Which one of the following indicates the correct order of atomic size

Options

A. `BegtFgtCgtNe`
B. `BeltCltFltNe`
C. `BegtCgtFgtNe`
D. `FltNeltBeltC`

Explanation

To determine the correct order of atomic size among Beryllium (Be), Carbon (C), Fluorine (F), and Neon (Ne), we need to consider the trends in atomic size in the periodic table.

### Step-by-step Solution:

1. **Understanding Atomic Size 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 generally **increases down a group** (from top to bottom) because additional electron shells are added, making the atom larger.

2. **Identifying the Elements**:
- 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. **Comparing Atomic Sizes**:
- Among these elements, since they are all in the same period (Period 2), we can directly compare their sizes:
- Beryllium (Be) has the largest atomic size because it is the furthest left in the period.
- Carbon (C) is next, as it is to the right of Beryllium.
- Fluorine (F) is smaller than Carbon, being further right.
- Neon (Ne) has the smallest atomic size in this group, being the furthest right.

4. **Establishing the Order**:
- Therefore, the order of atomic size from largest to smallest is:
- Beryllium (Be) > Carbon (C) > Fluorine (F) > Neon (Ne).

5. **Conclusion**:
- The correct order of atomic size is **Beryllium > Carbon > Fluorine > Neon**.

### Final Answer:
The correct order of atomic size is: **Beryllium (Be) > Carbon (C) > Fluorine (F) > Neon (Ne)**.

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