Outcomes:

After completing this class, students should be able to:

These course outcomes are effective for Fall 2009. We anticipate a change in these outcomes with the new textbook, starting Winter 2010--namely, to move bonding to Chem &161 and include thermochemistry .

• Ionic and Covalent Bonding
  • Describe the differences between covalent, ionic, and metallic bonds.
  • Apply the octet rule to predict the charge of common cations and anions; explain why there are exceptions to the octet rule.
  • Explain variations in electron configurations and ion formation for the transition metals.
  • Write Lewis structures for atoms, ions and molecules.
  • Predict bond lengths from periodic trends in radii.
  • Use bond energies to estimate enthalpies of reactions.
  • Explain how lattice energy varies with ionic charge and ionic radii, calculate the lattice energy.
  • Use resonance structures to model multiple bonding in molecules and poly-atomic ions and then select the most likely resonance structure by calculating formal charges.
  • Predict whether a bond will be ionic, polar covalent, or non-polar by using electronegativites.
• Molecular Geometry and Chemical Bonding Theory
  • Predict shapes of molecules and poly-atomic ions using VSEPR theory.
  • Explain deviations from ideal geometry in terms of loan-pair repulsions.
  • Predict the polarities of molecules.
  • Define isomers and illustrate with examples.
  • Describe the importance of spectroscopic methods in probing the structure of the molecule.
  • Describe the formation of a covalent bond in terms of valence bond theory and hybridization.
  • Demonstrate the formation of molecular orbitals; determine bond order for simple diatomic molecules.
• States of matter; Liquids and Solids
  • Compare the properties of the three states of matter and relate those properties to the distance between the particles, molecular motion, structure, and attractive forces.
  • Define dispersion forces, dipole-dipole attractions and hydrogen bonding and recognize when they occur.
  • Explain the liquid properties of surface tension, capillary action, viscosity, vapor pressure, and boiling point; describe how these properties are influenced by intermolecular forces.
  • Sketch heating an cooling curves for a substance; calculate the amount of heat absorbed or evolved during a phase change.
  • Identify features of phase diagrams.
  • Describe the structural units, interparticle forces, general properties and give some examples of each type of solid substance: ionic, metallic, network, and molecular.
  • Define a cubic unit cell in a crystalline lattice and perform simple calculations of unit cell mass and density.
• Solutions
  • Explain the factors that influence the solubility of one substance in another.
  • To define the heat of solution and discuss its various energy components.
  • Predict the influence of pressure and temperature on gas solubility.
  • Define and convert amount molarity, molality, mole fraction and mass fraction (percent, parts per million).
  • Describe and calculate the vapor pressure of a solution
  • Identify the colligative properties, explain the cause of each, and calculate the boinling point and freezing point of a solution of a nonvolatile solute.
  • Discuss the colligative properties of solutions and electrolytes.
  • Explain osmosis and describe its applications.
  • Rates of Reaction
  • List and discuss the factors which influence reaction rate.
  • Define reaction rate; obtain average reaction rates and instantaneous reaction rates from concentration versus time data.
  • Explain the terms in a rate equation or a rate law.
  • Use rate data to determine reaction order, write a rate equation, and use a rate equation to predict how a reaction rate varies with changing concentrations.
  • Describe the effect on reaction rate of changes in temperature.
  • Calculate the half-life of a first-order reaction.
  • Show by using an energy plot what happens as two reactant molecules interact to form product molecules and how a catalyst affects a reaction rate.
  • Define reaction mechanism and identify rate-determining steps, catalysts, and intermediates.
• Chemical Equilibrium; Gaseous Reactions
  • Discuss how equilibrium is established.
  • Use Q and K to predict whether a reaction is moving in the forward or the reverse direction.
  • Write equilibrium constant expressions, given balanced chemical equations (both homogeneous and heterogeneous).
  • Calculate the new equilibrium constant from the original constant when the equation is reversed or multiplied by some factor.
  • Make qualitative predictions about he extent of reaction based upon equilibrium constant values; that is, be able to predict whether a reaction is product- or reactant-favored.
  • Show how K and Kp are related.
  • Calculate a value of K using equilibrium concentrations or calculate an equilibrium concentration if K is known.
  • Show by using Le Chaterlier’s principle how changes in concentrations and temperature affect chemical equilibria.
• Thermodynamics and Equilibrium
  • Describe heat and work and the nature of energy transfer.
  • Distinguish between a state function and a path dependent property.
  • State the first, second and third laws of thermodynamics.
  • Explain the concept of entropy; give examples showing how spontaneous processes are accompanied by an increase in the disorder of the system and/or the surroundings.
  • Use entropy and enthalpy changes and Gibbs free energy to predict whether a reaction is product favored; describe the affect of temperature changes on spontaneity.
  • Define equilibrium in terms of minimum free energy; calculate standard free-energy changes form K and vice versa.
  • Relate work to the change in free energy.

• Organic Chemistry
  • Write names and formulas for straight chain alkenes.
  • Draw molecular diagrams for the chair and boat structures of cyclohexane; compare the energies of the two structures.
  • Write names and draw structures for the following functional groups; alkenes, alkynes, alkyl halides, alcohols, ketones, ethers, phenols, carboxylic acids, esters, amides, amines, mono saccharides.
  • Describe physical and chemical behavior of the above types of compounds.