From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy ( IE 2 ) should be determined. Concept Introduction: Periodic Table: The available chemical elements are arranged considering their atomic number , the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table. In periodic table the horizontal rows are called periods and the vertical column are called group . The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements. The s and p block elements together are called as main group elements. The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table. There are seven periods and 18 groups present in the table and some of those groups are given special name as follows, Group-1 → Alkali metal Group-2 → Alkaline metals Group-16 → Chalcogens Group-17 → Halogens Group-18 → Noble gases Cation: Removal of electron from the atom results to form positively charged ion called cation. Anion: Addition of electron to atom results to form negatively charged ion called anion. The net charge present in the element denotes the presence or absence of electrons in the element. First ionization energy: The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge. atom ( g ) → ion with positive charge ( g ) + electron Second ionization energy: Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization. Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z . The superscript presents on the left side of the symbol of the element.

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Answer 1

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Chapter 4.4, Problem 4.4.2SR

Interpretation Introduction

Interpretation: From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy (IE2) should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

atom(g) → ion with positive charge(g) + electron

Second ionization energy:

Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.

Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

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Answer 2

Question

Chapter 4.4, Problem 4.4.2SR

Interpretation Introduction

Interpretation: From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy (IE2) should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

atom(g) → ion with positive charge(g) + electron

Second ionization energy:

Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.

Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

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Answer 3

Question

Chapter 4.4, Problem 4.4.2SR

Interpretation Introduction

Interpretation: From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy (IE2) should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

atom(g) → ion with positive charge(g) + electron

Second ionization energy:

Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.

Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

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Answer 4

Question

Chapter 4.4, Problem 4.4.2SR

Interpretation Introduction

Interpretation: From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy (IE2) should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

atom(g) → ion with positive charge(g) + electron

Second ionization energy:

Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.

Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

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Answer 5

Chapter 4.4, Problem 4.4.2SR

Interpretation Introduction

Interpretation: From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy (IE2) should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

atom(g) → ion with positive charge(g) + electron

Second ionization energy:

Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.

Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Answer 6

Chapter 4.4, Problem 4.4.2SR

Interpretation Introduction

Interpretation: From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy (IE2) should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

atom(g) → ion with positive charge(g) + electron

Second ionization energy:

Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.

Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Answer 7

Chapter 4.4, Problem 4.4.2SR

Interpretation Introduction

Interpretation: From the given choices the correct choice that contains given elements in the order of their increasing second ionization energy (IE2) should be determined.

Concept Introduction:

Periodic Table: The available chemical elements are arranged considering their atomic number, the electronic configuration and their properties. The elements placed on the left of the table are metals and non-metals are placed on right side of the table.

In periodic table the horizontal rows are called periods and the vertical column are called group.

The elements placed on the left of the table are metals which contain its last electron on s-orbital hence considered as s-block elements and the elements placed on the right side of the table contains its last electron in p-orbital which is regarded as p-block elements.

The s and p block elements together are called as main group elements.

The elements with its last electron in d-orbital are called d-block elements also called as transition elements and elements with its last electron in f-orbital are called as inner-transition elements which are usually placed at the bottom of the periodic table.

There are seven periods and 18 groups present in the table and some of those groups are given special name as follows,

Group-1→Alkali metalGroup-2→Alkaline metalsGroup-16→ChalcogensGroup-17→HalogensGroup-18→Noble gases

Cation: Removal of electron from the atom results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The net charge present in the element denotes the presence or absence of electrons in the element.

First ionization energy:

The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.

atom(g) → ion with positive charge(g) + electron

Second ionization energy:

Repeating the same process that is removal of another electron that is second electron from the resulting ion of first ionization is called second ionization.

Atomic Number: Atomic number of the element is equal to the number of protons presents in nucleus of the element which is denoted by symbol Z. The superscript presents on the left side of the symbol of the element.

Answer 8

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Answer 10

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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 explains the periodic table's atomic number, electronic configuration, and properties. The ionization energy is the minimum energy required to remove the electron from the atom.

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