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Explain each answer briefly. (a) Rank the following in order of increasing atomic radius: O, S, and F. (b) Which has the largest ionization energy: P, Si, S, or Se? (c) Place the following in order of increasing radius: O 2− , N 3− , and F − . (d) Place the following in order of increasing ionization energy: Cs, Sr, and Ba.

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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 7, Problem 32PS
Textbook Problem
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Explain each answer briefly.

  1. (a) Rank the following in order of increasing atomic radius: O, S, and F.
  2. (b) Which has the largest ionization energy: P, Si, S, or Se?
  3. (c) Place the following in order of increasing radius: O2−, N3−, and F.
  4. (d) Place the following in order of increasing ionization energy: Cs, Sr, and Ba.

a)

Interpretation Introduction

Interpretation:    

The increasing order of atomic radius has to be predicted.

Concept Introduction:

Atomic radius: The concept explain chemical element is a measured of the size of its atoms, in other words to measure the distance from the center of the nucleus to the boundary of the surrounding cloud of number of electrons.

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)

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.

Explanation of Solution

  • Analyze increasing atomic radius values of Oxygen, Sulfur and Fluorine atoms.

Generally, atomic radii increase across a period table (move to right to left) and decreases down the group. Oxygen and Fluorine belong to same period; as per the rule, the atomic size of Oxygen is less than Fluorine. The Sulfur is located below oxygen in the same group; the atomic size of Sulfur is larger than Oxygen.

 The images of atomic radius (Figure-1) are shown below.

    

b)

Interpretation Introduction

Interpretation:    

The largest ionization energy has to be predicted.

Concept Introduction:

Atomic radius: The concept explain chemical element is a measured of the size of its atoms, in other words to measure the distance from the center of the nucleus to the boundary of the surrounding cloud of number of electrons.

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)

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.

c)

Interpretation Introduction

Interpretation:    

Increasing order of radius has to be ranked.

Concept Introduction:

Atomic radius: The concept explain chemical element is a measured of the size of its atoms, in other words to measure the distance from the center of the nucleus to the boundary of the surrounding cloud of number of electrons.

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)

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.

d)

Interpretation Introduction

Interpretation:    

The increasing order of ionization energy has to be ranked.

Concept Introduction:

Atomic radius: The concept explain chemical element is a measured of the size of its atoms, in other words to measure the distance from the center of the nucleus to the boundary of the surrounding cloud of number of electrons.

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)

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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Chapter 7 Solutions

Chemistry & Chemical Reactivity
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