General Chemistry Spring 2009

In this clip I go over several of the problems on the Review Problem Set by discussing what Chapters in the textbook should be reviewed to answer the questions. I have also included several podcasts from CHEM 1314 in this list to provide additional sample problems that are similar to the problems on the RPS.

This is a series of flash Cards and animations of molecules to help memorize the necessary information that relates number of bonding groups and lone pair electrons on the central atom with the bond angle and molecular geometry. Accompanying this information is an animation showing what the molecular geometry looks like.

In today's class we continued discussing the face-centered cubic and body centered cubic. We discussed the relationship between edge length and atomic radius for both of these systems and we did several sample problems. We also discussed ionic compounds and looked at how holes can accommodate ions.

In this lecture we continued our discussion of reaction types. In this class we covered neutralization reactions and single replacement reactions. There is a list of acids and bases that everyone must know, and you have to pay close attention to the strong acids and the weak acids because their ionic equations are different. We also looked at strong bases and weak bases. At the end of this lecture we defined molarity and looked at a few examples of problems using molarity.

In this lecture we began discussed Lewis structures for simple molecules. There are a specific series of steps that must be followed to drraw a complete Lewis structure. Several examples were discussed. The examples focused on how to draw a skeletal structure based on deciding from a chemical formula which atom(s) are terminal and which atom(s) are central. Examples with multiple bonds were also discussed.

In this lecture we continued our discussion over Lewis structures by looking at ethane, ethene and ethyne. These compounds are more complicated compared to the compounds discussed in the previous class due to the presence of mulitple central atoms. Bond order and bond lengths were introduced with these three compounds. Ethane has a carbon-carbon bond order of one, ethene has a carbon-carbon bond order of 2 and ethyne a carbon-carbon bond order of three. The next substance discussed was ozone. Ozone was interesting because the concept of resonance and resonance structures was introduced to completely represent the Lewis structure of the allotropic form of oxygen. The oxygen-oxygen bond order was determined. Next we drew the ressonance structures for nitrite (NO2^-) and nitrate (NO3^-). The next grop of compounds considered were the oxyacids such as sulfuric acid, nitric acid, carbonic acid and many others. At the end of the lecture formal charge was introduced and the formal charge for the atoms in a compound

In this lecture we began with a review of VSEPR models. Then we discussed polar bonds, and polar and nonpolar molecules. Then we discussed the types of orbitals that are involved in foming covalent bonds. In today's lecture we focused on examples of covalent bonds in substances that only used atomic orbitals. Right near the end of class we looked at methane, which is a case where atomic orbitals can NOT be used to described the orbitals on carbon that form covalent bonds. We talked about hybrid orbitals.

In today's class we discussed salts and how they can effect the pH of a solution. We started by looking at neutralization reactions to form salts. We did this as a way to classify salts. We then discussed the acid, base or neutral character of salts. For acidic and basic salts we determined how to calculate the equilibrium constant, and we did two sample calculations. Near the end of class we did an example of a common ion problem.

The majority of this class dwelled on administrative details of CHEM 1515 SPRING 2009 and the course web site. During the last 15 minutes of class we started discussing Chapter 20: Thermodynamics 2nd and 3rd Law.

In this clip I do two problems: the first is a solution stoichiometry/limiting reagent combination problem; the second is a calorimetry problem mixing hot and cold water in a calorimeter.