On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained. Conceptual Introduction: Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation. Ionization energy increases across the period as across the group, electrons start getting added. It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron. Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

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Answer 1

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Chapter 7, Problem 92QP

Interpretation Introduction

Interpretation:

On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained.

Conceptual Introduction:

Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation.

Ionization energy increases across the period as across the group, electrons start getting added.

It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron.

Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

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Answer 2

Question

Chapter 7, Problem 92QP

Interpretation Introduction

Interpretation:

On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained.

Conceptual Introduction:

Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation.

Ionization energy increases across the period as across the group, electrons start getting added.

It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron.

Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

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Answer 3

Question

Chapter 7, Problem 92QP

Interpretation Introduction

Interpretation:

On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained.

Conceptual Introduction:

Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation.

Ionization energy increases across the period as across the group, electrons start getting added.

It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron.

Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

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Answer 4

Question

Chapter 7, Problem 92QP

Interpretation Introduction

Interpretation:

On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained.

Conceptual Introduction:

Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation.

Ionization energy increases across the period as across the group, electrons start getting added.

It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron.

Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

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Answer 5

Chapter 7, Problem 92QP

Interpretation Introduction

Interpretation:

On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained.

Conceptual Introduction:

Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation.

Ionization energy increases across the period as across the group, electrons start getting added.

It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron.

Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

Answer 6

Chapter 7, Problem 92QP

Interpretation Introduction

Interpretation:

On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained.

Conceptual Introduction:

Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation.

Ionization energy increases across the period as across the group, electrons start getting added.

It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron.

Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

Answer 7

Chapter 7, Problem 92QP

Interpretation Introduction

Interpretation:

On the basis of electronic configuration, the given statement â€˜More energy is required to remove an electron from a bromine atom than from an iodine atomâ€™ is to be explained.

Conceptual Introduction:

Ionization energy.is the minimum energy that is required to remove an outermost electron from an isolated gaseous atom to convert it into gaseous cation.

Ionization energy increases across the period as across the group, electrons start getting added.

It increases the effective nuclear charge on the last electron and hence, a large amount of energy is required to remove an electron.

Ionization energy decreases down the group as down the group, a new shell is getting added which increases the distance of the last electron from the nucleus and hence, low amount of energy is required to remove the electron.

Answer 8

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Answer 9

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Answer 11

Ch. 7 - Prob. 1QC Ch. 7 - Prob. 2QC Ch. 7 - Prob. 3QC Ch. 7 - Prob. 4QC Ch. 7 - Prob. 5QC Ch. 7 - Prob. 6QC Ch. 7 - Prob. 7QC Ch. 7 - Prob. 1PP Ch. 7 - Prob. 2PP Ch. 7 - Prob. 3PP

Solution Summary: The author explains that more energy is required to remove an electron from a bromine atom than from an iodine

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