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Ch. 5.2b More hybrid orbitals | General Chemistry | YouTubeToText
YouTube Transcript: Ch. 5.2b More hybrid orbitals
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so we can look at another kind of
bonding and hybridization so let's look
at bh3 we draw the lewis structure for this
this
so this is one of those non octets we
know that we should get a 120 degree
bond angle based on vesper theory so how
does this
actually come about we see that we have
three electron domains
on here so what we're going to do is
we're going to take on the boron
three electron domains and hybridize
them so we're going to take the 2s
and 2 the two p's and we're going to
hybridize them
so that we end up forming degenerate
sp2 hybrid orbitals
and then we have one orbital left over
that is still the 2p that is left
over on here so this hybridization
creates these three sp orbitals
so what we're doing just like last time
we are taking the linear combination of the
the
one of the p orbitals and one of the perpendi
perpendi
the other perpendicular p orbitals and
then we
end up getting three different lobes
so we end up getting our sp hybridized orbital
orbital
which is our sp2 hybridized orbital
which is 120 degrees so if we look at the
the
valence bond theory picture of this we
can actually start off with
this sp2 hybrid orbital
and then we can take the hydrogens and form
form
our sigma bonds over here
and that is how we describe the bonding
in something like
bh3 we can go
from something a little bit more com
complex if we look at
methane and think about methane or in
the water complex
what were the water molecule what we're
looking at is
so that means we want to hybridize four
different orbitals
on here so we're gonna hybridize all of these
these
so we're gonna hybridize all these and
we're gonna form the classic
sp3 hybrid orbital and we actually
hybridize those we will actually form
something that looks like this
this is in a tetrahedron
type configuration so we can once again
have this three-dimensional picture
of this orbital and remember our water example
example
up here our water example up here starts
off with
a sp3 so there's four electron domains there
there
so the oxygen is sp3 hybridized
which gives us a base structure with a
bond angle
of 109.5 so this is your oxygen you have two
two
hydrogens over here so this is 109.5
but remember these electron pairs push these
these
a little bit so this squeezes in a
little bit to get our predicted
104 104.5 degrees so we expect it to
kind of squish
in there just a little bit now we can
get even more complicated so we're not
just gonna have
four things bonded to things sometimes
you'll have five different things bonded
and this comes up to the concept of
expanded octets
so if we think about another molecule
that has some sort of
five electron domains
around it we're going to go ahead and hybridize
hybridize
five of them so when we think about this
in general chemistry
we make sure that we can think about the
availability of the 3d electrons in our hybridization
hybridization
so if we have five electron domains what
we're going to create
now is an sp
3 d hybrid orbital
and that's going to look something like
this so remember here there are five
electron domains and this is
our trigonal bipyramid
and we can predict the bond is going to
look something
like this so our sp3d
we can start to think about this we uh
this kind of configuration and that's
where we get our octahedral
kind of uh electron domain configuration
our d's and then our p orbitals
we're going to take six of these
in there to get an sp3
d2 hybridization which will look something
something
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