Among the following, the molecule expected to be stabilized by anion formation is :
` C_2 ,O_2 , NO ,F_2`

Options

A. `NO`
B. `O_(2)`
C. `C_2`
D. `F_2`

Explanation

To determine which molecule among C₂, O₂, NO, and F₂ is expected to be stabilized by anion formation, we need to analyze the bond order of each molecule and how it changes upon the formation of an anion.

### Step-by-Step Solution:

1. **Understanding Bond Order**:
The bond order can be calculated using the formula:
\[ \text{Bond Order} = \frac{(\text{Number of Bonding Electrons} - \text{Number of Anti-bonding Electrons})}{2} \]
A higher bond order indicates greater stability of the molecule.

2. **Calculate Bond Order for C₂**:
- C₂ has 12 electrons.
- When it forms the anion (C₂⁻), it gains one additional electron, totaling 13 electrons.
- In the molecular orbital configuration, C₂ has 9 bonding electrons and 4 anti-bonding electrons.
- Thus, the bond order is:
\[ \text{Bond Order}_{C_2} = \frac{(9 - 4)}{2} = \frac{5}{2} = 2.5 \]

3. **Calculate Bond Order for O₂**:
- O₂ has 16 electrons.
- When it forms the anion (O₂⁻), it gains one additional electron, totaling 17 electrons.
- In the molecular orbital configuration, O₂ has 10 bonding electrons and 6 anti-bonding electrons.
- Thus, the bond order is:
\[ \text{Bond Order}_{O_2} = \frac{(10 - 6)}{2} = \frac{4}{2} = 2.0 \]

4. **Calculate Bond Order for NO**:
- NO has 11 electrons.
- When it forms the anion (NO⁻), it gains one additional electron, totaling 12 electrons.
- In the molecular orbital configuration, NO has 7 bonding electrons and 5 anti-bonding electrons.
- Thus, the bond order is:
\[ \text{Bond Order}_{NO} = \frac{(7 - 5)}{2} = \frac{2}{2} = 1.0 \]

5. **Calculate Bond Order for F₂**:
- F₂ has 18 electrons.
- When it forms the anion (F₂⁻), it gains one additional electron, totaling 19 electrons.
- In the molecular orbital configuration, F₂ has 10 bonding electrons and 9 anti-bonding electrons.
- Thus, the bond order is:
\[ \text{Bond Order}_{F_2} = \frac{(10 - 9)}{2} = \frac{1}{2} = 0.5 \]

6. **Comparison of Bond Orders**:
- C₂: Bond Order = 2.5
- O₂: Bond Order = 2.0
- NO: Bond Order = 1.0
- F₂: Bond Order = 0.5

Among these, C₂ has the highest bond order, which indicates that it will be the most stabilized by anion formation.

### Conclusion:
The molecule expected to be stabilized by anion formation is **C₂**.