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Molecular orbital (MO) theory can be used to describes the bonding in CO. CO bonding is specifically based on a heteronuclear Molecular Orbital theory. The different types of energy levels and overlapping of orbitals will be discussed through MO theory for CO.
The goal of MO theory is to allow us to produce a diagram that will give us information about the allow energy bonding between carbon and oxygen.
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For carbon monoxide, both carbon and oxygen uses sp because two things are attach to both carbon and oxygen. For example, carbon is connected to one lone pair (1 thing) and connected to oxygen (1 thing). So there are a total of two things attached to oxygen. Sp arrangement of its hybridized lopes are linear, so it is possible for one lone pair to be occupied in one of lopes, while the other is used for overlapping.
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The bonding order of CO is 3. It would make sense, carbon monoxide is triple bonded between carbon and oxygen. From the diagram we see that it is bonded by two pi overlaps and one sigma overlap.
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What does it mean by sigma and pi overlaps?
-sigma is connected by sp hybridization overlap, while pi are overlap by the pz and py overlaping.
Why is the oxygen 2p orbitals are lower in energy than carbon 2p orbitals?
-because oxygen is more electronegative and is more stable in energy, so is lower in energy.
Is it possible for [CO]2- to exist?
-It is not possible to exist, because two more electrons will be occupied in the antibonding orbital.
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