General Chemistry Spring 2009

In this segment I do go over how to answer PS6.1 - PS6.7. Review this problem set podcast in preparation for Exam #2 there are many good problem solving examples.

In this segment I do go over how to answer PS10.2, PS10.6 - PS10.9. Review this problem set podcast in preparation for Exam #3 there are many good problem solving examples.

In this clip I worked out all of the problems on the Spring 2003 CHEM 1515 Examination.

In this segment I Worked out all of the problems on the Exam #2 for the Fall 2006 semester. This will be an excellent review for the final.

In this segment I cover the orbital diagram for elements from hydrogen through krypton. I discuss the importance of spin pairing energy, Hund's rule and the exceptions for the electron configuration for chromium and copper.

In this clip I do a set of multiple choice questions covering a range of topics including; this clip begins with a density problem using mass percent; followed by a straightforward unit conversion problem; then a problem determining the fomula for a compound with an unknown metallic ion; a problem applying the definition of a compound and an element as viewed from the particulate level;then another limiting reagent problem with a twist; then a fun Hess' Law problem determining the enthalpy of formation for a compound; a simple problem based on formula units; and finally a set of three problems using electron configurations. Lots of fun problems on this exam....enjoy!

In this clip I worked out all of the problems on the Spring 2007 CHEM 1515 Examination 2.

In this segment I Worked out all of the problems on the Exam #2 for the Spring 2006 semester. This will be an excellent review for the final.

In this lecture we began by discussing the energy of the electron in the Bohr Model of the hydrogen atom. The lowest energy the electron can have is when it is in n = 1 level. As the electron moves to higher levels (n =2, n = 3, etc.) the electron must absorb energy. An atom with an electron in an energy level greater than n = 1 is said to be in an excited state. We talked more about the energy of the levels the electron can occupy in a hydrogen atom. Next we discussed the shell model for the atom. We reviewed the ionization energy of the first twenty elements in the periodic table. Based on the ionization energies and our understanding of the relationship between the charge on the nucleus and the distance the electron can be from the nucleus we arrived at the idea that electrons occupy different shells. We then looked at photoelectron spectra data and found that electrons in shells (shells greater than n = 1) had different energies. We introdcued the idea of subsehlls to explain the different energies of el

In this lecture we began by reviewing responses from the ACA and the PLE. We then covered two more examples of electron configurations for Europium and for rhenium. We talked about f-orbitals and how to manage the d-orbitals for elements just before the f-block, in the f-block and following the filling of the 4f-block. We looked at the orbital shapes for 's', 'p', 'd' and 'f' orbital. Then we looked at orbital diagrams for the element hydrogen through copper. Check the podcast on Orbital Diagrams for Multielectron Atoms for a brief review of this material.