General Chemistry 2

Learning objectives by module

Unit 2: Chemical Kinetics

 

Module 3: Reaction Rates

Calculate reaction rates from experimental data.

Describe the effects of chemical nature, physical state, temperature, concentration, and catalysis on reaction rates.

Determine relative rates of consumption and production of species from the balanced equation for a given chemical reaction.

 

Module 4: Rate Laws

Define half-life and carry out related calculations.

Perform integrated rate law calculations for zero-, first-, and second-order reactions.

Use rate and concentration data to identify reaction orders and derive rate laws.

 

Module 5: Reaction Mechanisms

Define the concepts of activation energy and transition state.

Derive the rate law consistent with a given reaction mechanism.

Explain the function of a catalyst in terms of reaction mechanisms and potential energy diagrams.

Use the Arrhenius equation in calculations relating rate constants to temperature.

Use the postulates of collision theory to explain the effects of physical state, temperature, and concentration on reaction rates.

 

Unit 3: Chemical Equilibrium

 

Module 8: Concepts of Chemical Equilibrium

Calculate values of equilibrium constants, using concentrations and pressures.

Calculate values of reaction quotients.

Explain the dynamic nature of equilibrium.

Given a reversible reaction and information about a system at equilibrium, determine values of K or concentration of species at equilibrium.

Predict directional shift of a reaction by comparing the values of the reaction quotient and equilibrium constant.

 

 

Module 9: Le Châtelier’s Principle

Predict the response of a stressed equilibrium using Le Châtelier’s principle.

 

Module 10: Equilibrium Calculations

Given a reversible chemical reaction with a large or small value of K, and the current state of a system, determine concentration of chemical species at equilibrium.

Given a reversible chemical reaction with an intermediate value of K and the current state of a system, determine the concentrations of the chemical species that will be present at equilibrium.

 

Unit 4: Acids and Bases

 

Module 13: Defining and Measuring Acids and Bases

Describe the acid-base behavior of amphiprotic substances.

Identify acids, bases, and conjugate acid-base pairs.

Perform calculations relating pH and pOH.

Use the ion-product constant for water to calculate hydronium and hydroxide ion concentrations.

 

Module 14: Strong and Weak Acids and Bases

Apply equilibrium concepts to acids and bases that may donate or accept more than one proton.

Calculate the concentrations of the various species in and pH of a salt solution.

Carry out equilibrium calculations for weak acid–base systems.

Perform calculations relating Ka and Kb and assess the relative strengths of acids and bases according to these ionization constants.

Perform calculations relating pH and pOH.

Predict whether a salt solution will be acidic, basic, or neutral.

Rationalize trends in acid–base strength in relation to molecular structure.

 

Module 15: Buffers

Calculate the pH of a buffer before and after the addition of added acid or base.

Describe the composition and function of acid–base buffers.

The graph, an illustration of buffering action, shows change of pH as an increasing amount of a 0.10-M NaOH solution is added to 100 mL of a buffer solution in which, initially, [CH3CO2H] = 0.10 M and [CH3CO2−] = 0.10M.

 

Module 16: Titrations

Compute sample pH at important stages of a titration.

Interpret titration curves for strong and weak acid-base systems.

 

Unit 5: Equilibria of Other Reaction Classes

 

Module 19: Solubility and Complex Ion Equilibria

Calculate values of solubility equilibrium constants, Ksp, using concentrations.

Determine conditions under which precipitation occurs.

Perform calculations relating Kf values and concentrations of species at equilibrium.

Perform calculations relating the solubility equilibrium constant, Ksp, to solubility using concentrations.

 

Unit 6: Thermodynamics

 

Module 21: The Second Law of Thermodynamics

Describe the characteristics of a spontaneous process.

Explain how the second law of thermodynamics can be used to determine spontaneity.

 

Module 22: Free Energy

Qualitatively and quantitatively determine free energy change for a process using enthalpies of formation and the entropies of reactants and products.

Use the relation between K and standard free energy change of a chemical reaction to connect observations about a system at equilibrium to the standard free energy.

Module 23

Thermodynamics: Unit Assessment

 

Unit 7: Electrochemistry

 

Module 25: Foundational Concepts of Electrochemistry

Define important associated terms of electrochemistry.

Produce balanced oxidation-reduction equations for reactions in acidic or basic solution.

 

Module 26: Galvanic Cells

Describe the basic components of galvanic cells.

Determine standard cell potentials for oxidation-reduction reactions.

Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants.

Use cell notation to describe galvanic cells.

Use the Nernst equation to determine cell potentials at nonstandard conditions.

 

Module 27: Other Applications of Electrochemistry

Describe batteries and fuel cells.

Describe electrolytic cells and their relationship to galvanic cells.

List methods used to prevent or slow corrosion.

Perform various calculations related to electrolysis.

 

Unit 8: Nuclear Chemistry

 

Module 29: Nuclear Reactions and Equations

Calculate mass defect and binding energy for nuclei.

Describe common types of nuclear reactions.

Describe nuclear structure in terms of protons, neutrons, and electrons.

Explain trends in the relative stability of nuclei.

Identify common particles and energies involved in nuclear reactions.

Write and balance nuclear equations.

 

Module 30: Applications of Nuclear Chemistry

Calculate kinetic parameters for decay processes, including half-life.

Describe and perform calculations for common radiometric dating techniques.

Describe the biological impact of ionizing radiation.

Explain nuclear fission and fusion processes.

List common applications of radioactive isotopes.

Summarize basic requirements for nuclear fission and fusion reactors.