Answer Fluorine has the highest electro negativity. Explanation On moving down a group in the periodic table, the electro negativity decreases due to an increase in the distance between valence electron shell and the nucleus. Atomic number of F is 9 and Br is 36. Therefore, Fluorine has the highest electro negativity. Electronegativity value of Fluorine is 3.98 and that of Bromine is 2.96. (b) Interpretation Introduction Interpretation: Whether Fluorine or Bromine has the highest ionic radius needs to be determined. Concept introduction: Ionic radius can be defined as the radius of the ion in an atom. Answer Bromine has the highest ionic radius. Explanation On moving down a group in the periodic table, the ionic radius of elements increases. This is because the number of shells increases on moving down a group. Atomic number of F is 9 and Br is 36. Therefore, Bromine has the highest ionic radius. Ionic radius of Fluorine is 147 pm and ionic radius of Bromine is 185 pm. (c) Interpretation Introduction Interpretation: Whether Fluorine or Bromine has the highest atomic radius needs to be determined. Concept introduction: The atomic radius of a particular element is the measure of the atoms size. It can also be defined as the distance between its boundary and nucleus of the element. Answer Bromine has the highest atomic radius. Explanation On moving down a group in the periodic table, the atomic radius of elements increases. This is because the number of shells increases on moving down a group. Atomic number of F is 9 and Br is 36. Therefore, Bromine has the highest ionic radius. Atomic radius of Fluorine is 147 pm and atomic radiusof Bromine is 185 pm. (d) Interpretation Introduction Interpretation: Whether Fluorine or Bromine has the highest ionization energy needs to be determined. Concept introduction: Ionization energy can be defined as the measure of amount of energy needed to extract an electron form an atom or an ion. The energy to remove the first electron is termed as first ionization energy. Similarly, the energy required to remove the second electron is termed as second ionization energy. Answer Fluorine has the highest ionization energy. Explanation On moving down a group in the periodic table, the ionization energy decreases. This is because the distance between the valence electrons and nucleus is more and so they experience greater shielding. Atomic number of F is 9 and Br is 36. Fluorine has the highest ionization energy. Ionization energy of Fluorine is 17, 4228 and ionization energy of Bromine is 11, 8138.

Glencoe Chemistry: Matter and Change, Student Edition

1st Edition

ISBN: 9780076774609

Author: McGraw-Hill Education

Publisher: MCGRAW-HILL HIGHER EDUCATION

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Question

Chapter 6.3, Problem 21SSC

Interpretation Introduction

(a)

Interpretation:

Whether Fluorine or Bromine has the highest electro negativity needs to be determined.

Concept introduction:

The tendency of attracting pair of shared electrons towards it self by an atom is defined as electro negativity.

Expert Solution

Answer to Problem 21SSC

Fluorine has the highest electro negativity.

Explanation of Solution

On moving down a group in the periodic table, the electro negativity decreases due to an increase in the distance between valence electron shell and the nucleus. Atomic number of F is 9 and Br is 36.

Therefore, Fluorine has the highest electro negativity. Electronegativity value of Fluorine is 3.98 and that of Bromine is 2.96.

(b)

Interpretation Introduction

Interpretation:

Whether Fluorine or Bromine has the highest ionic radius needs to be determined.

Concept introduction:

Ionic radius can be defined as the radius of the ion in an atom.

(b)

Expert Solution

Answer to Problem 21SSC

Bromine has the highest ionic radius.

Explanation of Solution

On moving down a group in the periodic table, the ionic radius of elements increases. This is because the number of shells increases on moving down a group. Atomic number of F is 9 and Br is 36.

Therefore, Bromine has the highest ionic radius. Ionic radius of Fluorine is 147 pm and ionic radius of Bromine is 185 pm.

(c)

Interpretation Introduction

Interpretation:

Whether Fluorine or Bromine has the highest atomic radius needs to be determined.

Concept introduction:

The atomic radius of a particular element is the measure of the atoms size. It can also be defined as the distance between its boundary and nucleus of the element.

