutral, acidic solution and apply to electrochemical cells and thermodynamics.
· Draw and explain an electrochemical cell
· Evaluate Gibbs free energy using the Nernst Equation, Free energy tables, and entropyenthalpy tables.
·

· Assess a problem in kinetics to determine what information is known/unknown and choose the necessary equations
· Assess a problem in solution chemistry and determine the type of problem (2 from: colligative property, concentration, acid/base, equilibrium) and equations needed to solve the problem.
· Assess a problem in equilibrium to determine what type of equilibrium (2 from: acid/base, buffer, solubility, complexion), relevant information, and necessary equations to solve the problem.
· Assess a problem in electrochemistry to determine type of cell (and be able to draw cell showing all components), evaluate information given and determine the equations necessary to solve the problem.
· Balance REDOX equations in neutral solution and apply to electrochemical cells and thermodynamics.
· Draw and explain an electrochemical cell
· Evaluate Gibbs free energy using the Nernst Equation, Free energy tables or entropyenthalpy tables.
·

· Assess a problem in kinetics to determine what information is known/unknown and choose the necessary equations
· Assess a problem in solution chemistry and determine the type of problem (1 from: colligative property, concentration, acid/base, equilibrium) and equations needed to solve the problem.
· Assess a problem in equilibrium to determine what type of equilibrium (1 from: acid/base, buffer, solubility, complexion), relevant information, and necessary equations to solve the problem.
· Be able to draw cell an electrochemical cell showing all components), evaluate information given and determine the equations necessary to solve the problem.
· Balance REDOX equations in neutral solution.
· Draw and explain an electrochemical cell
· Evaluate Gibbs free energy using Free energy tables.
·


Synthesis
outcome(s)
1, 2, 3, 4, 7

· Determine the rate of a reaction graphically and using initial rates
· Show how the rate is dependent on concentration by deriving the necessary equations, propose a mechanism for a set of appropriate equations for a given problem
· Mathematically manipulate a set of appropriate equations to fit the desired kinetic theory outcome and the information given
· Combine equations showing how physical properties (MW, concentration, etc) can be determined from colligative properties.
· Combine relevant equations in equilibria to obtain the solution to given questions.
· Combine the Nernst equation with those of equilibria and/or thermodynamics to obtain the solution to question.

· Determine the rate of a reaction graphically or using initial rates
· Use equations that relate the rate to concentration
· propose a mechanism for a set of appropriate equations for a given problem
· Mathematically manipulate a set of appropriate equations to fit the desired kinetic theory outcome and the information given
· Use equations that show how physical properties (MW, concentration, etc) can be determined from colligative properties.
· Combine relevant equations in equilibria to obtain the solution to given questions.
· Combine the Nernst equation with those of equilibria and/or thermodynamics to obtain the solution to question.

Do five of these:
· Determine the rate of a reaction graphically or using initial rates
· Use equations that relate the rate to concentration
· propose a mechanism for a set of appropriate equations for a given problem
· Mathematically manipulate a set of appropriate equations to fit the desired kinetic theory outcome and the information given
· Use equations that show how physical properties (MW, concentration, etc) can be determined from colligative properties.
· Combine relevant equations in equilibria to obtain the solution to given questions.
· Combine the Nernst equation with those of equilibria and/or thermodynamics to obtain the solution to question.

Do three of these:
· Determine the rate of a reaction graphically or using initial rates
· Use equations that relate the rate to concentration
· propose a mechanism for a set of appropriate equations for a given problem
· Mathematically manipulate a set of appropriate equations to fit the desired kinetic theory outcome and the information given
· Use equations that show how physical properties (MW, concentration, etc) can be determined from colligative properties.
· Combine relevant equations in equilibria to obtain the solution to given questions.
· Combine the Nernst equation with those of equilibria and/or thermodynamics to obtain the solution to question.


Analysis
outcome(s)
2, 3, 4, 5, 6, 7

· Determine the rate law for a given set of data
· Propose kinetic mechanisms
· Relate the halflife of a reaction to the rate constant
· Use the Arrhenius equation and use graphic interpretation
· Write equilibriumconstant expressions
· Identify acid and base species
· Identify Lewis acid/base
· Write solubility product expressions
· Determine the direction of spontaneity from electrode potentials
· Determine the direction of spontaneity from electrode potentials.
· Predict the halfreaction in aqueous electrolysis
· Analyze the outcome of a reaction predicted by DG.

Be able to do nine of:
· Determine the rate law for a given set of data
· Propose kinetic mechanisms
· Relate the halflife of a reaction to the rate constant
· Use the Arrhenius equation and use graphic interpretation
· Write equilibriumconstant expressions
· Identify acid and base species
· Identify Lewis acid/base
· Write solubility product expressions
· Determine the direction of spontaneity from electrode potentials
· Determine the direction of spontaneity from electrode potentials.
· Predict the halfreaction in aqueous electrolysis
· Analyze the outcome of a reaction predicted by DG.

