Introduction:
Tri methyl amine, di methyl amine, and methyl amine are all organic compounds that belong to the class of amines. Amines are organic derivatives of ammonia, where one or more hydrogen atoms are replaced by alkyl or aryl groups. These compounds can act as bases due to the presence of a lone pair of electrons on the nitrogen atom. However, the basicity of amines can vary depending on the substitution pattern and the electron-donating or electron-withdrawing nature of the substituents.

Basicity of amines:
Basicity is a measure of the ability of a compound to donate a pair of electrons. In the case of amines, the lone pair of electrons on the nitrogen atom can be donated to an electron-deficient species, forming a coordinate bond. The basicity of an amine is influenced by several factors, including the electron density on the nitrogen atom, steric hindrance, and resonance effects.

Comparison of basicity:
Tri methyl amine, di methyl amine, and methyl amine can be compared based on their basicity in aqueous solution.

1. Electronic effects:
The basicity of amines is primarily determined by the availability of the lone pair of electrons on the nitrogen atom. In this case, tri methyl amine has three methyl groups attached to the nitrogen atom, which are electron-donating groups. These groups increase the electron density on the nitrogen atom, making the lone pair of electrons less available for donation. On the other hand, di methyl amine has only two methyl groups, and methyl amine has no additional methyl groups. Therefore, the electron density on the nitrogen atom decreases in the order: tri methyl amine < di="" methyl="" amine="" />< methyl="" />

2. Steric hindrance:
Steric hindrance refers to the repulsion between bulky substituents, which can affect the basicity of amines. In this case, tri methyl amine has three methyl groups, which create more steric hindrance compared to di methyl amine and methyl amine. The bulky nature of the substituents in tri methyl amine hinders the approach of an electron-deficient species, reducing its basicity.

3. Resonance effects:
Resonance effects can also influence the basicity of amines. In this case, the resonance stabilization of the lone pair of electrons on the nitrogen atom is similar for all three compounds. Therefore, resonance effects do not significantly contribute to the difference in basicity between tri methyl amine, di methyl amine, and methyl amine.

Conclusion:
In aqueous solution, tri methyl amine is less basic than di methyl amine and methyl amine. This can be attributed to the electron-donating nature of the three methyl groups in tri methyl amine, which reduces the electron density on the nitrogen atom and decreases its basicity. Additionally, the steric hindrance caused by the bulky substituents in tri methyl amine further decreases its basicity compared to di methyl amine and methyl amine.