   Chapter 7, Problem 86SCQ

Chapter
Section
Textbook Problem

Sodium metal reacts readily with chlorine gas to give sodium chloride.Na(s) + 1/2CI2(g) → NaCI(s) (a) What is the reducing agent in this reaction? What property of the element contributes to its ability to act as a reducing agent? (b) What is the oxidizing agent in this reaction? What property of the element contributes to its ability to act as an oxidizing agent? (c) Why does the reaction produce NaCl and not a compound such as Na2CI or NaCl2?

a)

Interpretation Introduction

Interpretation:

The reducing agent and property of the element to act as reducing agent has to be discussed.

Concept Introduction:

Reducing agent: In a redox reaction, a reducing agent is an element or compound that loses an electron to another chemical species.

Explanation

Let us consider the given reaction

2Na(g)+Cl2(g)2NaCl(s)O.S:(0)

b)

Interpretation Introduction

Interpretation:

The oxidizing agent and property of the element to act as oxidizing agent has to be discussed.

Concept Introduction:

Oxidizing agent: In a redox reaction, a oxidizing agent is an element or compound that gains an electron from another chemical species.

c)

Interpretation Introduction

Interpretation:

The given reaction only produce NaCl but no other compounds ; the reason has to be discussed.

Concept Introduction:

Ionization energy (IE): The ionization energy is the required to remove an electron from an atom in the gas phase.

General formula of ionization energy= Atom in the ground state(g)Atom+(g)+eΔU=Ionizationenergy(IE)

As predicted by coulomb’s law, energy must be supplied to overcome the attraction between an electron and the nucleus and to separate the electron from the atom. Thus ionization energies always have positive values. An electron father from the nucleus generally has smaller ionization energy and electron closer to the nucleus has larger ionization energy.

Increase and decrease electro negativity: The less vacancy electrons an atoms has the least it will gain of electrons. Moreover the electron affinity decrease down the groups and from right to left across the periods on the periodic table, the reason is electrons are placed in a higher energy level far from the nucleus thus a decrease from its pull.

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