Chapter 17, Problem 17.78CP

Interpretation Introduction

Interpretation:

The reason for propanamide having higher boiling point comparing to methyl acetate even though both are soluble in water has to be determined.

Concept Introduction:

Hydrogen bonding is a type of dipole-dipole interaction of molecules when the hydrogen is bonded to strong electronegative atom in the molecules.

The boiling points of aliphatic amines are higher than those of alkanes or haloalkanes of similar relative molecular mass due to intermolecular hydrogen bonding.

The $\text{N-H}$ bond is more polar than the $\text{C-H}$ bond but less polar than $\text{O-H}$ bond.

Increasing order of boiling point of some organic compounds with similar molecular weight can be represented as follows,

$\text{Alkane}\text{<}\text{Ether}\text{<}\text{Alkyl}\text{halide}\text{<}\text{Amine}\text{<}\text{Ketone}\text{,}\text{aldehyde}\text{<}\text{Alcohol}\text{<}\text{Carboxylic}\text{acid}$