General Chemistry 2

Learning objectives by module

Unit : Chemical Kinetics

Module : Reaction Rates

• Calculate reaction rates from experimental data.
• Determine relative rates of consumption and production of species from the balanced equation for a given chemical reaction.
• Describe the effects of chemical nature, physical state, temperature, concentration, and catalysis on reaction rates.

Module : Rate Laws

• Use rate and concentration data to identify reaction orders and derive rate laws.
• Perform integrated rate law calculations for zero-, first-, and second-order reactions.
• Define half-life and carry out related calculations. 

Module : Reaction Mechanisms

• Use the postulates of collision theory to explain the effects of physical state, temperature, and concentration on reaction rates.
• Define the concepts of activation energy and transition state.
• Use the Arrhenius equation in calculations relating rate constants to temperature.
• 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. 

Unit: Chemical Equilibrium

Module: Concepts of Chemical Equilibrium

• Explain the dynamic nature of equilibrium.
• Calculate values of reaction quotients.
• Calculate values of equilibrium constants, using concentrations and pressures.
• Predict directional shift of a reaction by comparing the values of the reaction quotient and equilibrium constant. 

Module: LeChatelier’s Principle

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

Module: Equilibrium Calculations

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

Unit: Acids and Bases

Module: Defining and Measuring Acids and Bases

• Identify acids, bases, and conjugate acid-base pairs.
• Use the ion-product constant for water to calculate hydronium and hydroxide ion concentrations.
• Describe the acid-base behavior of amphiprotic substances.
• Perform calculations relating pH and pOH. 

Module: Strong and Weak Acids and Bases

• 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.
• Carry out equilibrium calculations for weak acid–base systems.
• Apply equilibrium concepts to acids and bases that may donate or accept more than one proton.
• Predict whether a salt solution will be acidic, basic, or neutral.
• Calculate the concentrations of the various species in and pH of a salt solution.
• Rationalize trends in acid–base strength in relation to molecular structure.

Module: Buffers

• Describe the composition and function of acid–base buffers.
• Calculate the pH of a buffer before and after the addition of added acid or base.

Module: Titrations

• Compute sample pH at important stages of a titration.
• Interpret titration curves for strong and weak acid-base systems. 

Unit: Equilibria of Other Reaction Classes

Module: Solubility and Complex Ion Equilibria

• Calculate values of solubility equilibrium constants, Ksp, using concentrations.
• Perform calculations relating the solubility equilibrium constant, Ksp, to solubility using concentrations.
• Determine conditions under which precipitation occurs.
• Perform calculations relating Kf values and concentrations of species at equilibrium. 

Unit: Thermodynamics

Module: 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: 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. 

Unit: Electrochemistry

Module: Foundational Concepts of Electrochemistry

• Define important associated terms of electrochemistry.
• Produce balanced oxidation-reduction equations for reactions in acidic or basic solution. 

Module: Galvanic Cells

• Describe the basic components of galvanic cells.
• Use cell notation to describe 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 the Nernst equation to determine cell potentials at nonstandard conditions.

Module: Other Applications of Electrochemistry

• Describe batteries and fuel cells.
• List methods used to prevent or slow corrosion.
• Describe electrolytic cells and their relationship to galvanic cells.
• Perform various calculations related to electrolysis.

Unit: Nuclear Chemistry

Module: Nuclear Reactions and Equations

• Describe nuclear structure in terms of protons, neutrons, and electrons.
• Calculate mass defect and binding energy for nuclei.
• Explain trends in the relative stability of nuclei.
• Identify common particles and energies involved in nuclear reactions.
• Write and balance nuclear equations.
• Describe common types of nuclear reactions.

Module: Applications of Nuclear Chemistry

• Calculate kinetic parameters for decay processes, including half-life.
• Describe and perform calculations for common radiometric dating techniques.
• Explain nuclear fission and fusion processes.
• Summarize basic requirements for nuclear fission and fusion reactors.
• List common applications of radioactive isotopes.
• Describe the biological impact of ionizing radiation.