chapter 7 covalent bonds and molecular architecturechickosj/chem11/lecture/lecture9.pdfyou recall...
TRANSCRIPT
![Page 1: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/1.jpg)
Chapter 7 Covalent Bonds and Molecular Architecture
![Page 2: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/2.jpg)
Octet rule: Main group elements tend to undergo reactions that leaves them with either 2 or 8 electrons in their outer or valence shell achieved by sharing electrons.
Exceptions to the rule includes all elements that have d levels close in energy. However, much of their chemistry can still be explained by the octet rule.
It is important to realize that this is a model that can also help us understand molecular structure.
![Page 3: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/3.jpg)
Main Group Elements
![Page 4: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/4.jpg)
Covalent bonding and Lewis structures
If H would form a covalent bond, how many bonds would it form?
Octet rule: Elements tend to undergo reactions to form covalent bonds that leaves them with either 2 or 8 electrons in their outer or valence shell.
Valence electrons are the electrons in orbitals with the highest principle quantum number.
![Page 5: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/5.jpg)
H2 has an electronic environment similar to He
One way chemists have of indicating a sharing of two electrons is to use a line to connect the two atoms, H2 is drawn H-H or H:H. These are called Lewis structures.
atomic orbitals
molecular orbitals
![Page 6: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/6.jpg)
If Cl would form a covalent bond with H, how many bonds would it form?
chlorine is 1 electron short of a filled 3p level
hydrogen is 1 electron short of a filled 1s level
How many valence electrons does each atom posses?
(valence electrons are the electrons with the highest principle quantum number)
How many electrons does H need to share to have an outer shell that resembles an inert gas? Which inert gas?
How many does Cl need to share to have an outer shell that resembles an inert gas? Which inert gas?
H Cl
![Page 7: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/7.jpg)
How many valence electrons does C posses?
If C forms covalent bonds, how many bonds would it form to satisfy the octet rule?
If H would form a covalent bond with C, how many bonds would it form?
H
H-C-H
H
4
4
Lewis structure
![Page 8: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/8.jpg)
How many valence electrons does N posses?
If N forms covalent bonds with H, how many bonds would it form
to satisfy the octet rule?
If H would form a covalent bond with N, how many bonds would it form?
H-N-H
H
5
3
1
![Page 9: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/9.jpg)
How many valence electrons does O possess?
If O forms covalent bonds with H, how many bonds would it form to satisfy the octet rule?
If H would form a covalent bond with O, how many bonds would it form?
6
2
1
H׀
:O:׀ H
![Page 10: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/10.jpg)
If B would form a covalent bond, how many bonds would it form?
If H would form a covalent bond with B, how many bonds would it form?
How many valence electrons does each atom posses?
How many does B need to share to have an outer shell that resembles an inert gas? Which inert gas?
Boron is a hopeless mess; much of its chemistry is very different from other elements in that the only way it can obtain an octet of electrons is by forming charged complexes; similarly with aluminum
H-B-H׀ H
H -1׀
Na+ H-B-H׀ H
![Page 11: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/11.jpg)
Geometry of molecules
Suppose two groups were attached at a single point in space, andsuppose these groups repelled each other, what geometric arrangement would these group chose to minimize their repulsion ( how would they arrange themselves to minimize repulsion)?
![Page 12: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/12.jpg)
Suppose two groups were attached at a single point in space, andsuppose these groups repelled each other, what geometric arrangement would these group chose to minimize their repulsion ( how would they arrange themselves to minimize repulsion)?
![Page 13: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/13.jpg)
Suppose three groups were attached at a single point in space, and suppose these groups repelled each other, what geometricarrangement would these group chose to minimize their repulsion?
![Page 14: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/14.jpg)
Suppose three groups were attached at a single point in space,
and suppose these groups repelled each other, what geometric
arrangement would these group chose to minimize their repulsion?
.
![Page 15: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/15.jpg)
Suppose four groups were attached at a single point in space, and suppose these groups repelled each other, what geometric arrangement would these group chose to minimize their repulsion?
