The two bonds N = O and N - O in `H_3CNO_2` are of same bond length due to

Options

A. Inductive effect
B. Hyperconjugation
C. Electrometric effect
D. Resonance effect

Answer

To solve the question regarding the bond lengths of the N=O and N-O bonds in H3CNO2 (nitromethane), we need to analyze the structure and bonding characteristics of the molecule.

### Step-by-Step Solution:

1. **Identify the Structure of H3CNO2**:
- The molecular formula H3CNO2 indicates that the compound is nitromethane. The structure consists of a carbon atom bonded to three hydrogen atoms (CH3) and a nitrogen atom, which is further bonded to two oxygen atoms.

2. **Draw the Lewis Structure**:
- In nitromethane, the nitrogen atom is bonded to one carbon atom and has two oxygen atoms attached to it. One of the oxygen atoms is connected by a double bond (N=O) and the other by a single bond (N-O).

3. **Understand Resonance**:
- The nitro group (NO2) can exhibit resonance. This means that the double bond and single bond can shift between the two oxygen atoms. This leads to the formation of multiple valid Lewis structures, where the double bond can be between nitrogen and either oxygen.

4. **Bond Length Consideration**:
- In general, a double bond is shorter than a single bond due to the increased overlap of orbitals. However, in the case of nitromethane, the resonance allows for the delocalization of electrons between the nitrogen and the oxygen atoms.

5. **Conclusion on Bond Lengths**:
- Due to resonance, the N=O and N-O bonds do not behave as typical double and single bonds. Instead, they exhibit characteristics of both bonds, leading to them having similar bond lengths. This is because the resonance hybrid does not favor one structure over the other, resulting in equal bond lengths.

### Final Answer:
The two bonds N=O and N-O in H3CNO2 are of the same bond length due to resonance, which allows for the delocalization of electrons and equalizes the bond characteristics.

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