Compare the relative basicity of the following amines.
I know that the higher the electron density on the nitrogen the higher will be its basicity. So here’s my take on each option.
(a)The Nitrogen lone pair undergoes resonance. It’s not good for basic strength
(b) A doubly bonded nitrogen lone pair does not undergo resonance. So, the Nitrogen lone pair are localised.
(c) Both nitrogen atoms are doubly bonded and so their lone pair won’t be delocalised and the electron density is localised here as well.
(d) There’s no question of resonance here so the lone pairs are localised anyway
From the above points my answer is (c)>(b)>(d)>(a) but the answer given is (d)>(b)>(c)>(a)
Is there any mistake in my reasoning?