Both assertion and reason are correct, but reason is not the correct explanation of assertion.. Actually, I think the reason should be that since in amides, the lone pair of nitrogen gets shifted off to oxygen.. U can also explain it through the - M effect of - C=O group, which promotes acidity rather than basicity..

Reasoning for Amines being more basic than amides:

Electronegativity of Nitrogen vs Oxygen:
- Nitrogen is less electronegative than oxygen, which means it has a greater ability to donate electrons.
- In a basic reaction, the amine donates a lone pair of electrons to a proton, forming a new bond and creating a positively charged ammonium ion. This process is facilitated by the nitrogen atom's ability to donate electrons.

Basicity of Amines:
- Amines have a lone pair of electrons on the nitrogen atom, making them excellent electron donors.
- This lone pair can readily form a bond with a proton, leading to the formation of an ammonium ion.
- The presence of this lone pair of electrons enhances the basicity of amines.

Basicity of Amides:
- Amides have a carbonyl group (C=O) attached to the nitrogen atom, which delocalizes the lone pair of electrons.
- This delocalization reduces the availability of the lone pair for donation, decreasing the basicity of amides compared to amines.
- The carbonyl group attracts electron density, making the lone pair less available for basic reactions.

Conclusion:
- Due to the lower electronegativity of nitrogen and the presence of a readily available lone pair of electrons, amines are more basic than amides. This difference in basicity can be attributed to the structural differences between amines and amides, specifically the presence of a carbonyl group in amides that reduces the basicity of the nitrogen atom.