Course Objectives by Chapter Title

Bonding: General Concepts

After completing this chapter, you should be able to:

  1. List and define three types of bonding:  Covalent, Ionic, Polar covalent

  2. Solve for the energy of interaction of an ionic solid

  3. Use the positions of atoms in the periodic table and their electronegativities to predict relative bond polarities

  4. Determine whether or not simple molecules have a dipole moment

  5. Predict the formulas of simple ionic compounds

  6. Predict the relative sizes of ions

  7. Explain the different steps involved when elements form ionic solids, especially concerning crystal lattice structures

  8. Define the following: Environment independent,  Model, Limitations

  9. Describe how a model is made

  10. Describe how a model is useful

  11. Calculate heats of reactions for bond energies

  12. Draw Lewis structures for a variety of covalent molecules

  13. Predict molecular geometry by using the VSEPR model

Covalent Bonding :  Orbitals

After completing this chapter, you should be able to:

  1. Use electronegativity to predict the ionic/covalent character of bonds.

  2. Draw electron dot structures from molecular formulas.

  3. Explain resonance in terms of electron-dot structures.

  4. Determine when a compound will exist as a resonance hybrid.

  5. Use formal charge to predict more favorable resonance structures.

  6. Use VSEPR theory to describe the structure of molecules.

  7. Use molecular geometry to predict bond angle.

  8. Explain covalent bonding and bond strength in terms of the Valence Bond Theory (VBT).

  9. Account for molecular geometries in terms of hybridization and VBT.

  10. Use Molecular Orbital (MO) theory to explain bonding and anti-bonding orbitals, multiple bonds, and s and p bonds.

  11. Combine the concepts of VBT and MO theory to explain resonance hybrids

Liquids and Solids

After completing this chapter, you should be able to:

  1. List intermolecular forces and describe some of the erects on liquids and solids:  Dipole-dipole forces, Hydrogen bonds, London forces

  2. Describe cohesive forces

  3. Describe adhesive forces

  4. Describe surface tension

  5. Explain viscosity

  6. Define the basic terms relating to the structure of solids

  7. Solve simple problem relating to x-ray diffraction by crystals

  8. Discuss bonding in metals

  9. Calculate the density of metals based on the structure of their unit cell

  10. Define and give examples of substitutional and interstitial alloys

  11. Discus the rationale for the packing that is observed in closest packed systems

  12. Classify substances according to the types of and properties of the solids they form

  13. Interconvert between vapor pressure, temperature, and enthalpy of vaporization

  14. Perform calculations regarding the energy of phase change

  15. Extract information from phase diagrams:  Boiling point, Freezing point, Critical temperature, Critical pressure, Triple point critical point

Properties of Solutions

After completing this chapter, you should be able to:

  1. Solve problems relating to the mass, percent, mole fraction, molality, and normality

  2. Determine the miscibility of a variety of solutions

  3. Predict relative solubilities of simple molecules based on structure

  4. Solve problems relating to Henry’s Law

  5. Calculate the vapor pressure of a variety of solutions

  6. Calculate the molar mass from vapor pressure information

  7. Use Raoult’s Law

  8. Solve problems relating to the colligative properties:  Boiling point elevation, Freezing point depression

  9. Solve problems regarding osmosis and molar mass

Chemical Kinetics

After completing this chapter, you should be able to:

  1. Use concentration vs. time data to determine relative reaction rates

  2. Define a rate law

  3. Write the expression for a rate law

  4. Describe the difference between a differential rate law and an integrated rate law

  5. Determine the proper units of a rate constant for any order rate law

  6. Determine the reaction order from concentration vs. time data

  7. Calculate the half-life of a first- or second-order reaction

  8. Evaluate the validity of simple reaction mechanisms

  9. State the criteria for reaction according to the collision model

  10. Solve problems relating to activation energy

  11. Define:  Catalyst, Enzyme, Heterogeneous catalyst, Absorption/adsorption, Hydrogenation, Homogeneous catalyst

Chemical Equilibrium

After completing this chapter, you should be able to:

