Question

Which of the following is not correct?
A.Basic strength:

B.Acidic strength:

C.Basic strength:

Answer 1

To answer this question, you should recall the concept of acidic strength and basic strength. Use the concept of inductive effect and resonance effect to find the correct relation for this question.

Complete Step by step solution:
We know that the resonance effect is more effective than the inductive effect. We can define the resonance effect as the resonance effect can be defined as a chemical phenomenon which is observed in the characteristic compounds having double bonds in the organic compounds.
We can define the inductive effect as when an electron-releasing or an electron-withdrawing species is introduced to a chain of atoms (generally a carbon chain), the corresponding negative or positive charge is relayed through the carbon chain by the atoms belonging to it. This causes a permanent dipole to arise in the molecule and is referred to as the inductive effect.
Let us analyze each option systematically:
A.This condition is correct as $+ {\text{M}}$ of amine group is stronger than $+ {\text{I}}$ thus, increases the basic character further of the molecule. Hence, this option can be eliminated
B.This condition is correct as the acidic strength of sulphonic acid is stronger than the carboxylic acid group. Hence, this option can be eliminated
C.The basic strength of the second molecule of more than the first molecule because the lone pair of the nitrogen atom is ore available in the second molecule as it is out of the plane with the benzene ring due to the steric hindrance from the methyl group while the lone pair of nitrogen in the first molecule is less available due to resonance. Hence, this option is the correct option as the given condition is incorrect.

Therefore, we can conclude that the correct answer to this question is option C.

Note: Make sure you remember the difference between different types of bases and acids:
Arrhenius Acid: Hydronium breaks up to yield a hydronium in solution. Arrhenius Base: Hydroxide is dissolved in water as $O{H^ - }$.
Bronsted-Lowry Acid: Hydronium is a ${H^ + }$ donor regardless of the solution. Bronsted-Lowry Base: Hydroxide attacks and accepts them ${H^ + }$ from hydronium.
Lewis Acid: The ${H^ + }$ on Hydronium accepts the attacking electron pair to form a bond. Lewis Base: Hydroxide donates electron pairs present over it to form a bond between itself and the Lewis acid.