The reason for the increase in chemical reactivity from top to bottom in group 1A and 2A” should be explained. Concept introduction: The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases. Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

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Answer 1

Question

Chapter 22, Problem 22.81SP

Interpretation Introduction

Interpretation:

The reason for the increase in chemical reactivity from top to bottom in group 1A

and 2A”

should be explained.

Concept introduction:

The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases.

Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

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Answer 2

Question

Chapter 22, Problem 22.81SP

Interpretation Introduction

Interpretation:

The reason for the increase in chemical reactivity from top to bottom in group 1A

and 2A”

should be explained.

Concept introduction:

The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases.

Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

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See solution

Answer 3

Question

Chapter 22, Problem 22.81SP

Interpretation Introduction

Interpretation:

The reason for the increase in chemical reactivity from top to bottom in group 1A

and 2A”

should be explained.

Concept introduction:

The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases.

Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

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Answer 4

Question

Chapter 22, Problem 22.81SP

Interpretation Introduction

Interpretation:

The reason for the increase in chemical reactivity from top to bottom in group 1A

and 2A”

should be explained.

Concept introduction:

The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases.

Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

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Check out a sample textbook solution

See solution

Answer 5

Chapter 22, Problem 22.81SP

Interpretation Introduction

Interpretation:

The reason for the increase in chemical reactivity from top to bottom in group 1A

and 2A”

should be explained.

Concept introduction:

The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases.

Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

Answer 6

Chapter 22, Problem 22.81SP

Interpretation Introduction

Interpretation:

The reason for the increase in chemical reactivity from top to bottom in group 1A

and 2A”

should be explained.

Concept introduction:

The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases.

Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

Answer 7

Chapter 22, Problem 22.81SP

Interpretation Introduction

Interpretation:

The reason for the increase in chemical reactivity from top to bottom in group 1A

and 2A”

should be explained.

Concept introduction:

The energy which is required to remove an electron from a gaseous atom or ion is called Ionization energy. Generally, in the periodic table; ionization energy increases from left to right across period and, in the group it decreases.

Atomic radius decreases in going from left to right across a period. This decrease in atomic radius results due to the increase in effective nuclear charge on going from left to right. This implies that the valence electrons are close to the nucleus, thus, the size of atom decreases. Due to increase in the orbital size and principal quantum levels, atomic radius increases from top to bottom.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 22 - Prob. 22.1P Ch. 22 - Prob. 22.2A Ch. 22 - Prob. 22.3P Ch. 22 - Prob. 22.4CA Ch. 22 - Prob. 22.5P Ch. 22 - Prob. 22.6P Ch. 22 - Prob. 22.7A Ch. 22 - Prob. 22.8CP Ch. 22 - Prob. 22.9A Ch. 22 - Prob. 22.10P

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Chapter 22 Solutions