Intermolecular Forces, Liquids, and Solids (Chapter 11) Very brief review of Lewis structures and molecular geometry Draw Lewis structures for and determine polarity of molecules through sp 3 8.45 8.64, 9.31 9.38 hybridization (8.5-8.7, 9.1-9.6) The kinetic-molecular description of gases, liquids and solids State assumptions of kinetic-molecular theory of gases (10.7) 10.71 10.74 Describe molecular level differences between gases, liquids, and solids (11.1) 11.1, 11.9 11.12 Intermolecular forces and their effect on properties Given a substance identify its intermolecular forces (11.2) 11.13 11.20 Properties of liquids and solids Define surface tension and viscosity and predict trends based on intermolecular forces (11.3) Arrange a series of compounds in order of increasing or decreasing boiling/freezing point (11.3) 11.29-11.31 11.5, 11.21-11.27, 11.79 11.83, 11.100, 11.110 Interpret a phase diagram and locate the triple point and critical points (11.4, 11.6) 11.6, 11.41-11.42, 11.51 11.56 Define vapor pressure and relate it to boiling point (11.5) 11.43 11.50, 11.91 Identify the three basic types of unit cell cubic, body-centered cubic, and facecentered cubic (11.7) Identify the bonding types molecular, covalent network, ionic, and metallic - in various solids (11.8) 11.59 11.68 11.69 11.78
Properties of Solutions (Chapter 13) The solution process - energetics Identify the endothermicity and exothermicity of steps in the solution process 13.13-13.14 (13.1) Identify the role of entropy in the solution process (13.1) 13.3 Define the terms unsaturated, saturated, and supersaturated (13.2) 13.5, 13.21-13.26 Predict solubilities based on intermolecular forces (13.3) 13.7, 13.15-13.16, 13.29-13.30, 13.87 State and predict effects of temperature and pressure on solubility (13.3) Methods of expressing concentrations Work numerically with the expressions of mass percentage, ppm, ppb, molarity, molality, and mole fraction (4.5, 13.4) Colligative properties Describe the four colligative properties of solutions and write the mathematical relationships that apply to each (13.5) Apply Raoult s Law and the relationships between concentration and freezing point, boiling point, and osmosis to a variety of problem situations (13.5) Colloids 13.8, 13.31-13.33, 13.89-13.90 13.9, 13.35-13.56 13.10-13.11, 13.57-13.80, 13.96, 13.100-13.103 Qualitatively describe colloids (13.6) 13.83-13.86
Chemical Kinetics (Chapter 14) Methods of expressing rates Given a chemical reaction, express the rate in terms of the stoichiometry (14.2) 14.1-14.4 Factors that affect reaction rates Identify factors that affect a reaction rate and their effect (14.1) Given experimental initial rate information, determine the rate law for a reaction 14.13-14.34 (14.3) Given sufficient concentration/time information, find missing information for 14.35-14.46 first- and second- order reactions (14.4) Use half-life relationships for first- and second-order reactions to find missing 14.6 information (14.4) Describe molecularly the effect of temperature on reaction rate (14.5) 14.5,14.7 Apply the Arrhenius equation (14.5) 14.47-14.60 Qualitatively describe the mechanisms of homogeneous, heterogeneous, and enzyme catalysis (14.7) Mechanisms and molecularity Identify the molecularity of an elementary step 14.61-14.64 Combine given chemical equations to result in a desired chemical equation 14.67, 14.70
Chemical Equilibrium (Chapter 15) The concept of equilibrium Describe the concept of a dynamic equilibrium (15.1) The equilibrium constant Write K c and K p for a given system to include heterogeneous systems (15.3-15.4) 15.11-15.14 Relate K c and K p (15.2) 15.17-15.18 Interpreting and working with equilibrium constants Relate chemical equations and equilibrium constants (reverse, take reciprocal, 15.19-15.26 etc.) (15.3) Given sufficient information, determine whether or not a system is at equilibrium 15.2-15.7 (15.2) Predict direction of equilibrium (to the left, to the right) based on value of 15.15-15.16 equilibrium constant (15.3) Calculating equilibrium constants Find the value of the equilibrium constant given equilibrium concentrations or 15.27-15.34 missing equilibrium concentrations given sufficient information (15.5) Use the equilibrium constant and given concentrations to predict the direction of 15.35 15.38 reaction (reaction quotient) (15.6) Calculate equilibrium concentrations given starting concentrations and the 15.39-15.50 equilibrium constant (15.6) LeChâtelier's Principle Predict shifts in equilibrium due to changes in concentration, volume, temperature, pressure, or the addition of catalyst (15.7) 15.8-15.9, 15.51-15.56 (in 15.50, CaCrO 4 should be a solid)
