chapter 1: structure and bonding mcmurry. coverage: 1. electron configurations. 2. lewis structures...
TRANSCRIPT
![Page 1: Chapter 1: Structure and Bonding mcmurry. Coverage: 1. Electron Configurations. 2. Lewis Structures 3. Covalent and Ionic bonds 4. Atomic and Molecular](https://reader035.vdocuments.net/reader035/viewer/2022070403/56649f285503460f94c40e43/html5/thumbnails/1.jpg)
Chapter 1: Structure and
Bondingmcmurry
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Coverage:1. Electron Configurations.2. Lewis Structures3. Covalent and Ionic bonds4. Atomic and Molecular Orbitals5. Hybridization
• Goals:
Write the electron configuration for any element in the periodic table.
Write Lewis line bond structures for simple organic molecules.
Know how to calculate formal charges on atoms.
Know the definitions of a sigma and pi bonds.
Draw energy diagrams for formation of pi and sigma bonds.
Predict the number of sigma and pi bonds in a molecule.
Predict the hybridization of an atom in a molecule.
Predict the approximate bond angles in a molecule.
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Hybridization of Atomic Orbitals
1. AOs on a single atom mix to form new, hybrid orbitals. These hybrid orbitals
have characteristics of both s and p orbitals.
2. Provides a means of explaining observed bond angles in organic molecules.
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1-4
Methane
sp3
CH
H
HH
109.50
The carbon atom is sp3 hybridized to obtain tetrahedral geometry. All bond angles are equal at 109.50.
E
__ s
__ __ __ p
__
__ __ __ __ __ __ __sp3
Promote e- Mix orbitals
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1-5
s + 3 p
=
4 sp3 orbitals
D:\rw32b2a.exe
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1-6
Ethylene sp2 sp2
CH
HC
H
H116.6o
121.7o
The carbon atom is sp2 hybridized to obtain trigonal planar geometry
E
__ s
__ __ __ p
__
__ __ __ __ p __ __ __ sp2 hybrid
Promote e- Mix orbitals
![Page 7: Chapter 1: Structure and Bonding mcmurry. Coverage: 1. Electron Configurations. 2. Lewis Structures 3. Covalent and Ionic bonds 4. Atomic and Molecular](https://reader035.vdocuments.net/reader035/viewer/2022070403/56649f285503460f94c40e43/html5/thumbnails/7.jpg)
1-7
s + 2 p
=
3 sp2 orbitals
sp2 Hybridization
There is one p orbital left over,and it would be along the z axis.
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1-8
Orbital Picture of Ethylene
D:\rw32b2a.exe
![Page 9: Chapter 1: Structure and Bonding mcmurry. Coverage: 1. Electron Configurations. 2. Lewis Structures 3. Covalent and Ionic bonds 4. Atomic and Molecular](https://reader035.vdocuments.net/reader035/viewer/2022070403/56649f285503460f94c40e43/html5/thumbnails/9.jpg)
1-9
Acetylene
C1
C2
HH
180o
spsp
E
__ s
__ __ __ p
__
__ __ __ __ __ p __ __ sp hybrid
promote e- Mix orbitals
D:\rw32b2a.exe
![Page 10: Chapter 1: Structure and Bonding mcmurry. Coverage: 1. Electron Configurations. 2. Lewis Structures 3. Covalent and Ionic bonds 4. Atomic and Molecular](https://reader035.vdocuments.net/reader035/viewer/2022070403/56649f285503460f94c40e43/html5/thumbnails/10.jpg)
1-10
s + p = sp + sp
Two sp orbitals
Remember, there are two p orbitalsleftover and these would be locatedon the y and z axes.
y
z
xEach sp orbital possesses 50% s characterand 50% p character.
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1-11
s + p = sp + sp
Two sp orbitals
Remember, there are two p orbitalsleftover and these would be locatedon the y and z axes.
y
z
xEach sp orbital possesses 50% s characterand 50% p character.
![Page 12: Chapter 1: Structure and Bonding mcmurry. Coverage: 1. Electron Configurations. 2. Lewis Structures 3. Covalent and Ionic bonds 4. Atomic and Molecular](https://reader035.vdocuments.net/reader035/viewer/2022070403/56649f285503460f94c40e43/html5/thumbnails/12.jpg)
Orbital Picture of Acetylene
D:\rw32b2a.exe