MO Diagrams for Diatomic Molecules

MO Diagrams for Diatomic Molecules

MO Diagrams for Diatomic Molecules Chapter 5 Friday, October 9, 2015 Homonuclear Diatomic Molecules What happens when we move to more complicated sy...

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MO Diagrams for Diatomic Molecules Chapter 5 Friday, October 9, 2015

Homonuclear Diatomic Molecules What happens when we move to more complicated systems? Consider O2. •

The Lewis dot structure famously predicts the wrong electronic structure for O2



We can use LCAO-MO theory to get a better picture:

Notice that Eσ > Eπ, because the σ bonds have more overlap than π bonds



2pa

2sa



2pb

2sb

Electron Configurations and Bond Orders Just as with atoms, we can write a molecular electron configuration for O2 σ2σ*2σ2π4π*2

We can also calculate the O–O bond order:

1 BO  # bonding e   # anti-bonding e  2 1  8  4   2 2 LCAO MO theory also predicts (correctly) that O2 has two unpaired electrons.

Orbital Mixing Orbitals of similar but unequal energies can interact if they have the same symmetry The 2s and 2pz orbitals form MOs with the same symmetry (σg and σu). sp mixing causes the σg and σu MOs to be pushed apart in energy:

The σ and π orbitals change order!

Orbital Mixing The size of the effect depends on the 2s-2p energy difference.

small Zeff = small energy difference = large sp mixing

order changes

large Zeff = large energy difference = small sp mixing

MOs of Homonuclear Diatomic Molecules The MO picture of homonuclear diatomic molecules depends on the amount of sp mixing.

Li2, Be2, B2, C2, N2

O2, F2, Ne2

Bond Order and Bond Distance The MO bond order is the main factor controlling the internucelar distance. B2 σ2σ*2π2 BO = 1 F2 2 2 σ σ* σ2π4π*4 BO = 1 O2– σ2σ*2σ2π4π*3 BO = 1.5 C2 2 σ σ*2π4

C22– σ2σ*2π4σ2 BO = 3

BO = 2

O2 2 2 σ σ* σ2π4π*2 BO = 2

N2+ σ2σ*2π4σ1 BO = 2.5

N2 2 σ σ*2π4σ2 BO = 3

O2+ σ2σ*2σ2π4π*1 BO = 2.5

Relative AO Energies for MO Diagrams Photoelectron spectroscopy gives us a pretty good idea of the relative energies for AOs.

Li H

Al

B

Na

C

Be

N

–13.6 eV

B

1s

2p C

He

O –18.6 eV

Ne

2s

P

Mg Al

F

Si

Si

S

3p 3s P S

N O F

–40.2 eV

Ne

Cl

Cl

Ar

Ar

MO Diagram for HF The AO energies suggest that the 1s orbital of hydrogen interacts mostly with a 2p orbital of fluorine. The F 2s is nonbonding. σ*

–13.6 eV 1s

Energy

nb σ

2p

–18.6 eV

So H–F has one σ bond and three lone electron pairs on fluorine

–40.2 eV

H

nb

2s

H–F

F

Relative AO Energies for MO Diagrams Photoelectron spectroscopy gives us a pretty good idea of the relative energies for AOs. Al

B

Li

C

Be

H

Na –10.7 eV

N

B

1s

–19.4 eV

He

2p C

O

–15.8 eV

Ne

2s

Al

S

3p 3s

O F Ne

Cl

P S

N –32.4 eV

P

Mg Si

F

Si

Cl

Ar

Ar

Heteronuclear Diatomic Molecules: CO In molecules with more than one type of atom, MOs are formed from AOs that have different energies. Consider CO: σ*

LUMO is on carbon too!

Energy

π*

HOMO is on carbon 2pa σ

2pb π σ*

Anti-bonding orbitals get polarized towards carbon

2sa

2sb

σ

C

C≡O

O

Bonding orbitals get polarized towards oxygen

Summary MO Theory •

LCAO-MO Theory is a simple method for predicting the approximate electronic structure of molecules.



Atomic orbitals must have the proper symmetry and energy to interact and form molecular orbitals.



Photoelectron spectroscopy provides useful information on the energies of atomic orbitals.



Next we’ll see that symmetry will help us treat larger molecules in the LCAO-MO theory framework.