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Ch 5.2a Hybridization | General Chemistry | YouTubeToText
YouTube Transcript: Ch 5.2a Hybridization
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all right so we can explain bonding
through the combination
of our atomic orbitals however if we
start to think about something like
water and we draw the lewis structure
for this and we start to think about this
this
overlap of s orbitals on the hydrogens
and maybe it's the p orbitals in the
oxygens that are overlapping
so if we draw our oxygen we know that we
can draw our p
orbitals we know from our quantum mechanics
mechanics
that a p orbital is 90 degrees to each other
so we can take this overlap and take the
hydrogen s
orbitals and explain the potential
bonding in there
but let's think about what this bond
this model
actually means our model actually means
is that the
bond angle for the hydrogen oxygen
hydrogen bond is 90 degrees
and that's just wrong if we actually
look at our data if we actually look at
we know that our bond angle is actually
right around
104 degrees so this produce to be
a problem for our drawings
so when we actually have to think about
this we have
to create new kinds of orbitals in here
so our next chapter is about hybridization
hybridization
and your two learning outcomes from
hybridization is to go ahead and
explain the concept of atomic orbital hybridization
hybridization
and you're also going to determine the
hybrid orbitals associated with
different molecular geometries
so let's just think about the different
ideas inside
of hybridization hybridization the first one
one
is that they only exist in covalent
molecules so you can forget about ionic
compounds we're not going to think about
that for this class
hybrid orbitals are going to have
different shapes
than the atomic orbitals so remember
your atomic orbitals your
s is going to be that dumbbell or the sphere
sphere
the p orbitals are going to be the
dumbbells the d's are kind of the clover leafs
leafs
but these are going to have new shapes
and they actually form from linear combinations
combinations
these are mathematical combinations of the
the
atomic orbitals another idea is each
hybrid orbital is going to have the same shape
shape
and the same energy so these are
these hybridized orbitals are going to
be degenerate
and we've already talked about vesper
theory that this hybridization
matches what we've already learned about
vesper theory
and anytime we have unhybridized orbitals
orbitals
they are going to able to form pi
interactions and all of your hybrid orbitals
orbitals
form sigma interactions so when we're
talking about hybrid orbitals they're
going to create
sigma bonds so let's look at one example
of this hybridization so let's look at
this molecule that we've drawn on here
uh based on vesper theory we know that
this is going to be a linear molecule
with a 180 degree bond angle
so that works out just great for for
vesper theory and lewis structures
but how can we think about this in terms
of hybridization
so when we look at the carbon atoms we
want to think about what it could
actually become
so in hybridization what we're going to
do for this is we're going to take the 2s
2s
and the 2p orbital over here
and hey we are going to form a hybrid orbital
orbital
is going to be called an sp
and there's going to be two of them and
then we're still going to have
our two p orbitals that are left over
so these are able to form the pi bonds
and these over here are able to form the
sigma bonds
so remember if we looked at our atomic
orbitals before
we see a triple bond here there should
be one sigma bond in here
and two pi bonds so remember that these
are going to form your pi bonds over here
here
your s and p or your sp orbital
hybridized orbitals are going to form
the sigma bonds
over here so if we actually hybridize
this s and p orbital what does this
actually look like
remember we are going to take linear combinations
combinations
so we look at our carbon atom we look at
the 2s
orbital and we're going to put on top of this
this
our p orbital so just remember our p
orbital has some sort of positive wave character
character
the other side of the lobe has some sort
of negative wave character
and then if we just arbitrarily choose
this as
a positive lobe we can see that we can have
have
d uh constructive interference
where we have the same signs over here
we have constructive
interference so we end up getting a
and then we actually have two of them so
this is one of them
the other one is just going to be
the other side of that
and that other side is that other p orbital
orbital
and that makes perfect sense for the
bonding that is happening in this molecule
molecule
that we have some sort of lobe that
looks like this
and our hydrogen s orbital can bond over here
here
and the other hydrogen 1s orbital can
bond over here
and then our hybrid orbitals match what
we're expecting
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