(c)

Expert Solution

Answer to Problem 21SSC

Bromine has the highest atomic radius.

Explanation of Solution

On moving down a group in the periodic table, the atomic radius of elements increases. This is because the number of shells increases on moving down a group. Atomic number of F is 9 and Br is 36.

Therefore, Bromine has the highest ionic radius. Atomic radius of Fluorine is 147 pm and atomic radiusof Bromine is 185 pm.

(d)

Interpretation Introduction

Interpretation:

Whether Fluorine or Bromine has the highest ionization energy needs to be determined.

Concept introduction:

Ionization energy can be defined as the measure of amount of energy needed to extract an electron form an atom or an ion. The energy to remove the first electron is termed as first ionization energy. Similarly, the energy required to remove the second electron is termed as second ionization energy.

(d)

Expert Solution

Answer to Problem 21SSC

Fluorine has the highest ionization energy.

Explanation of Solution

On moving down a group in the periodic table, the ionization energy decreases. This is because the distance between the valence electrons and nucleus is more and so they experience greater shielding. Atomic number of F is 9 and Br is 36.

Fluorine has the highest ionization energy. Ionization energy of Fluorine is 17, 4228 and ionization energy of Bromine is 11, 8138.

Chapter 6.3, Problem 20SSC

Chapter 6.3, Problem 22SSC

Chapter 6 Solutions

Glencoe Chemistry: Matter and Change, Student Edition

Ch. 6.1 - Prob. 1SSC Ch. 6.1 - Prob. 2SSC Ch. 6.1 - Prob. 3SSC Ch. 6.1 - Prob. 4SSC Ch. 6.1 - Prob. 5SSC Ch. 6.1 - Prob. 6SSC Ch. 6.1 - Prob. 7SSC Ch. 6.2 - Prob. 8PP Ch. 6.2 - Prob. 9PP Ch. 6.2 - Prob. 10PP

