Why ch3 2 is more basic than ch3 3n in an aqueous solution?
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With increase in alkyl group the +I effect will increase which will increase the ease of donation of lone pair electron. But in water one other factor is controlling the strength of basicity.
Amine will accept a proton and form cation. This cation will be stabilised in water by salvation (by hydrogen bonding). Better the salvation by hydrogen bonding, higher will be the basic strength. Thus with increase in methyl group, hydrogen bonding and stabilisation by salvation decreases. The net effect is when we move from secondary to tertiary amine basic strength actually decreases.
With increase in alkyl group the +I effect will increase which will increase the ease of donation of lone pair electron. But in water one other factor is controlling the strength of basicity.
Amine will accept a proton and form cation. This cation will be stabilised in water by salvation (by hydrogen bonding). Better the salvation by hydrogen bonding, higher will be the basic strength. Thus with increase in methyl group, hydrogen bonding and stabilisation by salvation decreases. The net effect is when we move from secondary to tertiary amine basic strength actually decreases.
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