Which of the following statements is correct?

Options

A. Methyl amine is slighty acidic.
B. Methyl amine is less basic than ammonia.
C. Methyl amine is less basic than dimethyl amine.
D. Methyl amine is less basic than aniline.

Explanation

To determine which of the given statements is correct regarding methyl amine and its basicity compared to other compounds, we will analyze each statement step by step.

### Step-by-Step Solution:

1. **Statement A: Methyl amine is slightly acidic.**
- Methyl amine (CH3NH2) has a nitrogen atom with a lone pair of electrons. This lone pair allows it to act as a Lewis base, meaning it can donate its electrons. Acidity refers to the ability to donate protons (H+), and since methyl amine does not donate protons but rather accepts them, this statement is incorrect.

**Hint:** Remember that basicity is associated with the presence of lone pairs that can accept protons, while acidity is related to the ability to donate protons.

2. **Statement B: Methyl amine is less basic than ammonia.**
- Ammonia (NH3) is a stronger base than methyl amine. The presence of the methyl group in methyl amine does provide some electron-donating effect, but it is not enough to make methyl amine less basic than ammonia. Therefore, this statement is also incorrect.

**Hint:** Consider how electron-donating groups affect the basicity of amines. More electron-donating groups typically increase basicity.

3. **Statement C: Methyl amine is less basic than dimethylamine.**
- Dimethylamine (CH3)2NH has two methyl groups that donate electron density to the nitrogen. This increased electron density enhances the ability of the nitrogen to donate its lone pair, making dimethylamine more basic than methyl amine. Thus, this statement is correct.

**Hint:** Compare the number of electron-donating groups attached to the nitrogen atom in both compounds to evaluate their basicity.

4. **Statement D: Methyl amine is less basic than aniline.**
- Aniline (C6H5NH2) has a nitrogen atom whose lone pair is involved in resonance with the aromatic ring. This delocalization reduces the availability of the lone pair for protonation, making aniline less basic than methyl amine. Therefore, this statement is incorrect.

**Hint:** Remember that resonance can stabilize lone pairs, making them less available for bonding with protons, which decreases basicity.

### Conclusion:
The only correct statement among the options provided is **Statement C: Methyl amine is less basic than dimethylamine**.