Why does CO generally not bind to a metal that is not a transition metal?

[plexus0208]

Please see title

 

[Borek]

What does you book say about complexes & their stability? What is a driving force behind?

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[quicknote]

Carbon monoxide (CO) is a diatomic molecule that is known to form strong bonds with transition metals. This is because transition metals have partially filled d-orbitals, which allows them to form coordination complexes with other molecules, including CO. These coordination complexes are formed through the donation of electron density from the metal to the CO molecule, resulting in a stable bond.

On the other hand, non-transition metals do not have partially filled d-orbitals and therefore do not have the ability to form coordination complexes with CO. This is because the energy required to promote electrons from the filled s and p orbitals to the higher energy d orbitals is too high and not favorable. As a result, CO generally does not bind to non-transition metals.

Additionally, non-transition metals tend to have smaller atomic radii compared to transition metals, making it difficult for CO to approach and form a bond. Non-transition metals also have a higher electronegativity, meaning they have a stronger attraction for electrons, making it less likely for them to donate electron density to form a bond with CO.

In summary, the lack of partially filled d-orbitals and unfavorable energy requirements make it difficult for non-transition metals to form bonds with CO. This is why CO generally does not bind to non-transition metals.