outline and discuss the following aromatic hydrocarbons. Aspartane, chlorobenzene, benzoic acid, aniline, phenol, and styrene. Discuss some common uses. Discuss ortho-meta-and para positions of additions to benzene. List and discuss 4-5 common properties of aromatic compounds. Outline that aromatics, like benzene do not undergo addition reactions, they undergo substitution reactions. Give examples of the 3 different types or substitutions

Correct and analyze the textbook homework problems which were due today. Define and discuss aromatic hydrocarbons, all of which are based on the benzene molecule. Structures and uses for toluene and naphthalin are discussed. Medicinal uses for tolu balsam also discussed.

Discuss alkene isomers. Show structurally why alkene isomers will only begin with a minimum of 4 carbons. Exhibit, using 1-butene as the hydrocarbon, why there are 4 isomers when the formula's indicate a maximum of 3.
Write the chemical reactions which occur during addition reaction of halogens or halogen halides. Indicate why the concentration of halogen will determine the additions formula of the alkenes. Discuss hydrogenation with hydrogen as the reagent. Indicate why hydrogenated oils are solids and act like a preservative. Discuss the Markovnokov rule, and show examples.

Work the nomenclature for typical alkane molecules. Discuss alkane properties, including boiling point, melting point, color, state, smell. Discuss how they react with oxygen to form carbon dioxide and water. Show how they also react with halogens in the presence of UV light. Introduce cycloalkanes, particularly cyclopropane and cyclobutane. Define strained hydrocarbons with bent angles and weak bonds. Introduce alkenes, the general formula and types of isotopes.

Discuss why carbon compounds are stable based on bond strength and speed of reaction. Introduce the five main subdivision of alkanes. Generate the general formula. Define which are gases, liquids, and solids. Sketch and name the 5 isotopes of hexane. Discuss the nomenclature regulation for naming alkanes. Present 2-3 examples on the board.

Elicit the 4 bond formations which carbon attains to complete an octet. Define isomers. Discuss and use examples of structural isomers and stereoisomers. Define with examples geometric isomers and optical isomers. Discuss rotation of light connected with optical isomers. Define and use examples of chiral molecules and the definition of enantiomers.

Use the formula E(cell) = E (cathode) - E(anode). Determine that when the total is positive, the reaction is product favored. Use table 19.1 to demonstrate that the more positive the E total, the better the oxidizing ability. The more negative the value of reduction potential, the less likely the 1/2 reaction will occur.

Measurement depends on half cell and net reaction, the concentration of reactants and products, and the pressure and temperature of gaseous reactants. Determination of standard potential, Ecell, is performed under standard conditions. The standard hydrogen electrode (SHE) is the favored reaction. The reduction of hydrogen at the electrode and the oxidation of zinc at the anode are listed as half reactions. The potential energy of this reaction produces a reading of 0.76 volts as standard.

Demonstrate in the lab the electrolysis of water, which is the reverse of how a battery works. Electrolysis uses electricity to produce chemical energy. Introduce electromotive force, EMF, as the difference in potential energy of electrons at the electrodes. Define it as the force needed to move the electrons between the electrodes. Define the units as volts. Define what one volt as 1 joule/ coulomb.

Label, define and describe the make up of the voltaic cell diagram, Write Both half cell formulas and then the net formula, Discuss the importance of the salt bridge. Have Joshua sketch a second voltaic cell using a different chemical formulation, label and describe each cell part. Introduce commercial voltaic cells (batteries). Use sketches of dry cells and describe the anode and cathode reactions, along the the paste needed transfer the electrons.