Chapter 10-11 

1.  Use the Ideal Gas Law to:
   a)   determine the effect of a change in one or more variables (n, T, P) on the value of another variable (e.g. V);  use the combined gas law
      b)   solve for one variable (P,n,V,T), knowing the values of the other three variables.
   c)   calculate the density or molar mass of a gas, given the necessary data (molar mass, pressure &  temp for density; temp, pressure and density for molar mass).
     d) relate the volume of a gas involved in a reaction to the amount of another reactant or product.
2.  Relate the volumes of gases (measured at the same T and P) in a reaction.
3.  Use Dalton's Law to find the partial pressure of a gas in a mixture.
4.  Use Graham's Law to relate the molar masses of two gases to their rates or times of effusion.

Chapter 12 

1. Draw a phase diagram for a pure substance, given appropriate data, and state what phases are present at any given point on the diagram.
2. Distinguish between ionic, molecular, network covalent, and metallic solids with regards to both particle structure and physical properties (melting point, conductivity, water solubility)
3.  Compare different molecular substances with respect to physical properties (melting point, boiling point) and types of intermolecular forces (dipole forces, hydrogen bonding, dispersion forces)

Chapter 13-14
 
1. Write balanced equations to represent the solution process for an electrolyte and a nonelectrolyte.
2.  Given the amounts (grams or moles) of the components of a solution, calculate mole fraction or molality.
3.  Describe how to prepare a solution to a desired molarity, starting either with a pure solute or a concentrated solution.
 4.  Relate the molarity of an electrolyte solution to the molarities of its ions.
 5.  Given appropriate data, convert between molarity, molality, mole fraction, and mass percent of solute.
 6.  Predict the effect of changes in temperature or pressure upon the solubilities of solids and gases.
 7.  Calculate the boiling point or freezing point of a nonelectrolyte solution, knowing or having calculated the molality.

Chapter 15-16
 

 1.  Given one of the three quantities, [H₃O+], [OH^-], pH, calculate the other two quantities.
 2.  Know properties and characteristics of acids and bases. Predict whether a given acid or base is strong or weak.
 3.  Write a net ionic equation to explain why a molecule, cation, or anion gives an acidic or basic solution.
 4.  Predict whether a given ion or ionic compound will give an acidic, basic, or neutral water solution.
 5.  Write net ionic equations and predict the pH for the reaction of a strong acid with a strong base, a weak acid with a strong base, and a strong acid with a weak base.
 6.  Choose an appropriate indicator for a given acid-base titration. 
 7.  Use titration data to calculate the concentration of an acidic or basic species in solution or and the pH at given points in the titration. 
 8.  Given the equation for an acid-base reaction, select the Bronsted acid and Bronsted base, the Lewis acid and Lewis base, the conjugate acid-base pairs. 

Chapter 17 

1.  Relate the direction of heat flow in a reaction (exothermic or endothermic) to the sign of ^H.

2.  Given a thermochemical equation, calculate
   a)  ^H for a specified amount of reactant or product.
   b)  the amount of product or reactant required to produce a specified ^H.
3.  Use Hess' Law to calculate ^H for
   a)  a stepwise reaction, knowing the value of ^H for each step.
   b)  a step in a reaction, knowing ^H for every other step and for the overall reaction.
4.  Use the general relation:  ^H = Sum^H (products) - Sum^H (reactants) to calculate: ^H for a reaction, knowing the heats of formation of all species.
^H_f for one species, knowing the heats of formation of all other species as well as ^H for the reaction.
5.  Use calorimetric data (temperature change, mass of water, specific heat of water, calorimeter constant) to determine the heat flow for a reaction.
6.  Use Tables to calculate ^H and ^S for a reaction.
7.  Use the Gibbs-Helmholtz equation to calculate the free energy change for a reaction.
8.  Given or having calculated ^H and ^S. determine the temperature at which a reaction is at equilibrium at 1 atm.
9.  Describe how the signs of ^H, ^S, and ^G relate to the spontaneity of a reaction.
10.  Determine the order of a reaction, given the initial rate as a function of concentration of reactants.
11.  For a first order reaction, calculate
    a)  The concentration of reactant after a given time, knowing its original concentration and the rate constant.
    b)  The time required for the concentration to drop by a given amount, knowing the rate constant.
    c)  Given either  the half life or the rate constant for a first order reaction, calculate the other quantity.

 Chapter 18

1.  Given a balanced equation for a reaction involving gases, write the corresponding expression for K_c
2.  For a given equation, calculate K_c , knowing:
   a)  The equilibrium concentrations of all species, or
   b)  The original concentrations of all species and the equilibrium concentration       of one species.
3.  Given the value of K_c, predict:
4.  The direction in which a chemical species will move to reach equilibrium.
5.  The equilibrium concentration of one species, given those of all other species.
6.  The equilibrium concentrations of all species, given their original concentrations.
7.  Using Le Chatelier's Principle, predict the effect of a change in the number of moles, volume, or temperature upon the position of an equilibrium
8.  Using the solubility rules, predict whether a precipitate will form when two electrolyte solutions are mixed and write a net ionic equation for an y reaction that occurs.
9.  Using the chemical equation for a precipitation reaction, relate the amounts of two different reactants.
10.  Given the formula of a slightly soluble ionic compound, write its K_sp
expression.
11.  Use the value of K_sp to:
    a)  Determine the concentration of an ion in solution, given that of the other ion in equilibrium with it.
    b)  Decide whether or not a precipitate will form when two solutions are mixed.
    c)  Calculate the solubility of an electrolyte in pure water or in a solution containing a common ion.
12.  Given the solubility of an electrolyte in pure water, calculate K_sp
13. Calculate K_a for a weak acid, HB, given the [H⁺] or pH of a solution prepared by dissolving HB in water to a known initial concentration.
14.  Given the initial concentration of a weak acid and the value of K_a calculate H⁺]
15.  Given the composition of a buffer system, determine its pH before and after the addition of known amounts of strong acid or base. 

Chapter 19 

1.  Given the formula of a species, determine the oxidation number of each atom.
2.  Given a redox equation, select the oxidizing agent; the reducing agent.
3.  Given the formulas of products and reactants, balance a redox equation by the half-equation method.
4.  Given a balanced equation or half-equation in acidic solution, write the corresponding balanced equation in basic solution.
5.  Contrast electrolytic with voltaic cells; identify anode and cathode in either type of cell and indicate the flow of current through all parts of the cell.
6.  Predict the products when an ionic solution is electrolyzed in water solution.
7.  Use standard electrode potentials to:
   a)  compare the relative strengths of different oxidizing agents;  different reducing agents.
   b)  calculate a cell voltage at standard concentrations.
   c)  decide whether or not a given redox reaction will occur spontaneously at standard concentrations.

Chapter 22 

1.,  Write a balanced equation for a nuclear reaction, given the identities of all but one of the reactants and products.
2.  Write typical nuclear equations to represent fission and fusion processes and discuss the characteristics of these reactions.