Draw possible Lewis structures for carbon monoxide. Include all formal charges.
We first draw a skeleton structure with only a single bond between the two atoms: This gives C-O.
Then we compare with the number of valence electrons in an isolated atom.
We see that in this structure C has five valence electrons — two from the lone pair and three from the C≡O triple bond, and O also has five valence electrons.
Since an isolated C atom has 4 valence electrons and here it has 5, it has gained an electron. It has a formal charge of -1.
Since an isolated O atom has 6 valence electrons and here it has 5, it has lost an electron. It has a formal charge of +1.
We might write the structure as :C⁻¹≡O:⁺¹. This structure satisfies the , but it contains formal charges.
We can avoid formal charges if we write the structure as :C=Ö: However, although this structure avoids formal charges, it does not give C an octet. There is just no single good Lewis structure for CO.
To know more about Lewis structures check this
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