A molecule is described by three Lewis structures having energies `E_1`, `E_2`, and `E_3`, respectively. The energies of these structures follow the order `E_1gtE_2gtE_3`, respectively. If the experimental energy of the molecules 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 described by the three Lewis structures with energies \( E_1 \), \( E_2 \), and \( E_3 \), we can follow these steps:

### Step 1: Understand the Concept of Resonance
Resonance refers to the phenomenon where a molecule can be represented by two or more valid Lewis structures (canonical forms) that differ only in the arrangement of electrons. The actual structure of the molecule is a resonance hybrid of these forms.

### Step 2: Identify the Energies of the Lewis Structures
The problem states that the energies of the three Lewis structures follow the order:
\[ E_1 > E_2 > E_3 \]
This means \( E_3 \) is the lowest energy structure, and thus, it is the most stable among the three.

### Step 3: Determine the Experimental Energy
The experimental energy of the molecule is given as \( E_0 \). This energy corresponds to the energy of the resonance hybrid, which is a more stable configuration than any individual Lewis structure.

### Step 4: Calculate the Resonance Energy
The resonance energy (\( RE \)) can be calculated using the formula:
\[ RE = E_0 - E_{\text{lowest}} \]
In this case, since \( E_3 \) is the lowest energy structure, we substitute it into the formula:
\[ RE = E_0 - E_3 \]

### Final Answer
Thus, the resonance energy of the molecule is:
\[ RE = E_0 - E_3 \]

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