![Page 16: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/16.jpg)
Suppose four groups were attached at a single point
in space, and suppose these groups repelled each other,
what geometric arrangement would these group chose
to minimize their repulsion?
.
![Page 17: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/17.jpg)
Suppose four groups were attached at a single point
in space, and suppose these groups repelled each other,
what geometric arrangement would these group chose
to minimize their repulsion?
.
![Page 18: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/18.jpg)
Suppose five groups were attached at a single point in space,
and suppose these groups repelled each other, what geometric
arrangement would these group chose to minimize their repulsion?
![Page 19: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/19.jpg)
Suppose five groups were attached at a single point in space,
and suppose these groups repelled each other, what geometric
arrangement would these group chose to minimize their repulsion?
![Page 20: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/20.jpg)
Suppose five groups were attached at a single point in space,
and suppose these groups repelled each other, what geometric
arrangement would these group chose to minimize their repulsion?
http://www.jcrystal.com/steffenweber/POLYHEDRA/p_10.html
![Page 21: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/21.jpg)
Suppose six groups were attached at a single point in space,
and suppose these groups repelled each other, what geometric
arrangement would these group chose to minimize their repulsion?
![Page 22: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/22.jpg)
Suppose six groups were attached at a single point in space,
and suppose these groups repelled each other, what geometric
arrangement would these group chose to minimize their repulsion?
![Page 23: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/23.jpg)
Suppose six groups were attached at a single point in space,
and suppose these groups repelled each other, what geometric
arrangement would these group chose to minimize their repulsion?
http://www.jcrystal.com/steffenweber/POLYHEDRA/p_10.html
octahedral geometry
![Page 24: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/24.jpg)
Let’s define a group as either an atom or a pair of valence electrons not involved in bonding, ignore bonding electrons and electrons in inner shellsdraw the Lewis structures, and predict the geometry of the following molecules
H2O
What is the central atom?
How many valence electrons around O?
How many groups around the central atom?
. 6 :O:
.
O
4 H:O:H What is the geometry of the molecule?
![Page 25: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/25.jpg)
The geometry of a molecule is determined only by location of thenuclei. The electrons can not be loprinciple
cated because of the uncertainty
![Page 26: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/26.jpg)
CCl4; CH4What is the central atom?
How many valence electrons around C?
What is the Lewis structure?
How many groups around the central atom?
What is the geometry of the molecule?
C
4
4
tetrahedral
H|
H-C-H|H
![Page 27: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/27.jpg)
![Page 28: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/28.jpg)
NH3
What is the central atom?
How many valence electrons around N?
What is the Lewis structure?
How many groups around the central atom?
What is the geometry of the molecule?
N
5
4
pyramidal
H|
H-N:|H
![Page 29: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/29.jpg)
![Page 30: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/30.jpg)
Draw Lewis structures and predict the shape of the following compounds:
1. SiCl4
2. CH5N
3. CH2O
4. C2H2Cl2
5. C3H4
![Page 31: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/31.jpg)
PCl5What is the central atom?
SF6What is the central atom?
Remember that we can only locate the position of a heavy atom; the position of electrons is not determined.
P
S
![Page 32: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/32.jpg)
![Page 33: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/33.jpg)
We have partially explained the geometry observed when atoms combine to form molecules. The geometry of the molecule is determined locally by the central atom. How do we identify central atoms?
Central atoms are determined by the number of bonds needed to complete the octet.
H, Halogens are seldom central atoms
B, C, N O in the first row
Al, Si, P, S in the second row …
![Page 34: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/34.jpg)
Shapes of molecules
1. linear
2. trigonal planar
3. bent
4. tetrahedral
5. trigonal pyramidal
6. trigonal bipyramidal
7. seesaw
8. T shaped
9. octahedral
10. square pyramidal
11. square planar
http://intro.chem.okstate.edu/1314F00/Lecture/Chapter10/VSEPR.html
![Page 35: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/35.jpg)
What experimental evidence is there that CH4 is tetrahedral and not square planar?
