Chapter 16, Problem 16.93QP

(a)

Interpretation Introduction

Interpretation:

• The reaction between the hydride ion ${\text{H}}^{\text{-}}$ and water in terms of a Bronsted acid-base reaction has to be described.

Concept Information:

Bronsted acid-base reaction:

Bronsted definition deals with the transfer of protons.

Bronsted's definition is based on the  chemical reaction that occur when both acids and bases are added with each other. In Bronsted's theory acid donates proton , while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

    $\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Redox reaction:

The oxidation and reduction taking place in a same reaction is termed as oxidation-reduction reaction or redox reaction.  Redox reactions, involves the transfer of electrons between two substances or species.

Oxidation: involves removal or loss of electrons

Reduction: involves addition or gain of electrons

The substance that has the tendency to oxidize other substance is said to be an oxidizing agent. It removes electron from other substance.  Since, it removes and accepts electron from other substance, it is called as an electron acceptor

The substance that has the tendency to reduce other substance is said to be an reducing agent. It transfers electrons to other substance.  Since, it transfers and donates electrons to other substance it is called as an electron donor

To Describe: The reaction between the hydride ion ${\text{H}}^{\text{-}}$ and water in terms of a Bronsted acid-base reaction and the oxidizing and reducing agents for the above reaction

(b)

Interpretation Introduction

Interpretation:

• The same reaction is also classified as redox reaction.  The oxidizing and reducing agents for this reaction has to be identified.

Concept Information:

Bronsted acid-base reaction:

Bronsted definition deals with the transfer of protons.

Bronsted's definition is based on the  chemical reaction that occur when both acids and bases are added with each other. In Bronsted's theory acid donates proton , while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

    $\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Redox reaction:

The oxidation and reduction taking place in a same reaction is termed as oxidation-reduction reaction or redox reaction.  Redox reactions, involves the transfer of electrons between two substances or species.

Oxidation: involves removal or loss of electrons

Reduction: involves addition or gain of electrons

The substance that has the tendency to oxidize other substance is said to be an oxidizing agent. It removes electron from other substance.  Since, it removes and accepts electron from other substance, it is called as an electron acceptor

The substance that has the tendency to reduce other substance is said to be an reducing agent. It transfers electrons to other substance.  Since, it transfers and donates electrons to other substance it is called as an electron donor

To Describe: The reaction between the hydride ion ${\text{H}}^{\text{-}}$ and water in terms of a Bronsted acid-base reaction and the oxidizing and reducing agents for the above reaction