a. The trend of first ionization energies from left to right in 3 rd period across the periodic table. b. The reason of having low 1 st ionization energy in case of Al as comparison to Mg and similarly, S having 1 st ionization energy than P . c. The trend of electron affinities from left to right in 3 rd period across the periodic table. d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si . e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

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Answer 1

Question

Chapter 3, Problem 141E

Interpretation Introduction

To determine:

a. The trend of first ionization energies from left to right in 3^rd period across the periodic table.

b. The reason of having low 1^st ionization energy in case of Al as comparison to Mg and similarly, S having 1^st ionization energy than P.

c. The trend of electron affinities from left to right in 3^rd period across the periodic table.

d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si.

e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

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Answer 2

Question

Chapter 3, Problem 141E

Interpretation Introduction

To determine:

a. The trend of first ionization energies from left to right in 3^rd period across the periodic table.

b. The reason of having low 1^st ionization energy in case of Al as comparison to Mg and similarly, S having 1^st ionization energy than P.

c. The trend of electron affinities from left to right in 3^rd period across the periodic table.

d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si.

e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

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Answer 3

Question

Chapter 3, Problem 141E

Interpretation Introduction

To determine:

a. The trend of first ionization energies from left to right in 3^rd period across the periodic table.

b. The reason of having low 1^st ionization energy in case of Al as comparison to Mg and similarly, S having 1^st ionization energy than P.

c. The trend of electron affinities from left to right in 3^rd period across the periodic table.

d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si.

e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

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Answer 4

Question

Chapter 3, Problem 141E

Interpretation Introduction

To determine:

a. The trend of first ionization energies from left to right in 3^rd period across the periodic table.

b. The reason of having low 1^st ionization energy in case of Al as comparison to Mg and similarly, S having 1^st ionization energy than P.

c. The trend of electron affinities from left to right in 3^rd period across the periodic table.

d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si.

e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

Expert Solution & Answer

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Answer 5

Chapter 3, Problem 141E

Interpretation Introduction

To determine:

a. The trend of first ionization energies from left to right in 3^rd period across the periodic table.

b. The reason of having low 1^st ionization energy in case of Al as comparison to Mg and similarly, S having 1^st ionization energy than P.

c. The trend of electron affinities from left to right in 3^rd period across the periodic table.

d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si.

e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

Answer 6

Chapter 3, Problem 141E

Interpretation Introduction

To determine:

a. The trend of first ionization energies from left to right in 3^rd period across the periodic table.

b. The reason of having low 1^st ionization energy in case of Al as comparison to Mg and similarly, S having 1^st ionization energy than P.

c. The trend of electron affinities from left to right in 3^rd period across the periodic table.

d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si.

e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

Answer 7

Chapter 3, Problem 141E

Interpretation Introduction

To determine:

a. The trend of first ionization energies from left to right in 3^rd period across the periodic table.

b. The reason of having low 1^st ionization energy in case of Al as comparison to Mg and similarly, S having 1^st ionization energy than P.

c. The trend of electron affinities from left to right in 3^rd period across the periodic table.

d. The reason of having more positive electron affinity in case of Mg as comparison to Na and similarly, P is more positive than Si.

e. The overall energy change, when one electron form Na is removed, and that electron is added to Cl and identify whether the exchange of electron is exothermic or endothermic.

Answer 8

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Answer 9

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Answer 10

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Answer 11

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Solution Summary: The author analyzes the trend of first ionization energies from left to right in 3 rd period across the periodic table.

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Chapter 3 Solutions