Consider CH2Cl2:
H H
H
Cl
CHCl
Cl
CCl
Are there two compounds with the formula CH2Cl2? No
![Page 36: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/36.jpg)
Are these the same?
Consider CHBrClF
![Page 37: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/37.jpg)
Are these the same?
Consider CHBrClF
![Page 38: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/38.jpg)
Are these the same?
Consider CHBrClF
![Page 39: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/39.jpg)
You recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain the structure of molecules using these same orbitals?
Remember the shape of these orbitals:
s: spherically symmetric
p: 3 orbitals each with two lobes touching each other at the nucleus and oriented 90 ° to each other.
d: 5 orbitals with a more complicated structure.
![Page 40: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/40.jpg)
sd
p
![Page 41: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/41.jpg)
Chemists like to think that the electrons are the glue that hold atoms together. Therefore, can the structure of the molecules we just described, for example, CH4, PCl5, be explained using the hydrogen atom atomic orbitals just shown?
![Page 42: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/42.jpg)
Schroedinger Equation is a differential equation. :
Properties of a differential equation:
1. the equation may have more than one solution.
2. any combination of solutions (sum or difference) is also a solution
Ψ2s = 1/4(1/2πa3).5(2-r/a)(2.718)r/2a
Ψ2p = 1/4(1/2πa3).5(r/a)(2.718)r/2acos θ
…
Linus Pauling: hybridization of atomic orbitals
![Page 43: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/43.jpg)
What were to happen if we combined ½ of a 2s orbital with one of the ½ 2p orbitals mathematically?
- + +a 2s + b 2p
a 2s - b 2p- + +
- +
- +
These hybrid orbitals are directional, pointing 180°away from each other and are called sp hybrid orbitals
2 s 2 p
![Page 44: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/44.jpg)
Combining a 2s orbital with 2 2p orbital can result in 3 sp2 hybrid orbital that point at 120 ° to each other
![Page 45: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/45.jpg)
Combining a 2s orbital with 2 2p orbital results in 3 sp2
hybrid orbital that point at 120 ° to each other; note that one p orbital remains unchanged by these mathematics.
![Page 46: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/46.jpg)
A summary of the types of hybridization necessary to product maximum electron density in the necessary direction as dictated by experimental geometries
sp hybridization: 2 orbitals pointing 180 ° to each other; 2 atomic p orbitals remain unchanged
sp2 hybridization: 3 orbitals pointing 120 ° to each other; 1 atomic p orbitals remains unchanged
sp3 hybridization: 4 orbitals pointing to the corners of a regular tetrahedron; all atomic p orbitals used
dsp2 hybridization: 4 orbitals pointing to the corners of a square; 4 d orbitals, 1 p orbital unchanged
dsp3 hybridization: 5 orbitals pointing to the corners of a trigonal bipramid; 4 d orbitals unchanged
d2sp3 hybridization: 6 orbitals pointing to the corners of a octahedron; 3d orbitals unchanged
![Page 47: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/47.jpg)
sp2
sp3
d2sp3
Shapes of the hybrid orbitals
![Page 48: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/48.jpg)
Draw the Lewis structure of C2H4 so that every carbon has a filled octet and each hydrogen has a He configuration
How many groups around each carbon?
3
What is the geometry at each carbon?
trigonal
![Page 49: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/49.jpg)
sp2 hybrid orbitals
Atomic p orbitals on each C
![Page 50: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/50.jpg)
![Page 51: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/51.jpg)
Draw the Lewis structure of C2H2 so that every carbon has
a filled octet and each hydrogen has a He configuration
How many groups around each carbon?
2
What is the geometry about each carbon?
digonal: 180 °
![Page 52: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/52.jpg)
H-C≡C-H
![Page 53: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/53.jpg)
Bond lengths
C-C 1.54 *10-10 m
C=C 1.34*10-10 m
C≡C 1.2* 10-10 m
![Page 54: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/54.jpg)
How do we explain the formation of CH4 using the electronic configuration of C
Valence electrons of C _____ _____ _____2p
____ 2s
hybridize
promote 1 electron: requires investment of energy
add electrons from H: allows the formation of 4 bonds instead of 2 and satisfies the octet rule
![Page 55: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/55.jpg)
How do we explain the structure of molecules such as SF4?
