What we've done so far:
Friday, December 2
Monday, December 5
Wednesday, December 7
Friday, December 9
Friday, December 4
The collision model works quite
well for many different reactions. This idea of collisions between molecules
can be combined with a known rate law to propose possible pathways for
the reaction with a nanoscale view. These step-by-step pathways are
called 13.5 Reaction Mechanisms.
Each step in the pathway is
called an elementary step: remember that adding together all
of the steps must give the overall balanced chemical equation. Note
that the overall balanced chemical equation shows what is happening on
Since an elementary step happens
on the nanoscale, there is a distinct advantage. The rate law for an elementary
step can be predicted based on the step itself. We talked about the
typical possible elementary steps in a pathway.The overall rate will be
dependent on the rate determining step.
Note that intermediates are formed and then consumed.
Read about how chemists deduce mechanisms through elegant experiments - bottom of page 564 and top of page 566.
based on the rate law, is a given mechanism valid?
Clickers! Click here for the document.
draw reaction profiles. Exercises: 51, 52, 54, 62
Monday, December 7
Catalysis allows a reaction to speed up by providing an alternative
route that has a lower Ea.
I drew you a diagram of what this looks like on the reaction coordinate diagram.
The catalyst takes part in the reaction but is not consumed based on
the overall reaction. It can either be inert or re-formed
depending on the type of catalyst.
Exercises: 70, 76, 86, 88, 94, 108, 110, 112.
A little review of MO theory...
Wednesday, December 9
Friday, December 11
Review Class - click here for the clicker questions I covered...
Good luck on the final exam!