The bond having the highest bond energy is :

Options

A. `C=C`
B. `C=S`
C. `C=O`
D. `P=N`

Explanation

To determine which bond has the highest bond energy among the given options, we can follow these steps:

### Step 1: Understand Bond Energy
Bond energy is the amount of energy required to break a bond between two atoms. It is influenced by the overlap of atomic orbitals and the size of the atoms involved in the bond.

### Step 2: Factors Affecting Bond Energy
1. **Overlap of Orbitals**: Better overlap leads to stronger bonds and higher bond energy.
2. **Size of Atoms**: Smaller atoms can form stronger bonds due to better overlap and less repulsion.

### Step 3: Analyze the Given Options
Assuming the options are:
- A) P=N (Phosphorus double bond Nitrogen)
- B) C=O (Carbon double bond Oxygen)
- C) C=S (Carbon double bond Sulfur)
- D) C=C (Carbon double bond Carbon)

### Step 4: Evaluate Each Option
- **Option A (P=N)**: Both phosphorus and nitrogen have lone pairs, leading to lone pair-lone pair repulsion, which decreases the bond energy.

- **Option B (C=O)**: Carbon and oxygen are relatively small atoms, and there is no lone pair-lone pair repulsion. This bond typically has a high bond energy due to effective overlap.

- **Option C (C=S)**: While carbon is small, sulfur is larger than oxygen, which may lead to less effective overlap and lower bond energy compared to C=O.

- **Option D (C=C)**: This bond is strong, but typically, double bonds involving oxygen (like C=O) have higher bond energies due to the electronegativity of oxygen.

### Step 5: Conclusion
Comparing the bond energies, the C=O bond generally has the highest bond energy among the options provided due to effective overlap and the small size of both atoms involved.

### Final Answer
The bond having the highest bond energy is **C=O (Carbon double bond Oxygen)**.

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