Atomic radius of F is greater than that of Ne.

Answer

To determine whether the atomic radius of fluorine (F) is greater than that of neon (Ne), we can analyze their electronic configurations and the trends in atomic size across a period in the periodic table.

### Step-by-Step Solution:

1. **Identify the Atomic Numbers and Electronic Configurations:**
- Fluorine (F) has an atomic number of 9. Its electronic configuration is:
\[ \text{F: } 1s^2 \, 2s^2 \, 2p^5 \]
- Neon (Ne) has an atomic number of 10. Its electronic configuration is:
\[ \text{Ne: } 1s^2 \, 2s^2 \, 2p^6 \]

2. **Determine the Period:**
- Both fluorine and neon are located in the same period (Period 2) of the periodic table.

3. **Understand the Trend in Atomic Radius Across a Period:**
- As we move from left to right across a period, the number of protons in the nucleus increases, which increases the nuclear charge.
- The electrons are added to the same energy level (shell), and thus the increased positive charge from the nucleus pulls the electrons closer, leading to a decrease in atomic radius.

4. **Compare the Atomic Radii:**
- In the case of fluorine, it has 9 protons and 9 electrons, while neon has 10 protons and 10 electrons.
- Despite both elements having their outermost electrons in the same shell, the increased nuclear charge in neon (10 protons) compared to fluorine (9 protons) results in a stronger attraction between the nucleus and the outermost electrons in neon.

5. **Consider the Noble Gas Stability:**
- Neon is a noble gas with a complete octet (8 valence electrons), which contributes to its stability.
- The complete octet leads to a slight increase in atomic size due to electron-electron repulsion in the filled outer shell, but this effect does not outweigh the increased nuclear charge.

6. **Conclusion:**
- Therefore, the atomic radius of fluorine is **not greater** than that of neon; rather, it is **smaller**. The statement "The atomic radius of F is greater than that of Ne" is **false**.

### Final Answer:
The atomic radius of fluorine (F) is less than that of neon (Ne).

---