Which is the correct order of size ?
`(O^(ɵ), O^(2-), F^(ɵ) and F )`

Options

A. `O^(2-) gt O^(ɵ) gt F^(ɵ) gt F`
B. `O^(ɵ) gt O^(2-) gt F^(ɵ) gt F`
C. `O^(2-) gt F^(ɵ) gt F gt O^(ɵ)`
D. `O^(2-) gt F^(ɵ) gt O^(ɵ) gt F`

Explanation

To determine the correct order of size among the ions and atoms given: \( O^{0}, O^{2-}, F^{0}, \) and \( F^{-} \), we can follow these steps:

### Step 1: Understand the Species
We have two elements, oxygen (O) and fluorine (F), and we need to compare:
- Neutral oxygen: \( O^{0} \)
- Oxide ion: \( O^{2-} \)
- Neutral fluorine: \( F^{0} \)
- Fluoride ion: \( F^{-} \)

### Step 2: Analyze the Charge Effect on Size
- Anions (negatively charged species) are larger than their neutral counterparts because the addition of electrons increases electron-electron repulsion, which expands the electron cloud.
- Therefore, \( O^{2-} \) will be larger than \( O^{0} \) and \( F^{-} \) will be larger than \( F^{0} \).

### Step 3: Compare Sizes of Ions and Atoms
- Between \( O^{0} \) and \( F^{0} \): As we move from left to right in the periodic table, the size of the atoms decreases due to an increase in effective nuclear charge. Thus, \( O^{0} \) is larger than \( F^{0} \).
- Between \( O^{2-} \) and \( O^{-} \): \( O^{2-} \) is larger than \( O^{-} \) because it has more electrons, leading to greater electron-electron repulsion.
- Between \( F^{-} \) and \( F^{0} \): \( F^{-} \) is larger than \( F^{0} \) for the same reason as above.

### Step 4: Establish the Order of Size
Now we can summarize the sizes based on the above analysis:
1. \( O^{2-} \) (largest)
2. \( O^{-} \)
3. \( F^{-} \)
4. \( F^{0} \) (smallest)

### Final Order of Size
Thus, the correct order of size is:
\[ O^{2-} > O^{-} > F^{-} > F^{0} \]