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Answer :
Final answer:
The statement 'Carbon monoxide contains resonance Lewis structures' is true. Resonance occurs when two or more Lewis structures can be written for a molecule with the same arrangement of atoms but different distributions of electrons. Carbon monoxide is an example of a molecule that exhibits resonance.
Explanation:
The statement 'Carbon monoxide contains resonance Lewis structures' is true.
Resonance occurs when two or more Lewis structures can be written for a molecule with the same arrangement of atoms but different distributions of electrons. Carbon monoxide, CO, is an example of a molecule that exhibits resonance. It can be represented by multiple Lewis structures, where the double bond can be formed between either the carbon or oxygen atom.
This phenomenon can be explained by the fact that carbon and oxygen have similar electronegativities, allowing for the delocalization of electrons and the formation of resonance structures.
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False. Carbon monoxide contains resonance Lewis structures.
Resonance structures are alternative Lewis structures for a molecule where the placement of electrons varies but the arrangement of atoms remains constant. These structures help describe the delocalization of electrons within certain molecules or ions. In the case of carbon monoxide (CO), it does not contain resonance structures.
The Lewis structure of CO features a triple bond between carbon and oxygen, with carbon having a lone pair and a formal charge of +1, and oxygen also having a lone pair and a formal charge of -1. There isn't an alternative arrangement for the electrons that would create a resonance structure.