Which one of the following indicates the correct order of atomic size?
(1). `C gt F gt Ne" "(2) Be lt C lt F lt Ne`
`(3). Be gt C gt F" "(4) F gt Ne gt Be gt C`

Explanation

To determine the correct order of atomic size among the elements given in the question, we need to analyze the atomic sizes of the elements: Beryllium (Be), Carbon (C), Fluorine (F), and Neon (Ne).

### Step-by-Step Solution:

1. **Understand the Periodic Trends**:
- Atomic size generally decreases across a period from left to right due to increasing nuclear charge, which pulls the electrons closer to the nucleus.
- Atomic size increases down a group due to the addition of electron shells.

2. **Identify the Elements and Their Positions**:
- Beryllium (Be) is in Group 2, Period 2.
- Carbon (C) is in Group 14, Period 2.
- Fluorine (F) is in Group 17, Period 2.
- Neon (Ne) is in Group 18, Period 2.

3. **Order the Elements by Atomic Size**:
- Since all these elements are in the same period (Period 2), we can compare their sizes directly.
- The order of atomic size from largest to smallest is:
- Beryllium (Be) > Carbon (C) > Fluorine (F) > Neon (Ne).
- Beryllium is the largest because it has the least nuclear charge pulling on its outer electrons. Carbon is smaller than Beryllium but larger than Fluorine. Fluorine is smaller than Carbon due to its higher nuclear charge, and Neon, being a noble gas, has a larger Van der Waals radius but is still smaller than Beryllium, Carbon, and Fluorine in terms of atomic size.

4. **Conclusion**:
- The correct order of atomic size is:
- Be > C > F > Ne.

5. **Identify the Correct Option**:
- From the options given:
- (1) C > F > Ne (Incorrect)
- (2) Be < C < F < Ne (Incorrect)
- (3) Be > C > F (Correct)
- (4) F > Ne > Be > C (Incorrect)
- Therefore, the correct answer is option (3) Be > C > F.