Find out the basic strength order.

Except the amines containing tertiary butyl group, all lower aliphatic amines are stronger bases than ammonia because of +I (inductive) effect. The alkyl groups, which are electron releasing groups, increase the electron density around the nitrogen thereby, increasing the availability of the lone pair of electrons to proton or Lewis acids and making the amine more basic. The observed order in the case of lower members is found to be as secondary > primary > tertiary. This anomalous behavior of tertiary amines is due to steric factors i.e. crowding of alkyl groups cover nitrogen atom from all sides and thus makes it unable for protonation. Thus the relative strength is in order CH3NH2<(CH3)2NH>(CH3)3N

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for tert butyl group the steric effect dominates and basicity is 0>1>2>3

Amines Basicity is 3>2>1>NH3 in gaseous state. But in Aqueous Media There is three factors which determine basicity 1)Inductive Effect 2)Solvation Of Ion 3) Steric Factor For CH3 there is no Steric Factors so Basicity is of Order 2>1>3 For C2H5 and others there is steric hindrance for formation of H-Bonding So it Becomes 2>3>1.

Explanation of above attached images Amines Basicity is 3>2>1>NH3 in gaseous state. But in Aqueous Media There is three factors which determine basicity 1)Inductive Effect 2)Solvation Of Ion 3) Steric Factor For CH3 there is no Steric Factors so Basicity is of Order 2>1>3 For C2H5 and others there is steric hindrance for formation of H-Bonding So it Becomes 2>3>1.

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