Final answer:
The correct Lewis structure for one of the isomers of butane is option c) H₃C-CH₂-CH=CH₂.
Step-by-step explanation:
Butane has multiple structural isomers due to the arrangement of its carbon atoms and the presence of double bonds. Option c) depicts one of these isomers, commonly known as 1-butene, a four-carbon molecule with a double bond between the first and second carbon atoms.
In the Lewis structure of option c), the central carbon (designated as CH=CH) forms a double bond with the adjacent carbon, implying a shared pair of electrons between these atoms. The structure adheres to the valency rules of carbon, which forms four bonds, including double bonds in certain instances, to satisfy its octet.
Options a), b), and d) represent different isomers of butane but do not correspond to the specific structure of 1-butene. Option a) signifies a different molecule (propene), possessing a double bond between the first and second carbon atoms, while option b) represents a linear butane structure with no double bonds. Option d) illustrates another isomer, specifically 2-butene, with a double bond between the second and third carbon atoms.
Among the choices provided, only option c) aligns with the structural arrangement of 1-butene, exhibiting the presence of a double bond between the first and second carbon atoms in the butane molecule. This arrangement is consistent with the molecular formula C₄H₈, characteristic of one of the isomers of butane possessing a double bond.