Choose the correct order of atomis radii of Fluorine and Neon (in pm) out of the options give below:

Options

A. 72, 160
B. 160, 160
C. 72,72
D. 160, 72

Explanation

To determine the correct order of atomic radii of Fluorine and Neon, we need to understand the definitions and characteristics of atomic radii for these elements.

### Step-by-Step Solution:

1. **Understanding Atomic Radii**:
- Atomic radii can be measured in different ways, with two common types being covalent radii and van der Waals radii.
- Covalent radii are typically used for elements that can form covalent bonds, while van der Waals radii are used for noble gases and non-bonded atoms.

2. **Identifying the Elements**:
- Fluorine (F) is a non-metal that typically forms covalent bonds.
- Neon (Ne) is a noble gas and does not form bonds in the same way that Fluorine does.

3. **Covalent Radii of Fluorine**:
- The covalent radius of Fluorine is the distance between the nuclei of two bonded Fluorine atoms divided by two. This value is relatively small due to the strong attraction between the nuclei and shared electrons.

4. **Van der Waals Radii of Neon**:
- The van der Waals radius of Neon is defined as half the distance between the closest approach of two non-bonded Neon atoms. This radius is generally larger than the covalent radius because it accounts for the space occupied by the electron cloud around the atom.

5. **Comparison of Radii**:
- Since the van der Waals radius (Neon) is larger than the covalent radius (Fluorine), we can conclude that:
\[ \text{Atomic radius of Neon} > \text{Atomic radius of Fluorine} \]

6. **Conclusion**:
- Therefore, the correct order of atomic radii in picometers (pm) is:
\[ \text{Atomic radius of Neon} > \text{Atomic radius of Fluorine} \]

### Final Answer:
The correct order of atomic radii is Neon > Fluorine.