what this will also allow us to do is to understand
understand
something else a little bit more
complicated and what we can also understand
understand
is this concept of delocalization
on here so this is actually the lewis
structure of the benzene model
model and it's very flawed because we
have to draw two different lewis structures
structures
to kind of explain what is actually
going on
in here because in reality what we have
is some sort of molecule
that we can express kind of like this
where we have electron density
that is in a circular kind of fashion
so all of these atomic orbital are these
uh carbon atoms
are all sp2 hybridized which means that
there is a p
orbital to form those pi interactions
and then all the carbon atoms will have
some sort of p
orbital that is available for bonding
and this creates the ring of electron density
density
the benzene ring
so to give you a better picture of this
what we can do is we can go to this
website kentube3d.com
and we can look at the benzene orbitals
on here
so here's a picture of the benzene
orbitals on here
so uh in the picture in the upper right
hand corner you can see the sp2
hybridized forms all the sigma bonds
on here so we can go ahead and first
think about all the sp2
hybridized orbitals and they form these
kind of orange kind of orbitals on here
so that works really great and then what
we have left over
are our remaining p orbitals that are
drawn above and below
and what we end up getting is a ring of
electron density
and this is what we call delocalized
electrons and that's really important
for this benzene molecule
so we end up getting these p orbitals
that can form this ring like of
electron density on here
and then if we actually show the
resulting bonding orbital
on here we see that we end up getting a
whole bunch of pi
interactions above and below
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