Question

Classify the following substances as a Bronsted-Lowry acid, Bronsted-Lowry base, Lewis acid, and/or Lewis base.

HCl, BF_3,

CCl_3, -H

CH_2O, CH_3Cl

-OCH_3 , NH_3

Answer 1

Answer :

HCl : Bronsted-Lowry acid

$BF_3\text{ and }^{+}CCl_3$ : Lewis-acid

$^-H, CH_2O,^-OCH_3\text{ and }NH_3$ : Bronsted-Lowry base

$^-H, CH_2O,^-OCH_3,CH_3Cl\text{ and }NH_3$ : Lewis-base

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.

HCl :

It is a Bronsted-Lowry acid that donates protons.

$BF_3\text{ and }^{+}CCl_3$ :

It is a Lewis-acid that accepts electron pairs.

$^-H, CH_2O,^-OCH_3\text{ and }NH_3$ :

It is a Bronsted-Lowry base that accepts protons.

$^-H, CH_2O,^-OCH_3,CH_3Cl\text{ and }NH_3$ :

It is a Lewis-base that donates electron pairs.