Question

All Bronsted acids are not Lewis acids. Explain.
Which of the following is strongest conjugate base? CH3-,
NH2-, OH-, F-​

Answer 1

Answer:

Any substance which can donate a pair of an electron can easily accept a proton. ... HCl, H2SO4 are Bronsted acids because they can donate protons, but they cannot accept a pair of electrons to form a coordinate bond, therefore, they are not Lewis acids. Thus all Bronsted acids are not Lewis acids.

2. CH3-

Explanation:

Answer 2

Answer:

1. Bronsted acids can donate H⁺ easily but they may not be able to donate electron like H₂SO₄ , HNO₃.

Therefore , All Bronsted acids are not Lewis acids.

Know more :

Bronsted - Lowry Concept :

According to this concept an acid is substance which can donate a proton H+ while base is substance which accepts proton.

For example :

$\sf HCl(ag)+H_2O(l) \rightleftharpoons H_3O^{+}(aq)+Cl^{-1}(aq)$

HCl is acid as it loses proton.

H₂O is base as it adds proton.

Conjugates acid - base :

The base which developed from an acid is called conjugates base.

Like wise acid which is formed from base is called conjugates acid.

2. CH₃⁻ is strongest conjugates base.

Read more :

In a gaseous reaction A + B ⇄ C + 2 D, 3 mol of inert gas is introduced into the vessel at constant pressure. What  will be its effect on equilibrium?

https://brainly.in/question/15893438

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