General Chemistry 2 - Part 2

- Definition of an acid-base reaction.

- Acidity constant.

- Predominance chart.

- Common examples of acids and bases: name, formula, and type—weak or strong—of sulfuric, nitric, hydrochloric, phosphoric, and acetic acids; sodium hydroxide; potassium hydroxide; the hydrogen carbonate ion; and ammonia.

- Buffer solutions.

- Temporal evolution of a chemical system and reaction mechanisms in a closed reactor of uniform composition. Rates of reactant consumption and product formation. Reaction rate for a transformation modeled by a single chemical reaction.

- Speed laws: reactions without order, reactions with simple order (0, 1, 2), global order, order

apparent.

- Half-life. The half-life of a radioactive nuclide. Document-based approach: Using documents related to radionuclides, explore, for example, issues related to their use, storage, or reprocessing.

- Arrhenius's empirical law; activation energy.

- Reaction mechanisms. Elementary reactions, molecularity, reaction intermediates, transition state. Kinetically determining step, quasi-steady-state approximation (AEQS).

Numerical approach: Use the results of a numerical method to identify approximations of the kinetically decisive step or the quasi-steady state.

• Identify the nature of reactions in aqueous solutions.
• Know how to construct and interpret a dominance diagram. Determine equilibrium constant values by reading distribution curves and dominance diagrams (and vice versa). Use dominance or presence diagrams to predict incompatible species or the nature of the dominant species.
• Understand the nature (acidic/basic, strong/weak) of the most common examples listed above.
• Calculate the pH of a buffer solution; calculate the concentration of each chemical species in a buffer solution.
• Understand the purpose of buffer solutions.
• Extract, from available resources, the relevant thermodynamic data to qualitatively predict the final state of a system in aqueous solution or to interpret experimental observations.
• Determine the value of the equilibrium constant for a reaction equation that can be written as a linear combination of equations whose thermodynamic constants are known.
• Predict whether a solution, solid, or gas is saturated or unsaturated.
• Use graphs showing how solubility changes as a function of a variable.
• Determine the effect of a parameter on the rate of a chemical reaction. Relate the reaction rate—when it is defined—to the rate at which a reactant is consumed or a product is formed.
• Derive a rate-of-change law based on the time-dependent behavior of a physical quantity.
• Express the rate law if the chemical reaction has an order, and determine the value of the rate constant at a given temperature.
• Determine the reaction rate at different times using a numerical or graphical method.
• Determine the order of a reaction using the differential method, the half-reaction times, or the integral method, strictly limiting the analysis to a decomposition of order 0, 1, or 2 involving a single reactant, or reducing the problem to such a case through order degeneracy or stoichiometric initial conditions.
• Determine the activation energy of a chemical reaction.
• Determine the activation energy of a chemical reaction based on values of the rate constant at different temperatures.
• Distinguish between a chemical equation representing a chemical reaction and an equation representing a step. Express the rate law for a step. Plot an energy profile corresponding to a single step or to several successive steps.
• Distinguish between a reaction intermediate and an activated complex (transition state).
• Interpreting the role of a catalyst. Recognizing a catalytic effect in a reaction mechanism.
• Identify the conditions under which the kinetically determining step approximation or the quasi-steady-state approximation can be used.
• Derive the rate law for the consumption of a reactant or the formation of a product based on a simple reaction mechanism, using standard approximations if necessary.

Stoichiometry, chemical formulas, states of matter, and the basics of differential calculus. 

3 ongoing assessments. Final grade = 20% OA1 + 30% OA2 + 50% OA3