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. The higher the bond energy, the stronger the bond.

### Step 2: Identify the Bonds
We need to identify the bonds in question. The bonds mentioned in the transcript are:
- C-C (Carbon-Carbon)
- C-S (Carbon-Sulfur)
- C=O (Carbon-Oxygen)
- P-N (Phosphorus-Nitrogen)

### Step 3: Analyze Electronegativity
Electronegativity plays a crucial role in determining bond strength. The more electronegative an atom is, the stronger it can attract electrons, leading to a stronger bond.

### Step 4: Compare Electronegativity of Atoms
- Carbon (C) has an electronegativity of about 2.5.
- Sulfur (S) has an electronegativity of about 2.5.
- Oxygen (O) has a higher electronegativity of about 3.5.
- Phosphorus (P) has an electronegativity of about 2.1.
- Nitrogen (N) has an electronegativity of about 3.0.

### Step 5: Determine the Strongest Bond
From the analysis:
- The C-C bond is relatively weak because it involves two atoms of the same element.
- The C-S bond is weaker than the C=O bond because sulfur is less electronegative than oxygen.
- The C=O bond is stronger due to the high electronegativity of oxygen.
- The P-N bond is weaker than the C=O bond because phosphorus is less electronegative than nitrogen.

### Conclusion
The bond with the highest bond energy is the **C=O (Carbon-Oxygen) bond** due to the high electronegativity of oxygen, which results in a stronger attraction between the atoms.

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