Question

Question: Explain why $\mathit{C}{\mathit{H}}_{\mathbf{3}}\mathit{C}{\mathit{H}}_{\mathbf{2}}\mathit{N}\mathit{H}\mathit{C}{\mathit{H}}_{\mathbf{3}}$has a higher boiling point than ${\left(C{H}_3\right)}_{\mathbf{3}}\mathit{N}$, even though they have the same molecular weight.

Short answer

Answer

The presence of hydrogen bonding results in$C{H}_{3}C{H}_{2}NHC{H}_3$ having a higher boiling point than${\left(C{H}_3\right)}_{3}N$.

Step-by-step solution

Boiling point

Various intermolecular forces regulate boiling point, and hydrogen bonding is an important intermolecular force.

Intermolecular forces

Intermolecular forcescan also be designated as “non-covalent interactions.”The interaction present in the molecule can be understood with the help of the functional groups present in them.

Comparison of the boiling points of CH3CH2NHCH3 and (CH3)3N

In the compound$C{H}_{3}C{H}_{2}NHC{H}_3$, hydrogen bonding takes place as the hydrogen atom is connected to the nitrogen atom.

However, in the case of the compound${\left(C{H}_3\right)}_{3}N$, hydrogen bonding is absent as the hydrogen is not directly linked to an electronegative atom in this compound.

Hence, the presence of hydrogen bonding results in$C{H}_{3}C{H}_{2}NHC{H}_3$ having a higher boiling point than${\left(C{H}_3\right)}_{3}N$.