Chapter 9 Chemical Bonding Theories

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Presentation transcript:

Chapter 9 Chemical Bonding Theories Valence Bond Theory: Uses Lewis Structures Bonds form using shared electrons between overlapping orbitals on adjacent atoms. Orbitals arrange around central atom to avoid each other. Two types of bonds: sigma and pi. Molecular Orbital Theory: Uses MO Diagrams Orbitals on atoms “mix” to make molecular orbtials, which go over 2 or more atoms. Two electrons can be in an orbital. Orbitals are either: bonding, antibonding, or nonbonding. Bonds are either: sigma or pi.

Sigma (s) Bonding Orbitals on bonding atoms overlap directly between bonding atoms Between s orbitals Between s and p orbitals Between p orbitals

Sigma (s) Bonding Consider VSEPR Shapes and bonding:

What’s wrong with this picture? Atoms bond by having their valence orbitals overlap

Orbitals don’t go in same directions as atomic orbitals. 2pz 2px 2py 2s Orbitals in CH4 Orbitals on C Orbitals don’t go in same directions as atomic orbitals.

Orbitals don’t go in same directions as atomic orbitals. 2pz 2px 2py 2s Orbitals in CH4 Orbitals don’t go in same directions as atomic orbitals. Conclusion: Atomic orbitals change shape when they make molecules.

Hybrid Orbitals Atomic valence orbitals “combine and mix” to form new “Hybrid Orbitals” Hybrid orbitals go in the VSEPR electron geometry directions.

Types of Hybrid Orbitals

4 Pairs: sp3 hybrid orbitals

4 Pairs: sp3 hybrid orbitals

sp3 bonding examples

3 Pairs: sp2 hybrid orbitals

sp2 bonding example

2 Pairs: sp hybrid orbitals

sp bonding example

More complex example:

Summary

Hybrid orbitals used for sigma bonds and lone pairs Hybrid orbitals used for sigma bonds and lone pairs. Unhybridized p orbitals used for pi bonds, or they are empty.

Sigma Bonding Orbitals overlap directly between two nuclei:

Sigma vs. Pi Bonding Sigma Bonding involves hybrid orbitals and/or H 1s orbitals. Pi bonding involves unhybridized p orbitals.

Pi Bond Formation

Bonding in Ethene

Bonding in Acetylene

Advanced: Allene Each end carbon is a flat trigonal. Are they co-planar or perpendicular?

Bonding in Allene

Bonding in Benzene

Summary

Conformations vs. Isomers Isomers: Molecules with same formula but different structure Conformers: Different temporary shapes of the same molecule

Bond Rotations CAN happen around single bonds Cannot happen around double bonds

Cis-Trans Isomerization When two groups are on a “side” of a molecule. cis trans

Can these molecules have cis-trans isomers?

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