Why pyridine is less basic

Pyridine has a cyclic system. Lone pair of nitrogen in pyridine is delocalized. Correct answer is option 'B'. Can you explain this answer? Answer to Question. Kriti Alam Jul 30, As the lone pair in Pyridine is sp2 hybrid. Thus pyridine is less basic than triethyl amine. Hardik Dahiya Apr 01, The sp2 hybrid has larger s-character NEET Among the following amines, the strongest Bronsted base is AMU Which of the following reactions is appropriate for converting acetamide to methanamine?

Chemistry Most Viewed Questions. Identify a molecule which does not exist. Identify the incorrect match. Which of the following set of molecules will have zero dipole moment? But why is pyrimidine less basic than pyridine? It is not the number of lone pairs that in any way explains basicity. Take a random sugar and it will have ten times the number of lone pairs albeit on oxygen, not on nitrogen without being significantly basic.

The problem is electronics. Going from pyridine to pyrimidine we need to double that. Thus, there is a perceived severe shortage of electrons in that ring since both nitrogens are trying to draw them towards themselves.

Now assume you protonate that species. We now have two nitrogens of which one is positively charged. Immediately, that positively charged nitrogen multiplies its electron-withdrawing force.

Equally immediately, the other nitrogen feels electron density leaving its vicinity. The whole system is much less favourable than the pyridine system with only a single nitrogen. Rephrasing that argument: Basicity is increased when electron- donating neighbours increase the electron density that equals a partial negative charge on an atom.

Both N are slightly basic. Apna phone number register karein. Ab aap Whatsapp pe solutions paa saktey h, hum aapko message karenge. Ab aap Whatsapp pe solutions paa saktey h, hum aapko ping karenge. Study Materials. Why use Doubtnut? Instant Video Solutions.