To determine the correct atomic radii of fluorine and neon, we first need to understand what atomic radius means. Atomic radius is essentially half the distance between the nuclei of two atoms of the same element in a molecule. For elements in the noble gas group, such as neon, the radius typically refers to the van der Waals radius, which is the radius of a hypothetical hard sphere representing the distance of closest approach for another atom. For other elements like fluorine, which readily forms molecules, the covalent radius (half the distance between nuclei in a single bond) is often considered.

The atomic radii values for fluorine (F) and neon (Ne) in angstrom units (Å) can be summarized as follows:

• Fluorine has a covalent radius of approximately 0.72 Å.
• Neon has a Van der Waals radius of approximately 1.60 Å.

Therefore, reviewing the provided options:

• Option A: 0.72 Å for fluorine and 1.60 Å for neon
• Option B: 1.60 Å for both fluorine and neon
• Option C: 0.72 Å for both fluorine and neon
• Option D: None of these values

Given the definitions and the typical atomic radius values for these elements, Option A is correct with fluorine having an atomic radius of about 0.72 Å, and neon having a radius of about 1.60 Å.