Arrange the following in increasing order of their basic strength :
C6H5 – NH2, C6H5 – CH2 – NH2, C6H5 – NH – CH3
C6H5-NH2 < C6H5-NH-CH3 < C6H5-CH2-NH2
C6H5-NH2 will be least basic because of the delocalisation of the lone pair of electrons present on the N-atom over the benzene ring due to the ‒R effect of the C6H5 group. However, C6H5-CH2-NH2 will be more basic than C6H5-NH-CH3 because of the electron-releasing nature of the CH3- group that increases the electron density on the N-atom, making the lone pair of electrons on the N-atom easily available for donation to a proton. The basicity of C6H5-NH-CH3 will be intermediate of C6H5-NH2 and C6H5-CH2-NH2 because the C6H5- group will tend to pull the electron density from the N-atom. On the other hand the CH3- group will tend to increase the electron density on the N-atom. Thus, the basic strength of the given amines will follow the above-mentioned order.