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Is there a reason carbon monoxide has a triple bond between the carbon and oxygen atoms? Aren't the formal charges more attractive when there's a double bond between them with two lone pairs on oxygen and one lone pair on carbon?
When drawing lewis structures, it is good to first make sure every element has a complete octet( unless it's in row 3 or after). Then I would start paying attention to how to create the most stable structure.
With a double bond, the molecule would have a +2 formal charge, while with a triple bond, the molecule would have +0 formal charge. Therefore, carbon monoxide needs a triple bond to be more stable.
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