General Chemistry Spring 2009

In today's class we continued our discussion of oxidation and reduction reactions. We discussed how to build an electrochemical cell containing an anode compartment and a cathode compartment. We used Dr. Greenbowe's simulations to construct the cell and measure the voltage of the cell. We discussed the standard hydrogen electrode and its importance.

In today's class we continued our discussion of oxidation and reduction reactions. We discussed the standard reduction potential table and we did several different types of problems using the SRP table. We also discussed free energy and equilibrium constants and their relationship with the standard cell potential.

In this lecture we began by reviewing the electron configurations of chromium and copper. Then we discussed the electron configuration of ions. We discussed electron configurations for cations and anions and how to determine which shells and subshells electrons would be removed from (cations) or added to (anions). Next we discussed effective nuclear charge, we learned how to calculate the effective nuclear charge for any electron in an atom. We then discussed how our electronic structure of the atom can be applied to experimental data for atomic radii and ionization energy. We looked at atomic radii for the elements and discussed how effective nuclear charge explains the trend in atomic radii going across a period. effective nuclear charge can not be used to explain the trend in atomic radii going down a group. That trend is explained in terms of the shell the valence electrons are located. We discussed first ionization energy trends going across a period in terms of ionization energy. We also looked at 1st

This is the lecture that Kerry covered. In this lecture Kerry introduced calorimetry measurements and calculations. She reviewed the relationship between heat, amount of substance, specific heat and change in temperature. She also discussed experiments using the OSU calorimeter and the bomb calorimeter.

In today's class we began our discussion on the concept of chemical equilibrium. We started by watching and discussing some video of a macroscopic equilibrium reaction. We then looked at an equilibrium reaction at the particulate level to better understand reversibility.

In today's class we discussed polarizibility and its importaqnce in dispersion forces. We then turned to vapor pressure, its definition, a particulate animation depicting vapor pressure, the comparison of vapor pressure and pressure due to vapor, and the temperature dependence of vapor pressure in the Clausius-Clapeyron equation.

In this clip I use Excel to plot Ln VP versus 1/T data for a problem similar to PS3.6.

In this clip I do several Lewis structures, discuss formal charge, VSEPR and do several gas law problems.

In this clip I discuss several multiple choice questions. The first multiple question we need to understand the concept of isoelectronic. In the second questions (3’ 35”) we use the concept of ionization energy. The third question (7’ 55”) the electron configuration of a transition metal cation is determined. The fourth question (11’ 38”) we use the energy level diagram for the hydrogen atom to reach the correct answer. The fifth question (14’ 00”) we must match an electron configuration with a particular group in the periodic table. The sixth question (18’ 6”) is a Hess’ Law problem that has some fun features. The seventh question (26’ 22”) we must calculate the enthalpy of combustion.

In this lecture we discuss naming ionic and covalent compounds. We worked several examples.