3d ____ _____ _____ ______ ____
3p ___ ____ ____
3s ____
hybridize
3d ____ _____ _____ ______ ____3p ___ ____ ____
3s ____
promote an electron
add electron from F
3d _____ _____ ______ ________ ___ ____ ____ _____ dsp3
![Page 56: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/56.jpg)
![Page 57: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/57.jpg)
3d ____ _____ _____ ______ ____
3p ___ ____ ____ 3s ____
3d ____ _____ _____ ______ ____
3p ___ ____ ____ 3s ____
How do we explain the structure of molecules such as SF6?
3d _____ _____ ______ ____ ___ ____ ____ _____ _____
promote 2 electrons
hybridize
add electron from F
![Page 58: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/58.jpg)
![Page 59: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/59.jpg)
How good are Lewis structures at explaining molecular properties?
For compounds of carbon: excellent very few exceptions
For other elements: very good, some exceptions
Consider the Lewis structures of the diatomic molecules of the elements
H2,
O2
N2
F2
Any exceptions?
![Page 60: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/60.jpg)
How good is this model at explaining molecular properties?
For compounds of carbon: excellent very few exceptions
For other elements: very good, some exceptions
Consider the Lewis structures of the diatomic molecules of the elements
H2,
O2
N2
F2
Any exceptions? O2 is paramagnetic
![Page 61: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/61.jpg)
![Page 62: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/62.jpg)
Molecular orbital Theory
Basic tenets: molecules are formed by combining atomic orbitalson each atom that have the proper orientation.
Whenever two atomic orbitals combine to form a molecular orbital, one combination is obtained by mathemetically adding the two together; this orbital goes down in energy relative to the atomic level. The other, obtained by the mathematical difference between the two orbitals, goes up in energy.
If a level goes down in energy relative to the atomic level, it is referred to as a bonding molecular orbital
If a level goes up in energy relative to the atomic level, it is called an antibonding level
If a level is not affected relative to the atomic level it is called a non-bonding orbital
![Page 63: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/63.jpg)
H2
![Page 64: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/64.jpg)
This model predicts that H2- should have some stability; the total
energy of He2 is the same as two isolated He atoms so nothing keeps the molecule together and it falls apart in two He atoms.
![Page 65: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/65.jpg)
![Page 66: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/66.jpg)
O2
![Page 67: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/67.jpg)
F2
![Page 68: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/68.jpg)
N2
![Page 69: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/69.jpg)
Draw the Lewis structure of ozone: O3
![Page 70: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/70.jpg)
Draw the Lewis structure of ozone
:O: :O::
::O:
:
+
-
![Page 71: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/71.jpg)
Resonance structures: two structures that are identical except for the location of the electrons
Symbol chemists use to denote resonance structures
![Page 72: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/72.jpg)
C
CC
C
CC
H
H
H
H
H
HC
CC
CC
C
H
H
H
H
H
H
Bond lengthsC-C 1.54 *10-10 mC=C 1.34*10-10 m
![Page 73: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/73.jpg)
Draw the structure of sulfuric acid; H2SO4
Draw the structure of the sulfate ion; SO4-2
![Page 74: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/74.jpg)
Why do covalent bonds form?
Covalent bonds: the sharing of electrons
![Page 75: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/75.jpg)
![Page 76: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/76.jpg)
![Page 77: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/77.jpg)
![Page 78: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/78.jpg)
![Page 79: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/79.jpg)
![Page 80: Chapter 7 Covalent Bonds and Molecular Architecturechickosj/chem11/Lecture/Lecture9.pdfYou recall that we were able to explain atomic structure using s, p , d, f orbitals. Can we explain](https://reader030.vdocuments.mx/reader030/viewer/2022020120/5aa6c74e7f8b9a6d5a8b6f54/html5/thumbnails/80.jpg)
Electronegativity: generally meant to identify the unevenness in sharing electrons in a covalent bond