Chapter 15, Problem 4RQ

(a)

Interpretation Introduction

Interpretation:

Lewis structure for bromide ion and reason it is called as base under Bronsted-Lowry and Lewis acid-base concept has to be written.

Concept Introduction:

Bronsted-Lowry acid outlined the definition of acids that donate ${\text{H}}^{+}$ or a proton while bases that accept ${\text{H}}^{+}$ or a proton.

As per the Bronsted definition, the most usual type of acid-base reaction involves lone pair of base that reaches out for an acidic proton as illustrated in the equation below.

In accordance with Lewis's concept, an acid species accepts an electron-pair from some other electron-rich species while a base that has generally more electron density donates it to another electron-deficient species.

In accordance with Lewis concept, an acid species accepts an electron-pair from some other electron-rich species while a base that has generally more electron density donates it to another electron-deficient species. For instance of Lewis acids that have electron-deficient central atom like ${\text{BF}}_3$ and ${\text{SO}}_3$. Similarly, Lewis bases include triethylamine, pyridine. These can form adducts with Lewis acids as illustrated in the equation below.

(b)

Interpretation Introduction

Interpretation:

Lewis structure for hydroxide ion and the reason it is called as base under Bronsted-Lowry and Lewis acid-base concept has to be written.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Lewis structure for cyanide ion and the reason it is called as base under Bronsted-Lowry and Lewis acid-base concept has to be written.

Concept Introduction:

Refer to part (a).