Acid-base equilibria (Chapter 16) Review of current acid-base concepts Arrhenius Theory (16.1) 16.15-16.16 Identify substances as Bronsted-Lowry acids or bases (16.2) Identify conjugate acid-base pairs (16.2) 16.17-16.24 Determine relative acidity or basicity of substances (16.2) 16.25-16.28, 16.107 The autoionization of water Given hydronium or hydroxide concentration, determine the other (16.3) 16.29-16.34 The ph scale Given hydronium, hydroxide, ph, and/or poh determine the other values (16.4) 16.35-16.42, 16.111 Calculations involving strong acids and bases Determine hydronium, hydroxide, ph, and/or poh values given a concentration of a strong acid or base (16.5) Calculations involving weak acids Given sufficient information, determine hydronium, hydroxide, ph, poh, K a, and/or percent ionization for a weak acid solution (16.6) Calculations involving weak bases Given sufficient information, determine hydronium, hydroxide, ph, poh, K a, and/or percent ionization for a weak base solution (16.7) 16.43-16.50, 16.110, 16.112, 16.122-16.123 16.51-16.70, 16.105-16.106, 16.113-16.115, 16.130 16.71-16.78, 16.118-16.119,16.127 Relationship between K a and K b Determine K a and K b for a conjugate acid/base pair given one of them (16.8) 16.79-16.82 Acid-base properties of salt solutions Given sufficient information, determine hydronium, hydroxide, ph, poh, K a, and/or percent ionization for a salt solution (16.9) 16.83-16.90, 16.116 Acid-base behavior and chemical structure Identify factors that affect acid and base strengths (16.10) 16.91-16.92 Evaluate the relative acidity or basicity of a series of compounds (16.10) 16.93-16.98, 16.120 Lewis acids and bases Identify materials as Lewis acids or bases (16.11) 16.99-16.104, 16.125
Other Aspects of Aqueous Equilibria (Chapter 17) The Common Ion Effect Identify common ions in a given solution (17.1) 17.13-17.14 Calculate the ph and associated quantities in systems made with compounds 17.15-17.18 containing common ions (17.1) Buffered solutions Define and identify buffer systems (17.2) 17.19-17.20 Calculate the ph and associated quantities in buffer systems (17.2) 17.21-17.26 Calculate changes in ph when acids and bases are added to buffer solutions (17.2) 17.27-17.28 Acid-base titrations 17.29-17.32 Generate titration curves for strong acid-strong base, weak acid-strong base, polyprotic acid titrations (17.3) Solubility equilibria 17.33-17.38 Given any chemical equation expressing the dissolution of a solid, write the 17.39-17.46 mathematical expression for the K sp (17.4) Given sufficient information, calculate missing information related to a solubility 17.49-17.50, 17.53- situation (17.4-17..5) 17.56, 17.59-17.62 Predict solubility based on the introduction of common ions (17.5) 17.57-17.58
Electrochemistry (Chapter 20) Oxidation States and Oxidation-Reduction Reactions Use oxidation number to identify the species oxidized, reduced, the oxidizing 20.11-20.16 agent and reducing agent in a redox reaction (20.1) Balancing Oxidation-Reduction Equations Use the half-reaction method to balance redox reactions in neutral, acidic, and 20.17-20.22 basic solution (20.2) Voltaic Cells Identify the anode and cathode in a voltaic cell (20.3) 20.25-20.26 Find the standard cell potential of a voltaic cell (20.4) 20.27-20.40 Identify the relative strengths of oxidizing agents and reducing agents from 20.41-20.48 standard reduction half-cell potentials (20.4) Determine the cell potential of a cell under nonstandard conditions using the 20.37-20.68 Nernst equation (20.6) Electrolysis Manipulate equations relating current, time, moles of electrons, and mass to determine missing information (20.9) 20.87-20.89, 20.91-20.92
Chemical Thermodynamics (Chapter 19) Spontaneous Processes Distinguish between the terms spontaneous process and nonspontaneous process (19.1) Distinguish between reversible and irreversible processes (19.1) 19.9-19.20 Entropy and the Second Law of Thermodynamics Describe the role of entropy in determining the spontaneity of a process (19.2) State and apply the Second Law of Thermodynamics (19.2) 19.25-19.26 Given sufficient information, determine the entropy change in a chemical or physical process (19.2, 19.4) Gibbs Free Energy Given sufficient information, calculate the Gibbs Free Energy change for a reaction (19.5) 19.21-19.24, 19.27-19.28, 19.43-19.50 19.53-19.60, 19.69-19.72 19.61-19.68 Determine temperature ranges of spontaneity based on enthalpy and entropy changes (19.6) Free Energy and the Equilibrium Constant Manipulate the relationships between ΔG and K and E (19.7) 19.73-19.82