Chapter 16, Problem 139AP

Interpretation Introduction

Interpretation:

The reaction between a hydride ion and water, in terms of Bronsted acid–base theory is to be described and its classification as a redox reaction is to be verified alongwith the identification of reducing and oxidizing agents.

Concept introduction:

According to the Bronsted–Lowry theory, a substance with the ability to donate a proton, acts as an acid. The acid is named as a Bronsted Acid.

A Bronsted base is a substance that accepts a proton and forms its conjugate acid.

Redox reactions are those in which both oxidation and reduction of the species takes place, simultaneously.

Loss of electrons leads to oxidation and gain of electrons leads to reduction

An element or compound that donates an electron to another chemical species in a redox chemical reaction is known as reductant or reducing agent. Reducing agent is said to have been oxidized, since it is losing electrons.

An oxidizing agent also known as oxidant, gains electrons and is reduced in a chemical reaction. Asoxidizing agentgain electrons and be reduced, it is normally in one of its higher possible oxidation states.