Question

relative basic strength of amines doesn't depend upon a)inductive effect b)mesomeric effect c)steric effect d) stabilisation of cation by hybridisation​

Answer 1

Answer:

mesomeric effect is correct answer

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Answer 2

Answer:

The answer is (b) the mesomeric effect

Explanation:

The other three options affect the relative basic strength of amines.

The Factors influencing the basic strength of amines are the Inductive effect, Steric Factor, and solvation of ions

• The basic character of amines is due to the presence of unshared electron pair on the nitrogen atom, which accepts the proton.

• Due to the positive inductive effect(+I effect) of alkyl groups the electron density at nitrogen atom increases and makes unshared electron pairs more available for protonation.

• The anomalous behavior of tertiary amines is due to the steric factors not due to the electronic effect.

• The inductive effect is maximum in tertiary amines but the presence of bulky substituents physically prevents the proton from combining with lone pair of electrons. Thus bulkier the alkyl group, the lower is the base strength

• When an amine is dissolved in water, the N-atom of amine forms a hydrogen bond with the H-atom of water.
• Thus the amine gets hydrated through hydrogen bonding. Consequently, bonding energy, called hydration energy is released.

• The greater the extent of hydrogen bonding in protonated amine, the greater will be the release of hydration energy which will directly influence the basicity of amines

The combined effects of steric effect, inductive effect, and solvation of ions, secondary amines are the strongest while the tertiary amines are the least basic

• The basic strength of primary, secondary, and tertiary amines are:

        Secondary amine> Primary amine > Tertiary amine

However aromatic amines are weaker bases than alkyl amines due to the electron-withdrawing nature of the aryl group.

• In Aryl amines (for example aniline) due to the +M effect of the ($-NH_{2}$ ) group or electron-withdrawing aryl group ( $Ar$ ), the lone pair of electrons on nitrogen is delocalized into the ring by resonance, and hence it is less available for protonation

• Therefore electron-withdrawing group decreases the basic strength of amines