  1. List some of the characteristics of reactions at equilibrium

  2. Write a mass action expression for a given balanced chemical equation

  3. Solve for Kc or Kp given appropriate data.

  4. Write equilibrium expressions for reactions involving pure solids and liquids

  5. Use the reaction quotient (Q) to predict the direction of chemical reactions toward equilibrium

  6. Use the reaction quotient to aid in solving simple equilibrium problems

  7. Solve many equilibrium problems, and test any assumptions you make

  8. Predict the response of a system to stresses placed on it

Acids and Bases

After completing this chapter, you should be able to:

  1. Define acids and bases using the Bronsted-Lowery model

  2. Identify conjugate acid/base pairs

  3. Write equilibrium expressions for acid dissociations

  4. Compare relative strengths of acids

  5. Solve problems regarding the autoionization of water

  6. Convert between pH, pOH, [OH-], and [H+]

  7. Calculate the pH of strong acid solutions

  8. Calculate the pH and percent dissociation of weak acids solutions

  9. Calculate the pH of a variety of basic solutions

  10. Solve the pH and concentrations of species of polyprotic acids in aqueous solutions

  11. Calculate the pH of a variety so salt solutions

  12. Identify the Lewis acids and bases in a reaction.

Applications of Aqueous Equilibria

After completing this chapter, you should be able to:

  1. Perform calculations on acidic solutions that involve a common ion

  2. Calculate the pH of a buffer solution

  3. Determine the effect of the addition of acids and bases on the pH of buffer solutions

  4. Calculate the pH of a solution where the buffer capacity has been exceeded

  5. Choose among alternatives, the best buffer system for a given pH

  6. Calculate the pH at any point along a curve for the following titrations:  Strong acid – weak base, Weak acid – strong base, Weak base – strong acid

  7. Select the proper indicator for an acid-base titration

  8. Interconvert between solubility and Ksp

  9. Solve problems relating to the common ion effect

  10. Determine whether the mixing of ttwo solutions will produce a precipitate

  11. Calculate the concentration of each ion in a solution in which a precipitate is produced

Spontaneity, Entropy, and Free Energy

After completing this chapter, you should be able to:

  1. Estimate reaction enthalpies from bond energies.
  2. Describe the differences between spontaneous and non-spontaneous events.
  3. Explain how energy changes are related to spontaneity.
  4. Describe how entropy is related to statistical probability and how entropy is related to spontaneous change.
  5. Understand the implications of the Second and Third Laws of Thermodynamics.
  6. Explain how DG is related to spontaneity.
  7. Calculate DS°, DH°, and DG° from tabulated values.
  8. Given a chemical equation or physical change, predict: if whether DH will be + or ­;  if whether DS will            be + or ­;  if whether DG will be + or ­ (or unpredictable due to conflicts between H and S);  if whether the change is spontaneous.
  9. Explain how DG is related to useful work, to equilibria, and to equilibrium constants.
  10. Determine from DH° and DS° how the position of equilibrium in a reaction is affected by changes in temperature.
  11. Use DGf° to determine whether a given reaction will be expected to occur (or be favored; spontaneous).

Electrochemistry

After completing this chapter, you should be able to:

  1. Define electrochemistry.
  2. Distinguish between the types of electrochemical cells.
  3. Given a galvanic cell, identify the cathode and anode, write half-reactions to describe each compartment, and identify the direction of electron and ion flow.
  4. Use and interpret shorthand notation for galvanic cells.
  5. Explain the relationship between DG, E, and spontaneity.
  6. Use the equation DG°=­nFE in calculations.
  7. Explain how standard reduction potentials are determined experimentally.
  8. Use standard reduction potential to calculate E° for a cell.
  9. Explain how changing concentrations may change cell voltage.
  10. Use the Nernst equation to determine E for cells at non-standard conditions.
  11. Explain the operation of an electrolytic cell in terms of E, DG, and spontaneity.
  12. Use standard reduction potentials to determine the electrode reactions for electrolytic cells in aqueous solution.
  13. Perform quantitative calculations given and electrolytic cell and appropriate data.
  14. Use and interpret visual representations of electrochemical cells.