Be able to do seven of:
· Determine the rate law for a given set of data
· Propose kinetic mechanisms
· Relate the halflife of a reaction to the rate constant
· Use the Arrhenius equation and use graphic interpretation
· Write equilibriumconstant expressions
· Identify acid and base species
· Identify Lewis acid/base
· Write solubility product expressions
· Determine the direction of spontaneity from electrode potentials
· Determine the direction of spontaneity from electrode potentials.
· Predict the halfreaction in aqueous electrolysis

Be able to do five of:
· Determine the rate law for a given set of data
· Propose kinetic mechanisms
· Relate the halflife of a reaction to the rate constant
· Use the Arrhenius equation and use graphic interpretation
· Write equilibriumconstant expressions
· Identify acid and base species
· Identify Lewis acid/base
· Write solubility product expressions
· Determine the direction of spontaneity from electrode potentials
· Determine the direction of spontaneity from electrode potentials.
· Predict the halfreaction in aqueous electrolysis


Application
outcome(s)
2, 3, 4, 5, 6, 7

· Write the mechanism for a multistep reaction
· Calculate solution concentration
· Convert concentration units
· Calculate vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure, molecular weights
· Determine colligative properties of ionic solutions
· Apply stoichiometry to an equilibrium mixture
· Obtain an equilibrium constant from reaction composition
· Obtain one equil. conc. Given the others and K.
· Calculate [H^{+}], [OH^{}], and pH
· Determine K_{a} or K_{b} from the solution pH
· Calculate concentrations of species in a weak acid (or base) using K_{a} or K_{b+.}
· Predict whether a salt solution is acidic, basic, or neutral
· Calculate concentration of species in a salt solution
· Calculate the commonion effect on acid ionization.
· Calculate the p H of a buffer solution, of a buffer when a strong acid or strong base is added, at the equivalence point in the titration of a weak acid by a strong base.
· Calculate K_{sp} from the solubility, or vice versa
· Calculate the solubility of a slightly soluble salt in a solution of a common ion
· Predict whether precipitation will occur
· Separate metal ions by sulfide precipitation
· Calculate the emf and Gibb’s Free Energy change from standard potentials
· Calculate the equilibrium constant from cell emf

Be able to do 19 of the following:
· Write the mechanism for a multistep reaction
· Calculate solution concentration
· Convert concentration units
· Calculate vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure, molecular weights
· Determine colligative properties of ionic solutions
· Apply stoichiometry to an equilibrium mixture
· Obtain an equilibrium constant from reaction composition
· Obtain one equil. conc. Given the others and K.
· Calculate [H^{+}], [OH^{}], and pH
· Determine K_{a} or K_{b} from the solution pH
· Calculate concentrations of species in a weak acid (or base) using K_{a} or K_{b+.}
· Predict whether a salt solution is acidic, basic, or neutral
· Calculate concentration of species in a salt solution
· Calculate the commonion effect on acid ionization.
· Calculate the p H of a buffer solution, of a buffer when a strong acid or strong base is added, at the equivalence point in the titration of a weak acid by a strong base.
· Calculate K_{sp} from the solubility, or vice versa
· Calculate the solubility of a slightly soluble salt in a solution of a common ion
· Predict whether precipitation will occur
· Separate metal ions by sulfide precipitation
· Calculate the emf and Gibb’s Free Energy change from standard potentials
· Calculate the equilibrium constant from cell emf

Be able to do 16 of the following:
· Write the mechanism for a multistep reaction
· Calculate solution concentration
· Convert concentration units
· Calculate vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure, molecular weights
· Determine colligative properties of ionic solutions
· Apply stoichiometry to an equilibrium mixture
· Obtain an equilibrium constant from reaction composition
· Obtain one equil. conc. Given the others and K.
· Calculate [H^{+}], [OH^{}], and pH
· Determine K_{a} or K_{b} from the solution pH
· Calculate concentrations of species in a weak acid (or base) using K_{a} or K_{b+.}
· Predict whether a salt solution is acidic, basic, or neutral
· Calculate concentration of species in a salt solution
· Calculate the commonion effect on acid ionization.
· Calculate the p H of a buffer solution, of a buffer when a strong acid or strong base is added, at the equivalence point in the titration of a weak acid by a strong base.
· Calculate K_{sp} from the solubility, or vice versa
· Calculate the solubility of a slightly soluble salt in a solution of a common ion
· Predict whether precipitation will occur
· Separate metal ions by sulfide precipitation
· Calculate the emf and Gibb’s Free Energy change from standard potentials
Calculate the equilibrium constant from cell emf

Be able to do 13 of the following:
· Write the mechanism for a multistep reaction
· Calculate solution concentration
· Convert concentration units
· Calculate vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure, molecular weights
· Determine colligative properties of ionic solutions
· Apply stoichiometry to an equilibrium mixture
· Obtain an equilibrium constant from reaction composition
· Obtain one equil. conc. Given the others and K.
· Calculate [H^{+}], [OH^{}], and pH
· Determine K_{a} or K_{b} from the solution pH
· Calculate concentrations of species in a weak acid (or base) using K_{a} or K_{b+.}
· Predict whether a salt solution is acidic, basic, or neutral
· Calculate concentration of species in a salt solution
· Calculate the commonion effect on acid ionization.
· Calculate the p H of a buffer solution, of a buffer when a strong acid or strong base is added, at the equivalence point in the titration of a weak acid by a strong base.
· Calculate K_{sp} from the solubility, or vice versa
· Calculate the solubility of a slightly soluble salt in a solution of a common ion
· Predict whether precipitation will occur
· Separate metal ions by sulfide precipitation
· Calculate the emf and Gibb’s Free Energy change from standard potentials
Calculate the equilibrium constant from cell emf

