The molecule having highest bond enegy is

Options

A. `N -N`
B. `F -F`
C. `C -C`
D. `O -O`

Explanation

To determine which molecule has the highest bond energy among nitrogen-nitrogen (N≡N), fluorine-fluorine (F-F), carbon-carbon (C-C), and oxygen-oxygen (O=O), we need to analyze the bond characteristics of 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. Higher bond energy indicates a stronger bond.

2. **Analyzing Each Bond**:
- **Nitrogen-Nitrogen (N≡N)**:
- This bond is a triple bond, which is generally very strong. However, nitrogen has one lone pair on each atom which can lead to some repulsion.
- **Fluorine-Fluorine (F-F)**:
- This bond is a single bond. Fluorine atoms have three lone pairs each, leading to significant lone pair-lone pair repulsion, which weakens the bond.
- **Carbon-Carbon (C-C)**:
- This bond is a single bond as well. Carbon atoms have no lone pairs, which means there is minimal repulsion, making the bond relatively strong.
- **Oxygen-Oxygen (O=O)**:
- This bond is a double bond. Each oxygen has two lone pairs, which contributes to some repulsion but is still stronger than the F-F bond.

3. **Comparing Bond Energies**:
- The bond energy can be ranked based on the type of bond and the presence of lone pairs:
- C-C bond has no lone pairs, making it strong.
- N≡N bond is strong due to the triple bond but has lone pairs.
- O=O bond is weaker than N≡N due to more lone pair repulsion.
- F-F bond is the weakest due to the high number of lone pairs causing significant repulsion.

4. **Conclusion**:
- Based on the analysis, the order of bond energies from highest to lowest is:
- C-C > N≡N > O=O > F-F
- Therefore, the molecule with the highest bond energy is **Carbon-Carbon (C-C)**.

### Final Answer:
The molecule having the highest bond energy is **C (Carbon-Carbon)**.