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According to Bronsted & Lowry , acids are proton donors and bases are proton acceptors. Lewis defined an acid as electron pair acceptor and base as an electron pair donor.
Thus if the electron pair is freely available the compound is more basic. For example in aniline, the lone pair of electrons on nitrogen is involved in resonance and is less available for protonation. Thus aniline is weaker base than aliphatic amines where the electron pair is freely available.
The relative basic strength ( availability electron pair) depends upon the following factors:
1.Resonance effect, 2.Inductive effect, 3.Internal H-bonding, 4.Orbital nature of electron pair, 5.Steric effect, 6.Solvent effect, 7.Bond length, 8. Electronegativity of the bonded atom.
Moderation Team
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