1Hybridization
HybridizationHow atomic orbitals form other orbitals that are directional
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2
Hybridization
The shapes of the atomic orbitals are inappropriatefor the formation of bonds within the molecules. For example, here are the shapes of the s and patomic orbitals:
X
Y
Z
pzs px py
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Hybridization
To share electrons, the electron wave needs to bein the direction of the atom be bonded. The sorbital is not directional and the p orbitals aredirected along the x, y and z axises, but equally inboth positive and negative directions.
X
Y
Z
pzs px py
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Hybridization
To solve this problem, recall that these are waves. As such one can recombine them in such a way asto form new waves that, although look different, areoverall identical. Here are the ways that they arecombined.
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Hybridization
The first combination is to combine the s orbital withone of the p orbitals. These are referred to as sphybrids. There are 2 to start with and 2 resultant.
– ½ !½
!+ ½ ½
Red here indicates a “trouth” in the wave functionand Green represents a “peak”.
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Hybridization
The first combination is to combine the s orbital withone of the p orbitals. These are referred to as sphybrids. There are 2 to start with and 2 resultant.
The small “trouth” in the hybrids are usually notshown in the overall picture since they are notinvolved in the final bonding. The two togetherlooks like this:
X
Along one of the axes.
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Hybridization
More complicated is the sp2 hybrid formed from an sorbital 2 of the p orbitals. There are 3 to startingorbitals and 3 resulting hybrid orbitals.
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Hybridization
The sp2 hybrid formations:
– ½ !
!½
– ¼
!+ ½
¼
+ ½
– ¼¼
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Hybridization
...or more simply for the sp2 hybrid formations:
!+
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Hybridization
The next more complicated combination is thecombination the s orbital with three of the p orbitals. These are referred to as sp3 hybrids. There are 4 tostart with and 4 resulting orbitals.
These are shown on the next slide.
11
Y
Hybridization
Combinating 1 s orbitalwith 3 p orbitals yield 4 sp3
hybrids.
X
! Z
X
Y
+
Z Z
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Hybridization
or, showing sp3 hybrid formations altogether:
Y
X
Y
+
Z
ZX!
13
X
Hybridization
So far these are the hybrids allowed for the rule of8. The geometry of these are:
X
Y
ZX
sp3 - tetrahedralsp - linear sp2 - trigonal
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Hybridization
There are 2 more hybrids which use the d orbitals. These hybrids are for those central atoms whichhave 10 or 12 electrons about them.
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Hybridization
For those central atoms which have 10 electronsabout them, a hybrid is formed from an s, 3 ps and1 d orbital to for 5 sp3d hybrids.
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Hybridization
For those central atoms which have 10 electronsabout them, a hybrid is formed from an s, 3 ps and1 d orbital to for 5 sp3d hybrids. These look like:
Z
Y
X
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X
Z
Y
Hybridization
This is a trigonal bipyramid. One can envision thisas two orbitals on the y-axis, up and down, andthree around the waist at 120E from each other:
back
to the side
forward
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Hybridization
For those central atoms which have 12 electronsabout them, a hybrid is formed from an s, 3 ps and2 d orbital to for 6 sp3d2 hybrids.
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Hybridization
For those central atoms which have 12 electronsabout them, a hybrid is formed from an s, 3 ps and2 d orbital to for 6 sp3d2 hybrids. This looks like:
X
Z
Y
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Hybridization
This is the octahedral arrangement with 2 orbital oneach of the axis in the + and – direction:
X
Z
Y
Hybridization
X
Z
Y
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Hybridization
Hybrids are formed from the following atomicorbitals, yielding the following shapes for the orbitalsformed:
1 s and 1 p - 2 sp hybrids - linear 1 s and 2 ps - 3 sp2 hybrids - trigonal1 s and 3 ps - 4 sp3 hybrids - tetrahedral1 s, 3 ps and 1 d - 5 sp3d hybrids - trigonal bipyramid1 s, 3 ps and 2 ds- 6 sp3d2 hybrids - octahedral
22The End of Hybridization Follow this up with the 2nd slideshow on hybridization
The End of HybridizationFollow this up with the 2nd slideshow on
hybridization
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