A molecule may be represented by three structures having energies `E_(1), E_(2) and E_(3)`, respetively. The energies of these structures follow the order `E_(2)ltE_(2)ltE_(1)`, respectively. If the experimantal bond energy of the molecule is `E_(0)`, the resonance energy is :

Options

A. `(E_(1)+E_(2)+E_(3))-E_(0)`
B. `E_(0)-E_(3)`
C. `E_(0)-E_(1)`
D. `E_(0)-E_(2)`

Answer

To find the resonance energy of the molecule represented by three structures with energies \( E_1, E_2, \) and \( E_3 \) (where \( E_1 > E_2 > E_3 \)), and given that the experimental bond energy of the molecule is \( E_0 \), we can follow these steps:

### Step 1: Understand the Concept of Resonance Energy
Resonance energy is defined as the difference between the energy of the most stable resonance hybrid (which is represented by the experimental bond energy \( E_0 \)) and the energy of the most stable canonical structure (which is the one with the lowest energy among the resonance structures).

### Step 2: Identify the Energies
From the problem, we have:
- \( E_1 \) (highest energy)
- \( E_2 \) (middle energy)
- \( E_3 \) (lowest energy)

### Step 3: Write the Formula for Resonance Energy
The resonance energy \( R \) can be calculated using the formula:
\[ R = E_0 - E_3 \]
where \( E_0 \) is the experimental bond energy of the molecule, and \( E_3 \) is the energy of the most stable canonical structure (the one with the lowest energy).

### Step 4: Substitute the Values
Now, we substitute the values into the formula. Since we don't have numerical values, we keep it in terms of the energies:
\[ R = E_0 - E_3 \]

### Conclusion
Thus, the resonance energy of the molecule is given by the expression \( R = E_0 - E_3 \).

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