Question

All Bronsted bases are also Lewis bases but all Lewis acids are not Bronsted acids. Justify.

Answer 1

A Lewis acid can accept an electron pair and form a bond. A Brønsted-Lowry acid can give up a proton which does exactly that, and thus every Brønsted-Lowry acid fits the definition of a Lewis acid. As you noted in the question, every Brønsted-Lowry baseis also a Lewis base, but the reverse isnot true.

Answer 2

Explanation:

According to the Bronsted Lowry conjugate acid-base theory, an acid is defined as a substance which donates protons and a base is defined as a substance which accepts protons.

According to the Lewis concept, an acid is defined as a substance that accepts electron pairs and base is defined as a substance which donates electron pairs.

Thus $NH_3$ which can accept a proton and can also donate its lone pair of electron to the proton an accepting it is both a Bronsted base and a lewis base.

But $AlCl_3$ which is lewis acid as it can accept electrons cannot donate a proton. Thus is a lewis acid but not a bronsted acid.

Learn more about bronsted and lewis concept

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https://brainly.com/question/1452785