Which of the following molecules has the maximum value of bond energy ?

Options

A. `F_(2)(g)`
B. `N_(2)(g)`
C. `CO(g)`
D. `HF(g)`

Explanation

To determine which molecule has the maximum bond energy among the given options, we will analyze the bond types and bond orders of each molecule.

### Step-by-Step Solution:

1. **Understanding Bond Energy**:
- Bond energy (or bond dissociation energy) is the amount of energy required to break one mole of a bond between two atoms. Generally, higher bond order corresponds to higher bond energy.

2. **Analyzing the Given Molecules**:
- **F2 (Fluorine)**:
- Bond: F-F
- Bond Order: 1 (single bond)
- Bond Energy: Relatively low due to the single bond.

- **N2 (Nitrogen)**:
- Bond: N≡N
- Bond Order: 3 (triple bond)
- Bond Energy: High due to the triple bond.

- **CO (Carbon Monoxide)**:
- Bond: C≡O
- Bond Order: 3 (triple bond)
- Bond Energy: Also high, but it is a polar molecule, which can influence bond energy.

- **HF (Hydrogen Fluoride)**:
- Bond: H-F
- Bond Order: 1 (single bond)
- Bond Energy: Lower compared to triple bonds.

3. **Comparing Bond Energies**:
- Non-polar bonds (like F2) generally have lower bond energies than polar bonds.
- Between N2 and CO, both have a bond order of 3, but CO is polar, which can lead to stronger interactions and thus higher bond energy compared to N2.
- HF has the lowest bond energy due to its single bond.

4. **Conclusion**:
- Among the given options, **CO (Carbon Monoxide)** has the highest bond energy due to its triple bond and polar nature, making it the correct answer.

### Final Answer:
**Carbon Monoxide (CO) has the maximum value of bond energy among the given molecules.**

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