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 order and the nature of the bonds in each molecule.

### Step-by-Step Solution:

1. **Understanding Bond Energy**:
- Bond energy is defined as the amount of energy required to break one mole of a bond in a molecule into its constituent atoms.
- Generally, higher bond energy indicates a stronger bond.

2. **Identifying the Molecules**:
- Let's consider the molecules mentioned: F2, CO, and HF.

3. **Analyzing F2**:
- In F2, each fluorine atom has 7 valence electrons. They share one pair of electrons to form a single bond.
- **Bond Order**: 1 (since there is one bond).
- **Bond Energy**: Relatively low due to the single bond.

4. **Analyzing CO**:
- Carbon has 4 valence electrons and oxygen has 6. They share two pairs of electrons to form a double bond.
- **Bond Order**: 3 (since there are three bonds: one double bond and one coordinate bond).
- **Bond Energy**: High due to the double bond and the nature of the bond.

5. **Analyzing HF**:
- In HF, hydrogen has 1 valence electron and fluorine has 7. They share one pair of electrons to form a single bond.
- **Bond Order**: 1 (since there is one bond).
- **Bond Energy**: Moderate, but lower than CO.

6. **Comparing Bond Energies**:
- F2 has a bond order of 1, HF has a bond order of 1, and CO has a bond order of 3.
- Since bond energy is directly proportional to bond order, CO will have the highest bond energy among the three.

7. **Conclusion**:
- The molecule with the maximum bond energy is **CO (Carbon Monoxide)**.