Catalog Description CHEM 106. Introductory Chemistry II. 3 3 0. Prerequisite: C or better in CHEM 105. A continuation of CHEM 105 with emphasis on solutions, chemical equilibrium, thermodynamics, kinetics, acid base chemistry, electrochemistry and ionic equilibrium. Degree credit will not be given for both CHEM 102 and 106. This course is also available via Internet. Basic computer knowledge is required for students enrolled in the Internet section.(40.0501)
STUDY GUIDE FOR CHEM 106
THERMOCHEMISTRY
____Sign convention for heat, work, and E
____Calculate PV work
____Calculate q for simple temperature change (no phase or chemical change)
____Calculate specific heat and heat capacity from q and T
____Calculate q for phase change
____Apply the concept of state function
____First Law of Thermodynamics: relate E, q, and w for system and surroundings
____Relate q to changes in state functions at constant V and at constant P
____Determine calorimeter constant
____Estimate heat capacity of dilute aqueous solutions
____Determine reaction enthalpy from calorimetric data
____Determine reaction enthalpy using Hess’ Law
____Write balanced equations for standard formation reactions
____Determine standard reaction enthalpy from standard enthalpies of formation
____Describe energy changes associated with bond breaking and bond formation
____Estimate reaction enthalpy from bond energies
PROPERTIES OF SOLUTION
____Calculate concentrations from amount of solute and solvent (or solution): molality,
Molarity, mole fraction, ppm, ppb, %(w/w) or mass percent, %(w/v) or g/dL
____Classify concentration units according to whether or not they depend on temperature
____Convert from concentration unit to another
____Describe and calculate four colligative properties of solution: vapor pressure lowering,
boiling point elevation, freezing point depression, osmotic pressure
____Determine concentration from colligative properties
____Determine molar mass from colligative properties
KINETICS
____Describe typical time profiles of reactants and products
____Describe factors that affect reaction rates: concentration, temperature, catalyst, surface area
____Interpret a rate law
____Deduce rate law from experimental data: initial rates method
____Deduce rate law from experimental data: half-life method
____Deduce rate law from experimental data: linear plot method
____Deduce pseudo-order from method-of-isolation data
____Identify molecularity of elementary reactions
____Write rate law of an elementary reaction
____Predict rate law from a mechanism
____Identify reaction intermediates in a mechanism
____Describe typical time profiles of reaction intermediates
____Identify catalyst in a reaction mechanism
____Define energy of activation
____Describe how energy of activation is affected by catalyst
____Calculate energy of activation from temperature dependence of rate constant
EQUILIBRIUM
____Define chemical potential and activities
____Calculate reaction quotient, Q
____Relate Q to Keq
____Determine Keq from experimental data
____Apply Le Chatelier’s principle to predict responses of systems in equilibrium to
stress
____Relate Le Chatelier’s principle to relationship between Q and Keq
____Determine extent of reaction given initial conditions and Keq
____Determine Keq when a balanced equation is flipped
____Determine Keq when two chemical equations are added
ACIDS AND BASES
____Write chemical equations associated with Kw, Ka, and Kb
____Identify conjugate acid/base pairs
____Relate pH, pOH, [H+] and [OH-]
____Classify solutions as acidic, basic, or neutral
____Calculate Ka of acid given Kb of conjugate base, and vice versa
____Calculate Keq for neutralization reaction
____Predict the typical magnitude of Keq for neutralization reactions
SOLUBILITY
____Write chemical equations associated with Ksp
____Relate solubility to Ksp
____Relate precipitation to Ksp
____Describe common ion effect on solubility
____Explain how addition of a strong acid helps dissolve an insoluble compound
____Explain how addition of a complexing agent helps dissolve an insoluble compound
THERMODYNAMICS
____Describe the second law of thermodynamics
____Calculate entropy change for simple temperature change
____Calculate entropy change for heat flow at constant temperature (as in phase changes)
____Describe the third law of thermodynamics
____Calculate entropy change for reactions at constant T using Third Law
or “standard” entropies
____Predict algebraic sign of entropy change for reactions at constant T, P
____Predict entropy change for system, surroundings, and universe for various processes
____Relate change in Gibbs free energy to enthalpy and entropy changes
____Relate Gibbs free energy to spontaneity
____Relate standard Gibbs free energy of reaction to Keq
ELECTROCHEMISTRY
____Distinguish between oxidation and reduction
____Put together two half reactions to get a balanced redox reaction
____Describe parts of a galvanic cell
____Interpret standard reduction potentials
____Calculate and interpret standard cell potentials
____Calculate cell potentials using Nernst Equation
____Relate standard cell potential to Keq