hybrid orbitals... used to describe the shapes of molecules. used to describe properties of various...
TRANSCRIPT
![Page 1: Hybrid orbitals... Used to describe the shapes of molecules. Used to describe properties of various types of bonds holding atoms together. Used to discuss](https://reader030.vdocument.in/reader030/viewer/2022032612/56649ef15503460f94c02863/html5/thumbnails/1.jpg)
Hybrid orbitals . . .
• Used to describe the shapes of molecules.
• Used to describe properties of various types of bonds holding atoms together.
• Used to discuss how molecules react.
• Used to make predictions about reactions.
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What are atomic orbitals?
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What are atomic orbitals?
• Atomic orbitals are equations that describe the probability of finding electrons in an atom.
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What are atomic orbitals?
• Atomic orbitals are equations that describe the probability of finding electrons in an atom.
• Atomic orbitals are 3-D surfaces.
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Shapes of Atomic Orbitals
• s orbitals are spherical surfaces
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Shapes of Atomic Orbitals
• s orbitals are spherical surfaces
• p orbitals are two-lobed surfaces
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There are three p orbitals and one s orbital.
• The p orbitals are orthogonal to each other.
• The spherical s orbital is centered at the origin.
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s
px
py
pz
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s
px
py
pz
The p orbitals liealong the x, y, and zaxes.
All are centered at the origin.
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Here are all four of the atomic orbitals relativeto each other.
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Adding Equations
• Equations can be added or subtracted.
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Adding Equations
• Equations can be added or subtracted.
• The result is a new equation.
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Let’s add some (relatively) simple equations. . .
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Y = sin x
Two sine waves. . .
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sin x + sin x
Adding the equations results in a functionwith twice the amplitude.
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sin x - sin x
Subtracting a sine wave results in a functionwith zero amplitude.
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sin x - sin x
Subtracting a sine wave results in a functionwith zero amplitude.
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We’re not limited to adding or subtracting just two equations . . .
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y = sin x
y = (1/3) sin 3x
y = (1/5) sin 5x
y = (1/7) sin 7x
y = (1/9) sin 9x
y = (1/11) sin 11x
y = (1/13) sin 13x
Here’s a bunch o’ sine functions . . .
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Remember that atomic orbitals are also mathematical equations, just a tad more
complicated . . .
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s
px
py
pz
1
2
1
2
3 ( )cos
1
2
3 ( )cos ( )sin
1
2
3 ( )sin ( )sin
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Hybridization of atomic orbitals
Hybridization is the combining of atomic orbitals to create new orbitals
The number of hybrid orbitals depends on how many atomic orbitals
one adds together.
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n AO’s n HO’s
S
P
P
P
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n AO’s n HO’s
2 sp hybridsS
P
P
P
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n AO’s n HO’s
2 sp hybridsS
P
P
P
s + p
s - p
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n AO’s n HO’s
3 sp2 hybridsS
P
P
P
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n AO’s n HO’s
3 sp2 hybridsS
P
P
P
s + p + ps + p - ps - p - p
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n AO’s n HO’s
4 sp3 hybrids
S
P
P
P
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n AO’s n HO’s
4 sp3 hybrids
S
P
P
P
s + p + p + ps + p + p - ps + p - p - ps - p - p - p
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Phases of Orbitals
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“s+p”
sp hybrid
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“s-p”
“s+p”
sp hybrid
sp hybrid
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LET’S HYBRIDIZE!
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Let’s add the s orbitalto one of the p orbitals.
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s + p
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s + p
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s + p
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s + p
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s + p
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s + p
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One sp hybrid orbital.
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Now let’s subtract s from p.
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p - s
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p - s
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p - s
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p - s
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p - s
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p - s
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Another sp hybrid orbital.
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p + s
p - s
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sp hybrid
sp hybrid
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sp hybrid
sp hybridWhere are theunhybridized
p orbitals?
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The unhybridized orbitals arestill there.
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pz
py
sp
sp
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