Molecular Orbital Theory

Molecular Orbital Theory - The diagram of the bonding and...

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Molecular Orbital Theory Below is how the 2p y and 2p z orbitals overlap Don’t forget to account for the 1s orbitals when doing electron configuration .
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First, we have the 1s + 1s -> sigma bonding MO, and then above this the σ* (sigma star) antibonding MO. Then, there are the pair 2s + 2s bonding σ (sigma) and antibonding σ* (sigma star) MOs. Next we come to the p + p interactions. These are a little more complicated because p orbitals are orientated in space along the x, y and z dimensions. The 2px + 2px orbital interaction gives a σ (sigma) bonding MO. The 2py + 2py and 2pz + 2pz interactions are equivalent, they only differ in spatial orientation. Both give rise to π bonding MOs. Next come a pair of π* (pi-star) antibonding MOs. Finally, we have the 2px + 2px σ* (sigma star) antibonding MO.
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Unformatted text preview: The diagram of the bonding and antibonding MOs is shown below: Heteronuclear Diatomic Molecules & Molecular Ions MO theory can be used to describe heteronuclear diatomic molecules & molecular Ions such as: LiH Lithium hydride HF Hydrogen fluoride CO Carbon monoxide CN Cyanide ion NO + Nitrosonium ion As the electronegativity differences increases the interacting orbitals will be at different energies. The result is that the covalent bonding energy decreases, but this is counteracted by an increasing electrostatic +/ attraction that is not represented on MO diagrams (see the Klopman equation , elsewhere in this web book.) The MO diagram for the diatomic carbon monoxide, CO, shows it to be isoelectronic with nitrogen, N2:...
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Molecular Orbital Theory - The diagram of the bonding and...

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