The quoted radius of neon ($160\mathrm{pm}$) is much larger than that of fluorine ($64\mathrm{pm}$), even though neon has a higher nuclear charge. The reason is that:

1. Aneon has an extra electron shell compared with fluorine
2. Bneon has a lower effective nuclear charge than fluorine
3. Cthe neon value is a van der Waals radius while the fluorine value is a covalent radius
4. Dneon forms bonds that are longer than those of fluorine