Which of the following compounds will not show resonance?

Options

A.
B. `CH_(2)=CH-CH=CH-overset(o+)CH_(2)`
C.
D.

Explanation

To determine which of the given compounds does not show resonance, we need to analyze the structures of each compound and identify whether they have the ability to delocalize electrons through resonance.

### Step-by-Step Solution:

1. **Understanding Resonance:**
- Resonance occurs when a molecule can be represented by two or more valid Lewis structures, which differ only in the placement of electrons. This typically involves the presence of conjugated double bonds or lone pairs adjacent to double bonds.

2. **Analyzing the Compounds:**
- Let's denote the compounds as A, B, C, and D for analysis.
- For each compound, we need to check for the presence of conjugated systems or charges that can participate in resonance.

3. **Compound A:**
- If Compound A has a structure with double bonds and adjacent lone pairs or charges, it is likely to show resonance.

4. **Compound B:**
- Similar to Compound A, if Compound B has conjugated double bonds or lone pairs adjacent to double bonds, it may also exhibit resonance.

5. **Compound C:**
- In this compound, if there is a nitrogen atom that is forming five bonds (which is not possible), it indicates that the structure cannot stabilize through resonance. This means that Compound C does not show resonance due to the violation of the octet rule for nitrogen.

6. **Compound D:**
- If Compound D has a structure that allows for resonance (like double bonds or lone pairs), it will show resonance.

7. **Conclusion:**
- Based on the analysis, Compound C is the one that does not show resonance because it involves a nitrogen atom that cannot form five bonds. Therefore, the correct option is C.

### Final Answer:
The compound that will not show resonance is **C**.