Final answer:
The correct option is D). The correct Lewis structure for BF₃ has no double bonds, as it adopts a trigonal planar geometry with single bonds between boron and each of the three fluorine atoms.
Step-by-step explanation:
The correct Lewis structure for BF₃ (boron trifluoride) would have no double bonds. The molecule has a trigonal planar molecular geometry with boron at the center forming single bonds with three fluorine atoms. Despite boron having less than an octet of electrons in its valence shell, this structure is more consistent with experimental evidence as it displays bond lengths closer to those expected for B-F single bonds and is also in line with the compound's reactivity. It is important to note that while it's theoretically possible to draw a Lewis structure with a double bond to fulfill the octet rule for boron, such a structure is inconsistent with the high electronegativity of fluorine which wouldn't favor a positive partial charge that a double bond would suggest.