Most basic compound is

Options

A. `C_(6)H_(5)NH_(2)`
B. `NH_(3)`
C. `CH_(3)NH_(2)`
D. `(C_(6)H_(5))_(2)NH`

Answer

To determine the most basic compound among the given options, we need to analyze the basicity of different amines. Here’s a step-by-step breakdown of the solution:

### Step 1: Understand Basicity
Basicity refers to the ability of a compound to accept protons (H⁺ ions). In the context of amines, the presence of a lone pair of electrons on the nitrogen atom allows it to act as a base.

### Step 2: Compare Alkyl and Aryl Amines
Alkyl amines (RNH₂) are generally more basic than aryl amines (C₆H₅NH₂) because the alkyl groups are electron-donating, which increases the electron density on the nitrogen atom, enhancing its ability to accept protons.

### Step 3: Analyze the Given Options
1. **C₆H₅NH₂ (Aniline)**: This is an aryl amine. The lone pair on the nitrogen is delocalized into the aromatic ring, reducing its availability to accept protons. Therefore, it is less basic.

2. **RNH₂ (Alkyl amine)**: Alkyl amines are more basic than aryl amines due to the electron-donating effect of the alkyl groups.

3. **NH₃ (Ammonia)**: Ammonia has a lone pair on nitrogen that is available for protonation, making it a good base, but it is less basic than alkyl amines.

4. **C₆H₅NH (Phenylamine)**: Similar to aniline, this compound will also be less basic due to the delocalization of the lone pair into the aromatic system.

### Step 4: Conclusion
Among the options, alkyl amines (RNH₂) are the most basic due to the electron-donating effect of the alkyl groups. Therefore, the most basic compound is the alkyl amine.

### Final Answer
The most basic compound is **RNH₂ (Alkyl amine)**.

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