Ch. 6.2 - Prob. 11SSC Ch. 6.2 - Prob. 12SSC Ch. 6.2 - Prob. 13SSC Ch. 6.2 - Prob. 14SSC Ch. 6.2 - Prob. 15SSC Ch. 6.3 - Prob. 16PP Ch. 6.3 - Prob. 17PP Ch. 6.3 - Prob. 18PP Ch. 6.3 - Prob. 19PP Ch. 6.3 - Prob. 20SSC Ch. 6.3 - Prob. 21SSC Ch. 6.3 - Prob. 22SSC Ch. 6.3 - Prob. 23SSC Ch. 6.3 - Prob. 24SSC Ch. 6 - Prob. 25A Ch. 6 - Prob. 26A Ch. 6 - Prob. 27A Ch. 6 - Prob. 28A Ch. 6 - Prob. 29A Ch. 6 - Prob. 30A Ch. 6 - Prob. 31A Ch. 6 - Prob. 32A Ch. 6 - Prob. 33A Ch. 6 - Prob. 34A Ch. 6 - Prob. 35A Ch. 6 - Prob. 36A Ch. 6 - Prob. 37A Ch. 6 - Prob. 38A Ch. 6 - Prob. 39A Ch. 6 - Prob. 40A Ch. 6 - Prob. 41A Ch. 6 - Prob. 42A Ch. 6 - Prob. 43A Ch. 6 - Prob. 44A Ch. 6 - Prob. 45A Ch. 6 - Prob. 46A Ch. 6 - Prob. 47A Ch. 6 - Prob. 48A Ch. 6 - Prob. 49A Ch. 6 - Prob. 50A Ch. 6 - Prob. 51A Ch. 6 - Prob. 52A Ch. 6 - Prob. 53A Ch. 6 - Prob. 54A Ch. 6 - Prob. 55A Ch. 6 - Prob. 56A Ch. 6 - Prob. 57A Ch. 6 - Prob. 58A Ch. 6 - Prob. 59A Ch. 6 - Prob. 60A Ch. 6 - Prob. 61A Ch. 6 - Prob. 62A Ch. 6 - Prob. 63A Ch. 6 - Prob. 64A Ch. 6 - Prob. 65A Ch. 6 - Prob. 66A Ch. 6 - Prob. 67A Ch. 6 - Prob. 68A Ch. 6 - Prob. 69A Ch. 6 - Prob. 70A Ch. 6 - Prob. 71A Ch. 6 - Prob. 72A Ch. 6 - Prob. 73A Ch. 6 - Prob. 74A Ch. 6 - Prob. 75A Ch. 6 - Prob. 76A Ch. 6 - Prob. 77A Ch. 6 - Prob. 78A Ch. 6 - Prob. 79A Ch. 6 - Prob. 80A Ch. 6 - Prob. 81A Ch. 6 - Prob. 82A Ch. 6 - Prob. 83A Ch. 6 - Prob. 84A Ch. 6 - Prob. 85A Ch. 6 - Prob. 86A Ch. 6 - Prob. 87A Ch. 6 - Prob. 88A Ch. 6 - Prob. 89A Ch. 6 - Prob. 90A Ch. 6 - Prob. 91A Ch. 6 - Prob. 92A Ch. 6 - Prob. 93A Ch. 6 - Prob. 94A Ch. 6 - Prob. 95A Ch. 6 - Prob. 96A Ch. 6 - Prob. 97A Ch. 6 - Prob. 98A Ch. 6 - Prob. 99A Ch. 6 - Prob. 100A Ch. 6 - Prob. 1STP Ch. 6 - Prob. 2STP Ch. 6 - Prob. 3STP Ch. 6 - Prob. 4STP Ch. 6 - Prob. 5STP Ch. 6 - Prob. 6STP Ch. 6 - Prob. 7STP Ch. 6 - Prob. 8STP Ch. 6 - Prob. 9STP Ch. 6 - Prob. 10STP Ch. 6 - Prob. 11STP Ch. 6 - Prob. 12STP Ch. 6 - Prob. 13STP Ch. 6 - Prob. 14STP Ch. 6 - Prob. 15STP Ch. 6 - Prob. 16STP Ch. 6 - Prob. 17STP Ch. 6 - Prob. 18STP Ch. 6 - Prob. 19STP

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Knowledge Booster

(a) Interpretation: Whether Fluorine or Bromine has the highest electro negativity needs to be determined. Concept introduction: The tendency of attracting pair of shared electrons towards it self by an atom is defined as electro negativity.

(a) Interpretation: Whether Fluorine or Bromine has the highest electro negativity needs to be determined. Concept introduction: The tendency of attracting pair of shared electrons towards it self by an atom is defined as electro negativity.

Answer to Problem 21SSC

Explanation of Solution

Interpretation: Whether Fluorine or Bromine has the highest ionic radius needs to be determined. Concept introduction: Ionic radius can be defined as the radius of the ion in an atom.

Answer to Problem 21SSC

Explanation of Solution

Interpretation: Whether Fluorine or Bromine has the highest atomic radius needs to be determined. Concept introduction: The atomic radius of a particular element is the measure of the atoms size. It can also be defined as the distance between its boundary and nucleus of the element.

Answer to Problem 21SSC

Explanation of Solution

Answer to Problem 21SSC

Explanation of Solution

Chapter 6 Solutions

Additional Science Textbook Solutions

(a)

Interpretation:

Whether Fluorine or Bromine has the highest electro negativity needs to be determined.

Concept introduction:

The tendency of attracting pair of shared electrons towards it self by an atom is defined as electro negativity.

Interpretation:

Whether Fluorine or Bromine has the highest ionic radius needs to be determined.

Concept introduction:

Ionic radius can be defined as the radius of the ion in an atom.

Interpretation:

Whether Fluorine or Bromine has the highest atomic radius needs to be determined.

Concept introduction:

The atomic radius of a particular element is the measure of the atoms size. It can also be defined as the distance between its boundary and nucleus of the element.