The given ionization energy has to be matched with the given electronic configuration of atoms. Concept Introduction: An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy . If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy . If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases. The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding. To compare: the ionization energies with the electronic configuration given

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Answer 1

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Chapter 4, Problem 4.55QP

Interpretation Introduction

Interpretation: The given ionization energy has to be matched with the given electronic configuration of atoms.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To compare: the ionization energies with the electronic configuration given

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Answer 2

Question

Chapter 4, Problem 4.55QP

Interpretation Introduction

Interpretation: The given ionization energy has to be matched with the given electronic configuration of atoms.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To compare: the ionization energies with the electronic configuration given

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Answer 3

Question

Chapter 4, Problem 4.55QP

Interpretation Introduction

Interpretation: The given ionization energy has to be matched with the given electronic configuration of atoms.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To compare: the ionization energies with the electronic configuration given

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Answer 4

Question

Chapter 4, Problem 4.55QP

Interpretation Introduction

Interpretation: The given ionization energy has to be matched with the given electronic configuration of atoms.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To compare: the ionization energies with the electronic configuration given

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Answer 5

Chapter 4, Problem 4.55QP

Interpretation Introduction

Interpretation: The given ionization energy has to be matched with the given electronic configuration of atoms.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To compare: the ionization energies with the electronic configuration given

Answer 6

Chapter 4, Problem 4.55QP

Interpretation Introduction

Interpretation: The given ionization energy has to be matched with the given electronic configuration of atoms.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To compare: the ionization energies with the electronic configuration given

Answer 7

Chapter 4, Problem 4.55QP

Interpretation Introduction

Interpretation: The given ionization energy has to be matched with the given electronic configuration of atoms.

Concept Introduction:

An atom can be converted into an ion by removing an electron from its outermost shell or adding electron to the outermost shell. An amount of energy is required to remove an electron from the outermost shell of an atom to form a cation. The minimum energy required for removing an electron from an atom in gaseous phase is known as ionization energy.

If one electron is removed from the atom to form a cation, the energy required is known as first ionization energy. If another electron is removed from the formed ion, the energy required is known as second ionization energy and this goes on. Second ionization energy is always higher than the first ionization energy because the effective nuclear charge increases.

The trend followed in a periodic table for ionization energy is, it increases across the period and decreases down the group. This is because; across the period, the electrons are added to the same orbital and hence decrease in shielding. However, down the group, the electrons are added to a new sub-shell and hence increase in shielding.

To compare: the ionization energies with the electronic configuration given

Answer 8

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Answer 11

Ch. 4.1 - Prob. 4.1WE Ch. 4.1 - Prob. 1PPA Ch. 4.1 - Prob. 1PPB Ch. 4.1 - Prob. 1PPC Ch. 4.1 - Prob. 4.1.1SR Ch. 4.1 - Prob. 4.1.2SR Ch. 4.1 - Prob. 4.1.3SR Ch. 4.2 - Prob. 4.2WE Ch. 4.2 - Without using a periodic table, give the...Ch. 4.2 - Identify the elements represented by (a)...

Solution Summary: The author compares the ionization energy with the electronic configuration of atoms.

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