[Disclaimer: All images were grabbed by doing an image
search on Google.]
As I’ve been teaching introductory chemistry to two
different groups of students (science majors and non-science majors), I’ve been
pondering how chemists use different representations to explain tiny things
that we cannot see. A chemistry demo in class gives the viewer a macroscopic
observation of a chemical reaction – the louder and brighter, the better! But
the whizz-bang of the demo is merely a prelude, at least in the mind of a
chemistry teacher, to the microscopic (or perhaps more accurately nanoscopic)
description that “explains” the observation.
The modern expensive chemistry textbook is fully illustrated
with colored balls and sticks connected to each other in a sometimes intricate
arrangement. “Atoms First” is the current fad in chemistry textbooks. What this
means is that the atomistic or molecular view takes center stage in the early
chapters. Older textbooks had fewer pictures and started with macroscopic
observations of chemical reactions but then used strange symbols and equations
to represent them.
As a quantum mechanic who spends time thinking about the
nature of the chemical bond, I personally like having atoms and molecules be
front and center. However, picking a suitable model of the atom to describe the
invisible (to us) particles can be challenging. It is clear that the heavily
mathematical quantum model that I teach in an upper division physical chemistry
course is unsuitable at the introductory level. In the non-majors class, we use
the Bohr/shell model, not just for the hydrogen atom (where it works
marvelously) but for every other atom in the periodic table where the
simplistic model is actually wrong. It is however very, very useful. Students
can get a feel for general trends in the periodic table and an atomistic level
description of chemistry just using the shell model.
In science majors chemistry, we wade into atomic orbitals.
This allows a finer grain description of atomic properties across the periodic
table and a more detailed description of chemical bonds. The students are
introduced to the “four quantum numbers” without much idea where they come from
or why they are used. (An alternative approach that I have used ignores the
numbers and makes use of photoelectron spectroscopy data.) We draw pictures of
circles, dumbbells and cloverleafs alongside energy diagrams – and it’s a
wonder that the students aren’t more confused as we throw a dizzying area of
symbols and representations at them – all in an attempt to make visible the
invisible.
Here’s an example. All my students recognize the symbolic
formula for the water molecule, H2O. (This is thanks to commercial
product advertising, much more than chemistry classes!) Even without my telling
them, I can project the following “space-filling” picture and they can all
automatically tell me that it is a molecule of H2O.
They have no problem recognizing the ball-and-stick model
either. Do either of these pictures represent what a water molecule “truly”
looks like? Why do we choose one representation over the other? (These are good
questions to toss at students who often haven’t stopped to think about it.)
Here’s a shell model showing just the valence electrons.
Which can be “reduced” to the Lewis structure of the water
molecule.
And after talking about Valence Shell Electron Pair
Repulsion (VSEPR) Theory to predict molecular shape, we talk about
“hybridization”. I’m pretty sure the students are rather clueless as to why we
teach them this. (Some instructors may be clueless too.)
And if you were a Molecular Orbital aficionado you might
show the students the following diagram from an Inorganic Chemistry textbook.
My students in both classes learn how to draw Lewis
structures. In the non-majors class we talk about the principle of keeping
electron clouds away from each other (explaining the difference between Pauli
repulsion and electrostatic repulsion is not helpful to them so we don’t delve
into it). I don’t use the term VSEPR theory since I want students to understand
the concept and not try to memorize a fancy term.
In the majors introductory class, they do need to know the
fancy term and we do discuss the qualitative difference between the
aforementioned types of repulsion (although it’s unclear to me that all but the
strongest students actually get the idea). Then I dutifully cover hybridization
because we have many General Chemistry sections, and students are expected to
have seen this before they get to Organic Chemistry. While I think I’ve managed
to persuade most of my colleagues that d-orbitals hardly contribute to
“hypervalent” molecules, it wasn’t until the textbooks (30 years late) started
mentioning this in passing that I’ve seen instructors move away from using it.
I do very little molecular orbital theory in my General Chemistry class even
though it is “covered” in the textbook, although I do cover it in great detail
when I teach upper division physical chemistry and/or inorganic chemistry.
We’ve got all these different representations to discuss the
different properties of a single water molecule. But that’s not how any of us
experiences water. We experience it in dollops of gazillions of molecules. Now
clearly no one is going to draw a mole (6.022 x 1023) of water
molecules, the amount of water you might experience cupped in your hands.
Instead, we have pictures like the one below to tell us
about the wonders of intermolecular forces! All represented by just five molecules.
Where am I going with all this? I don’t really know. But
writing about it has made me more acute to the myriad ways that chemistry is
represented. As an experienced practitioner, I see different symbols and my
trained brain knows what information to extract from them and to cut straight
to the salient points being illustrated. Students newly exposed to chemistry,
on the other hand, do not have that advantage. I guess I’m trying to remind
myself to be more judicious about the models that I use, to take wise advantage
of the power of illustration, but to point out to my students why certain
representations are being used and not to assume that the “picture tells a
thousand words”.
Finally, I’m amazed by the ability of the human brain that
conceptualizes all this abstract model with the aid of such pictures and
illustrations. This is how we see that which is unseen. Through Art!
So glad you are doing this! With my high school students I am working on being explicit about modeling and why it's useful. Every time we introduce a new model we discuss what it represents, what information it conveys, when it is most useful, and what the limitations are. I hope in doing this that they connect rather than compartmentalize these models and remember that they are all different ways of looking at a visible phenomenon!
ReplyDeleteThis is an area where I need to keep improving. Happy teaching!
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