Final answer:
In the Lewis structure for FeF3, there are zero lone pairs surrounding the iron atom since iron in this compound has an oxidation state of +3 after forming bonds with three fluorine atoms.
Step-by-step explanation:
In determining the number of lone pairs surrounding the iron (Fe) atom in the Lewis structure for FeF3, it's crucial to consider the electronic configuration and oxidation state of iron. Iron (III) fluoride, or FeF3, features an iron atom with a +3 oxidation state, as iron can lose three electrons from its valence shell. The atomic number of iron is 26, which corresponds to the electronic configuration [Ar] 4s2 3d6. After losing three electrons (two from the 4s orbital and one from the 3d orbital), the electron configuration becomes Fe3+: [Ar] 3d5. As a result, the iron atom has no remaining electrons to form lone pairs after forming bonds with the three fluorine atoms in FeF3.
Therefore, the correct answer is a. 0. There are zero lone pairs surrounding the iron atom in the Lewis structure for FeF3.