Transcripción de YouTube:
Ch. 5.2b More hybrid orbitals

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Transcripción del video

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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