Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Chapter 5, Problem 79QRT

Use electron configurations to explain why

  1. (a) sulfur has a lower electron affinity than chlorine.
  2. (b) boron has a lower first ionization energy than beryllium.
  3. (c) chlorine has a lower first ionization energy than fluorine.
  4. (d) oxygen has a lower first ionization energy than nitrogen.
  5. (e) iodine has a lower electron affinity than bromine.

(a)

Expert Solution
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Interpretation Introduction

Interpretation:

The reason for sulfur having lower electron affinity than chlorine has to be given using electron configurations.

Explanation of Solution

Electron affinity is the energy required to add an electron to the neutral atom.

  A+e-A-

The electronic configuration of neutral chlorine and chlorine anion is written as follows:

  ElectronicconfigurationofCl:[10Ne]3s23p5ElectroniccofigurationofCl-:[18Ar]

The electronic configuration of neutral sulfur and sulfuranion is written as follows:

  ElectronicconfigurationofS:[10Ne]3s23p4ElectroniccofigurationofS-:[10Ne]3s23p5

Addition of one electron to chlorine gives a noble gas configuration.  Hence, it has greater electron affinity than sulfur.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The reason for boron having lower first ionization energy than beryllium has to be given using electron configurations.

Explanation of Solution

The ionization energy is the energy required to remove the outermost electron in an atom.

  AA++e-

The electronic configuration of neutral boron and boroncation is written as follows:

  ElectronicconfigurationofB:[2He]2s22p1ElectroniccofigurationofB+:[2He]2s2

The electronic configuration of neutral beryllium and beryllium cation is written as follows:

  ElectronicconfigurationofBe:[2He]2s2ElectroniccofigurationofBe+:[2He]2s1

The beryllium atom has all subshells filled.  So, removing an electron requires more energy.  Hence, boron has lower first ionization energy.

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The reason for chlorine having lower first ionization energy than fluorine has to be given using electron configurations.

Explanation of Solution

The ionization energy is the energy required to remove the outermost electron in an atom.

  AA++e-

The electronic configuration of neutral chlorine and chlorine cation is written as follows:

  ElectronicconfigurationofCl:[10Ne]3s23p5ElectroniccofigurationofCl+:[10Ne]3s23p4

The electronic configuration of neutral fluorine and fluorine cation is written as follows:

  ElectronicconfigurationofF:[2He]2s22p5ElectroniccofigurationofF+:[2He]2s22p4

The electron from chlorine is removed from 3p orbital whereas in fluorine the electron is removed from 2p orbital.  Hence, chlorine has lower first ionization energy that fluorine.

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The reason for oxygen having lower first ionization energy than nitrogen has to be given using electron configurations.

Explanation of Solution

The ionization energy is the energy required to remove the outermost electron in an atom.

  AA++e-

The electronic configuration of neutral oxygen and oxygen cation is written as follows:

  ElectronicconfigurationofO:[2He]2s22p4ElectroniccofigurationofO+:[2He]2s22p3

The electronic configuration of neutral nitrogen and nitrogen cation is written as follows:

  ElectronicconfigurationofN:[2He]2s22p3ElectroniccofigurationofN+:[2He]2s22p2

The nitrogen atom attains half-filled p subshell, so removing an electron requires more energy.  Hence, oxygen has lower first ionization energy than nitrogen.

(e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The reason for iodine having lower electron affinity than bromine has to be given using electron configurations.

Explanation of Solution

Electron affinity is the energy required to add an electron to the neutral atom.

  A+e-A-

The electronic configuration of neutral iodine and iodine anion is written as follows:

  ElectronicconfigurationofI(Z=53):[36Kr]5s24d105p5ElectroniccofigurationofI-:[54Xe]

The electronic configuration of neutral bromine and bromine anion is written as follows:

  ElectronicconfigurationofBr (Z=35):[18Ar]4s23d104p5ElectroniccofigurationofBr-:[36Kr]

The electron added to bromine enters into 4p orbital and in iodine it enters into 5p orbital.  Hence, iodine has lower electron affinity than bromine.

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Chapter 5 Solutions

Chemistry: The Molecular Science

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