Chapter 9 Chemical Bonding Theories Valence Bond Theory: Uses Lewis Structures Bonds form using shared electrons between overlapping orbitals on adjacent.

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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.

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

Consider VSEPR Shapes and bonding: Sigma (s) 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. 2s 2p z 2p x 2p y Orbitals in CH 4 Orbitals on C

Orbitals don’t go in same directions as atomic orbitals. 2s 2p z 2p x 2p y Orbitals in CH 4 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

Types of Hybrid Orbitals: 2 Pairs

Types of Hybrid Orbitals: 3 Pairs

Types of Hybrid Orbitals: 4 Pairs

Types of Hybrid Orbitals

Sigma Bonding Orbitals overlap directly between two nuclei:

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

Pi Bond Formation

Bonding in Ethene

Bonding in Acetylene

Bonding in Formaldehyde

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

Bonding in Allene

Bonding in Benzene

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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